A111D3 DbbbbS

NBS SPECIAL PUBLICATION 513

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

National Bureau of Standards

library, E-01 Admin. BIdg.

OCT 1 1981

1310B7

/

Reaction Rate and

Photochemical Data for

Atmospheric Chemistry - 1977

Reaction Rate and Photochemical Data for

K

Atmospheric Chemistry - 1977 , ,

11

'

Edited by

Robert F. Hampson, Jr. and David Garvin

National Measurement Laboratory

National Bureau of Standards

Washington, D.C. 20234

Sponsored by the Department of Transportation

National Aeronautics & Space Administration

Office of Standard Reference Data, NBS

Office of Environmental Measurements, NBS

U.S. DEPARTMENT OF COMMERCE, Juanita M. Kreps, Secretary

Dr. Sidney Harman, Under Secretary

Jordan J. Baruch, Assistant Secretary for Science and Technology

^ NATIONAL BUREAU OF STANDARDS, Ernest Ambler, Director

Issued May 1978
Library of Congress Cataloging in Publication Data Main entry under title: Reaction rate and photochemical data for atmospheric

chemistry, 1977. (National Bureau of Standards special publication ; 513) Supt. of Docs, no,: CI3. 10:513

1. Atmospheric chemistry--Tables. 2. Chemical reaction, Rate of—Tables, etc. 3. Photochemistry—Tables. I. Hampson,

Robert F. II. Garvin, David, 1923- III. United States. Dept.

of Transportation IV. United States. National Bureau of Standards. V. Series: United States. National Bureau of Standards.

Special publication ; 513. QC100.U57 no. 513 [QC879.6] 602Ms [551.5'11] 78-606033

National Bureau of Standards Special Publication 513

Nat. Bur. Stand. (U.S.) Spec. Publ. 513, 111 pages (May 1978) CODEN: XNBSAV

U.S. GOVERNMENT PRINTING OFFICE

WASHINGTON: 1978

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

Stock No. 003-003-01924-1 Price $2.75

(Add 25 percent additional for other than U.S. mailing).
FOREWORD

The National Standard Reference Data System was established in

1963 for the purpose of promoting the critical evaluation and dissemination of numerical data of the physical sciences. The program

is coordinated by the Office of Standard Reference Data of the National

Bureau of Standards, but Involves the efforts of many groups in universities, government laboratories, and private industry. The primary

aim of the program is to provide compilations of critically evaluated

numerical data. These tables are published in the Journal of Physical

and Chemical Reference Data , The NSRDS-NBS Publication Series of the

National Bureau of Standards, and through other appropriate channels.

The present report consists of tables of data assembled for use

in modelling the chemistry of the stratosphere. It represents contributions from the Chemical Kinetics Information Center, other NSRDS

data centers, and a number of individual experts. Support for the

preparation of those tables has been provided by the Department of

Transportation under the High Altitude Pollution Program, by the

National Aeronautics and Space Administration under the Upper

Atmosphere Research Program, and by the Office of Standard Reference

Data, N.B.S. and the Office of Environmental Measurements, N.B.S.

David R. Lide, Jr.

Chief, Office of Standard

Reference Data
TABLE OF CONTENTS

Abstract 1

1. Introduction 1

„ Guide to the Table 3

3. Reaction Index 9

4. Table. Data for chemical reactions and photochemistry

of neutral species 16

5. Reference List 67

Appendices ;

1. Chemical Thermodynamic Properties of Selected

Molecular Species 90

2. Conversion Tables 104

iv
Reaction Rate and Photochemical Data for Atmospheric Chemistry - 1977

R. F. Hampson, D. Garvin, Editors

A table of data for gas phase chemical reactions

and photochemistry of neutral species is presented.

Specifically, it gives preferred values for

reaction rate constants, photoabsorption cross

sections, and quantum yields of primary photochemical

processes and also cites recent experimental work

(to December 1977) . It is intended to provide the

basic physical chemical data needed as input data

for calculations modelling atmospheric chemistry.

An auxiliary table of thermochemical data for the

pertinent chemical species is given in the appendix.

Key words: Air pollution; atmospheric chemistry; chemical kinetics;

data evaluation; gas phase; photoabsorption cross section; photochemistry;

quantum yield; rate constant.

1. Introduction

This technical note consists of a table of data on the kinetics

of chemical reactions and the photochemistry of neutral species. It

is designed for use in modelling the chemistry of the stratosphere

and, to a more limited extent, the polluted troposphere and also the

interpretation of laboratory experiments. The table of rate and

photochemical data is supplemented by a table of thermochemical

data for the species involved.

This work was supported by the High Altitude Pollution Program of the

Federal Aviation Administration, U. S. Department of Transportation, by

the Upper Atmospheric Research Program of the National Aeronautics and

Space Administration, and by the Office of Standard Reference Data, N.B.S.

and the Office of Environmental Measurements, N.B.S.

1
Earlier versions of this table have been issued as D. Garvin (editor)

"Chemical Kinetics Data Survey IV" NBSIR 73-203 (1973); D. Garvin and

R. F. Hampson (editors) "Chemical Kinetics Data Survey VII" NBSIR 74-430

(1974) ; and R. F. Hampson and D. Garvin (editors) "Chemical Kinetic and

Photochemical Data for Modelling Atmospheric Chemistry" NBS Technical

Note 866 (1975) . The table appearing in NBS Technical Note 866 was also

published in the U. S. Department of Transportation's Climatic Impact

Assessment Program Monograph 1 "The Natural Stratosphere of 1974"

E. Reiter, editor (1975). The present table supersedes all earlier

versions .

