Allioa 1 4 5 7 5 ^

NA1

iiLi IN®T STANDARDS & TECH R.I.C.

All 102145759

/NSRDS-NBS

1964 PLICATIONS

*°*tAU Of * NSRDS-NBS 51

U.S. DEPARTMENT OF COMMERCE / National Bureau of Standards

(Site

too

513

\o.5

1

<t15

N SRP S

Selected

Specific Rates of Reactions

of Transients from Water

in Aqueous Solution.

II. Hydrogen Atom

Hi
NATIONAL BUREAU OF STANDARDS

The National Bureau of Standards 1 was established by an act of Congress March 3, 1901. The Bureau’s overall goal is to strengthen and advance the Nation’s science and technology

and facilitate their effective application for public benefit. To this end, the Bureau conducts

research and provides: (1) a basis for the Nation's physical measurement system, (2) scientific and technological services for industry and government, (3) a technical basis for equity in trade,

and (4) technical services to promote public safety. The Bureau consists of the Institute for Basic Standards, the Institute for Materials Research, the Institute for Applied Technology,

the Institute for Computer Sciences and Technology, and the Office for Information Programs.

THE INSTITUTE FOR BASIC STANDARDS provides the central basis within the United

States of a complete and consistent system of physical measurement; coordinates that system

with measurement systems of other nations; and furnishes essential services leading to accurate and uniform physical measurements throughout the Nation’s scientific community, industry,

and commerce. The Institute consists of a Center for Radiation Research, an Office of Measurement Services and the following divisions: Applied Mathematics — Electricity — Mechanics — Heat — Optical Physics — Nuclear

Sciences 2 — Applied Radiation 2 — Quantum Electronics 3 — Electromagnetics 3 — Time

and Frequency 3 — Laboratory Astrophysics 3 — Cryogenics 3

. THE INSTITUTE FOR MATERIALS RESEARCH conducts materials research leading to improved methods of measurement, standards, and data on the properties of well-characterized

materials needed by industry, commerce, educational institutions, and Government; provides

advisory and research services to other Government agencies; and develops, produces, and

distributes standard reference materials. The Institute consists of the Office of Standard

Reference Materials and the following divisions: Analytical Chemistry — Polymers — Metallurgy — Inorganic Materials — Reactor

Radiation — Physical Chemistry.

THE INSTITUTE FOR APPLIED TECHNOLOGY provides technical services to promote

the use of available technology and to facilitate technological innovation in industry and

Government; cooperates with public and private organizations leading to the development of

technological standards (including mandatory safety standards), codes and methods of test; and provides technical advice and services to Government agencies upon request. The Institute consists of a Center for Building Technology and the following divisions and offices: Engineering and Product Standards — Weights and Measures — Invention and Innovation Product Evaluation Technology — Electronic Technology — Technical Analysis — Measurement Engineering — Structures, Materials, and Life Safety 4 — Building

Environment * — Technical Evaluation and Application 4 — Fire Technology.

THE INSTITUTE FOR COMPUTER SCIENCES AND TECHNOLOGY conducts research and provides technical services designed to aid Government agencies in improving cost effec- tiveness in the conduct of their programs through the selection, acquisition, and effective

utilization of automatic data processing equipment; and serves as the principal focus within the executive branch for the development of Federal standards for automatic data processing

equipment, techniques, and computer languages. The Institute consists of the following

divisions: Computer Services — Systems and Software — Computer Systems Engineering — Information Technology.

THE OFFICE FOR INFORMATION PROGRAMS promotes optimum dissemination and

accessibility of scientific information generated within NBS and other agencies of the Federal

government; promotes the development of the National Standard Reference Data System and

a system of information analysis centers dealing with , the broader aspects of the National

Measurement System; provides appropriate services to ensure that the NBS staff has optimum

accessibility to the scientific information of the world. The Office consists of the following

organizational units: Office of Standard Reference Data — Office of Information Activities — Office of Technical

Publications — Library — Office of International Relations.

* Headquarters and Laboratories at Gaithersburg, Maryland, unless otherwise noted; mailing address Washington, D.C. 20234. *

2 Part of the Center for Radiation Research.

3 Located at Boulder, Colorado 80302.

4 Part of the Center for Building Technology.
rtrt tiurUi toojiLhu . JUL 8 1975

n'-

Gc. loo

, US ')

3

r'€’.S' I Iq7<r

C.3-

Selected Specific Rates of

Reactions of Transients From Water

in Aqueous Solution.

II. Hydrogen Atom *

Michael Anbar

Stanford Research Institute,

Menlo Park, Calif. 94025

and

Farhataziz and Alberta B. Ross

Radiation Chemistry Data Center,

Radiation Laboratory,

University of Notre Dame,

Notre Dame, Ind. 46556

U.S. DEPARTMENT OF COMMERCE

NATIONAL BUREAU OF STANDARDS, Richard W. Roberts, Director

Issued May 1975
Library of Congress Catalog Number: 73-600329

NSRDS-NBS 51

Nat. Stand. Ref. Data Ser., Nat. Bur. Stand. (U.S.), 51, 56 pages (May 1975)

CODEN: NSRDAP

© 1975 by the Secretary of Commerce on Behalf of the United States Government

U.S. GOVERNMENT PRINTING OFFICE

WASHINGTON: 1975

For sale by the Superintendent of Documents, U.S. Government Printing Office, Washington, D.C. 20402

(Order by SD Catalog No. 03.48:51). Price $1.20
Foreword

The National Standard Reference Data System provides access to the quantitative data of physical science, critically evaluated and compiled for convenience and readily accessible through a

variety of distribution channels. The System was established in 1963 by action of the President’s

Office of Science and Technology and the Federal Council for Science and Technology, and

responsibility to administer it was assigned to the National Bureau of Standards.

NSRDS receives advice and planning assistance from a Review Committee of the National

Research Council of the National Academy of Sciences-National Academy of Engineering. A number of Advisory Panels, each concerned with a single technical area, meet regularly to examine

major portions of the program, assign relative priorities, and identify specific key problems in need of further attention. For selected specific topics, the Advisory Panels sponsor subpanels

which make detailed studies of users’ needs, the present state of knowledge, and existing data re- sources as a basis for recommending one or more data compilation activities. This assembly of advisory services contributes greatly to the guidance of NSRDS activities. The System now includes a complex of data centers and other activities in academic insti- tutions and other laboratories. Components of the NSRDS produce compilations of critically

evaluated data, reviews of the state of quantitative knowledge in specialized areas, and computations of useful functions derived from standard reference data. The centers and projects also establish criteria for evaluation and compilation of data and recommend improvements in ex- perimental techniques. They are normally associated with research in the relevant field. The technical scope of NSRDS is indicated by the categories of projects active or being

planned : nuclear properties, atomic and molecular properties, solid state properties, thermodynamic and transport properties, chemical kinetics, and colloid and surface properties.

Reliable data on the properties of matter and materials is a major foundation of scientific and technical progress. Such important activities as basic scientific research, industrial quality control, development of new materials for building and other technologies, measuring and correcting

environmental pollution depend on quality reference data. In NSRDS, the Bureau’s responsibility

to support American science, industry, and commerce is vitally fulfilled.

Richard W. Roberts, Director

III
Preface

This report is one of a series of data publications on radiation chemistry; the aim of the series

is to compile, evaluate, and present the numerical results on processes occurring in systems which

have been subjected to ionizing radiation. Various kinds of data are important in radiation chemistry. The quantities which were measured first were the observed radiation yields or G values (molecules formed or destroyed per 100 eV). Various indirect methods based on G values have been used to determine yields of transient species and relative rates of reactions. The spectral properties (optical,

electron spin resonance) of transients have provided a direct method for their identification, and rates of thfe very fast reactions of transients which occur in irradiated systems have been measured directly

by spectroscopic methods. Conductivity and luminescence methods have also provided a means of

measuring properties of transients and their kinetics. Some reactions which occur in irradiated systems

have also been studied by other methods, such as photochemistry, electric discharge, ultrasonics, chemical initiation, electron impact, etc. The emphasis in these publications is on the data of radiation

chemistry, but where other pertinent data exist, they are included.

The data of radiation chemistry are voluminous; thousands of systems have been investigated.

As a result there are certain collections, e.g. rate constants of particular types of reactions or certain

properties of transients, for which tabulations of the data are considered essential, but for which

critical assessment of each value is impossible. On the other hand, certain systems and properties

have been studied so extensively that critical examination of these data is desirable and timely.

Authors of this series of data publications have been asked to evaluate the extent to which the data can be critically assessed, to describe their criteria for evaluation, and to designate preferred values

whenever possible.

IV
Contents

Page Foreword Ill Preface IV

Introduction 1 Table 1. Values of k used for normalizing relative rates 4

Table 2. Reactions of H with transients from water (2.1-2.4K 5

Table 3. Reactions of H with inorganic solutes (2.5-2.103) 7

Table 4. Reactions of H with organic solutes (2.104-2.388) 16

Formula Index. 46

References 50

V

Selected Specific Rates of Reactions of Transients

from Water in Aqueous Solution

II. Hydrogen Atom

Michael Anbar

Stanford Research Institute, Menlo Park, Calif. 94025 Farhataziz and Alberta B. Ross

Radiation Chemistry Data Center , Radiation Laboratory ,* University of Notre Dame, Notre Dame, Ind . 46556

Rates of reactions of hydrogen atoms (from radiolysis of water and other sources) with organic

and inorganic molecules, ions, and transients in aqueous solution have been tabulated. Directly

measured rates obtained by kinetic spectroscopy or conductimetric methods, and relative rates determined by competition kinetics are included.

Key words: Aqueous solution; chemical kinetics; data compilation; hydrogen atom; radiation chemistry; rates.

Introduction

The radiolysis of water yields three major intermediates: the hydrogen atom, the hydrated electron,

and the hydroxyl radical. Tables of rates of hydrated electron reactions comprise part I of this series (73

0030). This compilation contains tables of rates of hydrogen atom reactions in aqueous solution and covers

the literature through 1972. The rate data for the hydroxyl radical have been compiled and will be

published in part III of this series.

The hydrogen atom is the simplest chemical species, carrying a single electron. Being such a fundamental entity, its reactivity with other chemical species is of special interest to theoretical chemists

as well as to anyone involved in the research of mechanisms of chemical reactions. In addition, the

hydrogen atom is one of the important products of the radiolysis of water and its reactivity determines,

therefore, the behavior of radiolyzed systems. As such the hydrogen atom reactions are of great importance

to .radiation chemists and radiobiologists.

The chemical behavior of hydrogen atoms may be summarized in the following examples:

H + Br2 —> HBr + Br (abstraction)

H + CH3 CH2 OH —» H2 + CH3CHOH (abstraction)

H + CH2 =CH-CH2 CH3 CH3 CHCH2 CH3 (addition)

H + C6 H6 —> C 6 H7 (addition)

H + H —> H2 (radical combination)

*The Radiation Laboratory is operated under contract with The Atomic Energy Commission. The work of the Center is supported jointly by The National Bureau of Standards,

Office of Standard Reference Data and The Atomic Energy Commission. This is AEC Document COO-38-815.

1
H + 02 -> H02 (addition)

H + Cu2+ —» Cu+ + H

+ (charge transfer)

H + OH" — + H2 0

These reacuons include abstraction reactions, some of which — like hydrogen abstraction — may be

defined as oxidation processes. Additions to double bonds or aromatic rings and to free radicals or biradicals may be considered as reducing processes. The third category of H atom reactions are reduction

processes which proceed probably via electron transfer mechanisms. Finally there are the H + OH- and H +

F" reactions which yield hydrated electrons and which have no simple analog in chemistry.

In acid solutions hydrated electrons are converted into hydrogen atoms,

+ H

+ -> H.q

with a specific rate of 2.3 x 10 10 dm3 /mol*s. In alkaline solutions hydrogen atoms are converted into

hydrated electrons (see 2.90);

H + OH' -* e;

q

thus, the amount of H present in strongly alkaline solutions is very small, but irradiated acidic and neutral

aqueous solutions contain hydrogen atoms which react with each other, with other transients from water,

and with organic and inorganic materials in the solution. A large number of such reactions have been

studied, although the number of H atom reactions for which rates are available is less than the nearly 700

e~q reactions listed in part I. One reason for the larger number of hydrated electron rates is the ease of

their direct measurement by kinetic spectroscopy. Hydrogen atom reactions have been studied in a number

of ways, but only a few of the data have been obtained by direct methods.

Methods for Specific Rate Determination

Generation of H by pulse radiolysis of aqueous solutions and direct observations of the hydrogen atom

by esr or optical spectroscopy, by conductivity methods, as well as by measurements on transients produced

by H addition or abstraction, can be used in some cases to determine rates. The reaction H + H —» H2 has been measured directly by following the decay of the optical

absorption of the hydrogen atom at 200 nm. The rate law is -d[H]/dt = 2k[H]2. In this compilation, values

of k are reported. In other cases, absolute specific rates of reactions have been measured by following the

growth of the optical absorption signal due to a product of the reaction. For reactions, where none of the

products has optical absorption, the relative rates have been measured by competition with reactions which

produce products with optical absorption. Interference by OH, or transients from OH reactions, must be

avoided in all optical studies by removing the OH from the solution. Alcohols such as /er/-butanol and

CD3 OH, which react much more slowly with H than with OH, have been used as scavengers for OH:

another method for removing OH is saturation with H2 at high pressures which converts OH to H hv the

reaction OH + H2 —» H + H20.

The esr signals of hydrogen atoms are observed in irradiated aqueous solutions as a result of their

enhancement by spin polarization effects. These signals decrease with time because of relaxation

processes. This relaxation has been used to measure relative and absolute rates of reactions of the

hydrogen atom bv steady state and pulse radiolysis, respectively.

There are about 60 reacuons in these tables for which specific rates have been determined directly;

the rates are listed in the column under k. More commonly, the kinetics of reactions of H are studied

indirectly by steady state radiolysis, or in a few cases by atomized hydrogen gas flow techniques, by

comparing measurements made on two reactants. The result is a ratio of rate constants obtained by

analyzing the data assuming a kinetic mechanism. The majority of the nearly 400 reactions in these table?

list relative rates which have been determined by competition kinetics, either by steady state or pulse

techniques. The measured rate ratios are included in the column under Ratio and are given in the form

2
k/kx , where kx

is k{ H + X) and X is the competing reactant. Certain values of k have been chosen for

normalization of the relative data; those values are listed in table 1. Values of k are calculated from the

ratios using those values and are designated as relative (rel.). The values listed in table 1 have been chosen

either because they are directly measured values or because they give the best agreement among various

values of relative rates. These values, some of which had to be chosen arbitrarily, are not presented as recommended values and are open for revision.

Abbreviations used for X, and other abbreviations and symbols used in the tables, are collected at the

end of this section.

Arrangement of Tables

Arrangement of these tables is similar to the arrangement in part I; reactions of H with other

transients from water are in table 2. Reactions of H with inorganic solutes are listed in table 3 in

alphabetical order by main element. Reactions of H with organic solutes are listed in table 4 in alphabetical

order by name. In most cases IUPAC nomenclature has been used. All reported values of specific rates have been included except when a measurement has been superseded by a more reliable measurement by

the same author. In a few cases values were omitted because it was apparent that the reported value did

not refer to the stated reaction or that the value was completely out of line with a number of wellestablished superseding measurements. Within the tables both solute and reaction have been included

when product identification has been made; otherwise only the solute is listed.

Columns are included identifying the source of the radical and the method of measurement; other

descriptive information is given under Comments. The serial number used in the Radiation Chemistry Data

Center files has been used for citing references; the first two digits of the number specify year. All

references are given following the tables. A formula index is also included, following the tables, as an aid

in locating specific compounds.

3
Abbreviations and Symbols M mol/dm3 abs. absorption mass spec. mass spectroscopy

abstr. abstraction Me methyl

acac acetylacetone MeOH methanol

AcO acetate MeOH(3D) methanol—d3 anal. analysis nat. natural (pH)

bipy bipyridine obs. observed

BzOH benzoic acid opt. optical spectroscopy

calc. calculated oxid. oxidation

chem. chemical oxy oxygen

c.k. competition kinetics p.b.k. product buildup kinetics concn. concentration perox hydrogen peroxide

condy. electrical conductivity phen 1, 10-phenanthroline

cor. corrected PhOH phenol

d.k. decay kinetics phot. photolysis

e.d. electrical discharge PNBA p-nitrobenzoic acid en ethylenediamine p.r. pulse radiolysis e-r. electron radiolysis 2-PrOH 2-propanol

esr electron spin resonance spectroscopy 2-PrOH(7D) 2-propanol-</7 estd. estimated Q benzoquinone

EtOH ethanol r. radiolysis

ferri ferricyanide ion rel. relative

g primary radiation yield (per 100 eV) soln. solution

G radiation yield (per 100 eV) son. sonolysis

y-r. gamma radiolysis unpubl. unpublished

k specific rate X-r. X-radiolysis

Table 1 . Values of k used to normalize relative rates

Reactant Reaction /c(dm

3 mol J s

*)

H (2.2)* H + H -» H2 1 x 10

10 Ag+ (2.5) H + Ag+ H

+ + Ag 3.1 x 10

10

ferri (2.63) H + Fe(CN)3 " H

+ + Fe(CN)J‘ 7 x 10

9 perox (2.69) H + H 2 02 ^ H2 0 + OH 6 x 10

7

nitrite (2.85) H + N02 ^ NO + OH" 7 x 10® oxy (2.89) H + 0 2 ^ H02 2 x 10

10 OH- (2.90) H + OH" —> e;q 1.5 x 10

7 BzOH (2.149) H + C6 Hs COOH C6 H6 COOH 1.0 x 10

9 Q (2.152) H + 0=C6 H4=0 0=C6 H4 0H 8.3 x 10

9 ClAcO" (2.178) H + ClCH2 COO" -> H2 + C1CHCOO” 1.9 x 10

6 dioxane (2.218) H + C 4 H8 0 2 -^ H 2 + C4 H 7 02 1.3 x 10

7 EtOH (2.224) H + CH3 CH2 OH ^ H2 + CHjCHOH 2.6 x 10

7 HCOO" (2.239) H + HCOO" —> H 2 + COO" 1.5 x 10® DCOO" (2.240) H + DCOO" —> HD + COO" 2.3 x 10

7 HCOOH (2.241) H + HCOOH -> H2 + COOH 7.5 x 10

s glucose (2.245) H + C6H12 06 ->H2 +C6Hu06 4.7 x 10

7 MeOH (2.296) H + CH3 OH -» H 2 + CH2 QH 2 x 10

6 MeOH(3D) (2.298) H + CD3 OH -> HD + CD2 OH 1 x 10

s PNBA (2.309) H + no2 c6 h4 cooh no2 c 6 h5 cooh 1 x 10

9 PhOH (2.320) H + OHC6 H5 -> OHC6 H6 1.8 x 10

9 2-PrOH (2.334) H + CH3 CHOHCH3 -> H2 + CH3 COHCH3 7.9 x 10

7 MeCDOHMe (2.335) H + CH3 CDOHCH3 ^ HD + CH3 COHCH3

1 x 10

7 2-PrOH(7D) (2.336) H + CD3 CDOHCD3 -> HD + CD3 COHCD3

1 x 10

7

‘Number in parentheses indicates the number of the reaction in the following tables.

4
Table 2. Reactions of H with water and transients from water

No. Solute and Reaction pH k(dm 3 mol x s

*) Ratio Source Method Comment Ref.

2.1 H + —* H2 + basic 2.5 x 10

10 (rel.) See 1.5, 1.6. 73-0030

OH2.2 H <1 7.5 x 10

9 (rel.) m^ = 125 p.r. chem. c.k.; obs. G(Hj) 62-0133

H + H -> H2 at various dose

rates. 0.4 1 x 10

10 (rel.) klk^ = 0.5 p.r. chem. obs. G(H 2 02 ); 63-0043

6.4 x 10

9 (rel.) k/k^ = 106 computer anal. <3 6 x 10

9 (rel.) — e-r. chem. obs. G(Hj) in Fe^ — H2 Oj soln.; 63-0043

1.5 x 10

10 km

lkj' 2+ = 6.3 computer anal. 0.8 p.r. opt. c.k.; obs. 63-0047

x 10~3 G(Fe3+

) at various dose rates. 0.4- 1.3 x 10

10 (rel.) — p.r. chem. obs. G(H2) and 64-0092

3 G(0 2 ) in H2 0 2 soln.; computer

anal. 2 2A#Fe3+ = 225 ± p.r. opt. c.k.; see however 64-0093

25 70-0063.

0.4 1 x 10

10 (rel.) — p.r. chem. c.k.; obs. G(H2 ) at various dose 65-0017

rates in H2 02 , 0 2 and Cu2+ solns.

1.1 — — y-r. chem. kfi/kfi = 3.5 ±

0.2. 66-0182

2-3 1.3 x 10

10 (rel.) klkfmi = 1.9 p.r. opt. c.k.; computer

anal. 68-0324

3 (7.8 ± 0.5) x 10

9 p.r. opt. d.k. at 200 nm;

e = 900 ± 30 dm3 mol

-1 cm_1

69-0083

<3 1.4 x 10

10 (rel.) p.r. opt. obs. GCFe^) in FeS04 - CuS04 soln. at various dose rates; best

fit.

70-0063

1 7.4 x 10

9

(rel.) p.r. opt. obs. GCFe^) in FeS04 soln. at various dose rates.

71-0268

acid — — p.r. chem.1 ’ kft/kj) = 3.2 ±

0.1. 72-0013

For other ratios see : 2.3, 2.4, 2.59, 2.67, 2.178, 2.179, 2.241, 2.301

2.3 OH <1 8 x 10

10 (rel.) *#0x7 = 4.1 * p.r. — — 60-0099

H + OH -* HjO 0.4 2 x 10

10 (rel.)

3.2 x 10 10 (rel.)

k/kji = 2 p.r. chem. obs. G(H2); computer anal. 63-0043

3 p.r. chem. obs. G(Hj) and

G(Oj) in Hj02 soln.; computer

anal.

64-0092

<1 6 x 10

11 (rel.) klk

= 30

k/k( OH + Fe

2+

) s

p.r. — see 70—0063. 64-0293

300

3 7 x 10

9

. p.r. opt. d.k. at 260 nm

(OH).

65-0010

5
Table 2. Reactions of H with water and transients from water — Continued

No. Solute and Reaction pH &(dm 3 mol *s *) Ratio Source Method Comment Ref.

<3 2 x 10

10 (rel.) p.r. chem. obs. G(Fe3+

) in FeS04 - CuS04 soln. at various dose rates; best fit.

70-0063

3 (1.5 ± 0.3) x 10

10 — p.r. opt. d.k. at 200 - 240 nm; computer anal. 70-0213

acid (2.5 ± 0.5) x 10

10 — p.r. chem. obs. G(H 2 ); computer anal. 72-0013

2.4 ho 2 0.4 2 x 10

10 (rel.) kl kH = 2 p.r. chem. obs. G(H 2); 63-0043

H + H02 -* H2 0 2 2 x 10

10 p.r. computer anal, assumed value. 64-0049

<3 2 x 10

10 (rel.) p.r. chem. obs. G(Fe3+

) in FeS04 - CuS04 soln. at various dose rates; best fit.

70-0063

6
Table 3. Reactions of H with inorganic solutes

No. Solute and Reaction ===

pH ^dmS mol~1 s

1

) Ratio Source Method Comment Ref.

2.5 Ag+ 2 ( 1.10 ± 0.06) x 10

10 — p.r. opt. p.b.k. at 310 nm; 67-0550

H + Ag+ -» Ag + H

+

2 (3.10 ± 0.30) x 10 10 p.r. opt.

superseded by

following value,

p.b.k. at 365 nm. 68-0436

1 2.83 x 10

10 p.r. opt. p.b.k. at 410 nm;

contains /er/-BuOH;

k increases with pressure 0 —» 6.72

kbar.

73-1053

For ratios see: 2.218, 2.224, 2.231, 2.249, 2.250, 2.2%, 2.301, 2.333, 2.334

2.6 As(III) H + As(III)

2.7 1.2 x 10

9 (rel.) = 20 X-r. chem. c.k. 62-0018

H

+ + As(II) 2.7 AsFg 5 8.8 x 10

s (rel.) ^/^MeCDOHMe ~ y-r. chem. c.k. 66-0401

8.8 x 10

"*

2.8 AuCl*

H(or e~%

) + AuCl* —

4 (5.7 ± 1.5) x 10

9 — p.r. opt. p.b.k. at 330 nm. 68-0302

H

+

(or HjO) +

AuClJ"

2.9 B 4 O?- -7 < 10

4 (rel.) is

1 A H son. chem. c.k.; B4 0

2 ”

is either nonreactive towards H or is less reactive than F”

67-0099

2.10 Br2 1 - 10

10 — p.r. opt. p.b.k. at 360 nm 65-0382

H + Br2 -» HBr + (Br^), uncertainty Br —> H

+ + Br" + in the value is Br —» H

+ + Br2 —0.8 4.2 x 10

10 (rel.) klk^ = 700 y-r. chem.

5-fold,

c.k., obs. G(-Br~) and

G(H 2 02 + Br2

).

67-0008

2. 10a Br" H + Br"-* HBr" - 7 2.0 x 10

7 (rel.) k/k^coQ— = 0.132 y-r. chem. c.k. 72-0264

2.11 Br0 3" 7 3.2 x 10

7 (rel.) ^/^2-PiOH = 0.4 y-r. chem. c.k. 66-0402

2.12 CO 1.2 k/kfe 2+ = 2.2 ± y-r. chem. c.k. 63-0014

H + CO - HCO 0.3

1 k/khcho = 14.8 ±

0 y-r. chem. c.k. 63-0014

3.8 x 10*

j — — Unpubl. data. 70-7235

2.13 C02 1 < 10

6 — p.r. opt. no abs. at 250 65-0384

H + C02 -> COOH nm. < 8 x 10

6 y-r. chem. estd. from yields

in carboxylation

of methanol.

65-0375

2.14 HCOJ 8 3.4 x 10

4 (rel.) k/kueOB = 1-7 X X--r. chem. c.k. 63-0049

10"2 2.15 HCN

H + HCN —> H2 CN — 1.1 x 10*(rel.) k/ki-ptOR =1-4 y-r. chem. c.k. 68-0593

2.16 CN" 7 4.1 x 10

9 (rel.) ^/^•2-PiOH = ^2 y-r chem. c.k. 66-0402

2.17 c 2 n2 6 < 10

7 — p.r. opt. react, not obs.

at low concn. 71-0038

2.18 CNS" 7 2.7 x 10* (rel.) ^•/^2-PiOH = 3.4 y-r. chem. c.k. 66-0402

2.19 Cd++ — < 3 x 10

5(rel.) k/k^oR < 10 y-r. chem. c.k. 65-0192

2.20 Cd(CN)*2" 5 > 2.4 x 10

9 (rel.) k/k^gCDOHMe > 235 y-r. chem. c.k. 66-0401

2.21 Ce4*

1 5.5 x 10 7 (rel.) k/kfjQR = 2.1 ± y-r. chem. c.k. 70-1059

0.4 2.21a cr -7 < 10

s (rel.) — y-r. chem. c.k. with HCOO" 72-0264

7
Table 3. Reactions of H with inorganic solutes — Continued

No. Solute and Reaction pH k(dm 3 mol *s *) Ratio Source Method Comment Ref.

2.22 Co(NH3)3+ 4-6 1.85 x 106 (rel.) — e.d. opt. calcd. from 65-0014

H + Co(NH3)j + — diffusion model;

Co(II) rel. to kH = 3 x

10

10

. 4-6 2 x 10

6 (rel.) ^/^MeOH<3D) = 20 y-r. chem. c.k.- 65-0085

1 < 9 x 10

4(rel.) kl

k

EtOH 3.4 x y-r. chem. c.k. 66-0010

10~3 2.23 Co(NH3 ) s H 2 0

3+ 1.8- 4.5 x 10

s (rel.) — e.d. opt. calcd. from 65-0014

H + Co(NH3 ) 5 H2 0

3+ 3.88 diffusion model; — Co(II) rel. to kt, = 3 x 10

10

. 1 < 7 x 10

s(rel.) ^/^EtOH < 2.6 X y-r. chem. c.k. 66-0010

10'2

Co(NH 3) s OH2+ 5 < 10

6 (rel.) ^MeCDOHMe < 0-1 y-r. chem. c.k. 66-0401

2.24 6.66- 3.1 x 10 7 (rel.) — e.d. opt. calcd. from 65-0014

H + Co(NH3 ) s OH2+ 11.0 diffusion model;

Co(II) rel. to kft — 3 x

10

10

. 7.5 3 x 10

7 (rel.) k/kMeCDOHMe = y-r. chem. c.k. 65-0085

2.95

2.25 Co(NH 3) 5 F

2+ 4-6 1.1 x 10

6 (rel.) — e.d. opt. calcd. from 65-0014

H + Co(NH3 ) 5 F

2+ —

»

diffusion model;

Co(II) rel. to kt, = 3 x 10 10

. 4-6 1.2 x 10

6 (rel.) k/kMeOH(3D) = ^ y-r. chem. c.k. 65-0085

1 < 1.4 x 106 (rel.) k/kEtOH 3.3 X y-r. chem. c.k. 66-0010

10“2 2.26 Co(NH3) 5 C1

2+ 4-6 7.3 x 10

7 (rel.) — e.d. opt. calcd. from 65-0014

H + Co(NH3 ) s C1

2+ -* diffusion model;

Co(II) rel, to kH = 3 x 10

10

. 4-6 2.6 x 10® (rel.) ^MeCDOHMe = 26 y-r. chem. c.k. 65-0085

1 1.1 x 10

9

(rel.) k/kEtOH = 42 y-r. chem. c.k. 66-0010

2.27 Co(NH 3) 5 Br

2+ 4-6 4.6 x 10® (rel.) — e.d. opt. calcd. from 65-0014

H + Co(NH3 ) s Br

2+ -* diffusion model;

Co(II) rel. to kH = 3 x

10

10

. 4-6 1.2 x 10

9 (rel.) ^MeCDOHMe = . y-r. chem. c.k. 65-0085

118

1 9.6 x 10

9 (rel.) k/kEtOH = 370 y-r. chem. c.k. 66-0010

2.28 Co(NH3) 5

I 2+ 4-6 3.3 x 10

9 (rel.) — e.d. opt. calcd. from 65-0014

H + Co(NH3 ) sI 2+ —

>

diffusion model;

Co(II) rel. to k H = 3 x 10

10

1 3.5 x 10

9 (rel.) kl k MeCDOHMe = y-r. chem. c.k. 65-0085

350

1 2.3 x 10

10 (rel.) kl ^e»oh = 370 y-r. chem. c.k. 66-0010

2.29 Co(NH3) 5 CN2+ 4-6 4.4 x 10

7 (rel.) kl ^MeCDOHMe = y-r. chem. c.k. 65-0085

H + Co(NH3 )5CN2+ ^ 4.35

Co(II) 1 4.2 x 10

7 (rel.) = 1-6 y-r. chem. c.k. 66-0010

2.30 Co(NH3) 5 NCS2+1 4.6 x 10

9 (rel.) k/k EtOH = 136 y-r. chem. c.k. 66-0010

2.31 Co(NH3) s N3 2+ 4-6 4.6 x 10* (rel.) ^/^MeCDOHMe = 46 y-r. chem. c.k. 65-0085

1 7.5 x 10® (rel.) k/keioh = 29 > y-r chem. c.k. 66-0010

2.32 Co(NH 3) s(H-fumarate)2+

1 4.2 x 10* (rel.) k/kEtOH = 130 y-r. chem. c.k. 66-0010

2.33 Co(NH 3) 5 N02+

1 1.1 x 10* (rel.) k/kfjoH = 4.2 y-r. chem. c.k. 66-0010

2.34 Co(NH3) 3(N02 ) 3

1 6.5 x 10* (rel.) k/kE»OH = 25 y-r. chem. c.k. 66-0010

2.35 Co(CN)3 -

1 1.4 x 10

7 (rel.) k/kEtOH = 0.53 y-r. chem. c.k. 66-0010

5 1.1 x 10

9

(rel.) k/k MeCDOHMe = 1®3 y-r. chem. c.k. 66-0401

8
Table 3. Reactions of H with inorganic solutes — Continued

No. Solute and Reaction pH &(dm 3 mol-1

s -1

) Ratio Source Method Comment Ref.