Since the publication of NBS Technical Note 866 in 1975, a major

effort in the evaluation of rate and photochemical data was undertaken

for the NASA chlorof luoromethane assessment by its Laboratory

Measurements Committee of which the present editors were members. The

recommendations of this committee covering 104 chemical reactions and

48 photochemical processes are given in NASA Reference Publication 1010

"Chlorof luoromethanes and the Stratosphere" R. D. Hudson, editor,

August 1977. These recommendations have been accepted by the editors

of this table and are given here as preferred values. These

recommendations are indicated either by the entry [ t*NASA(1977) eval] or by the symbols [t*] immediately preceding the author's name in the

reference column. The first notation is used to indicate that the

committee has synthesized a preferred value from a consideration of

all data sets. The latter designation is used when the committee has

accepted the results of a particular study or of an existing evaluation.

Recommended values also are given for reactions not considered

by the NASA Laboratory Measurements Committee. Some of these are drawn from other modern rate data evaluations, and the sources are indicated in the table. Other recommendations have been prepared

for this work.

Rate data evaluation is a small but growing branch of physical

chemistry. There are more recommended rate constants than contained

in this table, but it does contain most of those which are applicable

to atmospheric chemistry. Evaluations and compilations of rate

data and on-going programs in these areas have been described

in the recent review paper "Evaluation and Compilation of Reaction

Rate Data" by R. F. Hampson and D. Garvin, Journal of Physical

Chemistry 81^, 2317-2319 (1977) . A current extensive listing of sources of

evaluated rate data, NBS List of Publications 73 "Chemical Kinetics

Tables, Data Evaluations and Bibliographies. A Guide to the

Literature" is available on request from the NBS Chemical Kinetics

Information Center.

Three sets of detailed data sheets have been published by us in the course of preparing these tables. They are R. F. Hampson (editor)

"Survey of Photochemical and Rate Data for Twenty-eight Reactions of

Interest in Atmospheric Chemistry" J. Phys. Chem. Ref . Data 2^, 267 (1973);

2
R. F. Hampson (editor) "Chemical Kinetics Data Survey VI, NBSIR 73-207

(1973); and D. Garvin (editor) "Chemical Kinetics Data Survey V"

NBSIR 73-206 (1973) , all recommendations contained in them (and still

pertinent) are summarized in the present table.

We have also accepted many recommendations made by R. T. Watson in

"Rate Constants for Reactions of CtO of Atmospheric Interest"

X

J. Phys. Chem. Ref . Data 6, 871 (1977) and by D. L. Baulch, et al

"Evaluated Kinetic Data for High Temperature Reactions" Volume 1 (1972),

Volume 2 (1973) and Volume 3 (1976), Butterworth and Co., London.

In addition to recommendations on rate and photochemical data the

table includes listings of current research results. These data listings

serve several purposes. Some simply record measurements, usually limited

in number, on reactions for which it is not yet practical to give

recommended values. Others show the data upon which a new recommendation

is based. Still others show what has been done on a reaction since its

rate constant was last evaluated. These new data may support the

recommendation or suggest the need for modifications in the future.

2. Guide to the Table

2 . 1 General

This table provides current (December 1977) information on reaction

rate constants, quantum yields and absorption cross sections. For many

reactions, preferred values are given. The reactions included in the

table are summarized in the index of reactions given in section 3.

Most of the important stratospheric reactions are in the tables.

A number of the less important ones and some related systems are

included, often simply for comparison.

The following remarks summarize the content of the table. It lists

416 reactions and gives a preferred value of the rate constant for 194

reactions; 136 based on recent reviews and 58 based on recent (1975-1977)

experimental work. New data entries (1975-1977) are given for 252

reactions, showing substantial activity in the study of gas kinetics.

The following principles have been used in the selection and

presentation of data:

a. Where a preferred value is given for a rate constant or photochemical quantity, it is so indicated by an asterisk [*]

placed ahead of the entry in the reference column.

b. As indicated earlier an asterisk preceded by a dagger sjrmbol

[t"] is used to indicate those preferred values that have

been recommended by the NASA Laboratory Measurements Committee

and published in NASA Reference Publication 1010 "Chlorof luoromethanes and the Stratosphere" R. D. Hudson, editor, August 1977.

7>
c. Where there is a recent published evaluation of the data

and there are no newer data, the evaluation is adopted

and usually marked with an asterisk. The original data

covered by the evaluation are not listed separately.

However this latter rule has not been applied when the

evaluation has appeared within the past year.

d. Vfhere there is an evaluation but there are new data, both

are listed and a preferred value is indicated (marked by

an asterisk)

e. Where desirable, the available recent data sets are

listed, and a selection is made or a preferred value is

synthesized from them.

2.2 Uncertainty in Recommended Value of a Rate Constant

The uncertainty assigned here to the recommended value of

a rate constant is given in the column "Notes and reliability

of log k". This is an estimate by the evaluator of the absolute

accuracy of the preferred value. It is a subjective judgment

derived from intercomparison of data sets, consideration of related

reactions studied with the same technique, estimates of how well

the parameters could have been controlled, and comparison with

theory. It means that in the evaluators judgment, the true value

will lie within the indicated limits to a high level of confidence

(90 to 95 percent)

Usually the uncertainty is indicated by the term in the

expression: logio k = C ± D. This is equivalent to the statement

that k is uncertain to a factor of F where D = logigl''' The

statement that k has the value kg and is uncertain to a factor of

F means that ko/F < k < ko F.