2.36 Co(NH3) s (AcO)2+

1 < 9 x 10

s (rel.) ^/^EtOH < 3.4 X 10"2 y-T. chem. c.k. 66-0010

2.37 Co(NH3) s P04 1 < 5 x 10

s (rel.) kl

k

EtOH < 1-76 x 10"2 y-r. chem. c.k. 66-0010

2.38 £o(NH 3) s (OOCCF3 ) 2+

1 < 1.8 x 10

s (rel.) kl ^EtOH ^ 7.1 x

10“3 y-r. chem. c.k. 66-0010

2.39 Co(NH3) 5 (OCOC6 H5 ) 2+ 1.0 H + Co(NH3 ) 5 (OCOC 6 H5 ) 2+ Co(NH3 ) s (OCOC 6 H6 ) 2+

(1.6 ± 0.4) x 10

9 p.r. opt. p.b.k. at 345 nm. 71-0282

2.40 Co(en)3 H + Co(en)3 + —

>

Co(II)

3.5 6 x 10

s (rel.) e.d. chem. calcd. from

diffusion model;

rel. to ku — 3 x

10

10

.

71-9218

2.41 Co(en)2 (H 2 0) 2 + H + Co(en)2 (H 2 0) 2 + —> Co(II)

3.5 1.6 x 10

7 (rel.) e.d. chem. calcd. from

diffusion model;

rel. to = 3 x

10

10

71-9218

2.42 Co(en)2 F2 H + Co(en)2 F2 —

Co(II)

3.5 2.7 x 10

6 (rel.) e.d. chem. calcd. from

diffusion model;

rel. to = 3 x

10

10

.

71-9218

2.43 Co(en)2 Cl2 5 8.1 x 10

8 (rel.) k/kMeCDOHMe = ^1 y-r. chem. c.k. 66-0401

2.44 Co(en)2 C03 5 < 2.4 x 10

6

(rel.) kl k MeCDOHMe < 0-24 y-r. chem. c.k. 66-0401

2.45 Co(en)2 (C 2 04 ) + H + Co(en)2 (C 2 04) + -* Co(II)3.5 8 x 10

s (rel.) e.d. chem. calcd. from

diffusion model;

rel. to = 3 x

10

10

.

71-9218

2.46 Co(en)(C 2 04) 2 H + Co(en)(C 2 04) 2 ^ Co(II)

3.5 2.8 x 10

6 (rel.) e.d. chem. calcd. from

diffusion model;

rel. to kH = 3 x

10

10

.

71-9218

2.47 Co(C 2 04) 2 - H + Co(C 2 04) 3 —»

7 1.8 x 10

8 (rel.) ^nitrite = 0.15 y-r. chem. c.k.; assumed

*(H) = 2.8. 67-0498

Co(C 2 04) 2 + c 2 o

2_ + h

+ 3.5 4.2 x 10

6 (rel.) e.d. chem. calcd. from

diffusion model;

rel. to k H = 3 x 10

10

.

71-9218

2.48 Co(acac)3 1 1.3 x 10

9 (rel.) k/k2-PiOH = 17 y-r. chem. c.k. 70-0094

2.49 Cr(NH 3 ) 5 Cl

2+ 5 2.1 x 10

6 (rel.) ^/^MeCDOHMe =0'21 y-r. chem. c.k. 66-0401

2.50 crci2 (H 2 o); 5 2.4 x 10

7 (rel.) MeCDOHMe = 2.4 y-r. chem. c.k. 66-0401

2.51 Cr(C 2 04) 3 ~ H + Cr(C 2 04) 3 ~ —» Cr(II)3.5 1.1 x 10

6 (rel.) e.d. chem. calcd. from

diffusion model;

rel. to kH = 3 x

10

10

.

71-9218

2.52 CrO2- —

7.8 x 10

7 (rel.) 1.6 x 10

10 (rel.) HCOO - = 0.52

EtOH = 600 ±

300

y-r.

y-r. chem.chem.

c.k.

c.k. 66-0616

65-0192

2.53 Cr2 0

2 ' — 2.6 x 1010 (rel.) EtOH = (1 ±

0.2) X 10

3 y-r. chem. c.k. 65-0192

2.54

2+ Cu 1 4.2 x 10

7 (rel.) ^/^HCOOH = 36 X-r. chem. c.k. 56-0012

H + Cu2+ —> Cu+

1 6.6 x 10

7 (rel.) k/kMeOH = 33 X-r. chem. c.k. 58-0006 + H

+ ~6

1.5

0.4

9.8 x 10

8 (rel.)

6 x 10* (rel.) 1.2 x 10

9 (rel.)

6.8 x 10

7 (rel.)

6 x 10

9 (rel.)

^/^2-PrOH =

12.4 ± 3 k/kfMH = 23 ± 3

k/ke«oh = 45 ± 8

^/^e»oh = 2.64 ±

0.06 k/k^ = 0.3

y-r.

y-r.

y-r.

y-r.

y-r.

chem.

chem.

chem.

chem.

chem.

c.k.

c.k.; CuS04 used,

c.k.; Cu(N03) 2 used,

c.k.

c.k.; CuS04 -

Fe2+ - 02 system.

63-

0041,

64-

0095

65-

0192

65-

0192

66-

0138

66-0334,

68-0355

9
Table 3. Reactions of H with inorganic solutes — Continued

No. Solute and Reaction pH k(dm 3 mol *s

7

) Ratio Source Method Comment Ref.

7 5.9 x 10

8 (rel.) ^MeCDOHMe = 39 y-r. chem. c.k. 66-0401 — 2.5 x 10

8 (rel.) ^/^2-PrOH = 3.2 y-r. chem. c.k. 66-0616 ± 0.5 — 3.5 x 10

8 (rel.) kl kHcoo~ = 2.3 ± y-r. chem. c.k. 66-0616

0.5 1-2 7.6 x 10

7 (rel.) klkMeOH = 38 ± 2 y-r. chem. c.k. 68-0444

~7 4.2 x 10

7 (rel.) kl k Hcoo~ = 0.28 y-r. chem. c.k. 72-0264 For other ratios see: 2.110, 2.197, 2.256, 2.297 D + Cu 2+ —» D

+ 1.25 9.4 x 10

7 (rel.) ^/^EtOH ~ 3.62 — — — 66-0621 + Cu + 2.55 F~ 8.5 (1.9 ± 0.5) x 10

4 ^/^MeOH(3D) = y-r. mass c.k.; obs. 67-0099

H + F~-» e;q + HF (rel.) 0.19 spec. G(H 2 -HD)

~~7 1.5 x 10

4 (rel.) kl kci\cO~ = 8 x y-r.. chem. c.k.; obs. 67-0099

10"3 son. G(cn.

8.3 (1.0 ± 0.5) x 104 p.r. opt. effect of H2 concn. on e~q decay in 1.0 M KF.

67-0115

2.56 Fe

2+ 0.4 1.6 x 10

7 (rel.) ktk0TJ = 8.3 x y-r. chem. c.k. 57-0009

H + Fe

2+ (+H +

) -> 10

-4 Fe

3+ + H 2 2.1 1.3 x 10

7 (rel.) fc/£ oiy = 6.7 x X-r. chem. c.k. 58-0004 Fe

2+ + H ^ 10^

FeH 2+

(1) 0.8- 2 x 10

7 — p.r; chem. obs. G(Fe 3+

); 63-0047,

FeH2+ + H

+ ^ 1.2 effect of pulse 64-0049 Fe

3+ + H a (2) 0 (7.5 ± 2) x 10

6 p.r. opt.

length.

p.b.k. at 270 nm 69-0434

(rel.) (Fe

3+

); computer

anal.; rel. to = 2.6 x 10

10

; k2 = (1.06 ± 0.1) x 10

4

. 0.4 2.8 x 10

7 (rel.) k/koxr = 1.4 x y-r. chem. c.k. 70-0533

10~3

1.5 1.1 x 10

8 (rel.) klkOXJ = 5.5 x y-r. chem. c.k. 70-0534

10"3 For other ratios see: 2.2, 2.12, 2.57, 2.58, 2.60, 2.61, 2.83, 2.297

2.57 Fe

3+ <1 8 x 107 (rel.) klkOIJ = 4 x y-r. chem. c.k. in HC1 or 57-0008

Fe

3+ + H -> Fe2+ + 10~3 HC104

. H

+

1 6 x 10

6 (rel.) kl kMeOH = 3 X-r. chem. c.k. 58-0006

0.4 +

II O bCO y-r. chem. c.k. in H2 S04

. 57-0009 ± 0.010

2 1.4 x 10

8 (rel.) k/korj = 7 X 10"3 y-r. chem. c.k. 57-0010

1.57 k/ku2+ = 1.35 ± y-r. chem. c.k. 58-0004

0.1

2.1 k/kre 2+ = 7.2 ± y-r. chem. c.k. 58-0004

0.7 0.8 klkFc T+ = 170 y-r. chem. c.k. in HC1. 58-0011

~l-3 5 x 10

8 (rel.) k/kOI1 = 2.45 x y-r. chem. c.k. in HC104

. 63-0004

10'2 — 1-3 k/kFc 2+ <0.1 e.d. chem. c.k. in HC104

. 66-0345

0.4-3 k/kfe2+ = 0.1 e.d. chem. c.k. in H2 S04 ; reactant FeS04

. 66-0345

-1-2 < 2 x 10

6 (rel.) kl kUeOH < 1 y-r. chem. c.k. in HC104 soln.; kFeOH 2 + >

500 kFe 3+.

68-0444

For other ratios see: 2.2, 2.67, 2.68, 2.96, 2.98, 2.297

2.58 FeOH 2+ -1-3 k/kVe 2+ = 1.60 e.d. chem. c.k. in HC104

. 66-0345

-1-2 1 x 10

9 (rel.) kl kUeOH = 430 y-r. chem. c.k. in HC104

. 68-0444

10
Table 3. Reactions of H with inorganic solutes — Continued

No. Solute and Reaction pH k(dm 3 mol *s

7

) Ratio Source Method Comment Ref.

2.59 FeH 2+ 0.8- k*lkn

k\ = 0.25 p.r. chem. c.k.; reactant is 63-0047

FeH 2+ + H Fe

2+ + 1.2 produced from H + h 2 Fe

2+

; reaction 2

is FeH2+ + H

+ ^

Fe

3+ + H2

. 2.60 FeF 2+ + FeFj 0.8 klkTc 2+ = 0.04 e.d. chem. c.k. 66-0345

2.61 FeCl2+ 0.8 4.6 x 10

9 (rel.) k/k^ = 0.23 y-r. chem. c.k. in HC1. 57-0008

FeCl2+ + H ^ 0.8 k/kTe 2+ = 300 e.d. chem. c.k. in HC1. 66-0345 Fe

2+ + Cl" + H

+

2.63 Fe(CN)|~ (ferri) 2-9 1.5 x 10

9 (rel.) — e.d. opt. calcd. by 66-0345

H + Fe(CN)3 " diffusion model; Fe(CN)4 " + H

+

(I) assume kB = 3 x

10

10

. H + Fe(CN)j~ —

»

acid ku/k1 = 0.28 y-r. chem. c.k. 66-0286

Fe(CN)3 ~ + H

+ + 2-3 (6.5 ± 0.5) x 109 — p.r. opt. d.k. at 420 nm. 68-0324

CN~ (II) 1.9 7.5 x 10

9 — p.r. opt. d.k. at 410 nm. 71-0618

For other ratios see

:

2.2, 2.83, 2.85, 2.89, 2.90, 2.118, 2.150, 2.163, 2.194,

2.224, 2.225, 2.239, 2.241, 2.245, 2.249, 2.296, 2.316,

2.334, 2.346, 2.363

2.64 Fe(C 2 04 )l" 3.5 3.4 x 106 (rel.) — e.d. chem. calcd. from 71-9218

H + Fe(C 2 04 )3 _ —* diffusion model;

Fe(II) rel. to ka = 3 x

10

10

. 2.65 Fe(bipy)3+ 0.3 2.2 x 10

9 (rel.) e.d. opt. calcd. by

diffusion model; assume kH = 3 x 10

10

.

66-0345

2.66 Fe(phen)j

+ 0.3 2.9 x 10

9 (rel.) e.d. opt. calcd. by

diffusion model; assume = 3 x 10

10

.

66-0345

2.67 H

+ — 1-2 3.4 x 10

2 (rel.) ^/2iH = 1.2 x e.d. chem. c.k. 59-0008

H + H

+ ^ H2 10"5 <3.5 (2.6 ± 1.1) x 10

3 phot. chem. estd. from pH

effect on quantum

yields of N2 , I

2 and H2 in I" — N2 0 soln.

62-0057

<0.8 2.8 x 10

4 (rel.) k/k ^

= 1.4 x y-r. chem. c.k. 62-0096

10"6 2-3 klkTe 3+ = 2.8 x y-r. chem. c.k. 63-0004

10"3 <0 k/kTe 3+ = 3.6 x X-r, chem. c.k.; in 17.3 M 65-0371

10"4 y-r. h2 so4

. For other ratios see: 2.102 D + H

+ ^ HD+ acid 2 x 10

2 — y-r. — estd.; D2 soln. 58-0047

2.68 d 2 2.12 k/kje 3+ = 8.3 x y-r. chem. c.k. 59-0012

H + D 2 —* HD + D 10"3 2.69 H2 02 (perox) 2.85 > 6 x 10

6 (rel.) k/kmij > 3.3 x y-r. chem. c.k. 62-0051

H + H2 Oj -* H2 0 + 10^

OH 0.8- 4.4 x 10

7 (rel.) k/kaIJ = 2.2 x phot. chem. c.k. 62-7001

7 10"3 0.4 6.6 x 10

7 (rel.) k/kmT = 3.3 x p.r. chem. c.k. 63-0043

10"3

2.1 (9 ± 1) x 10

7 p.r. opt. p.b.k. (Cl 2 at 350 nm; soln. contains 0.2 M Cl").

64-0093 — 6.1 x 10

7 — p.r. — — 66-0559

-7 3.0 x 10

7 (rel.) kl ^hcoo - = 0-2 y-r. chem. c.k. 72-0264 For other ratios see: 2.2, 2.6, 2.10, 2.79, 2.100, 2.222, 2.224, 2.361

11
Table 3. Reactions of H with inorganic solutes — Continued

No. Solute and Reaction pH k(dm3 mol ! s

*) Ratio Source Method Comment Ref.

2.70 Hg2+ ~ 7 3.9 x 10

10 (rel.) k/kEtOH = (1*5 — y-r. chem. c.k. 65-0192

Hg2+ + H -> Hg+ + H

+ 0.1) x 10

3 ~ 7 1.7 x 10

9 (rel.) klkncoo~ — 11 — ^ y-r. chem. c.k.; 8 x

10"®

to 8 x 10~® M

HgCl2 and 2 x 10~s M HCOONa.

66-0616

1.5 2 x 10

9 (rel.) ^/^2-PrOH = 26 y-r- chem. c.k. 69-0275

1 (1.0 ± 0.5) x 10

10 — p.r. opt. p.b.k. at 330 nm. 73-0043

2.70a HgJ

+ — 4.7 x 109 (rel.) ^/^-2-P»OH ~ 0-60 y-r- chem. c.k. 72-0290

2.71 I 2 0.8 4 x 10

10 (rel.) 2 y-r. chem. c.k. 64-0245

I

2 + H HI + I — 1 x 10

10 (rel.) k/ktiMH x 10

3 — — c.k.; no details 67-0041

5.3 x 10

6 dm6 mol”2 s

_1 given. 2.72 r >0.4 — y-r. chem. c.k. assuming 69-0338

H + I - + H

+(or (rel.) k(H + I 3 or I

2 ) = HSO^) -* H2 + I 3 x 10

10 and

g(H) = 3.45-3.65. h + Hr ~7 2.4 x 10

7 (rel.) klkncoo~ = 0-162 y-r. chem. c.k. 72-0264

2.73 l~2 3.5- (1.8 ± 0.8) x 10

7 — phot. chem. estd. 62-0057

H + I 2 -> H

+ + 21" 11 2.74 I 3" 2.92 8 x 10

9 (rel.) klkueOH = 4 X phot. chem. c.k. 68-7194

h + i;-> h

+ + r 10"3 + I2 1.72- 2.3 x 10

10 (rel.) ^/^2-PiOH = 285 phot. che'm. c.k. 68-7194

2.92

1.5 3.3 x 10

10 (rel.) klk^ = 700 y-r. chem. c.k. 69-0338

2.75 103 7 9.5 x 10

7 (rel.) klk2-¥rOH = 1-2 y-r. chem. c.k. 66-0402

2.76 Mn2+ 6 3 x 10

7 (rel.) k/kMeCDOHMe = 3 y-r. chem. c.k. 66-0401

2.77 MnO; 3 2.8 x 10

10 — p.r. opt. d.k. 65-0044

H + MnO;-> 3 (2.36 ± 0.2) x 10

10 — p.r. opt. d.k. at 545 nm. 65-0385

H

+ + MnO$" acid 4.6 x 1010 (rel.) k/kOXJ = 2.3 p.r. opt. c.k. 65-0385

2.78 nh; 7 <2.3 x 10

4 (rel.) k/kx)coo~ < 10 y-r. chem. c.k. 64-0095

2.79 n2 h5+ 2 3 x 10

4 (rel.) klk^m = 5 x y-r. chem. c.k. 55-0004

H + N2 Hj-» N2 H3 4 10"4 H

+ + H2 ~0.7 1.7 x 10

4 (rel.) klk^ = 2.8 x y-r. chem. c.k. 69-0598

10"4 6 7.8 x 10

4 (rel.) klk^ = 1-3 x y-r. chem. c.k. 69-0598

10'3 2.80 nh3 1.2 1.1 x 10* (rel.) k/k^tOH =4.2 y-r. chem. c.k. 66-0010

2.81 Nj — 4.9 x 10® (rel.) klk^H = 19 y-r. chem. c.k. 66-0010 ~ 7 4.3 x 10

9 (rel.) ^/^2-PrOH = 64 y-r. chem. c.k. 71-0007

2.82 NO

H + NO -* HNO

7 1.1 x 10*° (rel.) klk^= 15 y-r. chem. c.k. 67-0231

2.83 N 2 0 ~ 2 k/krc 2+ = 1.7 x y-r. chem. c.k.; data from 60-0035

H + N 2 0 -» N2 + OH 10“2 60-0068.

3.5- (1.25 ± 0.5) x 10

4 — phot. chem. estd. 62-0057

11 < 10 > 1.7 x 104 (rel.) — y-r. chem. estd. by c.k. with H2 02

. 65-0011

7 ~ 10

5 (rel.) phot. chem. estd. from

k(OH + CH3OH)/k = 25.

65-7006

alk. 2.3 x 10

6 (rel.) klkfmi = (3.3 ± y-r. chem. c.k. 68-0693

1.8) x lO^1 2.84 HNOj 1 6.8 x 10® (rel.) k/k^ofi = 26 y-r. chem. c.k. 66-0010

H + HN02 -> HjO + NO

12
Table 3. Reactions of H with inorganic solutes — Continued

No. Solute and Reaction pH k(dm 3 mol *s *) Ratio Source Method Comment Ref.

2.85 NOj 7.6 1.5 x 10

9 (rel.) klk kni = 0.22 ± X-r. chem; c.k. 62-0017

H + N02 ^ NO + OH" 0.09 ~8 6 x 10

8 and k/k^eOH = 300 and X-r. chem. c.k. 62-0017

1 x 10

9 (rel.) 430. ~6 2.1 x 108 (rel.) ^/^2-PiOH = 2.7 ±. y-r. chem. c.k. 63-0041,

0.3 64-0095

nat. 1.4 x 10

9 (rel.) k/kueOH ~ 390 ± y—r. chem. c.k. 65-0192

70

nat. 2.1 x 10

9 (rel.) klk2-PrOH = 27 ±

Q y-r. chem. c.k. 65-0192

nat. 6.1 x 10

8 (rel.) k/k^coo — 4.1 ± y-r. chem. c.k. 65-0192

0.2

nat. 2.8 x 10

9 (rel.) klk ZtOH = 109 ± 7 y-r. chem. c.k. 65-0192

7-8 1.6 x 10

9 (rel.) k/k^oii = 63 y-r. chem. c.k. 66-0010

6 1.1 x 10

9 (rel.) ^/^MeCDOHMe = y-r. chem. c.k. 66-0401

1.06

nat. 8 x 10

8

(rel.) klk2-PrOH = 10 ±

1 y-r. chem. c.k. 66-0616

nat. 7.3 x 108 (rel.) k/kncoo ~ 4.8 ± y-r. chem. c.k. 66-0616

0.4

7 7.1 x 10

8 — p.r. esr d.k. (H signal). 71-0303 For other ratios see: 2.47, 2.82, 2.107, 2.245, 2.249

2.86 no3" ~ 6 4 x 10

7 (rel.) ^/^2-PiOH — 0.51 y-r. chem. c.k. 63-0041,

no3 + H no2 + ± 0.07 64-0095

OH" or N03 H" nat. 1.1 x 10

7 (rel.) k/k^tOH = 0.42 ± y-r. chem. c.k. 65-0192

0.05

5.6 1.4 x 10

7 (rel.) ^/^2-PiOH = 0.18 y-r. chem. c.k. 65-0372,

66-0114

5.7- 5.2 x 10

6 (rel.) k/k^xOH = 0.2 y-r. chem. c.k. 66-0147

7.1 3.0 x 10

6 (rel.) k/k^coo~ = 0.02 y-r. chem. c.k. 66-0147

4.7 x 10

6 (rel.) klk2-Pton = 0.06 y-r. chem. c.k. 66-0147

6 2.1 x 10

7 (rel.) k/k MeCDOHMe = y-r. chem. c.k. 66-0401

2.1

1 8.2 x 10

6 (rel.) k/k^cooH ~ 11 y-r. chem. c.k. 68-0343 ~ 7 2.9 x 10

6 (rel.) k/kjicoo~ ~ (1-0 y-r. chem. c.k. 70-0859 ± 0.3) x 10"2

2.5 1.4 x 10

6

| — p.r. esr d.k. (H signal); 71-0303

high concn. of N03 ; k concn. dependent. ~ 7 7.2 x 10

6 (rel.) klk \icoo~ = 4.8 y-r. chem. c.k. 72-0264

x 10“2 For other ratios see: 2.107

2.87 NO(SO^)2 (Fremy's 8.5 1.8 x 10

9 (rel.) k/ k\{QQo~ = 12 ± y-r. chem. c.k.; 0.1 M 69-0649

salt) 2 Na2 HP04 used to adjust pH.

2.88 Ni2+ nat. < 2.6 x 10s (rel.) ^/^“EiOH < 10 y-r. chem. c.k. 65-0192

2.89 02 (oxy) acid 1.2 x 10

10 — p.r. chem. obs. G(H 2 02 ); 63-0043

H + 02 -> H02 estd. value.

1.2 2.1 x 10

l° —

p.r. opt. p.b.k. at 240 nm. 64-0043

3 2.6 x 10

10 — p.r. opt. mathematical 64-0092

anal. — 2.x 10

10 (rel.) k/kueOH — 104 — — c.k.; details 67-0041

not given.

1.9 1.6 x 10

10 (rel.) klklmi = 2.3 p.r. opt. c.k.; obs. 71-0618

Fe(CN)4

" decay at 410 nm.

13
Table 3. Reactions of H with inorganic solutes — Continued

No. Solute and Reaction pH k(dm 3 mol J s

*) Ratio Source Method Comment Ref.

1.9 2.5 x 10

10 (rel.) k/k Q = 3.1 p.r. opt. c.k.; obs. benzoquinone Hadduct formn. at 410 nm.

71-0618

For other ratios see: 2.2, 2.3, 2.54, 2.56, 2.57, 2.61-62, 2.67, 2.69, 2.71, 2.77,

2.94, 2.95, 2.205, 2.224, 2.229, 2.245, 2.249, 2.271,

2.292, 2.296, 2.334, 2.374

2.90 OH - 11 - 1.4 x 10

7 (rel.) k/khcoo - = 0-09 X-r. chem. c.k. 63-0049

h + oh” —» <?:q 13 11.5 (1.5 - 2.3) x 10

7 — p.r. opt. p.b.k. 64-0108

11.6 ( 1.8 ± 0 . 6) x 10

7 p.r. opt. p.b.k.; soln. contains 100 atm h2

.

65-0009 — 2.3 x 10

7 — p.r. — — 66-0842

11 - 1.5 x 10

7 (rel.) */*£«ni=(2-l y-r., chem. c.k.; soln. 68-0693

13 ± 1.0) X 10

"3 X-r. contains N 2 0 and

Fe(CN)4 ”; obs. G(N 2 ); assume

k/k( H + N2 0) > 12.5. 10.5- 1.5 x 10

7 (rel.) ^•/^BiOH = 1-5 X e-T. esr decay of spin 72-0039

11.5 10”2 polarization,

compared with EtOH.

For other ratios see: 2.91, 2.107, 2.110, 2.178, 2.239

2.91 HPOj” 13.6 1.5 x 10

9 (rel.) ^/^OH — 100 y-r. chem. c.k. 65-0155

H + HPO3 - -* H2 + — ( 1.8 ± 0 . 6) x 109 — y-r. chem. c.k.; rel. to 69-0051

por (rel.) kOH (value not

given). 2.91a h 3 po4 0 (5 ± 3) x 10

s — p.r. opt. p.b.k. at 500 nm. 73-1049

H + H 3 P04 -» H2 + H 2 P04 2.91b h 2 po; 3.85- (5 ± 3) x 10

s — p.r. opt. p.b.k. at 500 nm. 73-1049

h + h 2 po;-> 4.0 h 2 + hpo;

2,92 HP04 ” ~ 7 < 5 x 10

3 (rel.) — y-r.. chem. c.k. with CH3 OH 67-0099

son. and Co(NH3 ) s F

2+

; obs. G(H2 ); also

c.k. with ClCH2 COO”, obs. G(C1”). 9.0- < 5 x 10

4 — p.r. opt. p.b.k. at 500 nm. 73-1049

12.3 2.92a Pr(III) 1.9 < 10

3 (rel.) — — — c.k. with CHjOH.

72-0066

2.93 Pt(CN)4

” 5 > 2.4 x 10

9 (rel.) ^/^MeCDOHMe > y-r. chem. c.k. 66-0401

235

2.93a Ru(bipy) 2+ ~ 2 9.5 x 10

9 — p.r. opt. p.b.k. at 420 nm. 72-0381

2.93b Ru(bipy)3 + <4.5 1.7 x 10

9 — — no details. 72-0462

2.93c D 2 S D + D 2 S —* D2 + DS 6 . 0- 1 x 10

9 (rel.) k/kncoo~ = 7.5 y-r. chem. c.k. 65-0013

6.5 2.94 s,oi- ~ 0 2.4 x 10

7 (rel.) (1.2 ± y-r. chem. c.k.; 70-0169

H + S 2 0

2 ”^ HS04 + 0.1) x 10”3 ceric - cerous S02a ~ system used.

2.95 H 2 so 5 ~ 0 2.2 x 10* (rel.) k/kOXJ =(1.06 ± y-r. chem. c.k.; 70-0169

H + H 2 SOs -» H 2 0 + 0.06) x 10

2 ceric - cerous hso4 system used.

2.96- Sn(II) 0.8 klkFe 3+ = 6 x y-r. chem. c.k. 59-0007

H + Sn(II) —> Sn(I) 10

4 + H

+ 2.97 SnF3” 5 2.4 x 10

9 (rel.) k/ku*CDOHMe = y-r. chem. c.k. 66-0401

235

14
Table 3. Reactions of H with inorganic solutes — Continued

No. Solute and Reaction . pH ^(dm 3 mol-1

8

x

) Ratio Source 5 'Method Comment Ref.

2.98 Sn(lV)

H + Sn(IV) ^ H

+ +

Sn(III)

0.8 fc/*F.3+ = 2 y-r. chem. c.k. 59-0007

2.99 SnF’- 5 1.1 x 10 7 (rel.) ^MeCDOHMe =

1.06 y-r. chem. c.k. 66-0401

2.100 Te(VI)

H + Te(VI) Te(V)

0.4 6.6 x 10

7 (rel.) */*p— = 1-1 y-r. chem. c.k. 68-0356

2.101 Tl

+ 1,5 1.2 x 10® (rel.) ^MeCDOHMe = 12 y-r. chem. c.k. 66-0401

2.102 U02+ H + U02+ ^ UO; +

0-2

H

+ k/kH+ = 1.2 y-r. chem. c.k. with Fe

2+

oxid. at varying

pH; authors assume

that Fe

2+ + Fe^+Hj.

61-0099

2.103 Zn 2+ — < 2.6 x 10s (rel.) kl ^EtOH < 10 y-r. chem. c.k. 65-0192

15
Table 4. Reactions of H with organic solutes

No. Solute and Reaction pH jt(dm

3 mol 's *) Ratio Source Method Comment Ref.

2.104 acetaldehyde 1 3.4 x 10

7 (rel.) kl kBiOH = 3.4 X e-r. esr Decay of spin 71-0003

H + CHjCHO - 10~2 polarization,

H 2 + CH2 CHO compared with

(or CHjCO) (I) 2-PrOH(7D).

H + CHjCHO 1 2.9 x 10

7 (I) (rel.) kilkn = 4.9 y-r. chem. 83% H abstr. 73-0053

CHjCHOH (II) 2.105 acetamide 1 1.3 x 10

s (rel.) kl kto*OH = 1.3 X e-r. esr decay of spin 71-0003

10

-4 polarization,

compared with 2-PrOH(7D).

1 1.9 x 10

s (rel.) kl kB»OH ~ 1-9 x y-r. chem. c.k. with 71-0017

10"4 2-PrOH(7D),

H abstr. 2.106 acetanilide 8-9 1.1 x 10

9 (rel.) kl k2-PrOH = 13.4 y-r. chem. c.k. 66-0500

H + C 6 H 5 NHCOCH, 1 1.1 x 109 (rel.) ^BiOH = 1-1 e-r. esr decay of spin 72-0025

-» C 6 H6 NHCOCH3 polarization,

compared with EtOH.

2.107 acetate ion ~ 8 3.2 x 10

s (rel.) */*nitrite = 4.5 X-r. chem. c.k. 62-0017

H + CH3 COO'-» x 10

-4 H 2 + CHjCOO" 7 2.8 x 10

s (rel.) kl k DCOO - = (1-2 y-r. chem. c.k. 63-0041, ± 0.1) X 10~2 64-0095 ~ 7 ^Bkme = 4 X X-r. chem. c.k. 63-0049

10'2 11- 2 x 10

s (rel.) klkOH - = (1.1-2) X-r. chem. c.k. 63-0049

12 X 10”2 7 3.5 x 10

s (rel.) k/kBxOh = 4-2 x e-r. esr decay of spin 72-0039

10"1 polarization, compared with EtOH.

2.108 acetate ion-d3 6 2 x 10

4 (rel.) kl kAco- = (4-5 ± y-r. chem. c.k. 64-0141

H + CDjCOO" —> 0.8) x 10"2 HD + CDjCOO"

2.109 acetic acid 1 7.5 x 10

4 (rel.) kl k HCOOH =0.10 X-r. chem. c.k. 56-0012

H + CH3 COOH -> 1 8 x 10

4 (rel.) klk BiOH = 8 X e-r. esr decay of spin 71-0003

Hj + CH2 COOH 10"5 polarization;

compared with CD3 CDOHCD3

.

1 1.3 x 10

s (rel.) klkBiOH = 1-3 X y-r. chem. c.k. with 71-0017

10^ 2-PrOH(7D).