Other forms used to indicate reliability are the following:

A < k < B means k lies in the range between A and B

k < (>) B means B is an upper (lower) limit

k

~ B means B is only a rough guide to value of k

k = A ± B alternative form for stating reliability limits
At times a rate constant expression is quoted from a paper

with individual uncertainties for the rate parameters as k =

(A ± a) exp(-B ± b/T) . These measures are those provided by the

author and often are indications of precision, not overall

reliability.

Some notes are in order, regarding the statement of the

uncertainty in the recommended value of the rate constant for

those recommended values recommended by the NASA Laboratory

Measurements Committee. Those recommendations were made for the

limited temperature range 200-300 K. The uncertainty is indicated

for T = 230 K, a typical midstratospheric temperature and in some

cases allowance for extrapolation from higher temperatures was

necessary. This is why occasionally the entry consists of the

value of a rate constant measured at 298 K, the symbols [^*]

immediately ahead of the entry in the reference column to show that

this value has been adopted by the Committee for the temperature

range 200-300 K, and a statement of the uncertainty in the preferred

value at T = 230 K. This stated uncertainty will generally be

larger than the uncertainty in the measured value (measured at

298 K) to allow for the additional uncertainty introduced by

extrapolation to T = 230 K.

For the recommendations made by the NASA Laboratory Committee

the indicated uncertainties in NASA Reference Publication 1010

have been doubled in the present table in order to make the

reliability statement analogous to a "95 percent confidence level".

2.3 Conventions Concerning Rate Constants

a. General Convention . Almost all of the reactions in the

table are elementary processes. For them the rate expression is

derivable from a statement of the reaction, e.g.

A + 2B ^ AB2

-d[A]/dt = -(1/2) d[B]/dt = d[AB2]/dt = k[A][B]^

Note that the stoichiometric coefficient for B, i.e. 2, appears in

the denominator before B's rate of change (which is equal to

2k[A][B]2) and as a power on the right hand side.

Wherever there may be any doubt an explicit rate expression

is given.

5
b. Dissociation and Combination Reactions . Some reactions

of these types are not of integral kinetic order over the

stratospheric pressure and temperature range. That is, although

they require an energy transfer agent, "M," they are in the

"pressure fall-off region". For some such reactions we tabulate

rate constants that include the effect of the energy transfer

agent and give rates for various altitudes. The reactions are written to demphasize "M," e.g.,

NO- + NOo (+M) ^ N_Oc (+M)

M

HNOo ^ HO + NO

The rate expressions to be used do not have the concentration of M

in them, e.g.. Rate = k[N02] [NO3] and k[HN03] respectively. The

units given for the k's, s~l for first order, and cm+3 molecule~ls~l

for second order, are consistent with this convention.

The altitude, temperature and number density regime used in

these cases is

_3 altitude/km temp./K log [M] /molecule cm

15 217 18.60

20 217 18.27

25 222 17.93

30 227 17.58

35 237 17.26

40 251 16.92

45 265 16.60

This table follov/s the U. S. standard atmosphere, 1976.

c. Forward and Reverse Reactions. In some cases there are no data on a reaction of interest but there are data on the "reverse"

reaction. Occasionally, for

A ^ B (f)

B -> A (r)

an evaluation will use the data on the "reverse" reaction together

with an equilibrium constant to obtain the other rate constant.

Obviously this is an approximation but it often is a useful method

of estimating non-measured physical properties.

6

i
The table contains notations to warn the reader when this

procedure has been used, such as "based on reverse reaction,"

or when both reactions f_ and r^ are listed together "kf = kj-Kgq or kj- = kj/Kgq. These expressions, which are those used

in the analyses, are based on equating the two rates at

equilibrium.

f r

kf[A] = k^[B]

K = [B]/[A] = \/\.

2.4 Convention Concerning Optical Absorption Coefficients

These are reported in the table as "absorption cross sections

per molecule, base e". They are defined by the equations.

I/I^ = exp(-a[N]]l)

a = (l/([N]Jl))ln (I^/I)

where Iq and I are the intensities of incident and transmitted

light, a is the absorption cross section, cm2molecule~l, [N] is the

concentration of absorbers, molecules cm"^^ and I is the path length,

cm. Other definitions and units are frequently used. The terms

"absorption coefficient" and "extinction coefficient" are common.

It is always necessary to know what concentration units, path length

units and type of logarithm (base e or base 10) are used in the

definition. To convert "cross-sections" to absorption coefficients

in (atm at 273 K)-l cm"!, base e, multiply by 2.69 x 10^^.

A table of conversion factors is given in the appendix.

7
3. Arrangement of the Table

Data on a reaction appear only once in the table. The normal

location for a reaction is determined by its reactants. Each species

has been assigned a sequence number (1 to 65) as shown in the index that

follows. These sequence numbers are the same as those used in NBS Technical

Note 866. New species have been inserted in appropriate positions and

assigned sequence numbers such as 34a, 34b, etc. A reaction is filed

under the lower numbered species. That is, the reaction of ozone (7)

with an oxygen atom (1) is filed under reactions of oxygen atoms. The

numbers for the reactants appear at the left margin of the table, preceding the statement of the reaction, e.g. 1,7 *-* ^3 ^2 ^2' "^^^^^ number pairs run in ascending order through the table.