2.110 acetone 1 2.8 x 10

6 (rel.) kl kBiOH ~ 2.8 X e-r. esr decay of spin 71-0003

H + CH3 COCH3 ^ 10"3 polarization.

prod. compared with CD3 CDOHCD3

. H + CH3 COCH3 ^ 1 2.5 x 10

s

(I) (rel.) k\lk HCOOH =0-34 X-r. chem. c.k. 56-0012

Hj + CHjCOCH3(I) -7 6.4 x 10

s

(I) (rel.) kllk DCOO~ - y-r. chem. c.k. 63-0041,

(2.8 ± 0.3) X 64-0095

10‘2 11- 1.2 x 10

6

(I) (rel.) kilkon~

= 8-3 x X-r. chem. c.k. 63-0049

13 10"2

1 kilkc%2+ = 1-4 x X-r. chem. c.k. 63-0049

10"2 — 2.3 x 10

6

(I) (rel.) k llkAknMMK = y-r. chem. c.k.; solvent 67-0222

0.18 dioxane contg.

2.2 M water.

1 1.7 x 10° (1) (rel.) kllkBMH = X y-r. chem. c.k. with 71-0017

10"3 2—PrOH(7D).

1 1.9 x 10

6

(I) (rel.) Arn

Ar, = 0.49 y-r. chem. 67% H abstr.; 2.5 x 10”*% enol. 73-0053

16
Table 4. Reactions of H with organic solutes — Continued

No. Solute and Reaction pH k(dm 3 mol *s

l

) Ratio Source Method Comment Ref. H + CH3 COCH3 -> - 7 k\\/k\ = 0.2 X-r. chem. — 63-0049

CH3 COHCH3 (II) 1 ^ii/^-i = 0.3 X-r. chem. — 63-0049

1.2 V*i = 0.33 ± y-r. chem. — 65-0016

0.06 < 1 fc n

/k, = 0.33 y-r. chem. • 68-0525

2.111 acetonitrile 1 1.5 x 106 (rel.) k/kb*oh = x e-r. esr Decay of spin 71-0003

H + CH3 CN 10~3 polarization,

CH2 CN + H2 (I) compared with H + CH3 CN - 2-PrOH(7D).

CH3 CNH (II) 1 8 x 10

4 (rel.) (I) ^l/^B*OH = 0 X — — estimated. 71-0017

10“5

1 2.7 x 106 (rel.) ^Il/^BiOH =2.7 y-r. chem. c.k. with 71-0017

(II) X 10"3 2-PrOH(7D).

1 1 x 10

s

(I) (rel.) *„/*, = 13.3 y-r. chem. 7% H abstr. 73-0053

2.112 acetophenone 8.9 2 x 10

9 (rel.) k/k2-P1OH = 26 y-r. chem. c.k. 66-0500

H + C 6H5 COCH3 -- 1 (1.1 ± 0.2) x 10

9 —I* p.r. opt. p.b.k.; CD3 OD 69-0001 c 6 h6 coch3

(I) as OH scavenger. H + C 6 H5 COCH3 ^ 1 1.2 x 10

9 (rel.) ^/^BiOH = 1-2 e-r. esr Decay of spin 72-0025

h2 + polarization.

C 6 Hs COCH2 (II) compared with EtOH.

1 ~ 1 x 10

7 (II) kn

/kl = 0.01 y-r. chem. ~ 1% H abstr. 73-0053

(rel.) 1.0 (3.4 ± 0.6) x 109 — p.r. opt. p.b.k. (H 72-0171

adduct); /er/-BuOH

as OH scavenger.

2.113 acetylacetone 1 8.2 x 10

7 (rel.) — e-r. esr unpubl. data. 73-0053

H + CH3 COCH2 COCH3 P. Neta and R.H. CH3 COC=C(OH)CH3 Schuler. + h2 (I) ~2 x 10

6

(I) (rel.) kn/ki = 0.3 y-r. chem. 23% H abstr.; 80% enol form. 73-0053

H + CH3 COCH2 COCH3 ^

no H2 (II) 2.114 acetylene 7 1.1 x 10® (rel.) k/kficoo~ = 0.73 y-r. chem. c.k. 68-0502

2.115 acetylenedicar- 1 1.0 x 109(rel.) klk^tOH = 1 e-r. esr decay of spin 71-0040

boxylic acid polarization,

compared with EtOH.

2.116 iV-acetylalanine 1 8.0 x 10

6 (rel.) k/kjitOH = 8-0 x e-r esr decay of spin 71-0003

10~3 polarization,

compared with 2-PrOH(7D).

2.117 N-acetylglycine 1 3.8 x 10

6 (rel.) k/kibOH — 3.8 x e-r. esr decay of spin 71-0003

10"3 polarization,

compared with 2-PrOH(7D).

2.118 acrylamide 1-2 3.5 x 10

10 (rel.) k/kfmi = 5.0 ± p.r. opt. c.k., Fe(CN)3 ' 70-0052

0.6 measured at 420 nm.

2.119 adenine 7-8 8.5 x 10

7 (rel.) ^/^DCOO~ = 3.7 ± y-r. chem. c.k. 68-3038

1 8.3 x 10

7 (rel.) k/kfaOH = 8.3 x e-r. esr decay of spin 71-0040

10“2 polarization.

compared with EtOH.

2 6 x 10

7 — e-r. esr decay of H

signal.

71-0303

7 1 x 10® — e-r. esr decay of H

signal.

71-0303

7 (0.9 - 1.5) x 10* klkftzoyi = 0.09 — e-r. esr decay of spin 71-0040

(rel.) 0.15 polarization,

compared with EtOH.

17
Table 4. Reactions of H with organic solutes — Continued

No. Solute and Reaction pH k(dm 3 mol *s

!

) Ratio Source Method Comment Ref.

2.120 adenosine 7-8 1.4 x 10

8 (rel.) k/kdcoo - = 6 y—r. chem. c.k. 68-3038

1 1.1 x 10

8 (rel.) ^/^B*OH = Oil e-r. esr decay of spin

polarization,

compared with EtOH.

71-0040

7 (1.4-2) x 10

8 (rel.) kik b,oh = 0.14— e-r. esr decay of spin 72-0039

0.2 polarization,

compared with EtOH.

2.121 adenosine-5-phos- 7-8 1.5 x 10

8 (rel.) k/ kf)QQQ~ = 6.5 y-r. chem. c.k. 68-3038

phate

2.122 a-alanine 1 2.4 x 10

s (rel.) — y-T. chem. c.k. assuming 68-0343

k(H + allyl ale.) = 2.8 x 10

9

.

1 2.9 x 10

s (rel.) ^/^BiOH = 2.9 X e-r. esr decay of spin 71-0003

10

-4 polarization,

compared with 2-PrOH(7D).

2.123 /3-alanine 1 3.4 x 10

5 (rel.) k/ ^BxOH = 3.4 x e-r. esr decay of spin 71-0003

10"4 polarization,

compared with 2-PrOH(7D).

2.124 allyl alcohol - 6 3.6 x 10

9 (rel.) ^/^2-PrOH = y-r. chem. c.k. 63-0041,

H + CH2 =CHCH2 OH 46 ± 5 64-0095

H 2 + C 3 Hs O (I) ~0.4 4.7 x 10

9 (rel.) klk+ = 100 y-r. chem. c.k. 68-0525

1 1.9 x 10

9 (rel.) k/k^cooH ~ 2-6 x y-r. chem. c.k.; author 68-0343

10

3 ealed. k = 2.8 x

10

9 assuming

^hcooh ~ 11 x 10

6

. H + CH2 =CHCH2 OH 1,7 JJf a

II nB o 1+ y-r. chem. c.k.; effect on 70-0468

C 3 H6 OH (II) 0.2) x 10~2 G(H 2 ) from water.

1 - 5 x 10

7 (I) (rel.) k\l

k

u = 2 x y-r. chem. — 2% H abstr. 73-0053

10“2 For rates relative to allyl alcohol see: 2.122, 2.125a, 2.204, 2.206, 2.247, 2.272,

2.282, 2.287, 2.292, 2.292a, 2.292b, 2.312a, 2.317a, 2.330, 2.353, 2.371, 2.387. 2.125 aminoacetonitrile 1 6.6 x 10

6 (rel.) ^/^BxOH — 6.6 X e-r. esr decay of spin 72-0039

H + H 2 NCH2 CN 10“3 polarization.

H 2 + H2 NCHCN (I) compared with EtOH.

H + H 2 NCH2 CN -» 7 5.6 x 10

7 (rel.) ^•/^•BiOH = 3.6 X e-r. esr decay of spin 72-0039

H2 NCH2 CHN (II) 10~2 polarization.

compared with EtOH.

1 - 6 x 10

4

(I) (rel.) k\lk u = 10 y-r. chem. — 1% H abstr. 73-0053

7 3.2 x 10

7 (I) (rel.) ki/k n = 1.4 (58% at pH7).

2.125a 2-aminobutyric 1 6.0 x 10

s (rel.) — y-r. chem. c.k. assuming 68-0343

acid k(H + allyl ale.) = 2.8 x 109

. 2.126 2-aminoethanol 1 3.0 x 10

6 (rel.) klkfoOH = 3.0 x e-r. esr decay of spin 71-0040

10"3 polarization,

compared with EtOH.

2.127 2 -amino-2- methyl- 1 8 x 10

4 (rel.) k/k^^oH = 8 x e-r. esr decay of spin 71-0003

propionic acid 10

_s polarization,

compared with 2-PrOH(7D).

2.128 aniline 8-9 2.8 x 10

9 (rel.) klk2-p^)H = 36 y-r. chem. c.k. 66-0500

H + C 6 Hs NH2 -> 7 2.6 x 10

9 (rel.) k/kfaOH — 2.6 e-r. esr decay of spin 72-0025, c 6 h6 nh2 polarization,

compared with EtOH.

72-0039 — (2.9 ± 0.7) x 10

9 — p.r. opt. p.b.k. at 350 nm. 72-0289

18
Table 4. Reactions of H with organic solutes — Continued

No. Solute and Reaction pH k(dm 3 mol *s

x

) Ratio Source Method Comment Ref.

2.129 anilinium ion 1 4.9 x 10

8 (rel.) kl ^BxOH = 0-49 e—r. esr decay of spin 72-0025

H + C 6 H5 NH3+ ^ polarization, c 6 h6 nh3+

3 (1.3 ± 0.2) x 10

9 p.r. opt.

compared with EtOH.

p.b.k. at 310 nm. 72-0289

2.130 anisole 1 1.2 x 10

9 (rel.) ^/^BxOH = 1-2 e-T. esr decay of spin

polarization;

compared with EtOH.

72-0025

2.131 anthracene 1.0 x 10

9 (rel.) ^Mdioxane = 78 y-r. chem. c.k.; solvent dioxane contg.

2.2 M water.

67-0222

2.132 9,10-anthraquinone— 1.0 (4.1 ± 0.3) x 10

9 p.r. opt. p.b.k. (H 72-0171

2-sulfonate ion adduct); fert-BuOH

as OH scavenger.

2.133 L-arabinose 1 5.7 x 10

7 (rel.) kl ^BiOH = 8 - 7 x e-r. esr decay of spin 71-0040

10'2 polarization,

compared with EtOH.

2.134 L-arginine 1 4.9 x 10

6 (rel.) kl ^BiOH = 4.9 x e-T. esr decay of spin 71-0040

10~3 polarization,

compared with EtOH.

2.135 ascorbate ion 7 (3-6) x 108 (rel.) kl ^BiOH = 0.3 — e-r. esr decay of spin 72-0039

0.6 polarization,

compared with EtOH.

2.136 ascorbic acid IS • 3.6 x 10

8 (rel.) k/k2-PiOH = 4.5 y-r. chem. c.k. 70-3023

H + C 5 H7 06 -» 1 1.1 x 10

8 (rel.) k/kBlOH ~ 0.11 e-r. esr decay of spin 71-0040

H 2 + C s H6 06

(I) polarization,

H + C 5 H7 06 —

>

compared with no H 2 (II) 1 ~ 2 x 10

6 (I) kfkn = 0.02 y-r. chem.

EtOH. — 2% H abstr. 73-0053

1 1.7 x 10

8 (rel.) k/k2-ptoh = 2.2 p.r. opt. c.k.; obs. 360 nm abs. 72-0266

2.137 DL -asparagine 1 4.7 x 10

5 (rel.) ^/^BxOH *4.1 X e-T. esr decay of spin 71-0040

10

-4 polarization,

compared with EtOH.

2.138 aspartate ion 7 2.9 x 10

6 (rel.) ^/^BiOH = 2.9 X e-r. esr decay of spin 72-0039

10“3 polarization,

compared with EtOH.

2.139 DL -aspartic acid 1 8 x 10 s (rel.) k/ ^BxOH = 8 X e-r. esr decay of spin 71-0040

10~* polarization,

compared with EtOH.

2.140 barbiturate ion 7 2.0 x 10

9 (rel.) ^•/^BiOH = 2.0 e-T. esr decay of spin

polarization,

compared with EtOH.

72-0039

2.141 barbituric acid 1 2.0 x 10

7 (rel.) kl ^BiOH = 0-02 e-T. esr decay of spin 71-0040

H + C 4 H4 N2 03 -* polarization,

H2 + C 4 H3 N2 03 compared with

(I) EtOH.

H + C 4 H4 N2 03 -» 1 2.4 x 10

6 (II) (rel.) knl ki= 7.3 y-r. chem. 12% H abstr. 73-0053

no H 2 (II)

19
Table 4. Reactions of H with organic solutes — Continued

No. Solute and Reaction pH /c(dm

3 mol_1 s *) Ratio Source Method Comment Ref.

2.142 benzaldehyde 1 1.5 x 10

9 (rel.) k/kBlOH =1-5 e-r. esr decay of spin 72-0025

C 6 H s CHO + H ^ polarization,

C 6 H s CO + H2 (I) compared with C 6 H s CHO + H — EtOH.

C 6 H 6 CHO (II) 1 6 x 10

7 (I) (rel.) knl ki = 24 y-r. chem. — 4 % H abstr. 73-0053

2.143 benzamide 1 8.9 x 10

8 (rel.) ^/^BiOH = 0.89 e-r. esr decay of spin

polarization,

compared with EtOH.

72-0025

2.144 benzene 0 9 x 10

8 (rel.) ^/^PhOH = 0-5 y-r. chem. compared effect 59-0006

H + C 6 H6 -» C 6 H 7 of C 6 H6 and

C 6 H5 OH on G(Fe3+

) in Fe

2+ soln. 3 (1.1 ± 0.1) x 10

9 p.r. opt. p.b.k. at 311 nm;

contains ~ 2 x 10~2 A/ CH3 OH,

assumed

67-0246

*(H + CH3 OH) =

1.6 x 10

6

. 2.0 5.3 x 10

8 (rel.) ^/^PNBA = 5.3 X p.r. opt. c.k.; build-up of 70-0211

10"1 /?-nitrobenzoic

acid-H adduct

2.145 benzenesulfonate 8-9 6.7 x 10

8 (rel.) ^/^2-PrOH =8.6 y-r. chem. c.k. 66-0500

ion 1 (8.2 ± 1.3) x 108 — p.r. opt. p.b.k. 69-0001

H + C 6 H5 S03-^ CD3 OD as OH

c 6 h 6 so 3-

6.3 x 10

8 scavenger. D + C 6 H5 SOJ—

>

1 — p.r. opt. p.b.k.; in D2 0. 69-0001 c 6 h 5 dso3 2.146 1,3,5-benzene— 1 6.5 x 10

8 (rel.) k/kb*oh = 0.65 e-r. esr decay of spin 71-0003

tricarboxybc acid

(1.0 ± 0.2) x 10

10

polarization,

compared with 2-PrOH(7D).

2.147 benzil 1.0 — p.r. opt. p.b.k. (H 72-0171

H + C 6 H5 COCOC6 H adduct); ferf-BuOH

C 6 H6 COCOC6 Hs as OH scavenger.

2.148 benzoate ion 8-9 1.4 x 10

9 (rel.) k/k2-PrOH =17.4 y-r. chem. c.k. 66-0500

H + C 6 H5 COO'^ 7 9.2 x 10

8 (rel.) ^/^•BiOH = 0.92 e-r. esr decay of spin 72-0039

C 6 H6 C00‘ polarization,

compared with EtOH.

2.149 benzoic acid 3 1.0 x 10

9 — p.r. opt. p.b.k. at 347 nm; 69-0001

(BzOH) CD3 OH as OH

H + C 6 H5 COOH scavenger. £ 6 H6 COOH — 1.2 x 10

9 (rel.) ^/^MeOH = 590 p.r. opt. c.k.; p.b.k. 69-0001

1 8.1 x 10

8 (rel.) k1 k 2-PrOHOt)) = e-r. esr decay of spin 71-0003

81 polarization. — 8.3 x 10

8 — e-r. esr decay of H

signal.

71-0303

1 8.8 x 10

8 (rel.) k/kfMH = 34 e-r. esr decay of spin

polarization.

72-0025

1 — — y-r. chem. < 1% H abstr. 73-0053 For other ratios see: 2.90, 2.104-5, 2.107, 2.109-12, 2.115--17, 2.119-20, 2.122-3, 2.125-30, 2.133-43, 2.146, 2.148-50, 2.153-4, 2.159-60,

2.162, 2.168-72, 2.175, 2.177, 2.181, 2.183-4, 2.189-91,

2.197, 2.200, 2.202, 2.205, 2.207, 2.209, 2.211-16, 2.218-9,

2.223-4, 2.229-32, 2.237, 2.239, 2.241 , 2.244, 2.245-7,

2.249, 2.250-5, 2.259, 2.261- 70, 2.272 -7, 2.279-83,

2.285-90, 2.294, 2.2%, 2.303, 2.305, 2.307, 2.311,

2.313, 2.315, 2.317--8, 2.320- 1, 2.323--7, 2.330, 2.332-9,

2.342-7, 2.349, 2.351, 2.353- 5, 2.357, 2.358, 2.360,

2.362, 2.365-8, 2.370-1, 2.374, 2.377, 2.380, 2.383-8

20
Table 4. Reactions of H with organic solutes — Continued

No. Solute and Reaction pH k(dm 3 mol x s

x

) Ratio Source Method Comment Ref.

D + C 6 H5 COOH 1 7.6 x 10

8 — p.r. opt. p.b.k.; in D 2 0. 69-0001

C 6 Hs DCOOH

2.150 benzonitrile 8-9 7.2 x 10

8 (rel.) k/k2-PrOH ~ 9.06 y-r. chem. c.k. 66-0500

H + C 6 Hs CN 1 6.8 x 10

8 p.r. opt. p.b.k.; CD 3 OH as 69-0001 c 6 h6 cn

8 x 10

8 (rel.) ^/^MeOH = 4 X p.r. opt. OH scavenger

c.k.; p.b.k. 69-0001

10“2 2 5.5 x 10

8 (rel.) */*fcrri= 7.8 X p.r. opt. c.k. 70-0657

10~2

1 6.4 x 10

s (rel.) k/k BiOH = 0-64 e-r. esr decay of spin

polarization,

compared with EtOH.

72-0025

2.151 benzophenone 3 x 10

8 (rel.) = 24 y-r. chem. c.k.; solvent is dioxane containing

2.2 M water.

67-0222

1.0 (5.6 ± 0.3) x 10

9 p.r. opt. p.b.k. (H

adduct); fert-BuOH

as OH scavenger.

72-0171

2.152 benzoquinone (Q) 1.0 2.3 x 10

9 (rel.) kl ^hcooh = 3000 X-r. chem. c.k. 56-0012

H + 0=C6 H4 =0 -* — 1.5 x 10

9 (rel.) ^/^MeOH = 750 ± y-r. chem. c.k. 58-0009 o=c 6 h4 oh 40 — 1.4 x 10

10 (rel.) = 350 ± y-r. chem. c.k. 65-0192

150

1.9 8.3 x 10

9 — p.r. opt. p.b.k. at 410 nm. 71-0618,

71-0619 For other ratios see: 2.89, 2.363

•2.152a 2—benzoylpyridine 1.0 (2.3 ± 0.4) x 10

9 p.r. opt. p.b.k. at 348 nm; H adduct formn. 72-0359

2.152b 3-benzoylpyridine 1.0 (3.7 ± 0.6) x 10

9 — p.r. opt. p.b.k. at 400 nm; H adduct formn. 72-0359

2.152c 4—benzoylpyridine 1.0 (2.4 ± 0.3) x 10

9 —

p.r. opt. p.b.k. at 375 nm; H adduct formn. 72-0359

2.153 benzyl alcohol 6 1 x 10

9 (rel.) ^/^2-PtOH = 13 ± y-r. chem. c.k. 63-0041,

H + C 6 H5 CH2 OH-+ 2.0 64-0095

h 2 + c 6 h5 choh ~0.4 9.4 x 10

8 (rel.) = 20 y-r. chem. c.k. 68-0525

(I) 1 1.1 x 10

9 (rel.) ^•/^BiOH = 1-1 e-r. esr decay of spin 72-0025

H + C 6 Hs CH2 OH polarization,

C 6 H6 CH2 OH (II)

1 8 x 10

7 (I) (rel.) kjkn = 0.07 y-r. chem.

compared with EtOH.

7% H abstr. 73-0053

2.154 betaine 1 8 x 10

4 (rel.) klk^zon = 8 x e-r. esr decay of spin 71-0040

10~5 polarization,

compared with EtOH.

2.155 biacetyl 1 4.7 x 10

6 (rel.) — e-r. esr unpubl. data, 73-0053

H + CH3 COCOCH3 ^ P. Neta and R.H. H2 + CH2 COCOCH3 Schuler.

(I) 1 9.4 x 10

s (I) (rel.) kx lkn = 0.25 y-r. chem. 20% H abstr. 73-0053

H + CH3 COCOCH3 -> no H 2 (II) 2.156 2,2'-bipyridine 1 1.5 x 10

8 — p.r. opt. p.b.k. 71-0582

2.157 4,4'-bipyridine 1 2 x 10

8

:— p.r. opt. p.b.k. 71-0582

2.158 bromoacetate ion H + BrCH2 C02 —

»

8.5 5.5 x 10* (rel.) ^/^•2-PrOH = 7.0 y-r. chem. c.k. 67-0050

HBr + CHjCOj

D + BrCH2 C02 ^ 8.5 3.2 x 10

6 (rel.) Ik 2-PrOH $ 4x y-r. chem. c.k. in DjO. 67-0050

HD + BrCHCOO" 10"2

21
Table 4. Reactions of H with organic solu[es — Continued

No. Solute and Reaction pH )t(dm

3 mol *sl )

y Ratio Source Method Comment Ref.

2.159 bromoacetic acid H + BrCH 2 COOH -> H 2 + CHBrCOOH (I

1

) < 3.6 x 10

6 (rel.)(I) ^i/^BiOH ^ 3.6 X

10

"3 y-r. estimated; c.k. with 2-PrOH(7D).

71-0017

H + BrCH2 COOH -* HBr + CH2 COOH

1.0 4.7 x 10

8 (rel.) (II) kill ^2-PiOH =

6.0 y-r. chem. c.k. 67-0050

(II) 1

1

~0.4

2.6 x 10

8 (rel.) (II)

3.6 x 10

8 (rel.) (II)

4.7 x 10

8 (rel.) (II)

^/^BiOH = 0-26

^Il/^BiOH = 0-36

10

e-r.

y-r.

y-r.

esr

chem.

chem.

decay of spin

polarization,

compared with 2-PrOH(7D).

c.k. with 2-PrOH(7D).

c.k.

71-0003

71-0017

68-0525

D + BrCH 2 COOH

HD + CHBrCOOH

1.0 < 4.7 x 10s (rel.) ^/^2-PrOH ^ 6 X 10'3 y-r. chem. c.k. in D2 0. 67-0050

2.160 bromoethane

H + BrCH2 CH3 H 2 + BrC 2 H4

(I) H + BrCH2 CH3 ->

1 1.7 x 10

8 (rel.) ^/^BiOH = 0.17 e-r. esr decay of spin

polarization,

compared with 2-PrOH(7D).

71-0003

2.161 HBr + C 2 H5 (II) 2-bromoethanol

1 - 5 x 10

6

(I) (rel.) kx !k n = 0.03 y-r. chem. — 3% H abstr. 73-0053

H + BrCH 2 CH2 OH

HBr + CH2 CH2 OH

1,9 2.7 x 10

8 (rel.) ^/^2-PrOH =3.4 y-r. chem. c.k. 67-0050

D + BrCH2 CH2 OH

HD + BrCHCH2 OH

1,9 2.7 x 10

7 (rel.) k/k2-PrOH = 0.34 y-r. chem. c.k. in D2 0. 67-0050

2.162 5-bromoorotic acid 1 2.1 x 10

8 (rel.) ^/^B*OH ~ 0.21 e-r. esr decay of spin

polarization,

compared with EtOH.

71-0040

2.163

2.164

p-bromophenol

2-bromopropionate io i

4.9 x 10

9 (rel.) i = 0-7 e.d. condy. obs. Br

_ formn. and ferricyanide reduction (opt.)

71-9384

H + CH3 CHBrCOO~ |8.5 -> HBr + CHjCHCOO"

1.3 x 10

9 (rel.) k/k2-PrOH = 17 y-r. chem. c.k. 67-0050

2.165

D + CHjCHBrCOO- |8.5 -* HD + CHjCBrCOO'

3-bromopropionate ion

2.5 x 10

7 (rel.) k/k2-P1OH = 0.32 y-r. chem. c.k. in D2 0. 67-0050

H + BrCH 2 CH2 COO"|8.5

-> HBr + CH2 CH2 COO'

3 x 10

8 (rel.) k/k2-P1OH =3.8 y-r. chem. c.k. 67-0050

2.166

D + BrCH2 CH2 COO"|8.5 ^ HD + BrCHCH2 COO”

2-bromopropionic acid

1.1 x 10

7 (rel.) klk2-ptOH = 0-14 y-r. chem. c.k. in D2 0. 67-0050

H + CHjCHBrCOOH |l.O

HBr + CH3 CHCOOH

1.5 x 10

9 (rel.) ^/^2-PrOH = 10 y-r. chem. c.k. 67-0050

2.167

D + CHjCHBrCOOH |l.O -> HD + CHjCBrCOOH

3-bromopropionic acid

6.3 x 10

6 (rel.) ^/^2-PrOH =0.08 y-r. chem. c.k. in D2 0. 67-0050

H+CH 2 BrCH2 COOH |l.O

HBr + CH2 CH2 COOH

2.7 x 10* (rel.) k/ki-PrOH = 3.4 y-r. chem. c.k. 67-0050

D+CH2 BrCH2 COOH |l.O -» HD + CHBrCH 2 COOH4.7 x 10

6 (rel.) k/k2-PrOH = 0.06 y-r. chem. c.k. in DjO. 67-0050

2.168 5-bromouracil 1 2.2 x 10* (rel.) k/kutoH — 0.22 e-r. esr decay of spin

polarization,

compared with EtOH.

71-0040

2.168a butadiene — 1 x 10

10 (rel.) klkntOR = 5 x 10 — — c.k.; no details given.

67-0041

22
Table 4. Reactions of H 'with organic solutes — Continued

No. Solute and Reaction pH k(dm 3 mol l s

*) Ratio Source Method Comment Ref.

2.169 butane 1 3.9 x 10

7 (rel.) k/k BxOH = 3.9 X e-r. esr decay of spin 71-0003

10~2 polarization,

compared with 2-PrOH(7D).

2.170 1-butanol 1 3.84 x 10

7 (rel.) k/k bioh = 3.84 x e—r. esr decay of spin 71-0003

H + CH3(CH2 ) 30H-^ 10'2 polarization.

h 2 + c 4 h8 oh

1 3.7 x 10

7 (rel.) k/k Bxoh = 3. 7 X y-T. chem.

compared with 2-PrOH(7D).

c.k. with 71-0017

10"2 2-PrOH(7D).

2.171 2-butanol

H + C 2 H5 CHOHCH3 1 1.3 x 10

8 (rel.) ^/^BxOH = 0-13 e-r. esr decay of spin 71-0003

-+ h2 + c 4 h8 oh

1 9.5 x 10

7 (rel.) klkhMB = 9.5 x y-T- chem.

polarization,

compared with 2-PrOH(7D).

c.k. with 71-0017

10~2 2-PrOH(7D).

2.172 ter/-butanol

H + (CH3 ) 3 COH -* 7 1.0 x 10

s (rel.) klkoQQQ— = 4.4 ± y-r. chem. c.k. 63-0041,

h2 + c 4 h8 oh 0.7) x 10"3 64-0095

1 8 x 10

4 (rel.) = 3 X e—r. esr decay of spin 71-0003

10'5 polarization,

compared with 2-PrOH(7D).

2 1.7 x 10

s p.r. esr decay of H

signal; high

concn.; k concn. dependent.

71-0303

2.173 1-butene -5.4 x 10

9 (rel.) k/ ^MeOH — 2.7 X — — c.k., no details 67-0041

H + C 4 H8 ^ C 4 H9 10

3 given. 2.174 butyrate ion 7 1.4 x 10

s (rel.) k/k MeCDOHMe ~ y-r. chem. c.k. 66-0422

H + CH3 CH2 CH2 COCT-* 1.4 x 10“2 h2 + c 3 h6 coo

_

2.175 butyric acid 1 8.6 x 10

6 (rel.) ^•/^BiOH = 3-6 X e—r. esr decay of spin 71-0003

H + CH3 CH2 CH2 COOH 10~3 polarization,

h2 + c 3 h6 cooh

1 7.4 x 10

6 (rel.) ^/^BxOH — 7.4 X y-r. chem.

compared with 2-PrOH(7D).

c.k. with 71-0017

10“3 2-PrOH(7D).

2.176 carbon disulfide 1 2.0 x 10

10 p.r. opt. p.b.k. at 310 nm. 73-1015

H + CS2 ^ H

+ + SCS"

2.177 carbon 1 4.8 x 10

7 (rel.) ^/^BiOH ~ 4.8 X e—r. esr decay of spin 71-0003

tetrachloride 10"2 polarization,

H + CCl4 -» H

+ + compared with cr + CC13 3.2 x 10

7 p.r. condy.

2-PrOH(7D).

p.b.k. 71-0778

2.178 chloroacetate ion 3-8 1.5 x 10

s (rel.) k/k H = 1.5 x e.d. chem. c.k. 62-9008

H + cich2 coct-» 10

_s H2 + C1CHCOO” 12.7 3.3 x 10

6 (rel.) k\lk()B ~ = 0.22 e.d. chem. c.k. 62-9011

(I) ~ 7 1.9 x 10

6 (rel.) klkocoQ~ = ^8.4 y-r. chem. c.k. 63-0041, ± 1.2) x 10"2 64-0095

H + ClCHjCOO" -* 3-8 knlkt = 0.09 e.d. chem. — 62-9008

HC1 + CHjCOO"

(II) For other ratios see: 2.9, 2.55

23
Table 4. Reactions of H with organic solutes — Continued

No. Solute and Reaction pH &(dm 3 mol l s *) Ratio Source Method Comment Ref.

2.179 chloroacetic acid 0.4-2 1.3 x 10

4 (rel.) k/kH = 1.3 x e.d. chem. c.k. 62-9008

H + ClCH 2 COOH -+ lO^6 H 2 + CHC1COOH 1 kulkt = 0.55 •y-r. chem. — 61-0025

.(I) < 2 kulki = 0-5 — e.d. chem. — 62-9008

H + ClCH 2 COOH -* 0.1 HC1 + CH 2 COOH ~ 0.4 kjk^ 0.61 y-r. chem. — 68-0525

(II) 2.180 p-chlorobenzoic 1 1.13 x 10

9 — p.r. opt. p.b.k.; CD3 OH as 69-0001

acid H + C 6 H4 C1C00H

OH scavenger.

C 6 H 5 C1C00H

2.181 chloroethane 1 1.8 x 10

6 (rel.) k/k BroH = 1-8 x e-r. esr decay of spin 71-0003

10~3 polarization,

compared with 2-PrOH(7D).

2.182 2— chloroethanol H + C1CH 2 CH2 0H 2.4 x 10

6 (rel.) ^2-PiOH ~ 3 X y-r. chem. c.k. 67-0050

HC1 + CH2 CH2 OH 10“2 D + C1CH 2 CH2 0H -> — 2.4 x 10

7 (rel.) ^/^2-PiOH = 0-3 y-r. chem. c.k. in D2 0. 67-0050

HD + CHC1CH 2 0H

2.183 chloroform H + CHC13 ^ HC1 + ~ 1 8.5 x 10

s (II) (rel.) — r. chem. c.k. in presence 62-0012,

CHC12 (II) of Fe

2+ assuming

k(OH + CHC13 ) =

7.4 x 10

6

.