If a reaction is not filed in the location described above, a cross reference is given there. The most common exception is the listing

together of data on the forward and reverse reactions of a pair,

i.e. A B, B A.

In the index that follows, bimolecular reactions are listed under

both reactants. Frequently the listing of reaction partners for a particular species is divided into two parts by three dashes, separating

species earlier in the list than the species indexed from those later in

the list. Reactions of the particular species with those species listed

before the three dashes should be sought under those reaction partners.

There is no indexing of products of reactions. A few species are listed

in the index for which there are no reactions in the table, in anticipation

of expansion of the data set.

8
REACTION INDEX

1. 0

0(^D)

0(^S)

02(^A)

Rxn with: 0, 0("^S), 0^, 0^, N, NO, NO2, NO^, N^, N^O,

N20^, NH^, NH^, H, HO, HO2, H^, H^O, H2O2,

HNO2, TM03» S^2» ^°3* ^2^» ^^2*

OCS, CIO, BrO, OCIO, HCI, HBr, NO^Cl, CI2,

CI2O, CO, CO2, CN, CHO, CH2O, CH^, CH2NO2,

CH^ONO, CH^, C2H^, C2Hg, C^Hg, alkane,

Rxn with: O2, 0^, NO, NO2, N2, N2O, NH^, E^, E^O,

H2O2, HCI, CO2, CH^, C2Hg, CP2CI2, CPCI^

Rxn with: 0, O2, 0^, NO, NO2, N2, N2O, NH^, H2O,

CO2, CH^

Rxn with; 0, 0(^D), 0(^S)

hv, N, NO, NO2, NO^, N2, H, H2, H2O, H2O2,

HNO. SO, HS, CI, CN, CHO. CH3. CH3O

Rxn with: O2, 0^, N, NO, N2, H, SO, SO2, H2S, CO,

CF2CI2, CCI|^, CH^CI, CH2CI2, CHCl^

02(^2)

0.

Rxn with: O2, N2, H2O

Rxn with: 0, O(-^D), O(-^S), 02('^A)

hv, M, N, NO, NO2, H, HO, HO2, SO, SO2,

H2S, CI, Br, CIO, BrO, CO, CH2O, CH^,

CH^02, CH^ONO, CH^, C2H^, C^Hg, allene,

butenes, butadiene,

9
8. N Rxn with: 0, O^, 02(''"A), 0^ - - -

N, NO, NO^, HO, SO, SO^, OCIO

9. NO Rxn with: 0, 0(^D), O(-^S), 0^, 02('^A), 0^, N

hv, M, NO, NO2 + H2O, NO^, NH, NH^, H, HO

HO^, H^, H^O, H^O^, CI, CIO, BrO, OCIO,

CH^, CH^O, CH2O2

10. NO2 Rxn with: 0, 0 ( ) , O(-^S), O2, 0^, N, NO + H2O

hv, M, NO2, NO^, NH2, NH^, H, HO, HO2,

SO2, CI, CIO, CH^, CH^O, CH2O2

11. NO^ Rxn with; 0, O2, NO, NO2

hv, M, NO^, H2O, SO2

12. N2 Rxn with: 0, O(-^D), O(-^S), O2, 02(^A), 0^{-^Z) ^ - «

M, HO

13. N2O Rxn with: 0, 0(^D), 0(^S)

hv, M, H, HO, CIO, CO

14. N20^ Rxn with: 0 hv, M, H2O, SO2

15. NH Rxn with: NO - - -

16. NH Rxn with: 0, NO H, HO, H2, H2O

17. NH^ Rxn with: 0, O(-^D), 0(^S), NO2

M, H, HO, CIO

10
17a.

18. H

Rxn with: H

19. HO

20

21

22

HO,

H^O

Rxn with;

Rxn with: 0, 0^, 02(^A), 0^, NO, NO^, N2O, NH^, NH^,

NpHzi

H, HO, HO^, H^O, H2O2, HNO, HNO^, HNO^,

SO2, HS, H^S, COS, OCIO, HCl, NOCl, 01^, CO,

CO2, CH^O, CH^OOH, CH^ONO, CH^Cl

0, 0^, N, NO, NO2, N^, N^O, NH^, NH^, H - - ^

M, HO, HO^, H^, D^, H^O, H2O2, HNO, HNO^,

HNO^, SO^, H^S, CI, HCl, DCl, HBr, NO^Cl,

CO, CH^O, CH^OH, CH^NO^, CH^ONO, CH^, C^H^,

C^H^, C^H^, C^Hg, C^H^Q, alkane, C^Hg,

CgH^CH^j C'F2Cl2, CFCl^j CH^Cl,

CH„C1„, CHCI3, CH.Cl.F,

2 2* 3* 1 J k

0, 0^, NO, NO2, H, HO

M, HO2, H2, H2O, SO2, CI, Br, CIO, CO, CH2O,

CH2O2J C2H^, C2H^, C^Hg, C|^H-|^Q

0, 0(^D), O2, NO, NH2, HO, HO2

M, CI, CIO

0, 0(^D), 0(^S), O2, 02(^2), NO, NO^, N20^,

NH2, H, HO, HO2 SO^

Rxn with;

Rxn with;

Rxn with;