66-9002

1 1.2 x 10

7 (rel.) k/kbxoh - 1-2 x e-r. esr decay of spin 71-0003

10“2 polarization,

compared with 2-PrOH(7D).

H + CHCl3 -» H 2 + 1 2.4 x 10

6

(I) (rel.) krfkn = 0.25 y-r. chem. 20% H abstr. 73-0053

CC13 (I) 2.184 chloromethane 1 7 x 10

4 (rel.) ^/^BzOH = 7 X e-r. esr decay of spin 71-0003

H + CH3 C1^ H 2 +

10“5 polarization,

CH2 C1 (I) compared with . 2-PrOH(7D).

H + CH3 C1^ no H21 3 x 10

4

(I) (rel.) ki/k n = 0.59 y-r. chem. 37% H ahstr. 73-0053

(II) 2.185 2-chloropropionate ion H + CH3 CHC1C0 2 ^ 8.5 1.9 x 10

7 (rel.) ^/^2-PiOH : 0.24 y-r. chem. c.k. 67-0050

HC1 + CH3 CHC02 D + CH 3 CHC1C0 2 -+ 8.5 4.7 x 10

6 (rel.) ^/^2-PrOH - 6 X y-r. chem. c.k. in D2 0. 67-0050

HD + CH3 CC1C02 10~2 2.186 3-chloropropionate ion H + CH2 C1CH2 C0 2 —>8.5 9.1 x 10

7 (rel.) ^/^2-PrOH =1-2 y-r. chem. c.k. 67-0050

hci + ch2 ch2 co: D + CH 2 C1CH 2 C02 —»8.5 2.4 x 10

7 (rel.) ^/^2-PiOH 0-3 y-r. chem. c.k. in D2 0. 67-0050

HD + CHClCHjCO2 2.187 2-chloropropionic acid H + CH3 CHClCOOH 1.0 5 x 10

6 (rel.) ^/^2-PK)H = 6.4 X y-r. chem. c.k. 67-0050

-» HCI + CH3 CHCOOH 10~2 D + CH3 CHC1C00H 1.0 4 x 10

6 (rel.) ^/^2-PrOH = 5 X y-r. chem. c.k. in D2 0. 67-0050

-> HD + CH3 CClCOOH 10"2

24
Table 4. Reactions of H with organic solutes — Continued

No. Solute and Reaction pH £(dm 3 mol *s *) Ratio Source Method Comment Ref.

2.188 3-chloropropionic acid H+CH 2 C1CH2 C00H 1.0 -> HC1 + CH2 CH2 COOH

3 x 10

7 (rel.) k/k2-PiOH = 0.38 y-r. chem. c.k. 67-0050

d+ch2 cich2 cooh 1.0 HD + CHClCHjCOOI1.6 x 10

7 (rel.) ^/^2-PrOH = 0-2 y-r. chem. c.k. in D 2 0. 67-0050

2.189 chlorotrifluoro- methane

1 < 10

6 (rel.) k/k b*oh < 103 e-r. esr decay of spin

polarization,

compared with 2-PrOH(7D).

71-0003

2.190 5-chlorouracil 1

7

1.6 x 10

8 (rel.)

2.2 x 10

8 (rel.)

^/^BxOH ~ 0.16

^/^BxOH =0.22

e-r.

y-r.

esr

chem.

decay of spin

polarization,

compared with EtOH.

c.k. with 2-PrOH(7D).

71-

0040 72-

0049

2.191 citric acid 1 4.3 x 10

s (rel.) 10

-4 e-r. esr decay of spin

polarization,

compared with EtOH.

71-0040

2.192 cyanoacetic acid H + NCCH2 COOH -

h 2 + ncchcooh

1

(I)

3.2 x 10

6 (rel.) kl ^BxOH = 3.2 x 10“3 e-r. esr decay of spin

polarization,

compared with 2-PrOH(7D).

71-0003

H + NCCH2 COOH ^1

HNCCH2 COOH (II) 4 x 10s

(I) (rel.) ki/k n = 0.14 y-r. chem. 12% H abstr. 73-0053

2.193 cyclobutanecarboxylic acid H + C 4 H7 COOH

1 1.3 x 10

7 (rel.) e—r. esr unpubl. data,

P. Neta and R.H.

Schuler.

73-0053

H2 + C 4 H6 COOH(I

H + C 4H7 COOH->

C 4 H8 COOH (II)

>1 9.2 x 10

6

(I) (rel.) ki/k u = 2.4 y-r. chem. 71% H abstr. 73-0053

2.194 cycloheptatriene — 8.4 x 109 (rel.) k/klari = 1.2 p.r. opt. c.k. 71-0710

2.195 1,3— cyclohexadiene 2.0 (9.8 ± 2.0) x 10

9

(rel.) ^/^PNBA = 9.8 ±

2.0

p.r. opt. c.k., p.b.k. at 400 nm.

70-0211

2.196 1,4— cyclohexadiene 2.0 (4.7 ± 1.0) x 10

9

(rel.)

k/kpffBA = 4.7 ±

1.0

p.r. opt. c.k., p.b.k. at 400 nm.

70-0211

2.197 cyclohexane — k/k Cjl 2 + = 1.2 y-r. chem c.k. 66-0810

H + CgH^ —

>

H 2 + C 6 Hjj

1 3 x 10

7 (rel.) klk^xoii = 0-03 e-r. esr decay of spin

polarization,

compared with 2-PrOH(7D).

71-0003

2.198 cyclohexene 2.0 (3.0 ± 0.6) x 10

9

(rel.) ^/^PNBA = 3.0 ±0.6

p.r. opt. c.k., p.b.k.

at 400 nm.

70-0211

2.199 cii-4— cyclohexene—

1,2— dicarboxylic

acid

1 1.0 x 10

9 (rel.) e-r. esr unpubl. data,

P. Neta and

R.H. Schuler.

73-0053

H + C 6 H8 (COOH)2 -^ H2 + C 6 H7 (COOH)j

H + C 6 H8 (COOH)2 -> no H 2 (II)

1

(I)

8 x 10

7 (I) (rel.) _k1 lk n s 0.08 y-r. chem. 8% H abstr. 73-0053

2.200 cyclopentane 1 3 x 10

7 (rel.) k/k^oE = 0.03 e-r. esr decay of spin

polarization,

compared with 2—PrOH(7D).

71-0003

2.201 1 -cyclopentane—

carboxylic acid H + C 5 H9 COOH ->

1 1.5 x 10

9 (rel.) e-r. esr Unpubl. data,

P. Neta and

R.H. Schuler.

73-0053

H2 + C s H8 COOH(I)

H + C 5 H9 COOH

no H2(II)

1 1.4 x 10

8

(I) (rel.) kjkn = 0.09 y-r. chem. 9% H abstr. 73-0053

25
Table 4. Reactions of H with organic solutes — Continued

No. Solute and Reaction pH /c(dm

3 mol *s *) Ratio Source Method Comment Ref.

2.202 cyclopropane 1 7 x 10

s (rel.) ^/^BiOH = 7 X e-r. esr decay of spin 71-0003

10-4 polarization,

compared with 2-PrOH(7D).

2.203 cyclopropane- 1 5.3 x 10

6 (rel.) — e-r. esr Unpubl. data 73-0053

carboxylic acid P. Neta and

H + C 3 H 5 COOH R.H. Schuler. h 2 + c 3 h 4 cooh 1 4 x 10

4

(I) (rel.) k{ lk n = 0.08 y-T. chem. 8% H abstr. 73-0053

(I) H + C 3 H 5 COOH -+ no H 2 (II) 2.204 cysteamine 2 3.0 x 10

9 — p.r. esr decay of H 71-0303

H + HSCH2 CH2 NH3 +

7.0 x 10

8 (rel.)

signal. -> H 2 (I) 1 — y-r. chem. c.k. assuming 73-0241

H + HSCH2 CH2 NH3 +(I + II) &(H + allyl ale.) -> H 2 S (II) 4.9 x 10

8

(I) (rel.) k\lk\\ ~ 2.3 ± = 2.8 x 10

9

. 2.1 x 10

8 (II) (rel.) 0.2 2.205 cysteine (positive 0.72 kilk u = 1.5 y-r. chem. c.k. 64-0151

ion) 1 2.5 x 10

9 (rel.) — — — c.k. with 66-0402

HSCH2 CH(NH^COOH + (I) cystine; cystine

H^H2 (D

0 kfk n = 3.5 y-r. chem.

formn. based on yields 67-0148

HSCH2 CH(NH^COOH + of H2 , H2 S and

H -» H 2 S (II)

1 4 x 10

9 (rel.) (I) k1 /k OIJ = 1.95 x y-r. chem.

cystine; ratio at 1°C = 8.6. c.k. 68-0540

10"1

1 kl /k u = 3.66 y-r. chem. c.k.; kjk^ =

5.4 x 10~2. 68-0540

1 4 x 10

9 (rel.) WkBrOH = 4 e-r. esr decay of spin

polarization,

compared with EtOH.

72-0025

2 3.0 x 10

9 — p.r. esr decay of H

signal.

71-0303

1 2.7 x 10

9

(I) (rel.) ki/k n =2.1 y-r. chem. 68% H abstr. 73-0053

1 1.5 x 10

9 (rel.) — y-r. chem. c.k. assuming 73-0241

(I + II) k(H + allyl ale.) 1.3 x 10

9

(I) (rel.) k\/k n = 5.2 ± = 2.8 x 10

9

. 2.5 x 10

8 (II) (rel.) 0.7 2.206 cysteine (zwitterion) HSCH2 CH(NH+)CO- 6 (1.0 ± 0.08) x 10

9 e.d. chem. d.k. for -SH 64-9012 + H H2 (I) (I) groups at ~ 5°C. HSCH2 CH(NH3+ )C02

, 6 (1.1 - 1.4) x 10

8 — e.d. chem. p.b.k. for H2 S 64-9012

+ H — H2 S (II) (II) at ~ 5°C. HSCH2 CH(NH+)CO~ 6 < 5 x 10

7 (III) — — — in D2 0; H abstr. 66-0402

+ D ^ HD (III) from C-H.

2.207 cystine 6 1.5 x 10

9 e.d. chem. p.b.k. for H2 S or -SH groups at ~ 5°C.

64-9012

1 7.9 x 10

9 (rel.) k/k 2-PjOH = 10® y-r. chem. c.k. 66-0402

1 2.15 x 10

9 (rel.) k/kncooH = 2870 y-r. chem. c.k. 68-0343

1 8 x 10

9 (rel.) klkfrOH = ® e-r. esr decay of spin

polarization,

compared with EtOH.

71-0040

26
Table 4. Reactions of H with organic solutes — Continued

No. Solute and Reaction pH k(dm 3 mol l s *) Ratio Source Method Comment Ref.

2.208 cytochrome-C ~ 7 7.5 x 10

9 (rel.) k/khcoo - = 30 X-r. chem. c.k. 62-3002

H + ferri-cytC —

»

— 1.5 x 10

10 — p.r. opt. p.b.k. at 550 nm 71-0930,

ferro-cytC + H

+ (ferro-cytC);

H2 -satd. 72-1002

H + ferri-cyt C —

2.5, 1 x 10

10 (rel.) — p.r. opt. p.b.k. (290- 71-3087

H adduct 6.5 325 nm); tert- BuOH as OH

scavenger.

2.209 cytosine 1 9 x 10

7 (rel.) klkuton =0.09 e-r. esr •decay of spin

polarization,

compared with EtOH.

71-0040

7 (1.0 - 1.5) x 108 k/kztOH = 0.1 - e-r. esr decay of spin 72-0039

(rel.) 0.15 polarization,

compared with EtOH.

2.210 2-deoxy-D-ribose 7 2.3 x 10

7 (rel.) kl k]ycOO~ — 1.0 ± y-r. chem. c.k. 64-0095

H + C 5 H 10O4 —

»

0.1 H 2 C s H9 04 2.211 dichlorodifluoro- 1 < 10

6 (rel.) ^/^BiOH < e-r. esr decay of spin 71-0003

methane polarization,

compared with 2-PrOH(7D).

2.212 dichloromethane 1 4 x 10

6 (rel.) k/kRt0n = 4 x e-r. esr decay of spin 71-0003

H + CH2 C12 ^ 10'3 polarization.

H 2 + CHC12(I) compared with H + CH2 C12 -^ 2-PrOH(7D).

no H2 (II) 1 1.1 x 10

6

(I) (rel.) k1 /ku = 0.37 y-r. chem. 27% H abstr. 73-0053

2.213 o-dicyanobenzene 1 5.5 x 10

8 (rel.) ^/^B*OH = 0.55 e-r. esr decay of spin

polarization,

compared with EtOH.

72-0025

2.214 m-dicyanobenzene 1 5.2 x 10

8 (rel.) ^/^BiOH — 0.52 e-r. esr decay of spin

polarization,

compared with EtOH.

72-0025

2.215 p-dicyanobenzene 1 2.8 x 10

8 (rel.) k/k^MH = 0.28 e-r. esr decay §f spin

polarization,

compared with EtOH.

72-0025

2 (3.5 ± 0.4) x 10

8 — p.r. opt. p.b.k. at 320 nm. 73-0121

2.216 2,3-dihydroxy- 1 9 x 10

7 (rel.) ^/^BiOH =0.09 e-r. esr decay of spin 71-0040

fumaric acid polarization,

H + (COHCOOH)2 -* compared with h2 + EtOH.

HOOCCOCOHCOOH (I) H + (COHCOOH)2 ^ 1 1.4 x 10

6

(I) (rel.) kt lk n = 0.19 y-r. chem. 16% H abstr. 73-0053

no H2 (II) 2.217 5,6-dihydrothymine 7-8 2.3 x 10

8 (rel.) k/kocoQ— = 10 y-r. chem. c.k. 68-3038

2.217a dimethyl fumarate 0.7 9.0 x 10

9 — p.r. opt. p.b.k. 73-0097

2.218 dioxane — 6.2 x 10

6 (rel.) kl k McCDOHMc t y-r. chem. c.k. 66-0422

H + C 4 H8 02 -» H2 + 6.2 x 10"1 c 4 h 7 o2 — 1.3 x 10

7 (rel.) k/k^+ = 4.18 x p.r. opt. c.k.; p.b.k. at 67-0550,

10

-4 ~ 310 nm (Ag£) 68-0436

1 1.3 x 10

7 (rel.) k/k^MH = 1-3 x e-r. esr decay of spin 71-0003

10“2 polarization,

compared with 2-PrOH(7D). For other ratios see: 2.110, 2.131, 2.151, 2.364

27
Table 4. Reactions of H with organic solutes — Continued

No. Solute and Reaction pH fc(dm

3 morl s

*) Ratio Source Method Comment Ref.

2.219 dithiodiglycolic 1 1 x 10

l ° (rel.) k/k BxOH = I® e-T. esr decay of spin 71-0040

acid

1 y-r. chem.

polarization,

compared with EtOH.

no H abstr. 73-0053

2.220 DNA 7-8 8 x 10“ (rel.)

1.1 x 10

s (rel.)

y-r. chem. c.k. with DCOO-

; mol. wt. = 5 x 10

6

; k = 5 x 10

7 per base unit.

68-3038

2.221 dodecyl sodium — ^/^2-PrOH(7D) = y-r. chem. c.k. 71-0586

sulfate 11 2.222 erythrosin See

tetraiodofluorescein 2.223 ethane 1 2.5 x 10

6 (rel.) ^/^BiOH - 2.5 X e-r. esr decay of spin 71-0003

10

-3 polarization,

compared with 2-PrOH(7D).

2.224 ethanol (EtOH) 1.0 2.0 x 10

7 (rel.) k/khcooh =14 y-r. chem. c.k. 56-0012

H 4- C 2 H 5 OH 1-3 2.8 x 10

7 (rel.) k/k fmi = 4 x X-r. chem. c.k. 62-0022,

h 2 + c 2 h 4 oh 10

-3 62-0033

1.2 4.2 x 10

7 (rel.) klklmi = 6 x X-r. chem. c.k. 62-0087

10

-3 ~ 6 1.5 x 10

7 (rel.) klkoQOQ- = (6.6 y-r. chem. c.k. 63-0041, ± 1.0) x 10

-1 64-0095 — 1.3 x 10

8 (rel.) k/k^ = 4.3 x y-r. chem. c.k. 65-0192

10

-3 ~ 7 3.9 x 10

7 (rel.) klkimi = 5.5 x y-r. chem. c.k. 65-0192

10

-3

1.1 2.4 x 10

7 (rel.) k/klmi = 3.45 y-r. chem. c.k. 65-0192

x 10

-3

1 3.8 x 10

7 (rel.) k/kOXy = 1.9 X y-r. chem. c.k. 66-0010

10

-3 — 1.7 x 10

7 (rel.) klkneOH = 8-4 y-r. chem. c.k., no details 67-0041

given. ~ 7 2.5 x 10

7 (rel.) klk„m = 0.41 y-r. chem. c.k. 67-0094 ~ 7 5 x 10

7 (rel.) k/k OXJ = 2.5 x y-r. chem. c.k. 67-0094

10”3 1.69 4.4 x 10

7 (rel.) klkOIJ = 2.2 x y-r. chem. c.k. 67-0094

10“3 — 3.7 x 10

7 (rel.) k/k A.+ = 12.0 x p.r. opt. c.k.; p.b.k. at 67-0550,

10

-4 313 nm (Ag£). 68-0436

~0.4 4.6 x 10

7 (rel.) k/kOXJ = 2.3 x y-r. chem. c.k. 68-0525

10

-3 >13 - 2 x 10

7 (rel.) — y-r. chem. c.k. with OH 69-0051

1 2.6 x 10

7 (rel.) k/kuzOH = 2.6 x e-r. esr decay of spin 71-0003

10"2 polarization,

compared with 2-PrOH(7D).

1 2.5 x 10

7 (rel.) k/ kjijQH = 2.5 x y-r. chem. c.k. with 71-0017

10"2 2-PrOH(7D).

1 1.3 x 10

7 — p.r. esr decay of H

signal.

71-0303

For other ratios see: 2.19, 2.21, 2.22, 2.23, 2.25-38, 2.52-54, 2.70, 2.80, 2.81,

2.84, 2.85, 2.86, 2.88, 2.103, 2.152, 2.226, 2.243, 2.310-12,

2.315, 2.316, 2.350, 2.352. D + C 2 H 5 OH -> 2 2.4 x 10

7 — p.r. esr decay of H 71-0303

HD + C 2 H 4 OH signal. 2.225 ethanol-d2 1.2 2.9 x 10

6 (rel.) k/kfmi = 9.5 x X-r. chem. c.k. 62-0087

H + CH3 CD 2 OH 10

-4 HD + CHjCDOH

2.226 ethoxide ion > 13 3.7 x 10

9 (rel.) k/kfMH = 1^4 y-r. chem. c.k. with OH-

. 69-0051

H + C 2 Hs O

- ^

c 2 h4 ct + h 2 28
Table 4. Reactions of H with organic solutes — Continued

No. Solute and Reaction pH k(dm 3 mol *s

l

) Ratio Source Method Comment Ref.

2.227 ethyl acetate H + CH3 COOC 2 H 5 ^

1.0 4.2 x 10

s (rel.) klkftcooH - 0.56 X-r. chem. c.k. 56-0012

h 2 + ch3 co2 c 2 h 4 2.228 ethyl acetoacetate 1 1.3 x 10

7 (rel.) — e—r. esr unpuhl. data, 73-0053

H + MeCOCH2 COOEt -> P. Neta and

H 2 + MeCOCHCOOEt R.H. Schuler. +MeC(OH)=CCOOEt 1 2.9 x 10

6

(I) (rel.) kx tk n = 0.27 y-r. chem. 22% H abstr.; 73-0053

(I) 8% enol formn. H + MeCOCH2 COOEt

no H 2 (II) 2.229 ethylene — 3.2 x 10

9 (rel.) ^/^MeOH = 1600 — — c.k. no details. 67-0041

H + CH2 =CH2 -^ 1 6.6 x 10® (rel.) k/koxy = 3.3 x y-r. chem. c.k. 68-0052 c 2 h5 1 3 x 10

9 (rel.)

10“2

^/^BiOH = 3 e-r. esr decay of spin

polarization,

compared with 2-PrOH(7D).

71-0003

2.230 ethylenediamine- 1 6.5 x 10

7 (rel.) k/kb,oh = 6-5 x e-r. esr decay of spin 71-0040

tetraacetic acid 10"2 polarization,

compared with EtOH.

2.231 ethyleneglycol ~ 7 1.0 x 10

7 (rel.) k/k dcoo~ = y-r. chem. c.k. 63-0041,

H + HOCH2 CH2 OH (4.3 ± 0.5) x 64-0095

HOCHCH2 OH + h2 10

_1 — 8.2 x 10

6 (rel.) ^/^MeCDOHMe = y-r. chem. c.k. 66-0422

8.2 x 10'1

2.1 x 10

7 (rel.) k/k

6.9 x p.r. opt. c.k.; p.b.k. at 67-0550,

10

-4 313 nm (Ag£). 68-0436

1 1.7 x 10

7 (rel.) ^/^BxOH = 1-7 X e-r. esr decay of spin 71-0003

10~2 polarization,

compared with 2-PrOH(7D).

1 2.1 x 10

7 (rel.) k/k^+ = 6.7 x p.r. opt. c.k.; obs. Ag at 73-1053

io4 410 nm; contains /ert-BuOH; k increases with pressure 0 —> 6.72

kbar. 2.232 ethyl ether 1 4.7 x 10

7 (rel.) k/kBioh = 4.7 x e-r. esr decay of spin 71-0003

10"2 polarization,

compared with 2-PrOH(7D).

2.233 ethyl dihydrogen

phosphate

1.3 2.1 x 106 (rel.) ^/^MeOH(3D) =21 phot. chem. c.k. 65-7019

H + C 2 H5 OPO(OH)2 -> H2 + CH3 CHOPO(OH)2 2.233a N-ethylmaleamic

acid

1.0 (1.3 ± 0.2) x 10

9 — p.r. opt. p.b.k. 72-0144

2.234 N-ethylmaleimide 1.0 (1.4 ± 0.2) x 10

10 — p.r. opt. p.b.k. 72-0144

2.235 fluorenone 1.0 (5.4 ± 0.6) x 10

9 p.r. opt. p.b.k. (H

adduct); tert-BuOH

as OH scavenger.

72-0171

2.236 fluoroacetate ion H + FCH 2 C02 -^ 8.5 5 x 10

s (rel.) ^MeOH(3D) = 3 y-r. chem. c.k. 67-0050

h2 + fchco2 H + FCH2 C02 -» 8.5 < 10

3 (rel.) y-r. chem. practically no 67-0050

HF + CH2 C02 F

_ formed.

29
Table 4. Reactions of H with organic solutes — Continued

No. Solute and Reaction pH k(dm 3 mol *s

l

) Ratio Source Method Comment Ref.

2.237 5-fluorouracil 1 1.8 x 10

8 (rel.) k/k B*OH = 0.18 e-r. esr decay of spin

polarization,

' compared with EtOH.

71-0040

2.238 formaldehyde 1.0 3.5 x 10

6 (rel.) k/kHCOOH =4.7 X-r. chem. c.k. 56-0012

H + HCHO -» H 2 1 5 x 10

6 (rel.) — e-r. esr unpubl. data, 73-0053 + CHO (I) P. Neta and

H + HCHO -*• R.H. Schuler. no H 2 (II) 1 4 x 10

6

(I) (rel.) kilk n — 5 y-r. chem. 83% H abstr. 73-0053 For other ratios see: 2.12 2.239 formate ion 7.6 3.9 x 10

8 (rel.) ^ferri = 5.5 x X-r. chem. c.k. 62-0017,

H + HC02 -» H 2 +

10~2 62-0024

C0 2 7 4.5 x 10

8 (rel.) k/k uni = 6.4 X X-r. chem. c.k. 62-0022,

10~2 62-0024

11- 1.7 x 10

8 (rel.) k/koh - = II X-r. chem. c.k. 63-0049

135.7- nitrate = 50 y-r. chem. c.k. 66-0147

7.1 7 3 x 10

8 (rel.) klklmi = 0.044 X-r. chem. c.k. 67-0064

7- 1.8 x 10

8 (rel.) k/koH~ = 12 X-r. chem. c.k. 67-0064

13.5

7 1.3 x 10

8 (rel.) ^/^B*OH ~ 0.13 e-r. esr decay of spin

polarization,

compared with EtOH.

72-0039

For other ratios see: 2.10a, 2.52, 2.54, 2.69, 2.70, 2.72, 2.8 5, 2.86, 2.87, 2.90, 2.93c, 2.114, 2.208, 2.240. 2.240 d-formate ion — 2.3 x 10

7 (rel.) k/knQoo ~ 1-51 x y-r. chem. c.k. 63-0041,

H + DCOCT —> HD J 10

_1 64-0095

C02 6 2.3 x 10

7 (rel.) klkyicoo~ = 1-53 x y-r. chem. c.k. 64-0141

10

_1 For other ratios see: 2.78, 2.107, 2.110, 2.119-2.121, 2.172, 2.178, 2.210,

2.217, 2.224, 2.231, 2.257, 2.296, 2.334, 2.372-4.

2.241 formic acid ~ 1 2.1 x 10

6 (rel.) klk{mi = 3 x X-r. chem. c.k. 62-0022,

H + HCOOH H 2 + 10

-4 62-0033

COOH ~ 2 7 x 10

6 (rel.) klkfmi = ~ 10-3 X-r. chem. c.k. 62-0033 ~ 3 7 x 10

7 (rel.) = ~ 10

_I X-r. chem. c.k. 62-0033

0.4 3.4 x 10

s (rel.) k/k H = 3.4 x 10"5 p.r. chem. at dose rate < 10

19 eV/gs.

62-0144

1 7.4 x 10

s klk^H = 7.4 x e-r. esr decay of spin 71-0003,

10~* (obs.) polarization,

compared with 2— PrOH(7D); cor.

for 40% formate ion.

72-0039

1 — — y-r. chem. 100% H abstr. 73-0053

For other ratios see: 2.54, 2.86, 2.109, 2.110, 2.124, 2.152, 2.207, 2.224, 2.227,

2.238, 2.242, 2.296, 2.298a, 2.324, 2.356, 2.382, 2.384. 2.242 d-formic acid 1 1.1 x 10

s (rel.) k/kucooH = 015 X-r. chem. c.k. 56-0012

H + DCOOH -> HD + COOH

2.243 fumarate ion. — 4 x 10

9 (rel.) k/kttoH s 150 y-r. chem. c.k.; reactivity 66-0010

hydrogen of the dianion is similar. 2.244 fumaric acid 1 9 x 108 (rel.) k/k^on = 0-9 e-r. esr decay of spin

polarization,

compared with EtOH.

71-0040

0.7 7.0 x 10

9 — p.r. opt. p.b.k. 73-0097

30
Table 4. Reactions of H with organic solutes — Continued

No. Solute and Reaction pH fc(dm

3 mol *s *) Ratio Source Method Comment Ref.

2.245 glucose 1.2 7 x 10

7 (rel.) klklmi ^ 10-2 X-r. chem. c.k. 62-0017

H + C 6 H 12 0 6 —;

H 2 ~ 8 3 x 10

7 (rel.) kl k nitrite = 4 x X-r. chem. c.k. 62-0017 + C 6 H u06 7 8 x 10 7 (rel.)

10"2 kl k fern = 1-2 X X-r. chem. c.k. 62-0024

10"2 ~0.4 1 x 10

8 (rel.) kl k0x7 = 5 x y-r. chem. c.k.; ratio at 68-0525

10~3 6.34 kbar.

1 4.7 x 10

7 (rel.) kl

k

bxoh = 4.7 x e-r. esr decay of spin 71-0040

10'2 polarization,

compared with EtOH.

For other ratios see: 2.74, 2.124, 2.153, 2.159. 2.246 glutamate ion 7 5.6 x 10

6 (rel.) ^/^BiOH ~ 5.6 X e-r. esr decay of spin 72-0039

10"3 polarization,

compared with EtOH.

2.247 L -glutamic acid 1 1 x 10

6 (rel.) y-r. chem. c.k. assuming

k(H + allyl ale.) = 2.8 x 10

9

.

68-0343

1 1.7 x 10

6 (rel.) = I -7 x e-r. esr decay of spin 71-0040

10“3 polarization,

compared with EtOH.

2.248 glutathione (red.) 0 k\ 1 kjj ~ 2.8 ± y-r. chem. c.k. 69-0022

H + GuSH

H2 + GuS (I) H + GuSH

0.4

H2 S + Gu (II) 2.248a glutathione 1.5- ( 1.0 ± 0 . 2) x 10

10 — p.r. opt. p.b.k. 72-0380

(oxid.) H + (GuS)2 —*2.5

GuS + GuSH or (GuS)2 H (?) 2.249 glycerol 1.2 3.5 x 10

7 (rel.) klkleni = 5 x X-r. chem. c.k. 62-0017

H + C 3 H8 03 —» 10~3 H2 + C 3H7O3 - 8 2.1 x 10

7 (rel.) */*»krite = 3 x X-r. chem. c.k. 62-0017

10"2

7 5,4 x 10

7 (rel.) klklmi = 7.7 X X-r. chem. c.k. 62-0024

10~3

2 4.1 x 10

7 (rel.) klk t-* = 13.2 x p.r. opt. c.k.; p.b.k. at 67-0550,

10

-4 313 nm (Ag£) 68-0436

-0.4 5.6 x 10

7 (rel.) k/kOXJ = 2.8 x y-r. chem. c.k. 68-0525

10"3

1 3.6 x 10

7 (rel.) klkftzou = 3.6 x e-r. esr decay of spin 71-0040

10“2 polarization,

compared with EtOH.

1 4.1 x 10

7 (rel.) klk u+ = 1.34 x p.r. opt. c.k.; obs. Ag at 73-1053

10

3 410 nm; contains terf-BuOH; k increases 0 —> 6.72 kbar. 2.250 glycine, positive 2 4.8 x 10

7 (rel.) k/ku+ = 15.5 x p.r. opt. c.k.; p.b.k. at 67-0550,

ion 10

-4 313 nm (Ag^). 68-0436

1 8 x 10

4 (rel.) kl kfaQH = 8 x e-r. esr decay of spin 71-0003

10

“s polarization,

compared with 2-PrOH(7D).

(Unexplained discrepancy in the above data).

31
Table 4. Reactions of H with organic solutes — Continued

No. Solute and Reaction pH k(dm 3 mol *s *) Ratio Source Method Comment Ref.

2.251 glycine, 7 9 x 10

4 (rel.) ^/^BiOH = 9 X e-T. esr decay of spin 72-0039

zwitterion 10"5 polarization,

compared with EtOH.

2.252 glycolate ion 7 4.0 x 10

7 (rel.) k/kBiOH = 4.0 x e-T. esr decay of spin 72-0039

10“2 polarization,

compared with EtOH.

2.253 glycolic acid 1 1.8 x 10

7 (rel.) ^/^BiOH = 1-8 X e-r. esr decay of spin 71-0003

H + CH2 OHCOOH 10"2 polarization.

h 2 + chohcooh compared with

(I) 2-PrOH(7D).

H + CH2 OHCOOH 1 1.7 x 10

7 (I) (rel.) k\lk u = 24 y-r. chem. 96% H abstr. 73-0053 —> no H 2 (II) 2.254 glycylglycine 1 2.6 x 10

6 (rel.) k/k BiOH = 2.6 X e-r. esr decay of spin 71-0040

10"3 polarization,

compared with EtOH.

2.255 glycylglycyl- 1 5.5 x 10

6 (rel.) ^/^BxOH = 5.5 X e-T. esr decay of spin 71-0040

glycine 10"3 polarization,

compared with EtOH.

2.256 glyoxal 1.3 k/k Ca2+ = 0.57 r. chem. c.k. 68-0503

H + CHOCHO -»• 1 — — y-r. chem. 80% H abstr. 73-0053

h 2 +.cocho

2.257 glyoxylate ion 7 3.7 x 10

7 (rel.) k/kjycoQ— = y-r. chem. c.k. 63-0041,

H + CH0C02 -* 1.6 ± 1 64-0095

h 2 + coco2 2.258 glyoxylic acid 1 2 x 10

7 (rel.) — y-r. chem. est. from G(H 2 ) 71-0925

H + CHOCOOH -> at different dose h 2 + cocooh rates and concn.; assume k H = 8 x 10

9

.

1 2.4 x 10

7 (rel.) e-T. esr Unpubl. data, P. Neta and

R.H. Schuler.

73-0053

1 2.4 x 10 ? (rel.) — y-r. chem. 100% H abstr. 73-0053

2.259 guanidine 1 1.3 x 10

6 (rel.) kl ^BiOH = 1-3 x e-r. esr decay of spin 71-0040

10

-3 polarization,

compared with EtOH.

2.260 hexadecyltri- — 1.5 x 10

8 (rel.) ^2-PrOH(7D) = y-r. chem. c.k. 71-0586

methyl ammonium

bromide

15.2

2.261 hexamethyleneimine 1 1.5 x 10

7 (rel.) k/k^QH = 1.5 x e-r. esr decay of spin 71-0040

10“2 polarization,

compared with EtOH.

2.262 hexane 1 1.5 x 10* (rel.) ^/^B*OH = 0.15 e-r. esr decay of spin

polarization,

compared with 2-PrOH(7D).

71-0003

2.263 1,6-hexanediamine 1 4.7 x 10

6 (rel.) k/kfcOH = 4.7 x e-r. esr decay of spin 71-0040

10“3 polarization,

compared with EtOH.

2.264 hexanoate ion 7 5.3 x 10

7 (rel.) k/kmoH = 5.3 x e-r. esr decay of spin 72-0039

l

10~2 polarization,

compared with EtOH.

32
Table 4. Reactions of H with organic solutes — Continued

No. Solute and Reaction pH k(dm 3 mol X s

X ) Ratio Source Method Comment Ref.

2.265 hexanoic acid 1 4.6 x 10

7 (rel.) k/k Bi0h = 4.6 x e—r. esr decay of spin 71-0003

10~2 polarization,

compared with 2-PrOH(7D).

2.266 hexanol 1 1.04 x 10

8 (rel.) */*BrfH = 0.104 e-T. esr decay of spin

polarization,

compared with 2-PrOH(7D).

71-0003

7 1.0 x 10

8 (rel.) k/kutOH = 0-1 e-r. esr decay of spin

polarization,

compared with EtOH.

72-0039

2.267 1-hexylammonium 1,7 3.5 x 10

7 (rel.) = 3.5 X e-T. esr decay of spin 72-0040,

ion 10~2 polarization,

compared with EtOH.

72-0039

2.268 hippuric acid 1 1.0 x 10

9 (rel.) ^/^BiOH = 1 e-T. esr decay of spin

polarization,

compared with EtOH.

71-0040

2.269 L -histidine, 1 4.8 x 10

7 (rel.) kl ^BiOH = ^-8 x e-r. esr decay of spin 71-0040

positive ion 10

-2 polarization,

H + ImCH2 CH(NHj)COOH compared with ImCH2 C(NH;f)COOH EtOH.

+ h2 (I) 3 5.1 x 10

7 (rel.) ^/^BiOH = 3.1 x e-T. esr decay of spin 72-0039

H + ImCH2 CH(NH£)COOH 10~2 polarization. —» no H2 (II) compared with EtOH.

Im = imadazolyl 1 ~ 1.5 x 10° (I) kx !k u = 0.03 chem. ~ 3 % H abstr. 73-0053

(rel.) 2.269a histidine, 7 2.5 x 10

8 (rel.) ^/^BxOH = 0.25 e-T. esr decay of spin 72-0039

zwitterion polarization,

compared with EtOH.

2.270 p-hydroxybenzoic 1 1.45 x 10

9 — p.r. opt. p.b.k. ; CD3 OH as 69-0001

acid OH scavenger H + HOC6 H4 COOH — 1.8 x 10

9 (rel.) k/kyieon = 900 p.r. opt. c.k.; p.b.k. 69-0001

HOC 6 H5 COOH

2.270a /7-hydroxyphenylpropionate ion9.0 (4.0 ± 1.0) x 10

9

“ p.r. opt. p.b.k. 73-0003

2.271 p-hydroxyphenyl- 2.0- 1.6 x 10

9 (rel.) k/k OXJ = 7.9 x p.r. opt. c.k.; p.b.k. at 69-0445

propionic acid 2.3 10“2 320 and 330 nm HOC 6 H4 CH2 CH2 COOH + (H adduct).

H —* adduct

2.272 L-hydroxyproline 1 1.6 x 10

6 (rel.) — y-r. chem. c.k. assuming 68-0343

k(H + allyl ale.) = 2.8 x 10

9

. 1 6.0 x 10

6 (rel.) ^/^BK)H = 6.0 X e-r. esr decay of spin 71-0040

10"3 polarization,

compared with EtOH.

2.273 imidazole 1 6.2 x 10

7 (rel.) klk^on = 6.2 x e-r. esr decay of spin 71-0040,

10"2 polarization,

compared with EtOH.

72-0025

2.274 iminodiacetic acid 1 4.0 x 10

s (rel.) ^/^BiOH = 4.0 X e-r. esr decay of spin 71-0040

10^ polarization,

compared with EtOH.

2.274a indole 1 4.4 x 10

9 (rel.) ^/^2-P»OH ~ 36 y-r. chem. c.k. 72-0541

33
Table 4. Reactions of H with organic solutes — Continued

No. Solute and Reaction pH k(dm3 mol

-1

s -1

) Ratio Source Method Comment Ref.

2.274b indole-3-acetic

acid

1 6.6 x 10

9 (rel.) ^/^2-PiOH = 84 y-r. chem. c.k. 72-0541

2.274c indole-3- propionic

acid

1 6.4 x 10

9 (rel.) ^2-PrOH = 81 y-r. chem. c.k. 72-0541

2.275 iodomethane 1 3* 2 x 10

9 (rel.) ^BiOH ^ 2 e-r. esr decay of spin

polarization,

compared with 2-PrOH(7D).

71-0003

2.276 isobutane 1 1.2 x 10

8 (rel.) ^/^BtOH = 0-12 e-r. esr decay of spin

polarization,

compared with 2-PrOH(7D).

71-0003

2.277 isobutyl alcohol 1 6.4 x 10

7 (rel.) ^/^BiOH = 6.4 X e-r. esr decay of spin 71-0003

H +(CH 3 ) 2 CHCH2 OH -* 10~2 polarization,

h 2 + c4 h 8 oh

1 5 x 10

7 (rel.) k/kBxOH = 5 X y-r. chem.

compared with 2-PrOH(7D).

c.k. with 71-0017

1 x 10

10 (rel.)

10“2 2-PrOH(7D).

2.278 isobutylene — k/k MeOH = 6.3 X — — c.k., no details 67-0041

H + C 4 H^ C 4 H9 10

3 given. 2.279 isobutyrate ion — 3.3 x 10

7 (rel.) ^/^MeCDOHMe = y-r. chem. c.k. 66-0422

H + (CH 3 ) 2 CHC02 -^ 3.3 h 2 + c 3 h6 co2 7 5.9 x 10

7 (rel.) k/k B*OH = 6-9 X e-r. esr decay of spin 72-0039

10~2 polarization,

compared with EtOH.

2.280 isobutyric acid 1 2.6 x 10

7 (rel.) k/k BlOH 2.6 X e-r. esr decay of spin 71-0003

10“2 polarization,

compared with 2-PrOH(7D).

2.281 isobutyronitrile 1 2.2 x 10

7 (rel.) k/k bioh 2.2 x e-r. esr decay of spin 71-0003

10"2 polarization,

compared with 2-PrOH(7D).

2.282 isoleucine 1 6.1 x 10

6 (rel.) y-r. chem. c.k. assuming

k(H + allyl ale.) 2.8 x 10

9

.

68-0343

1 8 x 10

6 (rel.) ^/^BiOH = 8 X e-r. esr decay of spin 71-0040

10~3 polarization,

compared with EtOH.

2.283 isoorotic acid 1 9 x 10

7 (rel.) k/kBioh = 9 x e-r. esr decay of spin 71-0040

10“2 polarization,

compared with EtOH.

2.284 isovalerate ion — 2.6 x 10

7 (rel.) k/kHeCDOHMe = y-r. chem. c.k. 66-0422

H + Me2 CHCH2 COO~ 2.6 -* H 2 + C 4 H8 COO~

2.285 lactic acid 1 2.2 x 10

7 (rel.) k/kmoH = 2-2 x e-r. esr decay of spin 71-0003

10"2 polarization,

compared with 2-PrOH(7D).

2.286 L-leucine 1 1.7 x 10

7 (rel.) klkmoH ~ 1-7 x e-r. esr decay of spin 71-0040

10~2 polarization,

compared with EtOH.

34
Table 4. Reactions of H with organic solutes — Continued

No. Solute and Reaction pH k(dm 3 mol *s *) Ratio Source Method Comment Ref.

2.287 L -lysine 1 9.9 x 10s (rel.) — y-r. chem. c.k. assuming 68-0343

k(H + allyl ale.) = 2.8 x 10

9

1 1.6 x 106 (rel.) k/kBiOH = 1-6 x e—x. esr decay of spin 71-0040

10"3 polarization,

compared with EtOH.

2.288 maleic acid 1 6 x 10® (rel.) ^/^BxOH = 0.6 e-x. esr decay of spin

polarization,

compared with EtOH.

71-0040

0.7 8.0 x 109 — p.r. opt. p.b.k. 73-0097

2.289 malic acid 1 2.2 x 10 7 (rel.) = 2.2 X e-r. esr decay of spin 71-0040

10

-2 polarization,

compared with EtOH.

2.290 malonic acid 1 4.2 x 10

s (rel.) kl ^BiOH = 4.2 x e-x. esr decay of spin 71-0003

H + CH2 (COOH)2 -^ lO^1 polarization,

H2 + CH(COOH)2 compared with

(I) 2-PrOH(7D).

H + CH2 (COOH)2 -> 1 4.4 x 10

s (rel.) ^/^BrOH ~ 4.4 X y-r. chem. c.k. with 71-0017

no H2 (II) 10^ 2-PrOH(7D).

1 3.3 x 10

s

(I) (rel.) kilk u = 3 y-r. chem. 75% H abstr. 73-0053

2.291 malononitrile 1 y-r. chem. 5% H abstr. 73-0053

2.292 2-mercaptoethanol 0 1.6 x 10

9

(I) (rel.) k\!korj = 0.08 p.r. opt. c.k. 71-0175

HSCH2 CH2 OH + H 0 .3.2 x 10® (II) (rel.) ki/k u = 5 X-r. chem. product analysis, 71-0175

-» h2 + sch2 ch2 oh G(H2 S).

(I) 1 1.6 x 10

9

(I + II) Tt^' y-r. chem. c.k. assuming 73-0241

HSCH2 CH2 OH + H ^ (rel.) &(H + allyl ale.) h 2 s + CH2 CH2 OH 1.3 x 10

9 (I) (rel.) kjkn = 5.7 ± = 2.8 x 10

9

(II) 2.3 x 10® (II) (rel.) 0.6 2.292a 2-mercaptopro- 1 2.7 x 10

9

(I + II) — y-r. chem. c.k. assuming 73-0241

pionic acid (rel.) k(H + allyl ale.) H + CH3 CH(SH)COOH 9.4 x 10® (I) (rel.) kx !kn = 0.52 ± = 2.8 x 10

9 H2 (I) 1.8 x 10

9

(II) (rel.) 0.05 H + CH3 CH(SH)COOH -> H2 S (II) 2.292b 3-mercaptopro- 1 1.1 x 10

9

(I + II) — y-r. chem. c.k. assuming 73-0241

pionic acid (rel.) k( H + allyl ale.) H + HSCH2 CH2 COOH 8.9 x 10® (I) (rel.) k\/k n = 4.0 ± = 2.8 x 10

9

. H2 (I) 2.2 x 10® (II) (rel.) 0.4 H + HSCH2 CH2 COOH

H2 S (II) 2.293 m'esitylene — ~ 7 x 10

9 — — — estd. by analogy 69-0503

H + C 6 H3 (CH3 ) 3 —

>

with benzene and

prod. toluene. T + C 6 H3 (CH3 ) 3 -> — k/kCu 2+ = ~ 22 — — effect of Cu2+ on 69-0503

prod. T exchange rate. 2.294 methane 1 < 10

s (rel.) ^/^B*OH ^ 10 e-x. esr decay of spin

polarization,

compared with 2-PrOH(7D).

71-0003

1 < 10

4 y-r. chem. deduced from

results with chloromethanes.

73-0053

2.295 methanethiol

H + CH3 SH

H2 + CH3 S (I) H + CH3 SH^

0.72 k\lkn = 6.4 y-r. chem. c.k. 64-0151

H2 S + CH3 (II)

35
Table 4. Reactions of H with organic solutes — Continued

No. Solute and Reaction pH k(dm 3 mol *s *) Ratio Source Method Comment Ref.

2.296 methanol (MeOH) 1 1.1 x 10

6 (rel.) klk HcooH = 1-5 X-r. chem. c.k. 56-0012

H + CH3 OH -* ~ 7 4.7 x 10

6 (rel.) klktmi = 6.7 x X-r. chem. c.k. 62-0024

H 2 + CH 2 OH

~ 6 1.7 x 106 (rel.) ^

-

1

0

i

0 1 II

1if* y-r. chem. c.k. 63-0041, ± 0.8) X 10

-2 64-0095

2 4.4 x 10

6 (rel.) k/k^ = 1.42 x p.r. opt. c.k.; p.b.k. at 67-0550,

10

-4 313 nm (Ag£). 68-0436

~0.4 5.8 x 10

6 (rel.) k/k ox1 = 2.9 x y-r. chem. c.k.; at 6.34 68-0525

10

-4 kbar k/kOIJ =

2.1 x 10

“3

. >13 ( 1.8 ± 0 . 6) x 10

6 — y-r. chem. c.k. with OH-

. 69-0051

(rel.)

1 2.4 x 10

6 — p.r. esr decay of H

signal.

71-0303

1 1.6 x 10

6 (rel.) k/kBxOH = 1-6 X e-r. esr decay of spin 71-0003

10

-3 polarization,

compared with 2-PrOH(7D).

1 2.9 x 10

6 (rel.) k/kBiOH = 2.9 x y-r. chem. c.k. with 71-0017

10

-3 2-PrOH(7D).

7 1.6 x 10

6 (rel.) ^/^BiOH = 1-6 X e-r. esr decay of spin 72-0039

10

-3 polarization,

compared with EtOH.

For other ratios see: 2.14, 2.54, 2.57, 2.58, 2.71, 2.74, 2.85, 2.89, 2.149,

2.150, 2.152, 2.173, 2.224, 2.229, 2.270, 2.278, 2.298, 2.308, 2.334, 2.340, 2.350, 2.352. D + CH3 OH 1 k/kfe 3+ = 0.38 X-r. chem. c.k. 58-0006

HD + CH2 OH 1 klkCa2+ = 0.04 X-r. chem. c.k. 58-0006

2 3.6 x 10

6 — p.r. esr decay of H

signal.

71-0303

2.297 methanol-d 1.2 k/kFt3+ = 0.38 X-r. chem. c.k. 58-0006

D + CH3 OD HD -» k/k Co 2 + = 3.7 x CH2 OD 10'2 k/k Fe 2+ = 0.42 2.298 methanol-d3 6 1 x 10

5 (rel.) ^MeOH = 5 X y-r. chem. c.k. 64-0141

(MeOH(3D))

H + CD 3 OH ->

10"2

HD + CD2 OH

For other ratios see: 2.22, 2.25, 2.55, 2.233, 2.236

2.298a methionine 1 6.0 x 10

8 (rel.) WkHCOOH - y-r. chem. c.k. 68-0343

2.299 methoxide ion H + CH3 0'-» > 13 1.8 x 10

9 (rel.) — y-r. chem. c.k. with OH-

. 69-0051

h 2 + CH2 0"

2.300 methyl acetate 7 6 x 10

4 (rel.) — — — c.k. with CDjOH. 66-0843

2.301 methylammonium ion 4 7 x 10

3 (rel.) k/(2k H) 112 = y-r. chem. estd. 65-0188

H + CH3 NH3 —

»

0.05 H 2 + CHjNHj 3 2.7 x 10

6 (rel.) ^/^PfcOH ~ 1*5 X p.r. opt.. c.k. 71-0595

10

-3

2.5 1.1 x 10

7 (rel.) k/k 1-+ = 3.65 x p.r. opt. c.k. 71-0595

10

-4 3-methylbutanoate ion See isovalerate ion 2.302 2 -methylbutanoic — 3.3 x 10

7 (rel.) ^/^UeCDOHMe = y-r. chem. c.k. 66-0422

acid 3.3 2-methyl-l-propanol See isobutyl alcohol 2-methylpropionate ion See isobutyrate ion 2-methylpropionic acid See isobutyric acid 2.303 6 -methyluracil 1 7 x 10

8 (rel.) ^/^B*OH =0.7 e-r. esr decay of spin

polarization,

compared with EtOH.

71-0040

36
Table 4. Reactions of H with organic solutes — Continued

No. Solute and Reaction pH k(dm 3 mol 7 s

7

) Ratio Source Method Comment Ref.

2.303a 1-naphthaleneacetic acid

1 3.2 x 10

9 (rel.) ^/^2-PrOH = 41 y-r. chem. c.k. 72-0541

2.304 1,4-naphtho- 1.0 (6.8 ± 0.4) x 10

9 — p.r. opt. p.b.k. (H 72-0171

quinone 2-sulfo- adduct); /ert-BuOH

nate ion as OH scavenger.

2.305 neopentyl alcohol 1 2.9 x 10

7 (rel.) kl ^B*oH = 2-9 x e-r. esr decay of spin 71-0003

5 x 10

8

10"2 polarization,

compared with 2-PrOH(7D).

2.306 nicotinic acid 1 — p.r. opt. p.b.k.;

/erf-BuOH as OH

71-0582

scavenger.

2.307 nitrilotriacetic 1 7.5 x 10

6 (rel.) kl ^b*oh = 7.5 x e-r. esr decay of spin 71-0040

acid 10~3 polarization,

compared with EtOH.

2.308 nitrobenzene 8-9 2.6 x 10

9 (rel.) ^/^2-PrOH = 33 y-r. chem. c.k. 66-0500

H + C 6 H5 N02 ^ 1 (5.6 ± 0.6) x 10

9 — p.r. opt. p.b.k. at 410 67-0458 c 6 h6 no2 nm; Tl

+ as OH

scavenger.

1 1.04 x 10

9

ft- f , p.r. opt. p.b.k.; CDjOH as OH scavenger. 69-0001 — 1.4 x 10

9 (rel.) k/kMeOH ~ 700 p.r. opt. c.k.; p.b.k. 69-0001

1 — — y-r. chem. no H abstr. 73-0053

2.309 p-nitrobenzoic 1 9.8 x 10

8 — p.r. opt. p.b.k.; CD3 OH as 69-0001

acid (PNBA) OH scavenger. H + PNBA 2 (1.0 ± 0.1) x 10

9 — p.r. opt. p.b.k. at 400 70-0211

-* 4-N02 C 6 H5 C00H nm; CD3 OH as OH

scavenger. For other ratios see: 2.144, 2.195, 2.196, 2.198

2.310 nitroethane — 7.15 x 10

7 (rel.) — 2.75 ± r. chem. c.k. 67-0180

0.10 2.310a an/i-5-nitro-2- 1,7 3 x 10

9 — p.r. opt. p.b.k. at 500 nm. 73-1018

furaldoxime (H adduct). 2.311 nitromethane ' 7.1 x 10

7 (rel.) klk^H 1 2.72 ±

- r. chem. c.k. 67-0180

0.10

1 4.4 x 10

7 (rel.) ^•/^BxOH = 4.4 X e-r. esr decay of spin 71-0003

10"2 polarization,

compared with 2-PrOH(7D).

1 — — y-r. chem. no H abstr. 73-0053

2.312 1-nitropropane — 7.4 x 10

7 (rel.) ~ 2.86 ± r. chem. c.k. 67-0180

0.10 2.312a norvaline 1 1.7 x 10

6 (rel.) y-r. chem. c.k. assuming

&(H + allyl ale.) = 2.8 x 10

9

.

68-0343

2.313 orotic acid 1.5 3.3 x 10

9 p.r. opt. p.b.k. at 345 nm (H adduct);

tert-BuOH as OH scavenger.

70-0567

1 5 x 10

8 (rel.) ^/^BrOH = 0.5 e-r. esr decay of spin

polarization,

compared with EtOH.

71-0040

2.314 oxalacetic acid 1 2.1 x 10

7 (rel.) — e-r. esr Unpubl. data, 73-0053

H + HOOCCOCH2 COOH P. Neta and ^ h2 + R.H. Schuler. HOOCCOCHCOOH 1 ~ 2 x 10

s

(I) (rel.) k^ku = 0.01 y-r. chem. ~ 1% H abstr. 73-0053

H + HOOCCOCH2 COOH

no H2 (II)

37
Table 4. Reactions of H with organic solutes — Continued

No. Solute and Reaction pH fc(dm

3 mol ! s

*) Ratio Source Method Comment Ref.

2.315 oxalate ion 7 1.6 x 10

6 (rel.) ^/^EtOH = 6 X y-r. chem. c.k. 69-0646

H + C 2 04 —> no H2 7 $ 4x 10

4 (rel.)

10'2

k/k BlOH $ 4x e-r. esr decay of spin 72-0039

10~5 polarization,

compared with EtOH.

2.316 oxalic acid + 1.3 Jcj + ^n/^ferri y-r. chem. c.k. 69-0646

oxalate ion *£ 10'4 (I)H + H2 C 2 04 -» 1.3 + ^iv/^E«OH y-r. chem. c.k. 69-0646

h 2 + co2 + cooh

(ii)H + hc 2 o;^

h 2 + co2 + coo

(III)H + H 2 C 2 04 ^

H 2 0 + C02 + CHO

(IV) H + hc 2 o;—

= 4.2 x 10~2

OH' + C02 + CHO

2.317 oxalic acid 1 3 x 10

s (rel.) k/k BiOH = 3 x y-r. chem. c.k. with 71-0017

H + H 2 C 2 Q4 — 10

-4 2-PrOH(7D);

no H 2 cor. for k(e~

q + H2 C 2 04) =

2.5 x 10

10

. 1 4.1 x 10

s (rel.) k/kBiOH = 4.1 x e-r. esr decay of spin 71-0003

10

-4 polarization,

compared with 2-PrOH(7D).

I — — y-r. chem. no H abstr. 73-0053

2.317a penicillamine 1 1.9 x 10

9

(I + II) — y-r. chem. c.k. assuming 73-0241

(RSH) (rel.) &(H + allyl ale.) H + RSH H 2 (I) 5.9 x 10

8

(I) (rel.) kjkn = 0.44 ± = 2.8 x 10

9

. H + RSH H 2 S[II) 1.3 x 10

9

(II) (rel.) 0.03 2.318 pentane 1 7 x 10

7 (rel.) k/k^jon = 0.07 e-r. esr decay of spin

polarization,

compared with 2-PrOH(7D).

71-0003

2.319 pentanoate ion — 1.9 x 10

7 (rel.) ^MeCDOHMe ~ y-r. chem. c.k. 66-0422

1.9 2.320 phenol (PhOH) 8-9 6.6 x 10

9 (rel.) kl k2-prOH = 0.84 y-r. chem. c.k. 66-0500

H + C 6 Hs OH 2.0 (1.8 ± 0.3) x 10

9 — p.r. opt. p.b.k. at 330 67-0122 c 6 h6 oh nm.

7 2.1 x 10

9 — p.r. esr decay of H

signal.

71-0303

1 1.4 x 10

9 (rel.) k/kuMH =1-4 e-r. esr decay of spin

polarization,

compared with EtOH.

72-0025

1 — — y-r. chem. ~ 3% H abstr. 73-0053 For other ratios see: 2.144, 2.301. 2.321 phenyl acetate 1 8.6 x 10

8 (rel.) k/k^on = 0.86 e-r. esr decay of spin

polarization,

compared with EtOH.

72-0025

2.322 phenylacetate ion 8-9 1.2 x 10

9 (rel.) ^/^2-PrOH =15 y-r. chem. c.k. 66-0500

2.323 phenylacetic acid 1 1.01 x 10

9 (II) — p.r. opt. p.b.k.; CDjOH as 69-0001

H + C 6 H5 CH2 COOH -» OH scavenger. h 2 + c 6 h5 chcooh 1 9.6 x 10* (rel.) k/kfaQH = 0.96 e-r. esr decay of spin 72-0025

(I) polarization,

H + C 6 H5 CH2 COOH compared with C 6 H6 CH2 COOH (II 1

1 2.5 x 10

9 (rel.) ^/^2-PtOH = 31 y-r. chem.

EtOH.

c.k. 72-0541

1 ~ 4 x 10

7 (rel.) (I) kt lk u = 0.042 y-r. chem. ~ 4% H abstr. 73-0053

38
Table 4. Reactions of H with organic solutes — Continued

No. Solute and Reaction pH /c(dm

3 mol ! s

l ) Ratio Source jMethod Comment Ref.

2.324 dl

phenylalanine 1 4.1 x 108 (rel.) k/kHCOOH = 346 y-r. chem. c.k. 68-0643

1 8.0 x 108

(rel.) ^/^B*OH = 0.8 e-r. esr decay of spin

polarization,

compared with EtOH.

71-0040

2.32b o-phenylenediamine 0 2.8 x 10

8 (rel.) k/kBiOH = 0.28 e-r. esr decay of spin 72-0025

1 7.3 x 10

8 (rel.) ^/^B*OH = 0.73 e-r. esr polarization, 2.0 1.0 x 10

9 (rel.) k/kmoH ~ 1-0 e-r. esr compared with

3.1 1.1 x 10

9 (rel.) klkjhoH =1.1 e-r. esr EtOH; at pHl

4.2 1.6 x 10

9 (rel.) klkvtOH =1-6 e-r. esr second amino

group is 50%

protonated;

at pH2-3 one amino group is protonated;

kc4c. ioT diamine = 2.1 x 109

. 2.326 m-phenylenediamine 1 3.4 x 10

8 (rel.) ^/^•BiOH = 0.34 e-r. esr decay of spin

polarization,

compared with EtOH.

72-0025

2.327 /?-phenylenediamine 1 3.0 x 10

8 (rel.) k/kfoOH ~ 0-3 e-r. esr decay of spin

polarization,

compared with EtOH.

72-0025

2.328 phenyl-/3-D-gluco- 1 3.5 x 10

7 — p.r. opt. p.b.k. at 320 71-0055

pyranoside nm.

pivalate ion See trimethylacetate ion 2.329 polyoxyethylene A— 2 x 10

9 (rel.) ^/^2-PrOH(7D) = y—r- chem. c.k.; at concn. 71-0586

1,5-nonylphenol 200 > 10

-4 M, ratio =

47. 2.330 L -proline 1 5.2 x 10

s (rel.) — y-r. chem. c.k. assuming 68-0343

k(H + allyl ale.) = 2.8 x 109

1 8 x 10

s (rel.) ^/^BiOH = 8 X e-r. esr decay of spin 71-0040

10^ polarization,

compared with EtOH.

2.331 1,3-propanediol 7 1.9 x 10

7 (rel.) ^/^MeCDOHMe = y-r. chem. c.k. 66-0422

1.9 2.332 propane 1 2.2 x 10

7 (rel.) ^/^BiOH = 2.2 X e-r. esr decay of spin 71-0003

10‘2 polarization,

compared with 2-PrOH(7D).

2.333 1-propanol 2 4 x 10

7 (rel.) k/kj^+ = 1.3 x p.r. opt. c.k.; p.b.k. at 67-0550,

H + CH3 CH2 CH2 OH —

>

10~3 313 nm (Ag^). 68-0436

h 2 + ch3 ch2 choh 1 2.7 x 10

7 (rel.) klkfcon = 2-7 x y-r. chem. c.k. with 71-0017

10~2 2-PrOH(7D).

1 2.5 x 10

7 (rel.) k/k bjoh = 2.5 x e-r. esr decay of spin 71-0003

10'2 polarization,

compared with 2-PrOH(7D).

2.334 2-propanol 1.2 8.4 x 107 (rel.) klk(mi = 1.2 x X-r. chem. c.k. 62-0017

(2-PrOH) 10

2

(I)H + (CH3 ) 2 CHOH 7 1.8 x 10

8 (rel.) klkfmi = 2.6 x X-r. chem. c.k. 62-0024

h 2 +

10"2 (CH3 ) 2 COH ~ 7 5.2 x 10

7 (rel.) k/kj)coo~ = 2.25 y-r. chem. c.k. 63-0041,

(II) H + CH3) 2 CHOH ± 0.2 64-0095

h2 + ~ 6 8.7 x 10

7 (rel.) klkfmi = 0.012 y-r. chem. c.k. 63-0041,

ch2 chohch3 acid A:,//: n = 110 y-r. chem.

64-0095

64-0141

39
Table 4. Reactions of H with organic solutes — Continued

No. Solute and Reaction pH k(dm 3 mol *s *) Ratio Source Method Comment Ref.

2.334 c >nt. — 5.3 x 10

7 (rel.) ^/^MeOH = 26.4 — — c.k.; no details 67-0041

given

2 1.1 x 10

8 (rel-.) k/k ^ = 3.58 x p.r. opt. c.k.; formn. of 67-0550,

10~3 Ag2 at 313 nm. 68-0436

-0.4 1.7 x 10

8 (rel.) k/kory ~ 8 ‘ 33 X y-r. chem. c.k. 68-0525

10"3

1 6.5 x 10

7 (rel.) ^/^BiOH = 6.5 x e-T. esr decay of spin 71-0003

10~2 polarization.

compared with 2-PrOH(7D).

1 7.9 x 10

7 — p.r. esr decay of H 71-0303

signal.

1 7.8 x 10

7 ^/^BxOH = 7.8 X y-r. chem. c.k. with 71-0017

10"2 2-PrOH(7D).

1 — — y-r. chem. 100% H abstr. 73-0053 For other ratios see: 2.11, 2.15, 2.16, 2.18, 2.48, 2.54, 2.70, 2.70a, 2.74, 2.75, 2.81, 2.85, 2.86, 2.106, 2.112 2.119, 2.124, 2.128, 2.136

2.145, 2.148, 2.150, 2.153, 2.158, 2.159, 2.161, 2.164, 2.165

2.166, 2.167, 2.182, 2.185-2.188, 2.207, 2.222, 2.308, 2.320

2.322, 2.335, 2.336, 2.345, 2.361, 2.385 D + (CH3 ) 2 CHOH 1 4.9 x 10

7 — p.r. esr decay of H 71-0303

HD + (CH 3 ) 2 COH signal. 2.335 2-propanol-2-d 6, 1 x 10

7 (rel.) k/k2-pioh = O-I 3 y-r. chem. detd. G(H2 ) and 64-0141

H + (CH3 ) 2 CDOH acid G(HD).

HD + (CH 3 ) 2 COH — 1.3 x 10

7 (rel.) kl ^2-PrOH = 0.17 — assumed value. 66-0422 — 1.1 x 10

7 (rel.) ^/^BiOH = 1-05 X -y-r. chem. c.k. 71-0017

10"2 For other ratios see: 2.6, 2.20, 2.23, 2.2'1, 2.26, 2.27-2.29, 2.31, 2.35, 2.43, 2.44, 2.49, 2.50, 2.54, 2.76, 2.86, 2.93, 2.97, 2.99, 2.101, 2.149, 2.174 2.218, 2.231, 2.279, 2.284, 2.302,

2.319, 2.331, 2.337, 2.341, 2.360, 2.378

2.336 2-propanol-d7 0 8 x 10

6 (rel.) ^/^2-PrOH - 10 y-r. chem. detd. G(H2 ) and 69-0500

H + (CD 3 ) 2 CDOH G(HD).