23 H2O2 Rxn with: 0, 0(^D), 0„, NO, H, HO

hv, M, CI, Br

11
24. HNO Rxn with: 0^, H, HO - - - M, HNO

25. HNO2 Rxn with: 0, H, HO - - - hv

26. HNO^ Rxn with: 0, H, HO - - - hv , M, CI

26a. S Rxn with: CS^, COS

27. SO Rxn with: 0, 0^, 0^{^^), 0^, N - - - SO, SO^

28. SO2 Rxn with: 0, O^C^A), 0^, NO^, NO^, ^2^5^

HO^ - - - CH^

29. SO^ Rxn with: 0, N, H^O, SO - - -

30. S^O Rxn with:

31. HS Rxn with: 0, 0^, H - - - HS

32. H2S Rxn with: 0, 02(''"A), 0^, H, HO - - -

33. HSO^ Rxn with:

34. H^SO^ Rxn with:

34a. CS Rxn with: 0 - - -

34b. CS^ Rxn with: 0, S - - -

34c. COS Rxn with: 0, H, S

12
35. CI Rxn with: 0^, 0^, NO, NO^, HO, HO^, H^, H^O^,

HNO^ - - - CI, OCIO, ClOO, NOCl, NO^Cl,

NO^Cl, Cl^O, CH^, C^Hg

Br Rxn with: 0^, HO^, H^O^ - - -

36. CIO

BrO

Rxn with: 0, 0^, NO, NO^, N^O, NH^, HO^,

hv, CIO, BrO, CO, CH^, C^H^, C^H^

Rxn with: 0, 0^, NO, CIO - - - BrO

37. ClOO Rxn with: CI hv, M

OCIO Rxn with: 0, N, NO, H, CI - - - hv

38. CIO. Rxn with:

39. HCl Rxn with: 0 , 0 ( D )

, H , HO - - - hv

HBr Rxn with: 0, HO - - -

40. HOCl

41. HOCIO

42. NOCl

Rxn with: hv

Rxn with

Rxn with: H, CI - - - hv

43. NO^Cl Rxn with: CI - - - hv

43a. NO^Cl Rxn with: 0, HO, CI - - - hv

44. CI, Rxn with: 0, H - - - hv

44a. Cl^O Rxn with: 0, CI - - -

13
45. CO Rxn with: 0, O^C'^A), 0^, N^O, H, HO, HO^, CIO

CH^O

46. CO^ Rxn with: 0, O(-^D), 0(^S), H - - - M

46a. CN Rxn with: 0, O2 - - -

47. CHO Rxn with: 0, 0^ - - -

48. CH^O Rxn with: 0, 0^, H, HO, HO^ - - - hv

49. CH^ Rxn with: 0, 0^, 0^, NO, NO^, SO^ - - -

50. CH^O Rxn with: 0^, NO, NO^, CO

51. CH^O^ Rxn with: 0^, NO, NO^, HO^ - - - CH^O^

52. CH^OH Rxn with: HO -

53. CH^OOH Rxn with: H - - -

54. CH^NO^ Rxn with: 0, HO - - -

CH^ONO Rxn with: 0, 0^, H, HO - - - hv

55. CH^NO^ Rxn with:

56. CH^ Rxn with: 0, 0 ( ) , 0(^S), 0^, HO, CI, CIO - -

56a. C^H^ Rxn with: HO, CIO - - -

57. C^H^ Rxn with: 0, 0^, HO, HO2, CIO - - -

14
58. C^Hg Rxn with: 0, O(-^D), HO,

*59. C^Hg Rxn with: 0, 0^, HO - -

t60. C^Hg Rxn with: 0, HO, HO^ - -

V60a. CgHg Rxn with: 0 , HO - - -

61. CP^Cl^ Rxn with: 0(^D), 02("^A),

62. CFCl^ Rxn with: 0 ( )

, HO - -

63. CC1|^ Rxn with: HO - - - hv

64. CH.Cl. Rxn with: 0, 0,,(^A), 0^,

/65. CH.Cl.P, Rxn with: HO - - -

1 J k

* and higher alkenes

t and higher alkanes

V and other aromatics

/ and other halocarbons

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REFERENCES

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and Third Body Effects on The Rate Constants for H 0^, H Ne,

and H ce, " J. Chem. Phys. 57. 3736-3745 (1972)

Albers, E, A., Hoyermann, K. , Wagner, H. Gg., and Wolf rum J,, "Study of

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(Combustion Institute, Pittsburgh, 1969 > 313-321

Albers, E. A., Hoyermann, K, , Wagner, H, Cg,, and Wolfrum J,, "Absolute

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Albers, E, A,, Hoyermann, K. , Schacke, H. , Schmatjko, K. J,, Wagner, H. Gg,,

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Clyne, M. A. A., and Down, S. , "Kinetic Behaviour of 6H X^n and A^E* using

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Clyne, M. A. A., and McDermld, I. S. , "Mass Spectrometrlc Determinations of

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Clyne, M. A. A., and Nip, W. S. , "Study of Elementary Reactions by Atomic

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Cox, R. A., "The Photolysis of Nitrous Acid in the Presence of Carbon Monoxide

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Cox, R. A., Derwent, R. G. , and Holt, P. M. "The Photo-flxidation of Ammonia

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Cox, R. A., Derwent, S. G. , and Holt, P. M., "Relative Rate Constants for

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2031-2043 (1976)

Cox, S. A., Derwent, R. G. , Holt, P. M. , and Kerr, J. A., " Photo-Qxidati on of Methane in the Presence of N6 and Ndg," J. Chem. Soc Faraday

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Cupitt, L. T., and Glass, G. P., "Reactions of SH with Atomic 6xygen and

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Daubendiek, R. L., and Calvert, J. G., "A Study of the NgSg-Seg-e^ Reaction

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Davidson, J. A., Schiff, H. I., Streit, G. E. , McAfee, J. R.