HD + (CD3 ) 2 COH 1 1.1 x 10

7 (rel.) kl k2-pjOH ~ T34 y-r. chem. c.k. 71-0017

x 10'1

1 1.1 x 10

7 (rel.) ^/^BxOH = 1-05 x y-'. chem. c.k. 71-0017

10'2 For other ratios see: 2.221, 2.260, 2.329

2.337 propionate ion — 1.3 x 10

7 (rel.) ^/^MeCDOHMe y-r. chem. c.k. 66-0422

H + CH3 CH2 C02 -^ 1.3 h2 + c 2 h4 co2 7 1.8 x 10

7 (rel.) k/k^oH = 1-8 x e-r. esr decay of spin 72-0039

10"2 polarization.

compared with EtOH.

2.338' propionic acid 1 5.9 x 10

6 (rel.) ^/^B*OH = x y-r. chem. c.k. with 71-0017

H + CH3 CH2 COOH 10'3 2-PrOH(7D).

H 2 + C 2 H4 COOH (I) 1 6.4 x 10

6 (rel.) k/k^oH = 0-4 x e-r. esr decay of spin 71-0003

H + CH3 CH2 COOH 10~3 polarization, no H 2 (II) compared with 2-PrOH(7D).

1 5.1 x 10

6

(I) (rel.) ki/k n = 24 y-r. chem. 96% H abstr. 73-0053

2.339 propionitrile 1 1.06 x 10

7 (rel.) kl kBiOH = 106 x e-r. esr decay of spin 71-0003

10"2 polarization.

compared with 2-PrOH(7D).

2.340 propylene — 4 x 10

9 (rel.) = 2000 — — c.k.; no details 67-0041

H + CH3 CH=CH2 -» given. c 3 h 7

40
Table 4, Reactions of H with organic solutes — Continued

No. Solute and Reaction pH k(dm 3 mol *s *) Ratio Source Method Comment Ref.

2.341 propylene glycol — 1.9 x 10

7 (rel.) kl ^ MeCDOHMe = y-r. chem. c.k. 66-0422

H + HOCH2 CH2 CH2 OH -* 1.9 h2 + hoch2 ch2 choh

2.342 purine 1 1.2 x 10

8 (rel.) k/kBiOH = 0.12 e—r. esr decay of spin

polarization,

compared with EtOH.

72-0025

2.343 pyrazine 1 3.3 x 10

8 (rel.) ^/^b*oh = Q-33 e—r. esr decay of spin

polarization,

compared with EtOH.

72-0025

2.344 pyridazine 1 2.9 x 10

8 (rel.) ^/^BrOH = 0.29 e-r. esr decay of spin

polarization,

compared with EtOH.

72-0025

2.345 pyridine ~ 6 1.0 x 10

9 (rel.) kl ^2-PtOH = 13 ± y-r. chem. c.k. 64-0095

h + c 5 h5 n-^ 2.5 c 5 h6 n 7 6.5 x 10

8 (rel.) ^“/^BxOH = 0.65 e—r. esr decay of spin

polarization,

compared with EtOH.

72-0039

2.346 pyridinium ion 1 2.9 x 10

8 (rel.) klkleni = 4 - 2 x p.r. opt. c.k. 67-0251

H + C S HS NH+ ^ 10“2 c 5 h6 nh+

1 1.7 x 10

8 — p.r. opt. p.b.k.;

rert-BuOH as OH

71-0582

2.2 x 10

8 (rel.) scavenger.

1 = 0-22 e-r. esr decay of spin

polarization,

compared with EtOH.

72-0025

2.347 pyrimidine 1 1.0 x 10

8 (rel.) k/kfoon =0.1 e-r. esr decay of spin 72-0025,

polarization,

compared with EtOH.

71-0040

2.348 ribonuclease 2.2- 1.5 x 10

10 — p.r. opt. p.b.k. 71-3087,

H + RNase —

6.7 72-1004,

H adduct 72-3094

2.349 D-ribose 1 5.5 x 10

7 (rel.) kl ^BxOH = 3.5 x e—r. esr decay of spin 71-0040

H + C s H 10 O5 —

»

10~2 polarization,

H2 +Cs H9 O s (I) compared with h + c 5 h 10 o 5 ^ EtOH.

no H 2 (II) 1 4.6 x 10

7 (I) (rel.) kikn = 5 y-r. chem. 83% H abstr. 73-0053

2.350 salicylate ion 2 (2.4 ± 0.4) x 10

9 — p.r. opt. p.b.k. at 390 nm. 68-0305

H + OHC6 H4 COCT 2 1.1 x 10

9 (rel.) = 330 p.r. opt. c.k. 68-0305

OHC6 H5 COO" 2 1.7 x 10

9 (rel.) ^/^•EtOH ~ 66 p.r. opt. c.k. 68-0305

2.351 sarcosine 1 1.2 x 10

s (rel.) = 1-2 X e-r. esr decay of spin 71-0040

10

-4 polarization,

compared with EtOH.

2.352 selenourea 6.5 6.3 x 10

8 — p.r. opt.. p.b.k. at 410 nm 70-0240

H + NH2 CSeNH2 —

»

(NH2 C(=NH)Se“)2 H 2 + NH2 C(=NH)Se — 1.2 x 10

9 (rel.) k/kfjtofi — 47 p.r. opt. c.k. 70-0240 — 8 x 10

8 (rel.) k/k^eoh = 400 p.r. opt. c.k. 70-0240

2.353 DL-serine 1 3.6 x 106 (rel.) — y-r. chem. c.k. assuming 68-0343

k(H + allyl ale.) = 2.8 x 10

9

1 1.3 x 10* (rel.) kl ^b*oh = 1-3 x e-r. esr decay of spin 71-0040

10'3 polarization,

compared with EtOH.

41
Table 4. Reactions of H with organic solutes — Continued

No. Solute and Reaction pH k(dm 3 mol ! s

l ) Ratio Source Method Comment Ref.

2.354 succinate ion 7 1.1 x 10

7 (rel.) k/ ^BiOH = 1 • 1 x e-r. esr. decay of spin 72-0039

10

-2 polarization,

compared with EtOH.

2.355 succinic acid 1 2.3 x 10

6 (rel.) k/kb»oh = 2.3 x y-T. chem. c.k. with 71-0017

H + (CH 2 COOH)2 -+ 10"3 2-PrOH(7D).

h 2 + 1 3.5 x 10

6 (rel.) k/k b«oh = 3.5 x e-r. esr decay of spin 71-0003

HOOCCH2 CHCOOH 10"3 polarization,

(I) compared with H + (CH 2 COOH)2 ^ 2-PrOH(7D).

no H 2 (II) 1 2.7 x 10

6

(I) (rel.) *„/*, = 0.05 y-r. chem. 95% H abstr. 73-0053

2.356 sucrose 1.0 2.6 x 10

7 (rel.) ^/^HCOOH =35 X-r. chem. c.k. 56-0012

H + C —

>

H 2 + C 12 H 2 iO u

2.357 tartaric acid 1 1.7 x 10

7 (rel.) ^/^BiOH = 1.7 X e-r. esr decay of spin 71-0003

10"2 polarization,

compared with 2-PrOH(7D).

2.358 tartronic acid 1 2.3 x 10

7 (rel.) k/k BlOH = 2.3 X e-r. esr decay of spin 71-0040

10"2 polarization,

compared with EtOH.

2.359 tetrafluoromethane — — — —

— — 71-0026

H + CF4 -> no reaction 2.360 tetrahydrofuran — 3.4 x 10

7 (rel.) k/k MeCDOHMe = y-r. chem. c.k. 66-0422

H + C 4 H8 0 3.4 h 2 + c 4 h 7 o 1 7.8 x 10

7 (rel.) k/k BiOH = 7.8 x e—r. esr decay of spin 71-0003

10"2 polarization,

compared with 2-PrOH(7D).

2.361 tetraiodofluore- 8.3 1.8 x 10

9 (rel.) k/k2-PiOH = 23 ± X-r. phot. c.k. 71-0354

scein 4

8.4 5.3 x 10

9 (rel.) = 88 X-r. phot. c.k. 71-0295

2.362 N,N,N',N'-ietra- 1 2.4 x 10

8 (rel.) BiOH = 0-24 e-r. esr decay of spin 72-0025

methyl-p-phenyl- polarization,

lenediamine compared with EtOH.

2.363 2,2,6,6-tetra- 1.9 5.3 < 10

9 (rel.) k/k(mi = 0.76 p.r. opt. c.k.i d.k. at 71-0618 m ethyl-4- piperi- 410 nm (ferri). done N-oxyl (TAN) 6.7 x 10

9 (rel.) k/kQ = 0.81 p.r. opt. c.k.; p.b.k. at 410 nm

(benzoquinone-H

adduct).

71-0618

2.364 tetranitromethane — (2.6 ± 1.0) x 10

9 — p.r. opt. p.b.k. 64-0133

H + C(N02 ) 4 ^ 2 5.5 x 10

8 — p.r. opt. p.b.k. at 366 nm 65-0183

H

+ + C(N02 )j + (nitroform anion);

NOj — 1.4 x 10

8 (rel.) klkd = 11 y-r. chem.

cor. for k H and

^OHc.k.; solvent dioxane contg.

2.2 M water.

67-0222

2.365 thioacetamide 1 6 x 10

9 (rel.) ^/^BiOH = 6 X e-r. esr decay of spin 71-0040

10'3 polarization,

compared with EtOH.

2.366 thiodiglycolic 1 2 x 10

9 (rel.) k/ k BrOH = 2 e-r. esr decay of spin 71-0040

acid

1 y-r. chem.

polarization,

compared with EtOH.

no H abstr. 73-0053

42
Table 4. Reactions of H with organic solutes — Continued

No. Solute and Reaction pH fc(dm

3 mol *s *) Ratio Source Method Comment Ref.

2.367 thioglycolic acid 1 4 x 10

9 (rel.) ^/^BiOH = 4 e-i. esr decay of spin

polarization,

compared with EtOH.

71-0040

2.368 thiomalic acid 1 3 x 10

9 (rel.) e-r. esr decay of spin

polarization,

compared with EtOH.

71-0040

2.369 thiophenol 1 4.0 x 10

9 (rel.) — e-r. esr Unpubl. data. 73-0053

H + C 6 H5 SH P. Neta and

H 2 +C6H5 S (I) R.H. Schuler. H + C 6Hs SH 1 2.8 x 10

9

(I) (rel.) kjku = 2.45 y-r. chem. 71% H abstr. 73-0053

C 6 H6 SH (II) 2.370 thiourea 1 6 x 10

9 (rel.) k/kB*OH = 6 x e-r. esr decay of spin 71-0040

10"3 polarization,

compared with EtOH.

2.371 threonine, 1 7.9 x 10

6 (rel.) — y-r. chem. c.k. assuming 68-0343

positive ion fc(H + allyl ale.) = 2.8 x 10

9

. 1 8 x 10

6 (rel.) k/k Bxoh = 8 x e-r. esr decay of spin 71-0040

10"3 polarization,

compared with EtOH.

2.372 thymidylic acid 7-8 2.3 x 10

8 (rel.) klk^QQQ— = 10 y-r. chem. c.k. 68-3038

2.373 thymidine 7-8 2.5 x 10® (rel.) kl ^DCOO~ = H y-r. chem. c.k. 68-3038

2.374 thymine 1 8 x 10

8 (rel.) kl kOIJ = 4 x y-r. chem. c.k. 68-0359

10

-2

0.7 7 x I0

8 — p.r. opt. p.b.k. at 400 68-0597 nm. 7-8 2.3 x 10

8 (rel.) ^/^DCOO~ = y-r. chem. c.k. 68-3038

1 5 x 10

8 (rel.) k/k^xOH ~ 8-5 e-r. esr decay of spin

polarization,

compared with EtOH.

71-0040

0.65 (6.8 ± 0.2) x 10

8 — p.r. opt. p.b.k. at 400 71-0529 nm.

2.375 toluene 3 (2.6 ± 0.5) x 10

9 — p.r. opt. p.b.k.; methanol 67-0246

H + C 6 H5 CH3 —

»

as OH scavenger; c 6 h6 ch3 cor. for fc MeOH . 2.376 p-tolyl-5-/3-D~

thioglucopyranoside — 2.1 x 10

9

(rel.) 1 | p.r. — — 70-1056

2.377 trichlorofluoro- 1 1.7 x 10

6 (rel.) ^•/^BiOH = 1-7 * e-r. esr decay of spin 71-0003

methane 10"3 polarization,

compared with 2-PrOH(7D).

2.378 trimethylacetate — 2 x 10

6 (rel.) ^/^MeCDOHMe = y-r. chem. c.k. 66-0422

ion 2 x 10

_1 H + (CH3) 3 CC02--> H2 + (CH3 ) 2 C(CH 2 )COO"

2.379 trimethylaceto- 1 1.5 x 10

7 (rel.) — e-r. esr Unpubl. data. 73-0053

nitrile P. Neta and

H + (CH3) 3 CCN -* R.H. Schuler. h2 + 1 7.5 x 10

s

(I) kl /k n = 0.053 y-r. chem. 5% H abstr. 73-0053

(CH3 ) 2 (CH2 )CCN (rel.)

(I) H + (CH3 ) 3 CCN -* (CH3 ) 3 CCNH (II)

43
Table 4. Reactions of H with organic solutes — Continued

No. Solute and Reaction pH k(dm 3 mol *s *) Ratio Source Method Comment Ref.

2.380 trimethylanilinium 1 4.5 x 10

8 (rel.) BiOH = 0.45 e-r. esr decay of spin 72-0025

ion polarization,

compared with EtOH.

2.381 tropylium ion h + c 7 h;-» — (7 ± 2) x 10

9 — p.r. opt. p.b.k. at 315 nm. 71-0710

c 7 h 7 + h 3 o

+ 2.382 L-tryptophan 1 2.25 x 10

9 (rel.) k/k hcooh = 3000 y-r. chem. c.k. 68-0343

1 (7.4 ± 1) x 10

9 p.r. opt. p.b.k. at 325 nm;

methanol as OH

69-0459

2 x 10

8

scavenger; cor. for k(H + MeOH)

and &(OH +

tryptophan). 2.383 DL -tryptophan ~ 6 e.d. opt. d.k. at 278 nm;

cor. for product absorption and H + H.

64-9012

1 & 2.3 x 10

9 (rel.) ^/^BiOH ^ 2.3 e-r. esr decay of spin

polarization

compared with EtOH.

71-0040

2.384 DL -tyrosine ~ 6 ~ 4 x 10

8 e.d. opt. d.k. at 274 nm;

cor. for product

absorption and

H + H.

64-9012

1 8.2 x 10

8 (rel.) ^/^HCOOH = 1090 y-r. chem. c.k. (l isomer). 68-0343

1 1.1 x 10

9 (rel.) WkBlOH =1-1 e-r. esr decay of spin

polarization,

compared with EtOH.

71-0040

1.0 (9.8 ± 0.4) x 10

9 — p.r. opt. p.b.k. 71-0143

9.0 (2.0 ± 0.5) x 10

9 — p.r. opt. p.b.k. 73-0003

2.385 uracil 6 4.7 x 10

9 (rel.) ^2-PiOH = 59 ±

7 y-r. chem. c.k. 64-0095

2 (5.6 ± 0.6) x 10

9 p.r. opt. p.b.k. at 420 nm;

formaldehyde as OH scavenger;

cor. for H + ch2 o.

69-0571

2 2.8 x 10

8

2.8 x 108 (rel.) — p.r. esr decay of H

signal.

71-0303

1 BlOH = 0.28 e-r. esr decay of spin

polarization,

compared with EtOH.

71-0040

7 2-3 x 10

8 (rel.) k/kBlOH = 0.2 — e-r. esr decay of spin 72-0039

0.3 polarization,

compared with EtOH.

7 2.4 x 10* (rel.) ^/^BiOH = 2.4 X y-r. chem. c.k. with 72-0049

10'1 2-PrOH(7D).

2.386 urea 1 < 3 x 10

4 (rel.) k/kBiOH < 3 X e—r. esr decay of spin 71-0003

10~s polarization,

compared with 2-PrOH(7D).

valerate ion See pentanoate ion

1

44
Table 4. Reactions of H with organic solutes — Continued

No. Solute and Reaction pH k(dm 3 mol *s

3

) Ratio Source Method Comment Ref.

2.387 valine,

positive ion

1 3.3 x 10

6 (rel.)' — y-r. chem. c.k. assuming

k(H + allyl ale.) = 2.8 x 10

9

68-0343

1 9 x 10

6 (rel.) k/kBlOH = 9 x

10~3 e-r. esr decay of spin

polarization,

compared with EtOH.

71-0040

2.388 valine, zwitterion

7 1.3 x 10

7 (rel.) kl ^BxOH = 1*3 x 10'2 e-r. esr decay of spin

polarization,

compared with EtOH.

72-0039

45
Formula index

Ag+

, 2.5

As(III) Arsenic(III) ion, 2.6 AsF6

~ Hexafluoroarsenate(V) ion, 2.7 AuC14 Tetrachloroaurate(III) ion, 2.8 B 4 0 7

2 Tetraborate ion, 2.9 Br Bromide ion, 2.10a Br0 3 ~ Bromate ion, 2.11 Br2 Bromine, 2.10 CC1F3 Chlorotrifluoromethane, 2.189 CC12 F2 Dichlorodifluoromethane, 2.211 CC13 F Trichlorofluoromethane, 2.377 CC14 Carbon tetrachloride, 2.177 CD02 d-Formate ion, 2.240 CF4 Tetrafluoromethane, 2.359 CHClj Chloroform, 2.183 CHD02 d-Formic acid, 2.242 CHD3 O Methanol-d3 , 2.298 CHN Hydrogen cyanide, 2.15 CH02 ~ Formate ion, 2.239 CHO3 Bicarbonate ion, 2.14 CH2 C1 2 Dichloromethane, 2.212 CH2 0 Formaldehyde, 2.238 CH2 0 2 Formic acid, 2.241 CH3 CI Chloromethane, 2.184 CHjDO Methanol-J, 2.297 CH3

I Iodomethane, 2.275 CH3 N02 Nitromethane, 2.311 CH3 0 Methoxide ion, 2.299 CH4 Methane, 2.294 CH4 N 2 0 Urea, 2.386 CH4N 2 S Thiourea, 2.370 CH4N 2 Se Selenourea, 2.352 CH40 Methanol, 2.296 CH4 S Methanethiol, 2.295 CHS N 3 Guanidine, 2.259 CH6 N

+ Methylammonium ion, 2.301 CH 15 CoN6 2+ Cyanopentaamminecobalt(III) ion, 2.29 CH 15 CoN 6 S

2+ Thiocyanatopentaamminecobalt(III) ion, 2.30 CN Cyanide ion, 2.16 CNS Thiocyanate ion, 2.18 CN40 8 Tetranitromethane, 2.364 CO Carbon monoxide, 2.12 C02 Carbon dioxide, 2.13 CS2 Carbon disulfide, 2.176 C 2 D 3 0 2 - Acetate ion-J3 , 2.108 C 2 H03 _ Glyoxylate ion, 2.257 C 2 H04 Oxalate ion, hydrogen, 2.316 C 2 H 2 Acetylene, 2.114 C 2 H2 Br0 2 _ Bromoacetate ion, 2.158 C 2 H2 C10 2 Chloroacetate ion, 2.178 C 2 H2 F0 2 ~ Fluoroacetate ion, 2.236 C 2 H 2 0 2 Glyoxal, 2.256 C 2 H2 03 Glyoxylic acid, 2.258 C 2 H2 04 Oxalic acid, 2.316-7

C 2 H3 Br0 2 Bromoacetic acid, 2.159 C 2 H3 C10 2 Chloroacetic acid, 2.179 CjH3 N Acetonitrile, 2.111 C 2 H3 02 _ Acetate ion, 2.107 C 2 H3 0 3 ~ Glycolate ion, 2.252 C 2 H4 Ethylene, 2.229 C 2 H4 D 2 0 Ethanol-d2 , 2.225 C 2 H4 N 2 Aminoacetonitrile, 2.125 C 2 H4 0 Acetaldehyde, 2.104

C 2 H4 0 2 Acetic acid, 2.109 C 2 H4 0 2 S Thioglycolic acid, 2.367 C 2 H4 0 3 Glycolic acid, 2.253 C 2 H 5 Br Bromoethane, 2.160 C 2 H 5 BrO 2-Bromoethanol, 2.161 C 2 H 5 C1 Chloroethane, 2.181 C 2 H5 C10 2-Chloroethanol, 2.182 C 2 H s NO Acetamide, 2.105 C 2 Hs N02 Glycine, 2.250-2.251; Nitroethane, 2.310 C 2 H5 NS Thioacetamide, 2.365 C 2 Hs O" Ethoxide ion, 2.226 C 2 H6 Ethane, 2.223 C 2 H6 0 Ethanol, 2.224 C 2 H6 OS 2 -Mercaptoethanol, 2.292 C 2 H6 0 2 Ethylene glycol, 2.231 C 2 H 7 NO 2 -Aminoethanol, 2.126 C 2 H7 NS Cysteamine, 2.204 C 2H7 04P Ethyldihydrogen phosphate, 2.233 C 2 H 15 CoF3 N 5 2+ Trifluoroacetatopentaamminecobalt(III) ion, 2.38 C 2 H 18 CoN5 0 2

2+ Acetatopentaamminecobalt(III) ion, 2.36 C 2 N2 Cyanogen, 2.17 C 2 04

2 Oxalate ion, 2.315 C 3 HD 7 0 2-Propanol-d7 , 2.336 C 3 H2 N 2 Malononitrile, 2.291 C 3 H3 N02 Cyanoacetic acid, 2.192 C 3 H4 Br0 2 ~ 2-Bromopropionate ion, 2.164; 3-Bromopropionate ion, 2.165 C 3 H4 C10 2 _ 2-Chloropropionate ion, 2.185; 3-Chloropropionate ion, 2.186 C 3 H4 N 2 Imidazole, 2.273 C 3 H4 04 Malonic acid, 2.290 C 3 H4 O s Tartronic acid, 2.358 C 3 H5 Br0 2 2 -Bromopropionic acid, 2.166; 3-Bromopropionic acid, 2.167 C 3 H5 C10 2 2-Chloropropionic acid, 2.187; 3-Chloropropionic acid, 2.188 C 3 H5 N Propionitrile, 2.339 C 3 H5 NO Acrylamide, 2.118 C 3 H5 0 2 _ Propionate ion, 2.337 C3H6 Cyclopropane, 2.202; Propylene, 2.340 C 3 H6 0 Acetone, 2.110; Allyl alcohol, 2.124 C 3 H6 0 2 Methyl acetate, 2.300; Propionic acid, 2.338 C 3 H6 0 2 S 2 -Mercaptopropionic acid, 2.292a;

3 —Mercaptopropionic acid, 2.292b C 3 H6 03 Lactic acid, 2.285 C3 H 7 DO 2-Propanol-2-<7, 2.335 C 3 H 7 N02 a-Alanine, 2.122; /3-Alanine, 2.123;

1 -Nitropropane, 2.312; Sarcosine, 2.351 C 3 H 7 N02 S Cysteine, 2.205-2.206 C 3 H 7 N03 Serine, 2.353 C 3 H8 Propane, 2.332 C 3 H8 0 1 -Propanol, 2.333; 2-Propanol, 2.334 C 3 H8 0 2 1,3-Propanediol, 2.331 C 3 H8 03 Glycerol, 2.249 C 4 CdN4 2_ Tetracyanocadmate(II) ion, 2.20 C 4 H 2 0 4 Acetylenedicarboxylic acid, 2.115 C 4H3BrN 2 0 2 5-Bromouracil, 2.168 C 4 H 3 C1N 2 0 2 5-Chlorouracil, 2.190 C 4 H3 FN 2 0 2 5-Fluorouracil, 2.237 C 4 H3 N 2 0 3 _ Barbiturate ion, 2.140 C 4 H3 0 4 _ Fumarate ion, hydrogen, 2.243 C 4 H4 N 2 Pyrazine, 2.343; Pyridazine, 2.344;

46
Pyrimidine, 2.347 C 4H4 N2 02 Uracil, 2.385 C 4 H4 N 2 03 Barbituric acid, 2.141 C 4 H404 Fumaric acid, 2.244; Maleic acid, 2.288 C 4 H40 4

2~ Succinate ion, 2.354 C 4H4 O s Oxalacetic acid, 2.314 C4H4 06 2,3-Dihydroxyfumaric acid, 2.216 C4 Hs N 3 0 Cytosine, 2.209 C 4H6 Butadiene, 2.168a C 4H6 N03 N-Acetylglycine, 2.117 C 4H6 N04 _ Aspartate ion, 2.138 C 4H6 0 2 Biacetyl, 2.155; Cyclopropanecarboxylic acid, 2.203 C4H6 04 Succinic acid, 2.355 C 4H604 S Thiodiglycolic acid, 2.366; Thiomalic acid, 2.368 C 4H6 04 S 2 Dithiodiglycolic acid, 2.219 C 4H6 Os Malic acid, 2.289 C 4H6 06 Tartaric acid, 2.357 C 4H7 N Isobutyronitrile, 2.281 C 4H7 N04 DL-Aspartic acid, 2.139; Iminodiacetic acid, 2.274 C 4H 7 0 2 ~ Butyrate ion, 2.174; Isobutyrate ion, 2.279 C4 H8 1-Butene, 2.173; Isobutylene, 2.278 C 4H8 N2 03 DL-Asparagine, 2.137; Glycylglycine, 2.254 C 4H8 0 Tetrahydrofuran, 2.360 C 4 H8 0 2 Butyric acid, 2.175; Dioxane, 2.218; Ethyl acetate, 2.227; Isobutyric acid, 2.280 C 4 H9 N02 2-Aminobutyric acid, 2.125a; 2-Amino-2-methylpropionic acid, 2.127 C 4H10 Butane, 2.169; Isobutane, 2.276 C 4H10 NO3 + Threonine, positive ion, 2.371 C 4 H 10 O 1-Butanol, 2.170; 2-Butanol, 2.171; ferf-Butanol, 2.172; Ethyl ether, 2.232; Isobutyl alcohol, 2.277 C 4H 16 C12 CoN4 + Dichlorobis(ethylenediamine)-

cobalt(III) ion, 2.43 C 4H 16 CoF2 N4 + Difluorobis(ethylenediamine)-

cobalt(III) ion, 2.42 C 4 H 18 CoNs 04 + Fumarylpentaamminecobalt(III) ion, 2.32 C 4 H20 CoN4O 2 3+ Diaquobis(ethylenediamine)-

cobalt(III) ion, 2.41 C 4N4 Pt

2_ Tetracyanoplatinate(II) ion, 2.93 C 5 H3 BrN 2 04 5-Bromoorotic acid, 2.162 C 5 H4N2 04 Orotic acid, 2.313; Isoorotic acid, 2.283; ant/-5-Nitro-2-furald oxime, 2.310a C S H4 N4 Purine, 2.342 C 5 H5 N Pyridine, 2.345 C 5 Hs N5 Adenine, 2.119 C 5 H6 N

+ Pyridinium ion, 2.346 C 5 H6 N 2 02 Thymine, 2.374 C 5 H6 N2 S 2 6-Methyluracil, 2.303 C s H8 N03 N-Acetylalanine, 2.116 C sH8 N04 _ Glutamate ion, 2.246 C 5 H8 N2 02 5,6-Dihydrothymine, 2.217 C 5 H8 0 2 Acetylacetone, 2.113; Cyclobutanecarboxylic acid, 2.193 C 5 H9 N Trimethylacetonitrile, 2.379 C 5 H9 N02 Proline, 2.330 C sH9 N03 Hydroxyproline, 2.272 C s H9 0 2 _ Isovalerate ion, 2.284; Pentanoate ion, 2.319; Trimethylacetate ion, 2.378 C S H 10 Cyclopentane, 2.200 C 5 H 10 NO4 + Glutamic acid, positive ion, 2.247 C 5 H 10 O 2 2-Methylbutanoic acid, 2.302 C 5 H 10 O 4 Deoxyribose, 2.210

C 5 H 10 O 5 Arabinose, 2.133; Ribose, 2.349 C 5 H n N0 2 Norvaline, 2.312a; Valine, 2.387-8

C 5 H uN0 2 S Methionine, 2.298a; Penicillamine, 2.317a C 5 H

i

2 Pentane, 2.318 C 5 H 12 N0 2 + Betaine, 2.154 C 5 H 12 0 Neopentyl alcohol, 2.305 C 5 H 16 CoN4 0 3 + Carbonatobis(ethylenediamine)-

cobalt(III) ion, 2.44 C 6 CoN6 3_ Hexacyanocobaltate(III) ion, 2.35 C 6 Co0 12 3- Trioxalatocobaltate(III) ion, 2.47 C6 Cr0 12

3 Trioxalatochromate(III) ion, 2.51 C 6FeN6

3 Hexacyanoferrate(III) ion, 2.63 C6Fe0 12 3~ Trioxalatoferrate(III) ion, 2.64 C 6 H4 0 2 Benzoquinone, 2.152 C 6 H5 BrO p-Bromophenol, 2.163 C6 Hs N02 Nicotinic acid, 2.306; Nitrobenzene, 2.308 C 6 Hs 03 S~ Benzenesulfonate ion, 2.145 C 6 H6 Benzene, 2.144 C 6 H6 0 Phenol, 2.320 C 6 H6 S Thiophenol, 2.369 C 6 H 7 N Aniline, 2.128 C 6 H 7 N02 N-Ethylmaleimide, 2.234 C 6 H 7 0 6 ~ Ascorbate ion, 2.135 C 6 H8 1,3-Cyclohexadiene, 2.195; 1,4-Cyclohexadiene, 2.196 C 6 H8 CoN2 0 8 Dioxalatoethylenediaminecobaltate(III) ion, 2.46 C 6 H8 N

+ Anilinium ion, 2.129 C 6 H8 N2 o-Phenylenediamine, 2.325; m-Phenylenediamine, 2.326; p-Phenylenediamine, 2.327 C 6 H8 0 4 Dimethyl fumarate, 2.217a C 6 H8 06 Ascorbic acid, 2.136 C 6 H8 0 7 Citric acid, 2.191 C 6 H9 N03 N-Ethylmaleamic acid, 2.233a C6H9 N3 Nitrilotriacetic acid, 2.307 C 6 H9 N3 02 Histidine, 2.269 C 6 H 10 Cyclohexene, 2.198 C 6 H 10 O2 1-Cyclopentanecarboxylic acid, 2.201 C 6 H 10 O3 Ethyl acetoacetate, 2.228 C 6H u 02 _ Hexanoate ion, 2.264 C 6H n N3 04 Glycylglycylglycine, 2.255 C 6 H 12 Cyclohexane, 2.197 C6 H 12 N2 04 S 2 Cystine, 2.207 C 6 H 12 02 Hexanoic acid, 2.265 C 6 H 12 06 Glucose, 2.245 C 6 H 13 N Hexamethyleneimine, 2.261 C 6 H 13 N02 Isoleucine, 2.282; Leucine, 2.286 C 6 H 14 Hexane, 2.262 C 6 H mN2 02 Lysine, 2.287 C 6 H 14 N4 02 L-Arginine, 2.134 C 6H 14 0 1-Hexanol, 2.266 C 6 H 16 CoN4 04 + Oxalatobis(ethylenediamine)-

cobalt(III) ion, 2.45 C 6 Hi6 N

+ 1-Hexylammonium ion, 2.267 C 6 Hi6 N 2 1,6-Hexanediamine, 2.263 C 6 H24 CoN6 3+ Tris(ethylenediamine)cobalt(III) ion, 2.40 C 7 H5 C10 2 p-Chlorobenzoic acid, 2.180 C 7 H5 N Benzonitrile, 2.150 C 7 H5 N04 p-Nitrobenzoic acid, 2.309 C 7 H s 0 2 _ Benzoate ion, 2.148 C 7 Hs 0 3 _ Salicylate ion, 2.350 C 7 H6 0 Benzaldehyde, 2.142 C 7 H6 0 2 Benzoic acid, 2.149 C 7 H6 0 3 p— Hydroxybenzoic acid, 2.270 C 7 H 7 + Tropylium ion, 2.381 C 7 H 7 NO Benzamide, 2.143 47
C 7 H8 Cycloheptatriene, 2.194; Toluene, 2.375 C 7 H8 0 Anisole, 2.130; Benzyl alcohol, 2.153 C 7 H2oCoN 5 0 2 2+ Benzoatopentaamminecobalt(III) ion, 2.39 C 8 H4 N 2 o-Dicyanobenzene, 2.213; m-Dicyanobenzene, 2.214; /?-Dicyanobenzene, 2.215 C 8 H 7 N Indole, 2.274a C 8 H7 02 ~ Phenylacetate ion, 2.322 C 8 H8 0 Acetophenone, 2.112 C 8 H8 02 Phenyl acetate, 2.321; Phenylacetic acid, 2.323 C 8 H9 NO Acetanilide, 2.106 c 8 h 10 o4 c/s-4-Cyclohexene-l,2-dicarboxylic acid, 2.199 C,H6 06 1,3,5-Benzenetricarboxylic acid, 2.146 C,H9 NOj Hippuric acid, 2.268 C 9 H9 03 - p-Hydroxyphenylpropionate ion, 2.270a C 9 H 10 O3 p-Hydroxyphenylpropionic acid, 2.271 C 9 HjjN0 2 Phenylalanine, 2.324 C 9 H n N03 Tyrosine, 2.384 C 9 H 12 Mesitylene, 2.293 C 9 H 14 N