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Schmeltekopf , A. L., and Howard, C. J., "Temperature Dependence of

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Davidson, J. A,, and Thrush, B. A., "Reaction of 6xygen Atoms with Methyl

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Volman, D. H., and Gorse, R. A., "Rate Constant for the Reaction of Hdg with

Carbon Monoxide," J. Phys. Chem. 76, 3301-3302 (1972)

von Rosenberg, C. W., Jr., and Trainor, D. W., "vibrational Excitation of

©zone Formed by Recombination," J. Chem. Phys. 61., 2442-2456 ( 1974) von Rosenberg, C. W., Jr., and Trainor, D. W., "Excitation of Qzone formed by

Recombination. II," J. Chem. Phys. 63, 5348-5353 (1975)

Wagner, H. Gg. , Welzbacher, 0., and Zellner, R., "Rate Measurements for the

Reaction H Clg HCl Cl by Lyman-O! Fluorescence," Ber. Bunsenges.

Phys. Chem. 8£, 902-908 (1976)

Wagner, H. Gg. , Welzbacher, U., and Zellner, R., "Rate Measurements for

the Reactions H NO^ - e)H NO and H NflCl - HCl N9

by Lyman-a Fluorescence, Ber. Bunsenges. Phys. Chem. 80 . 1023-1027 (1976)

Walker, R. W. , Ph.D., thesis, Univ. of London, Queen Mary College, 1973

Walker, S. W. , Comments on "Gas-Phase Sxidation of Butene-2 : The Role of

Acetaldehyde in the Reaction," by Ray, D. J, M, , Diaz, R. R. , and

Wassington, D. J., Symp. Combust. 14th (Combustion Institute, Pittsburgh,

1973) 265-266

Walker, R. W., "Rate Constants lor Reactions in Gas-Phase Hydrocarbon

6xidatlon," Chapter 7 in "Gas Kinetics and Energy Transfer - Volume 2" A Specialist Periodical Report, The Chemical Society,

London ( 1977 ) Washida, N. , and Bayes, K. D., "The Reactions of Methyl Radicals with Atomic

and Molecular ©xygen," Int. J. Chem. Kinet. 8, 777-794 (1976)

Washida, N. , Martinez, R. I., and Bayes, K. D. , "The dxidation of Formyl

Radicals," Z. Naturforsch. A 29, 251-255 (1974)

Watson, R, T. , "Rate Constants for Reactions of Clet^ of Atmospheric

Interest," J. Phys. Chem. Ref. Data 6, 871-918 (1977)

Watson, R., Machado, G, , Fischer, S. , and Davis, D. D., "A Temperature

p Dependence Kinetics Study of the Reaction of ^'^^ P^/z'^ with 6^, CH^ and

HgOg*" Chem. Phys. 65, 2126-2138 ( 1976 ) Watson, R, T, , Machado, G,, Conaway, B., Wagner, S, , and Davis, D. D.,

"a Temperature Dependent Kinetics Study of the Reaction of 0H with

CHgClF, CHClgF, CHClFg, CH^CClg CH^CFgCl, and CFgClCFClg,"

J. Phys. Chem. 8i, 256-262 (1977)

Weaver, J., Meagher, J,, Shortridge, R, , and Heicklen, J., "The 6xldation of

Acetyl Radicals," J. Photochem. 4, 341-360 (1975)

87
Wei, C. N. , and Timmons, R. B. , "ESR Study ot the Kinetics of the Reactions

o* e(^P) Atoms with CSg and eCS," J. Chem. Phys. 62, 3240-32A5 (1975)

Westenberg, A. A., and deHaas, N. , " St eady-Sta t e Intermediate Concentrations

and Rate Constants. Some Results," J. Phys. Chem. 76, 1586'>1593 < 1972a)

Westenberg, A. A., and deHaas, N. , "Measurement of the Rate Constant for

H HgCa - HC6 at 297-652*K," J. Phys. Chem. 76, 2213-2214 (1972b)

Westenberg, A. A., and deHaas, N. , "Rates of C0 6H and Hg dH ever an Extended Temperature Range," J. Chem. Phys. 58, 4061-4065 (1973a)

Westenberg, A. A., and deHaas, N. , "Rate of the Reaction 6R an -» HgC* * 6,"

J. Chem. Phys. 58, 4066-4071 (1973b)

Westenberg, A. A., and deHaas, N, , "Rates of H CH^X Reactions," J. Chem.

Phys. 6£, 5321-3325 (1975a)

Westenberg, A. A., and deHaas, N. , "Reaction Rates of 6 CH^Br and 6 CH^Cl, " J. Chem. Phys. 62, 4477-4479 (1975b)

Westenberg, A. A., and deHaas, N. , "Rate of the 6 30^ Reaction," J. Chem.