+ Trimethylanilinium ion, 2.380 C 9 H 16 N02 2,2,6,6-Tetramethyl-4-piperidone N-oxyl, 2.363 C 10 H5 O5 S“ l,4-Naphthoquinone-2-sulfonate ion, 2.304 Ci0 H8N2 2,2'-Bipyridine, 2.156; 4,4'-Bipyridine, 2.157 C 10 H9NO2 Indole-3-acetic acid, 2.274b C 10 H 13 N 5 O4 Adenosine, 2.120 Ci0H 14 N 2 O5 Thymidine, 2.373 C 10 H 14 N5 O 7 P Adenosine-5'-phosphate, 2.121 Ci0H 15 N2 O8 P Thymidylic acid, 2.372 C 10 H 16 N 2 N,N,Af',Ar-Tetramethyl-p-phenylenediamine, 2.362 Ci0 H 16 N2 O8 Ethylenediaminetetraacetic acid, 2.230 Ci0 H 16 N 3 O6 S Glutathione, 2.248 C u H uN02 Indole-3-propionic acid, 2.274c ChH 12 N 2 02 Tryptophan, 2.382-3

C uH9 NO 2-Benzoylpyridine, 2.152a; 3-Benzoylpyridine,

2.152b; 4-Benzoylpyridine, 2.152c C 12 H 10 O 2 1-Naphthaleneacetic acid, 2.303a C^HjgOg Phenyl-/3-D~glucopyranoside, 2.328 C^HaOjj Sucrose, 2.356 C 12 H2S Na04S Dodecyl sodium sulfate, 2.221 C^HgO Fluorenone, 2.235 C uH l0 O Benzophenone, 2.151 C^HjgC^S p-Tolyl-5-/3-D-thioglucopyranoside, 2.376 C 14 H8 Os S 9,10-Anthraquinone-2-sulfonate ion, 2.132 Cj4 H 10 Anthracene, 2.131 C mH10O2 Benzil, 2.147 CisHjjCoOj^ Tris(acetylacetonato)cobalt(III) ion, 2.48 C^H^BrN Hexadecyltrimethylammonium bromide, 2.260 C»H8Os

I 4 Tetraiodofluorescein, 2.361 CjoHJ4FeN6 3+ Tris(2,2'— bipyridyl)iron(III) ion, 2.65 CggH^NgRu^ Tris(2,2'-bipyridyl)ruthenium(II) ion, 2.93a CsoH^NgRu3* Tris(bipyridyl)ruthenium(III) ion, 2.93b C MFeN 6 3+ Tris(l , lO-phenanthroline)iron(III)

ion, 2.66 C4sHM0 16 Polyoxyethylene(l,5)nonyl phenol, 2.329 Cd2+ Cadmium(II) ion, 2.19 Ce4*, 2.21 Cl Chloride ion, 2.21a ClCrH ls N s 2+ Chloropentaamminechromium(III) ion, 2.49 ClFe 2+ Chloroiron(III) ion, 2.61 Cl2 CrH8 04

+ Dichlorotetraaquochromium(III) ion, 2.50 Cl2 Fe

+ Dichloroiron(III) ion, 2.62 CoBrH ls N5 2+ Bromopentaamminecobalt(III) ion, 2.27 CoC1H 15 N s 2+ Chloropentaamminecobalt(III) ion, 2.26

CoFH 15 N 5 2+ Fluoropentaamminecobalt(III) ion, 2.25 CoH9 N6 06 Trinitrotrisamminecobaltflll), 2.34 CoH 15 IN 5 2+ Iodopentaamminecobalt(III) ion, 2.28 CoH 15 N 5 04 P Phosphatopentaamminecobalt(III), 2.37 CoH 1s N602 2+ Nitropentaamminecobalt(III) ion, 2.33 CoH 15 N8 2+ Azidopentaamminecobalt(III) ion, 2.31 CoH 16 N 5 0

2+ Hydroxopentaamminecobalt(III) ion, 2.24 CoH nN 5 0

3+ Aquopentaamminecobalt(III) ion, 2.23 CoH 18 N6 3+ Hexaamminecobalt(lil) ion, 2.22 Cr04

2 Chromate(VI) ion, 2.52 Cr2 0 7 2- Dichromate(VI) ion, 2.53 Cu2+ Copper(II) ion, 2.54 D 2 Deuterium, 2.68 D2 S Deuterium sulfide, 2.93c F~ Fluoride ion, 2.55 FFe 2+ Fluoroiron(III) ion, 2.60 F2 Fe + Difluoroiron(III) ion, 2.60 F3 Sn Trifluorostannate(II) ion, 2.97 F6 Sn2~ Hexafluorostannate(IV) ion, 2.99 Fe

2+ Iron(II) ion, 2.56 Fe

3+ Iron(III) ion, 2.57 FeH0 2+ Hydroxoiron(III) ion, 2.58 FeH2+ Hydroiron(III) ion, 2.59 H Hydrogen atom, 2.2 H

+

, 2.67 HN02 Nitrous acid, 2.84 HO Hydroxyl radical, 2.3 HO- Hydroxide ion, 2.90 H02 Perhydroxyl radical, 2.4 H03 P

2 Hydrogen phosphite ion, 2.91 H04P

2 Hydrogen phosphate ion, 2.92 H2 0 2 Hydrogen peroxide, 2.69 H2 04P~ Dihydrogenphosphate ion, 2.91b H2 Os S Peroxysulfuric acid, 2.95 H3 N Ammonia, 2.80 H3 04P Phosphoric acid, 2.91a H4N

+ Ammonium ion, 2.78 HsN2 + Hydrazinium ion, 2.79 Hg2+

, 2.70 Hg2 2+

, 2.70a

1 Iodide ion, 2.72

I

2 Iodine, 2.71

I 2 ~, 2.73

I3 ', 2.74 I03 Iodate ion, 2.75 Mn 2+ Manganese ion, 2.76 Mn04 ~ Permanganate ion, 2.77 NO Nitric oxide, 2.82 N02 _ Nitrite ion, 2.85 N03 _ Nitrate ion, 2.86 N07 S 2

2~ Nitrosyldisulfonate ion (Fremy's salt), 2.87 N2 0 Nitrous oxide, 2.83 N3 ~ Azide ion, 2.81 Ni2+ Nickel(II) ion, 2.88 02 Oxygen, 2.89 0 2 U

2+ Uranyl(VI) ion, 2.102 08 S 2

2- Peroxydisulfate ion, 2.94

Pr(III) Praseodymium(III) ion, 2.92a

Sn(II) Tin(II) ion, 2.96 Sn(IV) Tin(IV) ion, 2.98 Te(VI) Tellurium(VI) ion, 2.100

Tl

+ Thallium(I) ion, 2.101 Zn

2+ Zinc(II) ion, 2.103

48
Acknowledgements

The assistance of the staff of the Radiation Chemistry Data Center in preparation of these tables is gratefully acknowledged. Our thanks go especially to Mary Early for proofreading and indexing and to Joyce Ross for typing of the manuscript. We are grateful to those persons who have provided unpublished

data for inclusion in these tables.

49
55-

0004 56-

0012 57-

0008

57-0009 57-

0010 58-

0004

58-0006

58-0009

58-0011

58-

0047

59-

0006

59-0007

59-0008

59-

0012

60-

0035

60-

0099

61-

0025

61-0099

References

Dewhurst, H.A.; Burton, M., Radiolysis of aqueous solutions of hydrazine, J. AMER.

CHEM. SOC. 77: 5781-5 (1955). Baxendale, J.H.; Smithies, D.H., Die

Strahlenchemie in Wasser geloester

organischer Verbindungen, Z. PHYSIK.

CHEM. (FRANKFURT) 7: 242-64 (1956). Schwarz, H.A., The radiation chemistry

of ferrous chloride solutions, J. AMER.

CHEM. SOC. 79: 534-6 (1957). Allen, A.O.; Rothschild, W.G., Studies in the radiolysis of ferrous sulphate solutions.

I. Effect of oxygen concentrations in 0.8 N

sulphuric acid, RADIAT. RES. 7: 591-602 (1957). Allen, A.O.; Hogan, V.D.; Rothschild, W.G.,

Studies in the radiolysis of ferrous solutions.

II. Effect of acid concentration in solutions containing oxygen, RADIAT. RES. 7: 603—8

(1957). Rothschild, W.G.; Allen, A.O., Studies in the

radiolysis of ferrous sulfate solutions. III. Air-free solutions at higher pH, RADIAT. RES

8: 101-110 (1958). Baxendale, J.H.; Hughes, G., The X-irradiation

of aqueous methanol solutions. Part II. Reaction in D 2 0, Z. PHYSIK. CHEM. (FRANKFURT)

14: 323-38 (1958). Baxendale, J.H.; Hughes, G., The X-irradiation

of aqueous methanol solutions. Part I. Reactions in H 2 0, Z. PHYSIK. CHEM. (FRANKFURT)

14: 306-22 (1958). Schwarz, H.A.; Hritz, J.M., The radiation chemistry of deaerated ferrous chloride

solutions, J. AM. CHEM. SOC. 80: 5636-8 (1958). Friedman, H.L.; Zeltmann, A.H., Hydrogen

conversion and exchange reactions in aqueous

solutions induced by gamma rays, J. CHEM.

PHYS. 28(5): 878-90 (1958). Kurien, K.C.; Phung, P.V.; Burton, M.,

Radiolysis of aqueous solutions of benzene

and of phenol, RADIAT. RES. 11: 283-90 (1959). Boyle, J.W.; Weiner, S.; Hochanadel, C.J., Kinetics of the radiation-induced reaction of

iron(III) with tin(II), J. PHYS. CHEM. 63: 892-6 (1959). Czapski, G.; Jortner, J.; Stein, G., The

oxidation of iodide ions in aqueous solution by atomic hydrogen, J. PHYS. CHEM. 63: 1769-74 (1959). Riesz, P.; Hart, E.J., Absolute rate constants

for H atom reactions in aqueous solutions,

J. PHYS. CHEM. 63: 858-61 (1959). Czapski, G.; Jortner, J., Role of ferrous hydride in the oxidation of ferrous ion by

hydrogen atoms, NATURE (LONDON) 188: 50-1 (1960). Rotblat, J.; Sutton, H.C., The effects of high dose rates of ionizing radiations on solutions

of iron and cerium salts, PROC. ROY. SOC.

(LONDON) SER. A 255: 490-508 (1960). Hayon, E.; Allen, A.O., Evidence for two kinds

of "H atoms" in the radiation chemistry of water, J. PHYS. CHEM. 65: 2181-5 (1961). Firsov, V.G., The retarding effect of the uranyl ion in the radiation-chemical

62-0012

62-0017

62-0018

62-0022

62-0024

62-0033

62-0051

62-0057

62-0087

62-0096

62-0133

62-0144

62-3002

62-7001

62-9008

62-9011

oxidation of bivalent iron, DOKL. PHYS. CHEM.

PROC. ACAD. SCI. USSR 138(5): 483-5 (1961) (translated from DOKL. AKAD. NAUK SSSR. 138(5): 1155-7 (1961)). Chutny, B.; Bednar, J., Geschwindigkeitskonstanten fuer die Reaktionen

von Radikalen mit chloroform, COLLECT. CZECH.

CHEM. COMMUN. 27: 1496 (1962). Rabani, J.; Stein, G., Yield and reactivity

of electrons and H atoms in irradiated aqueous solutions, J. CHEM. PHYS. 37: 1865—73

(1962). Daniels, M., The radiation chemistry of arsenite. Part II. Oxygen—free solution,

J. PHYS. CHEM. 66: 1475-7 (1962). Czapski, G.; Rabani, J.; Stein, G., The

reactivity of hydrogen atoms with ethanol and formate in aqueous solution, TRANS.

FARADAY SOC. 58: 2160-7 (1962). Rabani, J., On the two forms of hydrogen atoms

in neutral solutions irradiated by X-rays,

J. AMER. CHEM. SOC. 84: 868-9 (1962). Rabani, J., On the reactivity of hydrogen atoms in aqueous solutions, J. PHYS. CHEM.

66: 361-2 (1962). Czapski, G.; Allen, A.O., The reducing

radicals produced in water radiolysis: Solutions of oxygen-hydrogen peroxide-hydrogen

ion, J. PHYS. CHEM. 66: 262-6 (1962). Dainton, F.S.; Sills, S.A., The rates of some

reactions of hydrogen atoms in water at 25°C,

PROC. CHEM. SOC.: 223 (1962).

Lifshitz, C.; Stein, G., Isotope effects in the abstraction of hydrogen from ethanol by

hydrogen atoms in irradiated aqueous solutions,

J. CHEM. SOC.: 3706-12 (1962). Boyle, J.W., The decomposition of aqueous

sulfuric acid solutions by cobalt gamma rays,

II. Yields of solvent decomposition and

reducing radicals from Fe(II) solutions in 0.4 to 18 M acid, RADIAT. RES. 17: 450-64

(1962). Thomas, J.K.; Hart, E.J., The radiolysis

of aqueous solutions at high intensities. RADIAT. RES. 17: 408-18 (1962). Hart, E.J.; Boag, J.W., Effect of dose-rate

on the radiolysis of aqueous formic acid, BRIT. J. RADIOL. 35(417): 650 (1962). Rabani, J.; Stein, G., The radiation chemistry

of aqueous solutions of cytochrome c, RADIAT.

RES. 17: 327-40 (1962). Hochanadel, C.J., Photolysis of dilute hydrogen peroxide solution in the presence

of dissolved hydrogen and oxygen. Evidence

relating to the nature of the hydroxyl

radical and the hydrogen atom produced in the radiolysis of water, RADIAT. RES. 17: 286-301 (1962). Jortner, J.; Rabani, J., The decomposition of chloroacetic acid in aqueous solutions by

atomic hydrogen. I. Comparison with radiation chemical data, J. PHYS. CHEM. 66: 2078-81

(1962). Jortner, J.; Rabani, J., The decomposition of 50
chloroacetic acid in aqueous solutions by

atomic hydrogen. II. Reaction mechanism in alkaline solutions, J. PHYS. CHEM. 66: 2081-4 (1962). 63-0004 Shubin, V.N.; Dolin, P.I., The method of a competitive scavenger in radiation chemistry,

RADIAT. RES. 19: 345-58 (1963). 63-0014 Raef, Y.; Swallow, A.J., Action of y-rays on aqueous solutions of carbon monoxide, TRANS.

FARADAY SOC. 59: 1631-40 (1963). 63-0041 Appleby, A.; Scholes, G.; Simic, M.,

Reactivities of the primary reducing species

formed in the radiolysis of aqueous solutions,

J. AMER. CHEM. SOC. 85: 3891-2 (1963). 63-0043 Thomas, J.K., The rate constants for H atom

reactions in aqueous solutions, J. PHYS. CHEM.

67: 2593-5 (1963). 63-0047 Schwarz, H.A., Absolute rate constants for some hydrogen atom reactions in aqueous

solution, J. PHYS. CHEM. 67: 2827-30 (1963).

63-

0049 Nehari, S.; Rabani, J., The reaction of H

atoms with OH- in the radiation chemistry

of aqueous solutions, J. PHYS. CHEM. 67: 1609-13 (1963).

64-

0043 Gordon, S.; Hart, E.J.; Thomas, J.K., The

ultraviolet spectra of transients produced

in the radiolysis of aqueous solutions,

J. PHYS. CHEM. 68: 1262-4 (1964). 64-0049 Schwarz, H.A., Intensity effects, pulsed-beam

effects, and the current status of diffusion

kinetics, RADIAT. RES. SUPPL. 4: 89-113 (1964). 64-0092 Fricke, H.; Thomas, J.K., Pulsed electron beam

kinetics, RADIAT. RES. SUPPL. 4: 35-53 (1964). 64-0093 Sweet, J.P.; Thomas, J.K., Absolute rate constants for H atom reactions in aqueous

solutions, J. PHYS. CHEM. 68: 1363-8 (1964). 64-0095 Scholes, G.; Simic, M., Reactivity of the hydrogen atoms produced in the radiolysis of aqueous systems. J. PHYS. CHEM. 68: 1738-43

(1964). 64-0108 Matheson, M.S., The formation and detection

of intermediates in water radiolysis, RADIAT.

RES. SUPPL. 4: 1-23 (1964). 64-0133 Asmus, K.-D.; Henglein, A.; Ebert, M.; Keene, J.P., Pulsradiolytische Untersuchung

schneller Reaktionen von hydratisierten

Elektronen, freien Radikalen und Ionen mit Tetranitromethan in waessriger Loesung,

BER. BUNSENGES. PHYSIK. CHEM. 68: 657-63

(1964). 64-0141 Anbar, M.; Meyerstein, D., Isotope effects in the hydrogen abstraction from aliphatic

compounds by radiolytically produced hydrogen atoms in aqueous solutions, J. PHYS. CHEM.

68: 3184-7 (1964). 64-0151 Armstrong, D.A.; Wilkening, V.G., Effects of pH

in the y-radiolysis of aqueous solutions of cysteine and methyl mercaptan, CAN. J. CHEM.

42: 2631-5 (1964). 64-0245 Rama Rao, K.V.S.; Kamala, R.; Jain, S.K.,

Effect of iodine and methyl iodide on

radiolysis of water, Proc. Nucl. Radiat. Chem.

Symposium, Bombay, India, Mar. 16-9, 1964, p.73-8. 64- 0293 Pikaev, A.K.; Glazunov, P.Ya., Radiolysis

of aqueous ferrous sulphate solutions under

64-9012

65-0009

65-0010

65-0011

65-0013

65-0014

65-0016

65-0017

65-0044

65-0085

65-0155

65-0183

65-0188

65-0192

65-0371

65-0372

the action of decimicrosecond electron pulses.

DOKL. PHYS. CHEM., PROC. ACAD. SCI. USSR

154 (5): 181-4 (1964) (translated from

DOKL. AKAD. NAUK 154(5): 1167-70 (1964)). Navon, G.; Stein, G., The reactivity of atomic

hydrogen with cysteine, cystine, tryptophan

and tyrosine in aqueous solution, ISRAEL J. CHEM. 2: 151-4 (1964). Matheson, M.S.; Rabani, J., Pulse radiolysis

of aqueous hydrogen solutions. I. Rate

constants for reaction of e^,

- with itself and other transients. II. The

interconvertibility of e tq

~ and H, J. PHYS.

CHEM. 69: 1324-35 (1965). Thomas, J.K., Rates of reaction of the hydroxyl

radical, TRANS. FARADAY SOC. 61: 702-7 (1965). Dainton, F.S.; Walker, D.C., The radiation chemistry of aqueous solutions of nitrous oxide, PROC. ROY. SOC. (LONDON) SER. A

285: 339-59 (1965). Meissner, G.; Henglein, A., Die Reaktionen

des Schwefelwasserstoffs mit hydratisierten Electronen und freien Wasserstoffatomen. BER. BUNSENGES. PHYSIK. CHEM. 69: 3-7 (1965). Navon, G.; Stein, G., Electron transfer between atomic hydrogen and cobalt(III) complexes in aqueous solution, J. PHYS. CHEM.

69: 1390-4 (1965). Riesz, P., The radiolysis of acetone in air-free aqueous solutions, J. PHYS. CHEM.

69: 1366-73 (1965). Thomas, J.K., The nature of the reducing

species in the radiolysis of acidic aqueous

solutions at high intensities, INTERN. J. APPL. RADIAT. ISOTOPES 16: 451-6 (1965). Baxendale, J.H.; Fielden, E.M.; Keene, J.P., The pulse radiolysis of aqueous solutions of some inorganic compounds, PROC. ROY. SOC.

(LONDON) SER. A 286: 320-36 (1965). Anbar, M.; Meyerstein, D., Effect of ligands on the rate of reduction of cobalt(III) complexes by radiolytically produced hydrogen

atoms, NATURE (LONDON) 206: 818-9 (1965). Haissinsky, M., Radiolyse y de solutions

alcalines et neutres. II. Effet du pH sur les rendements, J. CHIM. PHYS. 62: 1149-54 (1965). Rabani, J.; Mulac, W.A.; Matheson, M.S., The

pulse radiolysis of aqueous tetranitromethane.

I. Rate constants and the extinction

coefficient of e„,”. II. Oxygenated solutions,

J. PHYS. CHEM. 69: 53-70 (1965). Riesz, P.; Morris, T., The radiolysis of aqueous methylammonium ion, RADIAT. RES. 26: 1-11 (1965). Hayon, E.; Moreau, M., Reactivite des atomes H avec quellques composes organiques et mineraux en solutions aqueuses, J. CHIM. PHYS.

62: 391-4 (1965). Kuan-lin, H.; Bugaenko, L.T., The radiolysis

of iron ions in sulphuric acid solutions,

RUSS. J. INORG. CHEM. (ENGLISH TRANSL.) 10: 401-5 (1965). Sawai, T.; Shinozaki, Y.; Meshitsuka, G., Radical yields in the radiolysis of neutral aqueous solutions, ANN. REPT. TOKYO

METROPOLITAN ISOTOPE RES. CENTER (4):

51
43-50 (1965). 65-Q375 Guetlbauer, F.; Getoff, N., Kinetic studies

in the radiochemical carboxylation of methanol, Z. PHYSIK. CHEM. 47(5-6): 299-305

(1965). 65-0382 Sutton, H.C.; Adams, G.E.; Boag, J.W.;

Michael, B.D., Radical yields and kinetics in the pulse radiolysis of potassium bromide

solutions, Pulse Radiolysis, Ebert, M.,

Keene, J.P., Swallow, A.J., Baxendale, J.H.

(eds.). Academic Press, New York, 1965,

p.61-81.

65-0384 Keene, J.P.; Raef, Y.; Swallow, A.J., Pulse

radiolysis studies of carboxyl and related

radicals, Ibid, p.99-106.

65-0385 Baxendale, J.H.; Keene, J.P.; Stott, D.A.,

Determination of some fast reaction rates using the pulsed radiolysis of permanganate

solutions, Ibid, p.107-15.

65-7006 Dainton, F.S.; Fowles, P., The photolysis of aqueous systems at 1849 A. I. Solutions containing nitrous oxide, PROC. ROY. SOC.

(LONDON) SER. A 287: 295-311 (1965).

65-

7019 Halmann, M.; Platzner, I., The photochemistry

of phosphorus compounds. Part III. Photolysis

of ethyl dihydrogen phosphate in aqueous

solution, J. CHEM. SOC.: 5380-5 (1965).

66-

0010 Halpern, J.; Rabani, J., Reactivity of hydrogen atoms toward some cobalt(III) complexes in aqueous solutions, J. AMER. CHEM.

SOC. 88: 699-704 (1966). 66-0114 Sawai, T., Radical yields in the radiolysis of neutral aqueous solutions, BULL. CHEM. SOC.

JAPAN 39(5): 955-60 (1966). 66-0138 Micic, O.; Draganic, I., A study of some

free-radical reactions in aqueous y radiolysis

by direct measurements of Cu+ intermediates during irradiation, J. PHYS. CHEM. 70(7): 2212-19 (1966). 66-0147 Chouraqui, M.; Sutton, J., Origin of primary

hydrogen atom yield in radiolySis of aqueous

solutions, TRANS. FARADAY SOC. 62(8): 2111-20

(1966). 66-0182 Anbar, M.; Meyerstein, D., H/D isotope effects

in the formation of hydrogen from the combination of two radicals in aqueous

solutions, TRANS. FARADAY SOC. 62(524): 2121-31 (1966). 66-0286 Haissinsky, M.; Koulkes, A.-M.; Masri, E., Radiolyse y de solutions de ferro- et ferric-cyanures de potassium. II. Solutions acides degazees. III. Solutions alcalines,

J. CHIM. PHYS. 63: 1129-34 (1966). 66-0334 Koulkes-Pujo, A.-M.; Mantaka, A., Effect des

rayons y de ^Co sur le systeme

Fe^-Fe^-Cu^-O2 en solution aqueuse. Determination des rapports des constantes de

vitesse pour les intermediaires H, H02 et Cu+

, COMPT. REND., SER. C 263(5): 371-4 (1966). 66-0345 Navon, G.; Stein, G., The reactivity of some

high— and low-spin iron(III) complexes with atomic hydrogen in aqueous solution, J. PHYS.

CHEM. 70(11): 3630-40 (1966). 66-0401 Anbar, M.; Meyerstein, D., Unpublished data quoted in 67-0103.

66—0402 Anbar, M.; Neta, P., Unpublished data quoted

in 67-0103.

66-0422

66-0500

66-0559

66-0616

66-0621

66-0810

66-0842

66-0843

66-

9002

67-

0008

67-0041

67-0050

67-0064

67-0094

67-0099

67-0103

67-0115

67-0122

Anbar, M.; Meyerstein, D.; Neta, P., Reactivities of aliphatic compounds toward

bromine and hydrogen atoms in aqueous solution,

J. CHEM. SOC. PT. A: 572-5 (1966). Anbar, M.; Meyerstein, D.; Neta, P., Reactivity

of aromatic compounds towards hydrogen atoms,

NATURE 209: 1348 (1966). Baxendale, J.H.; Stott, D.A., Unpublished

data quoted in 67-0103.

Sutton, J.; Moreau, M., On the origin of the

yield of primary hydrogen atoms in water

radiolysis, Proc. of the Second Tihany

Symposium on Radiation Chemistry, Dobo, J., Hedvig, P. (eds.). Publishing House of the Hungarian Acad, of Sci., Budapest, 1967,

p.95-103.

Draganic, I., Some competition studies in gamma irradiated aqueous solutions at various pH, Ibid, p.129-32.

Rama Rao, K.V.S.; Srinivasan, K.;

Shastri, L.V., Radiolysis of aqueous solutions, Proc. of the Nuclear and Radiation Chemistry

Symposium, Bombay, Jan. 20-2, 1966, p.109-18.

Brown, D.M., Unpublished data quoted in 67-0103.

Anbar, M.; Meyerstein, D.; Neta, P., Unpublished data quoted in 67-0103.

Chutny, B., Contribution to the oxidation mechanism of ferrous ions by hydroxyl radicals

in the presence of organic compounds, COLLECT.

CZECH. CHEM. COMMUN. 31: 358-61 (1966). Farhataziz, Cobalt-60 y radiolysis of solutions

of potassium bromide in 0.8 N sulfuric acid,

J. PHYS. CHEM. 71: 598-602 (1967). Thomas, J.K., Pulse radiolysis of aqueous

solutions of methyl iodide and methyl bromide.

The reactions of iodine atoms and methyl

radicals in water, J. PHYS. CHEM. 71(6): 1919-25 (1967). ^

Anbar, M.; Neta, P., Reactions of halogenoaliphatic acids with free radicals in aqueous solution. Part I. Reactions with hydrogen atoms, J. CHEM. SOC. PT. A: 834-37

(1967). Burchill, C.E.; Dainton, F.S.; Smithies, D., Radical and molecular product yields in x-irradiated alkaline aqueous solutions, TRANS.

FARADAY SOC. 63(4): 932-43 (1967). Seddon, W.A.; Allen, A.O., Radiation chemistry

of aqueous solutions of ethanol, J. PHYS. CHEM.

71: 1914-8 (1967). Anbar, M.; Neta, P., Reaction of fluoride ions with hydrogen atoms in aqueous solution. TRANS.

FARADAY SOC. 63(529): 141-6 (1967). Anbar, M.; Neta, P., A compilation of specific

bimolecular rate constants for the reactions

of hydrated electrons, hydrogen atoms, and

hydroxyl radicals with inorganic and organic

compounds in aqueous solution, INT. J. APPL.

RADIAT. ISOTOP. 18: 493-523 (1967). Anbar, M.; Hart, E.J., The formation of hydrated electrons by the reaction of hydrogen atoms with fluoride ions. J. PHYS.

CHEM. 71(13): 4163-5 (1967). Land, E.J.; Ebert, M., Pulse radiolysis studies

of aqueous phenol. Water elimination from

dihydroxycyclohexadienyl radicals to form

52
phenoxyl, TRANS. FARADAY SOC. 63: 1181-90

(1967). 67-0148 Wilkening, V.G.; Lai, M.; Arends, M.;

Armstrong, D.A., The y-radiolysis of cysteine

in deaerated 1 N HC104 solutions. CAN. J. CHEM.

45: 1209-14 (1967). 67-0180 Sutton, J.; Tran Dinh Son, Vitesses de reaction de trois nitroparaffines avec les atomes

d'hydrogene et les electrons solvates en milieu aqueux, J. CHIM. PHYS. 64(4): 688-90 (1967). 67-0222 Baxendale, J.H.; Rodgers, M.A.J., Hydrogen

yields in the y-radiolysis of 1,4-dioxan and

dioxan + water mixtures, TRANS. FARADAY SOC.

63: 2004-11 (1967). 67-0231 Knight, R.J.; Sutton, H.C., Radiolysis of aqueous solutions of nitric oxide, TRANS.

FARADAY SOC. 63: 2628-39 (1967). 67-0246 Sauer, M.C.Jr.; Ward, B., The reactions of hydrogen atoms with benzene and toluene studied by pulsed radiolysis: Reaction rate constants and transient spectra in the gas phase and

aqueous solution, J. PHYS. CHEM. 71(12): 3971-83 (1967). 67-0251 Cercek, B.; Ebert, M., Pulse radiolysis studies

of the reaction of H and OH radicals and

hydrated electrons with pyridine, TRANS.

FARADAY SOC. 63: 1687-98 (1967). 67-0458 Asmus, K.D.; Cercek, B.; Ebert, M.;

Henglein, A.; Wigger, A., Pulse radiolysis of nitrobenzene solutions, TRANS. FARADAY SOC.

63(10): 2435-41 (1967). 67 0498 Murgulescu, I.G.; Oncescu, T.; Paun, J.; Mihalcea, I., The radiolysis of the complex

oxalates in aqueous solutions. I. Kinetics and

mechanism of the radiolysis of Co-trisoxalato-complex in aqueous solution,

REV. ROUM. CHIM. 12(5): 573-81 (1967).

67-

0550 Baxendale, J.H.; Bevan, P.L.T., Absolute rates

of hydrogen atom reactions in aqueous solution. The Chemistry of Ionization and Excitation,

Johnson, G.R.A. and Scholes, G. (ed.), Taylor

and Francis Ltd, London, 1967, p.253-7.

68-

0052 Basson, R.A.; duPlessis, T.A., The radiolytic oxidation of ethylene in aqueous solution,

RADIAT. RES. 33: 183-93 (1968). 68-0302 Ghosh-Mazumdar, A.S.; Hart, E.J., A pulse

radiolysis study of bivalent and zerovalent

gold in aqueous solutions, ADVAN. CHEM. SER.

81: 193-209,(1968).

68-0305 Amphlett, C.B.; Adams, G.E.; Michael, B.D., Pulse radiolysis studies of deaerated aqueous

salicylate solutions, ADVAN. CHEM. SER. 81: 231-50 (1968). 68-0324 Rabani, J.; Meyerstein, D., Pulse radiolytic studies of the competition H + H and H +

ferricyanide. The absolute rate constants,

J. PHYS. CHEM. 72(5): 1599-1603 (1968). 68-0343 Volkert, W.A.; Kuntz, R.R., The reactions of hydrogen atoms in aqueous solutions. Some

amino acids. J. PHYS. CHEM. 72(10): 3394-3400

(1968). 68-0355 Mantaka, A.; Koulkes-Pujo, A-M., Radiolyse du

melange Fe

2+ -Fe3+ -0 2 -Cu2+ en solution aqueuse

et sulfurique, J. CHIM. PHYS. 65(7-8):

1291-300 (1968). 68-0356 Haissinsky, M., Radiolyse de solutions

68-0359

68-0436

68-0444

68-0502

68-0503

68-0525

68-0540

68-0593

68-0597

68-0643

68-0693

68-3038

68-7194

69-0001

69-0022

69-0051

69-0083

aqueuses du tellure par les rayons y. III. Solutions acides, J. CHIM. PHYS. 65(7-8):

1386-92 (1968). Loman, H.; Blok, J., On the radiation chemistry

of thymine in aqueous solution, RADIAT. RES.

36: 1-13 (1968). Bevan, P.L.T., Radiolysis studies in aqueous

solution, Ph.D., Thesis, Univ. of Manchester,

Sept., 1968, 172p.

Baxendale, J.H.; Dixon, R.S.; Stott, D.A.,

Reactivity of hydrogen atoms with Fe 3*, FeOH2+ and Cu2+ in aqueous solutions, TRANS. FARADAY

SOC. 64(549): 2398-2401 (1968).

Fiti, M.; Sutton, J., Vitesses des reactions de l'acetylene avec les especes radicalaires produites dans l'eau irradiee, Unpublished

data. Draganic, I.; Markovic, V., Unpublished data. Hentz, R.R.; Farhataziz, Milner, D.J., y Radiolysis of liquids at high pressures. VI. Hydrogen-atom reactions in aqueous 0.8 N H2 S04 solutions, J. CHEM. PHYS. 49(5): 2153-7 (1968). Al-Thannon, A. A-M., Kinetics of the gamma

radiolytic decomposition of aqueous cysteine

solutions, Ph.D, Thesis, Univ. of Delaware,

Newark, 1968, 147p.

Ogura, H., Radiolysis of hydrogen cyanide in an aqueous system. Part II. Effects of additives and reaction mechanism, BULL. CHEM.

SOC. JAPAN 41(12): 2871-6 (1968). Theard, L.P.; Peterson, F.C., Pulse radiolysis

study of protection of pyrimidine base components of nucleic acid by aminothiols in aqueous solution, GA-8872, lllp., Sept. 1968.

(Gulf General Atomic, San Diego, Calif.) Pleticha-Lansky, R., Oscillo-polarographic

studies of the effects of y-radiation on

adenine in aqueous solution, INT. J. RADIAT.

BIOL. 14(4): 331-39 (1968). Czapski, G.; Peled, E., On the pH-dependence

of GredndB< in the radiation chemistry of aqueous solutions, ISRAEL J. CHEM. 6: 421-36 (1968). Scholes, G.; Simic, M., Radiolysis of aqueous

solutions of DNA and related substances:

reaction of hydrogen atoms, BIOCHIM. BIOPHYS.

ACTA 166: 255-8 (1968). Czapski, G.; Ottolenghi, M., Scavenging

kinetics in the photochemistry of some ions in aqueous solution, ISRAEL J. CHEM. 6(2): 75-83 (1968). Neta, P.; Dorfman, L.M., Pulse radiolysis studies. XIV. Rate constants for the reactions

of hydrogen atoms with aromatic compounds in aqueous solution, J. PHYS. CHEM. 73(2): 413-17 (1969). Lai, M.; Armstrong, D.A.; Wieser, M., The

cobalt-60 gamma-radiolysis of reduced

glutathione in deaerated aqueous solutions,

RADIAT. RES. 37: 246-52 (1969). Moreau, M.; Sutton, J., Influence of pH on

yield of hydrogen atoms in radiolysis of aqueous solutions, TRANS. FARADAY SOC.

65(554): 380-9 (1969). Pagsberg, P.; Christensen, H.; Rabani, J.; Nilsson, G.; Fenger, J.; Nielsen, S.O.,

53
Far- ultraviolet spectra of hydrogen and

hydroxyl radicals from pulse radiolysis of aqueous solutions. Direct measurement of 70-0211

the rate of H + H, J. PHYS. CHEM. 73(4): 1029-38 (1969). 69-0275 Faraggi, M.; Desalos, J., Effect of positively

charged ions on the "molecular" hydrogen yield

in the radiolysis of aqueous solutions, INT. J. RADIAT. PHYS. CHEM. 1: 335-44 (1969). 70-0213

69-0338 Hentz, R.R.; Johnson, C.G.Jr., y Radiolysis of liquids at high pressures. VII. Oxidation of iodide ion by hydrogen atoms in aqueous

solutions, J. CHEM. PHYS. 51(3): 1236-41

(1969). 69-0434 Jayson, G.G.; Keene, J.P.; Stirling, D.A.; Swallow, A.J., Pulse-radiolysis study of some 70-0240

unstable complexes of iron, TRANS. FARADAY SOC.

65(561): 2453-64 (1969). 69-0445 Chrysochoos, J., Pulse-radiolysis studies of p-hydroxyphenylpropionic acid, J. PHYS. CHEM. 70-0468

73(12): 4188-93 (1969). 69-0459 Armstrong, R.C.; Swallow, A.J., Pulse- and

gamma-radiolysis of aqueous solutions of 70-0533

tryptophan, RADIAT. RES. 40(3): 563-79 (1969). 69-0500 Vacek, K.; von Sonntag, C., H-D isotope effect

in the reaction of hydrogen radicals with

isopropyl alcohol in 6M-H2 S0 4 in the liquid and

in the glassy state, CHEM. COMMUN. 1256-7 70-0534

(1969). 69-0503 Adsetts, J.R.; Gold, V., Kinetics of hydrogen

isotope exchange reactions. Part XVI. Aromatic

exchange under the influence of /3-radiation on aqueous solutions of mesitylene, J. CHEM. SOC. 70-0567 PT. B (9): 1108-14 (1969). 69-0571 Greenstock, C.L.; Hunt, J.W.; Ng, M., Pulse

radiolysis studies of uracil and its 70-0657

derivatives. Primary species attack, TRANS.

FARADAY SOC. 65: 3279-87 (1969). 69-0598 Belloni, J.; Haissinsky, M., Radiolyse y de

solutions aqueuses d'hydrazine, INT. J. 70-0859

RADIAT. PHYS. CHEM. 1: 519-27 (1969). 69—0646 Micic, O.; Draganic, I., Some reactions of hydrated electron in acid medium (pH 0. 6-4.0), 70-1056

INT. J. RADIAT. PHYS. CHEM. 1(3): 287-95

(1969).

69-

0649 Moreau, M.; Schmidt, M.; Sutton, J., The 70-1059

radiolysis of aqueous solutions of Fremy's

salt: Rate constants for the reactions with

solvated electrons and hydrogen atoms, INT.

J. RADIAT. PHYS. CHEM. 1(4): 433-40 (1969).

70-

0052 Chambers, K.W.; Collinson, E.; Dainton, F.S., 70-3023

Addition of e H- and OH to acrylamide in aqueous solution and reactions of the adducts,

TRANS. FARADAY SOC. 66: 142-62 (1970). 70-7235

70-0063 Feng, P.Y.; Brynjolfsson, A.; Halliday, J.W.;

Jarrett, R.D., High-intensity radiolysis of aqueous ferrous sulfate-cupric sulfate-sulfuric

acid solutions, J. PHYS. CHEM. 74(6): 1221-7 71—0003

(1970). 70-0094 Rama Rao, K.V.S.; Shastri, L.V.; Shankar, J., Radiation chemistry of tris(acetylacetonato)

cobalt(III) in aqueous solutions, RADIAT. EFF.

2(3): 193-200 (1970). 71-0007

70—0169 Matthews, R.W.; Mahlman, H.A.; Sworski, T.J., Kinetics of the oxidation of cerium(III) by

peroxysulfuric acids induced by cobalt-60

y radiation, J. PHYS. CHEM. 74(12): 2475-9

(1970). Michael, B.D.; Hart, E.J., The rate constants

of hydrated electron, hydrogen atom, and

hydroxyl radical reactions with benzene,

I, 3-cyclohexadiene, 1,4-cyclohexadiene, and

cyclohexene, J. PHYS. CHEM. 74(15): 2878-84

(1970). Neilsen, S.O.; Pagsberg, P.; Hojberg, K.S.; Christensen, H.C.; Nilsson, G., Direct spectrophotometric determination of the rate

of H + OH in aqueous solution, Internat. Meeting on Primary Radiation Effects in Chemistry and Biology, Buenos Aires, Argentina,

March 9-14, 1970, Abstr. No. A-2.

Badiello, R.; Fielden, E.M., Pulse radiolysis

of selenium-containing radioprotectors: I. Selenourea, INT. J. RADIAT. BIOL. 17(1): 1-14 (1970). Sawai, T.; Hamill, W.H., Evidence for very

early effects in the radiolysis of water,

J. PHYS. CHEM. 74(22): 3914-24 (1970). Tsuda, S.; Kikuti, Y., Studies in the

radiolysis of ferrous sulfate solutions. I. Effect of oxygen concentration of 0.8 N

sulfuric acid, DOITAI TO HOSHASEN 4(3): 206-13 (1970). Tsuda, S.; Kikuti, Y., Studies in the

radiolysis of ferrous sulfate solutions. 2. Effect of oxygen concentration in 0.05 N

sulfuric acid, DOITAI TO HOSHASEN 4(3): 214-20 (1970). Greenstock, C.L., Radiation chemistry of orotic acid as studied by pulse radiolysis, TRANS.

FARADAY SOC. 66: 2541-50 (1970). Chutny, B.; Swallow, A.J., Aromatic anions and

free radicals in the pulse radiolysis of aqueous solutions of benzonitrile, TRANS

FARADAY SOC. 66: 2847-54 (1970). Hickel, B., Radiolysis of concentrated nitrate and formate solutions, CEA-R-4046, Aug., 1970,

64p. (Saclay, France).

Christie Hospital and Holt Radium Inst., Paterson Laboratories Annual Report, 1970,

188p. (Manchester, England).

Nichiporov, F.G.; Byakov, V.M., Reactivity of Ce 4* ions in irradiated aqueous solutions of sulfuric acid, HIGH ENERGY CHEM. 4(6): 496-7

(1970) (translated from KHIM. VYS. ENERG. 4(6): 546-7 (1970)). Ogura, H.; Murata, M.; Kondo, M., Radiolysis

of ascorbic acid in aqueous solution, RADIOISOTOPES (TOKYO) 19: 89-91 (1970). Getoff, N.; Lehmann, H.P., Reactions of methanol and carbon monoxide in water

photolysis at 184.9 nm, INT. J. RADIAT. PHYS.

CHEM. 2(2): 91-6 (1970). Neta, P.; Fessenden, R.W.; Schuler, R.H., An

electron spin resonance study of the rate constants for reaction of hydrogen atoms with organic compounds in aqueous solution, J. PHYS.

CHEM. 75(11): 1654-66 (1971). Peled, E.; Mirski, U.; Czapski, G., On the contribution of H atoms to GHl in the

radiation chemistry of aqueous solutions, J. PHYS. CHEM. 75(1): 31-5 (1971).

54
71-0017 Neta, P.; Holdren, G.R.; Schuler, R.H., On the

rate constants for reaction of hydrogen atoms

in aqueous solutions, J. PHYS. CHEM. 75(4): 449-54 (1971). 71-0026 Balkas, T.I.; Fendler, J.H.; Schuler, R.H.,

The radiation chemistry of aqueous solutions of CFC13 , CFjClj, and CF3 CI, J. PHYS. CHEM. 75(4): 455-66 (1971). 71-0038 Draganic, I.G.; Draganic, Z.D.; Holroyd, R.A., Pulse radiolysis of aqueous cyanogen solution,

J. PHYS. CHEM. 75(5): 608-12 (1971). 71-0040 Neta, P.; Schuler, R.H., Rate constants for reaction of hydrogen atoms with compounds of biochemical interest, RADIAT. RES. 47: 612-27

(1971). 71-0055 Phillips, G.O.; Filby, W.G.; Moore, J.S.; Davies, J.V., Radiation studies of aryl

glycosides. Part II. Mechanism of radiolysis

of phenyl j8-d-glucopyranoside in aqueous

solution, CARBOHYDRATE RES. 16(1): 89-103 (1971). 71-0143 Feitelson, J.; Hayon, E., Unpublished data. 71-0175 Jayson, G.G.; Stirling, D.A.; Swallow, A.J., Pulse- and X-radiolysis of 2-mercaptoethanol

in aqueous solution, INT. J. RADIAT. BIOL.

19(2): 143-56 (1971). 71-0268 Frunze, T.A.; Kabakchi, S.A.; Shubin, V.N.;

Dolin, P.I., Radiolysis in a periodic source

field, HICH ENERGY CHEM. 5(1): 73 (1971) (translated from KHIM. VYS. ENERG. 5(1): 85 (1971)). 71-0282 Cohen, H.; Meyerstein, D., Oxidation of benzoatopentaamminecobalt(III) by hydroxyl

radicals, J. AMER. CHEM. SOC. 93(17): 4179-83 (1971). 71-0295 Chrysochoos, J.; Shihabi, D.S., X-radiolysis

of aqueous erythrosin, RADIAT. RES. 47: 392-401

(1971). 71-0303 Smaller, B.; Avery, E.C.; Remko, J.R., EPR

pulse radiolysis studies of the hydrogen atom

in aqueous solution. I. Reactivity of the hydrogen atom, J. CHEM. PHYS. 55(5): 2414-8

(1971). 71-0354 Chrysochoos, J.; Shihabi, D.S., Reactivity of hydrogen atoms and hydrated electrons toward aqueous erythrosin. X-radiolysis, J. PHYS.

CHEM. 75(19): 3020-2 (1971). 71-0529 Theard, L.M.; Peterson, F.C.; Myers, L.S.Jr., Nanosecond pulse radiolysis studies of aqueous

thymine solutions, J. PHYS. CHEM. 75(25): 3815-21 (1971). 71-0582 Simic, M.; Ebert, M., Pulse radiolysis of aqueous solutions of carboxy, carbamido and

pyridyl derivatives of pyridine, INT. J. RADIAT. PHYS. CHEM. 3: 259-72 (1971). 71-0586 Bansal, K.M.; Patterson, L.K.; Fendler, E.J.; Fendler, J.H., Reactions of hydrated electrons, hydrogen atoms and hydroxyl radicals in micellar systems, INT. J. RADIAT. PHYS. CHEM.

3(3): 321-31 (1971). 71-0595 Getoff, N.; Schwoerer, F., Pulsradiolyse von Methylamin in waesseriger Loesung, INT. J. RADIAT. PHYS. CHEM. 3(3): 429-39 (1971). 71-0618 Willson, R.L., Pulse radiolysis studies on

reaction of triacetoneamine-N-oxyl with radiation-induced free radicals, TRANS.

FARADAY SOC. 67(10): 3008-19 (1971).

71-0619 Willson, R.L., Pulse radiolysis studies of electron transfer in aqueous quinone solutions, TRANS. FARADAY SOC. 67(10): 3020-9 (1971). 71-0710 Schoeneshoefer, M., Pulse radiolysis of the tropylium ion, tropylcarbinol and tropilidene

in aqueous solution, Z. NATURFORSCH. PT. B

26(11): 1120-4 (1971). 71-0778 Koester, R.; Asmus, K.D.; Die Reduktion von

Tetrachlorkohlenstoff durch hydratisierte

Elektronen, H-Atome und reduzierende Radikale,

Z. NATURFORSCH. PT. B 26(11): 1104-8 (1971). 71-0925 Sehested, K.; Markovic, V., Radiolysis of aqueous solutions of some simple compounds

containing aldehyde groups. Part II. Glyoxylic acid, Proc. of the Third Tihany

Symposium on Radiation Chemistry, Vol. 2,

J. Dobn and P. Hedvig (eds.), Akademiai

Kiado, Budapest, Hungary, 1971, p. 1225-67. 71-0930 Nilsson, K.; Fagsberg, P., The reduction of ferricytochrome C to ferrocytochrome C

studied by pulse radiolysis, Ibid. p. 131 1—7. 71-3087 Lichtin, N.N.; Ogdan, J.; Stein, G., Fast consecutive intramolecular processes involving

protein and Fe(III) in ferri-cytochrome-c in aqueous solution, ISRAEL J. CHEM. 9(5): 579-82 (1971). 71-9218 Shagisultanova, G.A.; Tikhonov, A.S.; Karaban, A. A., Determination of the reaction

rate constants for hydrogen atoms with some

complex compounds of Co(III), Fe(III), and

Cr(III), HIGH ENERGY CHEM. 5(2): 173-4 (1971) (translated from KHIM. VYS. ENERG. 5(2): 189-90

(1970)).

5(2): 173-4 (1971).

71-

9384 Kongshaug, M.; Steen, H.B., New method for the study of reactions of H atoms in aqueous

solutions, NATURE PHYS. SCI. 234(45): 37-8

(1971).

72-

0013 Boyd, A.W.; Willis, C.; Lalor, G.C., Isotope

effects and hydrogen yields in the radiolysis

of HjO—

D

2 0 mixtures at very high dose rates, CAN. J. CHEM. 50(1): 83-92 (1972). 72-0025 Neta, P.; Schuler, R.H., Rate constants for reaction of hydrogen atoms with aromatic and

heterocyclic compounds. The electrophilic nature of hydrogen atoms, J. AMER. CHEM. SOC.

94(4): 1056-9 (1972). 72-0039 Neta, P.; Schuler, R.H., The effect of ionic dissociation of organic compounds on their rate of reaction with hydrogen atoms, J. PHYS.

CHEM. 76(19): 2673-9 (1972). 72-0049 Patterson, L.K.; Bansal, K.M., Pulse radiolysis studies of 5-halouracils in aqueous solutions,

J. PHYS. CHEM. 76(17): 2392-9 (1972). 72-0066 Faraggi, M.; Feder, A., Pulse radiolysis studies in lanthanide aqueous solutions.

II. Formation, spectrum, and some chemical

properties of praseodymium (IV) in aqueous

solution. J. CHEM. PHYS. 56(7): 3294-7 (1972). 72-0144 Hayon, E.; Simic, M., Radiation sensitization reactions of N-ethylmaleimide with model

compounds, RADIAT. RES. 50(3): 464-78 (1972). 72-0171 Hayon, E.; Ibata, T.; Lichtin, N.N.; Simic, M.,

Electron and hydrogen atom attachment to aromatic carbonyl compounds in aqueous

solution. Absorption spectra and dissociation

55
constants of ketyl radicals, J. PHYS. CHEM.

76(15): 2072-8 (1972). 72-0264 Draganic, Z.D.; Draganic, I.G., Studies on the formation of primary hydrogen atom yield (G H) in the y radiolysis of water, J. PHYS. CHEM.

76(19): 2733-7 (1972). 72-0266 Schoeneshoefer, M., Pulsradiolytische

Untersuchung zur Oxidation der Ascorbinsaeure

durch OH-Radikale und Halogen-Radikal-Komplexe

in waessriger Loesung, Z. NATURFORSCH. PT. B

27(6): 649-59 (1972). 72-0289 Christensen, H., Pulse radiolysis of aqueous

solutions of aniline and substituted anilines, INT. J. RADIAT. PHYS. CHEM. 4(3): 311-33

(1972). 72-029U Faraggi, M.; Amozig, A., Pulse radiolysis of metallic ions in aqueous solutions. I. Pulse

radiolysis in Hg2+ and Hg2 2+ ions aqueous

solutions, INT. J. RADIAT. PHYS. CHEM. 4(3): 353-8 (1972). 72-0359 Nelson, D.A.; Hayon, E., Ketyl radicals of benzoylpyridines. J. PHYS. CHEM. 76(22): 3200-7 (1972). 72-0380 Shafferman, A., The free-radical cleavage of the disulfide bond (studied by pulse

radiolysis), ISRAEL J. CHEM. 10(3): 725-33

(1972). 72-0381 Baxendale, J.H.; Fiti, M., Transient species

in the reactions of some pyridyl complex ions with hydrated electrons, J. CHEM. SOC. DALTON

TRANS. (18): 1995-8 (1972). 72-0462 Martin, J.E.; Hart, E.J.; Adamson, A.W.;

Gafney, H.; Halpern, J., Chemiluminescence from

the reaction of the hydrated electron with

tris(bipyridyl)ruthenium(III), J. AM. CHEM.

SOC. 94(26): 9238-40 (1972). 72-0541 Shetiya, R.S.; Rao, K.N.; Shankar, J., Determination of rate constants for the

reactions of H, OH and e iq ~ with indole-3-acetic

acid and other plant hormones, RADIAT. EFF.

14(3-4): 185-9 (1972). 72-1002 Nilsson, K., The reduction of ferricytochrome

C studied by pulse radiolysis. ISRAEL J. CHEM.

10(6): 1011-9 (1972). 72-1004 Lichtin, N., Consecutive radical reactions and

the role of protein in the pulse radiolysis of enzymes. ISRAEL J. CHEM. 10(6): 1041-58 (1972). 72-3094 Lichtin, N.; Ogdan, J.; Stein, G., Fast consecutive radical processes within the ribonuclease molecule in aqueous solution.

I. Reaction with H atoms. BIOCHIM. BIOPHYS.

ACTA 263: 14-30 (1972). 73-0003 Feitelson, J.; Hayon, E., Electron ejection and

electron capture by phenolic compounds, J. PHYS.

CHEM. 77(1): 10-5 (1973). 73-0030 Anbar, M.; Bambenek, M.; Ross, A.B., Selected

specific rates of reactions of transients from

water in aqueous solution. I. Hydrated

electron, NSRDS-NBS—43, 1973, 54p.

73-0043 Nazhat, N.B.; Asmus, K.-D., Reduction of mercuric chloride by hydrated electrons and reducing radicals in aqueous solutions. Formation and reactions of HgCl, J. PHYS.

CHEM. 77(5): 614-20 (1973). 73-0053 Witter, R.A.; Neta, P., On mode of reaction

of hydrogen atoms with organic compounds in aqueous solutions, J. ORG. CHEM. 38: 484-7

(1973). 73-0097 Hayon, E.; Simic, M., Acid-base properties of

radical anions of cis and trans isomers.

I. Fumarates and maleates, J. AMER. CHEM. SOC.

95(8): 2433-9 (1973). 73-0121 Robinson, E.A.; Schulte-Frohlinde, D., Pulse

radiolysis of 1,4-dicyanobenzene in aqueous

solutions in the presence and absence of T1(I) ions. J. CHEM. SOC. FARADAY TRANS. I 69(4): 707-18 (1973). 73-0241 Tung, T.-L.; Kuntz, R.R., The reactions of hydrogen atoms in aqueous solutions: Thiols. RADIAT. RES. 55: 10-7 (1973). 73-1015 Roebke, W.; Schoeneshoefer, M.; Henglein, A., Die y-Radiolyse und Pulsradiolyse des

Schwefelkohlenstoffs in waessriger Loesung.

Z. NATURFORSCH. PT. B 28(1-2): 12-22 (1973). 73-1018 Greenstock, C.L.; Dunlop, I., Pulse

radiolysis studies of nitrofurans. Radiation chemistry of nifuroxime.

J. PHYS. CHEM. 77(15): 1834-8 (1973). 73-1049 Grabner, G.; Getoff, N.; Schwoerer, F., Pulsradiolyse von H3 P04 , H2 P04 , HPO2- und

P2O7

- in waessriger Loesung. I. Geschwindigkeitskonstanten der Reaktionen

mit den Primaerprodukten der Wasserradiolyse, INT. J. RADIAT. PHYS. CHEM. 5: 393-403 (1973). 73-1053 Farhataziz; Mihalcea, I.; Sharp, L.J.; Hentz, R.R., Pulse radiolysis of liquids at high pressures. IV. Hydrogen-atom reactions in aqueous 0.1M HC104 solutions, J. CHEM. PHYS.

59(5): 2309-15 (1973).

56
FORM NBS-114A d-71)

2. Gov’t Accession No.

U.S. DEPT. OF COMM.

BIBLIOGRAPHIC DATA

SHEET

1. PUBLICATION OR REPORT NO.

NSRDS-NBS 51

3. Recipient’s Accession No.

4. TITLE AND SUBTITLE

Selected Specific Rates of Reactions of Transients from Water

in Aqueous Solution. II. Hydrogen Atom.

5. Publication Date May 1975

6. Performing Organization Code

7. AUTHOR(S)

Michael Anbar, Farhatazi z, Alberta B. Ross

8. Performing Organization

10. Project/Task/Work Unit No. 9. PERFORMING ORGANIZATION NAME AND ADDRESS

NATIONAL BUREAU OF STANDARDS

DEPARTMENT OF COMMERCE

WASHINGTON, D.C. 20234

11. Contract/Grant No.

12. Sponsoring Organization Name and Address

Same as No. 9.

13. Type of Report & Period

Covered

NA

14. Sponsoring Agency Code

15.

SUPPLEMENTARY NOTES

Library of Congress Catalog Card Number: 73-600329

16.

ABSTRACT (A 200-word or less factual summary of most significant information. If document includes a significant

bibliography or literature survey, mention it here.)

Rates of reactions of hydrogen atoms (from radiolysis of water and other sources)

with organic and inorganic molecules, ions, and transients in aqueous solution

have been tabulated. Directly measured rates obtained by kinetic spectroscopy

or conductimetric methods, and relative rates determined by competition kinetics

are included.

17.

KEY WORDS (Alphabetical order, separated by semicolons)

Aqueous solution; chemical kinetics; data compilation; hydrogen atom; radiation

chemistry: rates.

19. SECURITY CLASS

(THIS REPORT)

21. NO. OF PAGES

56

UNCL ASSIFIED

20. SECURITY CLASS

(THIS PAGE)

22. Price

UNCLASSIFIED $1.20

18. AVAILABILITY STATEMENT

fXl UNLIMITED.

I I FOR OFFICE AL DISTRIBUTION. DO NOT RELEASE

TO NTIS.

USCOMM-DC 66244-P71

*U.S. GOVERNMENT PRINTING OFFICE: 1975-582-653/130

NBS TECHNICAL PUBLICATIONS

PERIODICALS JOURNAL OF RESEARCH reports National Bureau

of Standards research and development in physics,

mathematics, and chemistry. It is published in two sections, available separately:

• Physics and Chemistry (Section A)

Papers of interest primarily to scientists working in these fields. This section covers a broad range of physical and chemical research, with major emphasis on

standards of physical measurement, fundamental constants, and. properties of matter. Issued six times a

year. Annual subscription: Domestic, $17.00; Foreign,

$21.25. • Mathematical Sciences (Section B)

Studies and compilations designed mainly for the mathematician and theoretical physicist. Topics in mathematical statistics, theory of experiment design, numerical analysis, theoretical physics and chemistry, logical

design and programming of computers and computer

systems. Short numerical tables. Issued quarterly. Annual subscription: Domestic. $9.00; Foreign, $11.25.

DIMENSIONS/NBS (formerly Technical News Bulletin) —This monthly magazine is published to inform

scientists, engineers, businessmen, industry, teachers,

students, and consumers of the latest advances in science and technology, with primary emphasis on the work at NBS. The magazine highlights and reviews such

issues as energy research, fire protection, building tech- nology, metric conversion, pollution abatement, health and safety, and consumer product performance. In addition, it reports the results of Bureau programs in measurement standards and techniques, properties of matter and materials, engineering standards and services, instrumentation, and automatic data processing.

Annual subscription: Domestic, $9.45; Foreign, $11.85.

NONPERIODICALS Monographs—Major contributions to the technical liter- ature on various subjects related to the Bureau’s scientific and technical activities. Handbooks—Recommended codes of engineering and

industrial practice (including safety codes) developed

in cooperation with interested industries, professional

organizations, and regulatory bodies. Special Publications—Include proceedings of confer- ences sponsored by NBS, NBS annual reports, and other

special publications appropriate to this grouping such

as wall charts, pocket cards, and bibliographies.

Applied Mathematics Series—Mathematical tables, manuals, and studies of special interest to physicists,

engineers, chemists, biologists, mathematicians, computer programmers, and others engaged in scientific and technical work.

National Standard Reference Data Series—Provides

quantitative data on the physical and chemical properties of materials, compiled from the world’s literature and critically evaluated. Developed under a world-wide

program coordinated by NBS. Program under authority

of National Standard Data Act (Public Law 90-396).

NOTE: At present the principal publication outlet for these data is the Journal of Physical and Chemical

Reference Data (JPCRD) published quarterly for NBS

by the American Chemical Society (ACS) and the American Institute of Physics (AIP). Subscriptions, reprints,

and supplements available from ACS, 1155 Sixteenth

St. N. W., Wash. D. C. 20056. Building Science Series—Disseminates technical infor- mation developed at the Bureau on building materials,

components, systems, and whole structures. The series presents research results, test methods, and performance criteria related to the structural and environmental functions and the durability and safety characteristics of building elements and systems.

Technical Notes—Studies or reports which are complete

in themselves but restrictive in their treatment of a

subject. Analogous to monographs but not so comprehensive in scope or definitive in treatment of the subject area. Often serve as a vehicle for final reports of work performed at NBS under the sponsorship of other government agencies.

Voluntary Product Standards—Developed under pro- cedures published by the Department of Commerce in Part 10, Title 15, of the Code of Federal Regulations.

The purpose of the standards is to establish nationally

recognized requirements for products, and to provide

all concerned interests with a basis for common under- standing of the characteristics of the products. NBS

administers this program as a supplement to the activities of the private sector standardizing organizations. Federal Information Processing Standards Publications (FIPS PUBS)—Publications in this series collectively constitute the Federal Information Processing Standards Register. Register serves as the official source of information in the Federal Government regarding stand- ards issued by NBS pursuant to the Federal Property

and Administrative Services Act of 1949 as amended,

Public Law 89-306 (79 Stat. 1127), and as implemented

by Executive Order 11717 (38 FR 12315, dated May 11, 1973) and Part 6 of Title 15 CFR (Code of Federal

Regulations).

Consumer Information Series—Practical information, based on NBS research and experience, covering areas

of interest to the consumer. Easily understandable language and illustrations provide useful background

knowledge for shopping in today’s technological

marketplace.

NBS Interagency Reports (NBSIR)—A special series of interim or final reports on work performed by NBS for outside sponsors (both government and non-government). In general, initial distribution is handled by the sponsor; public distribution is by the National Technical Information Service (Springfield, Va. 22161) in paper copy or microfiche form.

Order NBS publications (except NBSIR’s and Biblio- graphic Subscription Services) from: Superintendent of Documents, Government Printing Office, Washington,

D.C. 20402. BIBLIOGRAPHIC SUBSCRIPTION SERVICES

The following current-awareness and literature-survey

bibliographies are issued periodically by the Bureau:

Cryogenic Data Center Current Awareness Service A literature survey issued biweekly. Annual subscription: Domestic, $20.00; foreign, $25.00.

Liquefied Natural Gas. A literature survey issued quarterly. Annual subscription : $20.00.

Superconducting Devices and Materials. A literature

survey issued quarterly. Annual subscription: $20.00.

Send subscription orders and remittances for the pre- ceding bibliographic services to National Technical Information Service, Springfield, Va. 22161. Electromagnetic Metrology Current Awareness Service Issued monthly. Annual subscription: $100.00 (Special rates for multi-subscriptions). Send subscription order and remittance to Electromagnetics Division,

National Bureau of Standards, Boulder, Colo. 80302.
U.S. DEPARTMENT OF COMMERCE

National Bureau of Standards

Washington. D.C. 20234