Phys. 6g, 725-730 (1975c)

Westenberg, A. A., and deHaas, N. , "Rate of the Reaction of 9 Sdg M - SO^ * M> " ^- Chem. Phys. 63, 5411-5415 (1975d)

Westenberg, A. A., Roscoe, J. M. , and DeHaas, N. , "Rate Measurements on

N ^a^^^g* - Ne 6 and H ®2*^^g' - <3H * Chem. Phys. Lett. 7,

597-599 ( 1 970 ) Whytock, D. A., Michael, J. V., and Payne, W. A,, "Absolute Rate Constants for

for e Ne Ng - NOg N2 from 217 - 500 K, " Chem. Phys. Lett. 42,

466-471 (1976)

Whytock, D. A., Lee, J. H. , Michael, J. V., Payne, W, A., and Stief, L. J.,

"Absolute Rate of the Reaction of Cl( ^P ) with Methane from 200-500 K,

J. Chem. Phys. 66, 2690-2695 (1977)

Whytock, D. A., Timmons, R. B. , Lee, J. H. , Michael, J. V., Payne, W. A., and

Stief, L. J., "Absolute Rate of the Reaction of e( ^P ) with Hydrogen

Sulfide ever the Temperature Range 263 to 495 K," J. Chem. Phys. 65,

2052-2 055 ( 1976 ) Wilson, Wm. E., Jr., "A Critical Review of the Gas-Phase Reaction Kinetics

of the Hydroxyl Radical," J. Phys. Chem. Sef. Data 1., 535-573 ( 1972 ) Wong, E. L. , and Belles, F. E. , "Rate Measurements for the Reaction of

Hydrogen Chloride and Deuterium Chloride with Atomic 6xygen," Lewis

Research Center, NASA, Cleveland, Ohio, NASA Tech. Note, NASA TN-D-6495

(1971); Chem. Abstr. 76:18326q (1972)

Wong, W. , and Davis, D. D., "A Flash Photolysis-Resonance Fluorescence Study

of the Reaction of Atomic Hydrogen with Molecular 6xygen: H flg * M HCg M," Int. J. Chem. Kinet. 6, 401-416 (1974)

Wu, C. H. , Morris, E. D., Jr., and Niki, H., "The Reaction of Nitrogen

Dioxide with Bzone," J. Phys. Chem. 7Z. 2507-2511 (1973)

Wyrsch, D., Wendt, H. R., and Hunzlker , H, E,, "Modulation Kinetic Spectroscopy

of Hg/Hg/eg/Ce Mixtures: Reactions of HgH and HOg," XI. Int. Symp. on Free Radicals ( Berchtesgaden-Konlgssee, Sept. 4-7, 1973 ) Paper No. 36; see also, Ber. Bunsenges. Physik. Chem. 7_8, 204 (1974)

Yaron, M. , von Engel, A., and Vidaud, P. H., "The Collislonal Quenching of

02(^Ag) by Ne and COg," Chem Phys. Lett. 37, 159-161 (1976)

2^hniser, M. S. , Berquist, B. M, , and Kaufman, F,, "Kinetics of the

Reaction CI CH^ CH3 HCl from 200 to 500 K, " Int. J. Chem.

Kinet. 10. 15-29 (1978)

88
Zahnlser. M. S. , Chang, J. S,, and Kaufman, F. , "Chlorine Nitrate:

Kinetics of Formation by CIG * NQg M and of Reaction with eH,"

J. Chem. Phys. 67, 997-1003 (1977)

Zahniser, M, S. , and Kaufman, Fo, "Kinetics of the Reactions of CIS with

0 and with we," J. Chem. Phys. 66, 3673-3681 (1977)

Zahniser, M. S. , Kaufman, F., and Anderson, J. G., "Kinetics of the Reaction

of 0H with HCl," Chem. Phys. Lett. 27, 507-510 (1974)

Zahniser, M. S. , Kaufman, F. , and Anderson, J. G., "Kinetics of the Reaction

CI 63 - Cle Og," Chem. Phys. Lett 37, 226-231 (1976)

Zellner, R. , Erler, K. , and Field, D. , "Kinetics of the Recombination

Reaction 6H H M Hgfl M at Low Temperatures," Symp. Combust.

16th (Combustion Institute, Pittsburgh, 1977) 939-948

Zellner, R. , and Steinert, W., "Flash Photolysis Study of the Rate of the

Reaction 0H CH^ CH^ HgG over an Extended Temperature Range,"

Int. J. Chem. Kinet. 8, 397-409 (1976)

89
APPENDIX 1.

Chemical Thermodynamic Properties of Selected Molecular Species

E. S. Domalski, D. Garvin, and D. D. Wagman

Two tables are provided showing chemical thermodynamic properties

of selected molecular species of interest in stratospheric chemistry. In

these tables there are sufficient data for the usual calculations of

heats of reaction and equilibria.

The first table lists enthalpy and Gibbs energy of formation,

entropy and heat capacity data. The information was extracted from

"Selected Values of Chemical Thermodynamic Properties" (D. D. Wagman,

et al, NBS Technical Note 270-3, January 1968) except as indicated

in the Notes. The thermodynamic properties tabluated are:

1. enthalpy of formation at OK and 298. 15K,

2. Gibbs energy of formation at 298. 15K,

3. enthalpy increment between OK and 298. 15K,

4. entropy at 298. 15K,

5. heat capacity at constant pressure at 298. 15K.

The values given for the heats of formation are based on experimental thermodynamic and spectroscopic measurements except

where otherwise indicated; the values of S° , C

° and H° -H° for

p zy o u gaseous species were calculated by standard statistical-mechanical

equations, using corrections for vibrational anharmonicities

,

rotational stretching, and rotation-vibration interactions where

these data were available.

The second table presents bond dissociation energies or bond

strengths. These usually are the enthalpies of simple bond scission

reactions. However, there are some cases in which there is a substantial contribution from rearrangement of electronic structure

in the products (reducing the bond energy)

.

The values given here for some molecules may differ slightly from

values adopted by the CODATA Task Group on Key Values for Thermodynamics

(see CODATA Bulletin 17, published by the International Council of

Scientific Unions Committee on Data for Science and Technology,

January 1976) . These differences will have no significant effect on the

enthalpies or free energies of reaction calculated from the tables.

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i

Notes

1. Hampson, R. F. et al, J. Phys. Chem. Ref . Data _2, 267-312 (1973)

[Data sheet on 0^ + hv (u.v.)] p. 303.

2. Contributions of the higher electronic states of molecular oxygen

to the enthalpy, entropy, and heat capacity at 298 K are

insignificant

.

3. Stull, D. R. and Prophet, H. "JANAF Thermochemical Tables" 2nd.

ed. NSRDS-NBS 37 (1971).

4. Tsang, W. Estimated from kinetic data on the decomposition of

N2H^. Chapter 12, NBS Report 10904, 1 July 1972,

5. NBS Report 10904, 1 July 1972, pp. 239-307.

6. R. A. Fletcher and G. Pilcher, Trans Faraday Soc. 66, 794-799

(1970) provide more recent data for AHf° , 298.15 K.

7. Data obtained from Benson and O'Neal ("Kinetic Data on Gas

Phase Unimolecular Reactions", NSRDS-NBS-21, Feb 1970, page 55).

8. Heat formation value from S. W. Benson "Thermochemical

Kinetics" Second Edition, John Wiley and Sons (1976)

.

9. Values for AHf° , S° , and Cp° at 298.15 K were calculated using

the group additivity method described by Benson and O'Neal

("Kinetic Data on Gas Phase Unimolecular Reactions", NSRDS-NBS21, Feb. 1970, pp. 40-42).
The value for mf" [CH^ONOCg)] = -16.5 kcal mol"''" was derived

from the combustion data of Geiseler and Thierfelder (Z. physik.

Chem., N. F., 29, 248-257 (1961)), and the equilibrium data of

Leermakers and Ramsperger (J. Am. Chem. Soc. 54, 1837-1845

(1932)) for: CH30H(g) + NOC^(g) = CH30N0(g) +HC^(g).

o -1

The value for ^f (CH30N02(g)) = -29.8 kcal mol was derived

from the work of Ray and Ogg (J. Phys. Chem. 63j 1522-1523

(1959)) on the enthalpy of reaction of N20^ with CH^ONO.

o -1 -1

We have chosen S [CH30N02(g)] = 76.1 cal mol K based upon

low temperature thermal data of Gray and Smith (J. Chem. Soc.

1953

,

2380-2385). Calculations from microwave studies by

Dixon and Wilson (J. Chem. Phys. 35^ 191-198 (1961)) give S* =

72.15 cal mol "''"k"'''.

Davies, J. V., and Pritchard, H. 0., J. Chem. Thermodynamics

4, 23-29 (1972) provide more recent AHf° data.

Data on mf , S , Cp obtained from S. W. Benson and H. E.

O'Neal ("Kinetic Data on Gas Phase Unimolecular Reactions",

NSRDS-NBS-21, Feb. 1970, page 567).

Rossini, F. D., Pitzer, K. S., Amett, R. L., Braun, R. M.

and Pimentel, G. C, "Selected Values of Physical and Thermodynamic Properties of Hydrocarbons and Related Compounds",

API Research Project 44, Carnegie Press, Pittsburgh, 1953.

98
16. AHf° data from Pittam and Pilcher (J. Chem. Soc, Faraday

Trans. I, 68, 2224-2229 (1972).

17. AHf° data frcjm R. L. Nuttall, A. H. Laufer and M. V. Kilday.,

J. Chem. Thermodynamics 3, 167-174 (1971).

18. Devore, J. A., and O'Neal, H. E., J. Phys. Chem. 73, 2644-

2648 (1969).

O 19. Data on S° and C^ were obtained from Note (14), page 589;

data on AHf° came from Note (18).

20. Spectroscopic studies of N. Basco and R. D. Morse, J. Molec.

Spectres. 45, 35 (1973); R. A. Durie and D. A. Ramsay, Can.

J. Phys. 36, 35 (1958); P. A. G. O'Hare and A. C. Wahl, J.

Chem. Phys. 54, 3770 (1971); L. Andrews and J. I. Raymond,

J. Chem. Phys. 55, 3087 (1971); D. R. Johnson and F. X. Powell,

Bull. Am. Phys. Soc. 13^, 594 (1968); A. Carrington, P. N. Dyer,

and D. H. Levy, J. Chem. Phys. 47 , 1756 (1967) were examined

and used to calculate the thermodynamic properties.

21. Arkell, A., and Schwager, I., J. Am. Chem. Soc. 89, 5999

(1967); Johnston, H., Morris, E. D., and Van den Bogaerde, J.,

J. Am. Chem. Soc. _91, 7712 (1969), Clyne, M. A. A. and White,

I. F., Trans. Faraday Soc. 67., 2068 (1971).

22. Studies by D. J. Gardiner, J. Mol. Spectroscopy 38, 476 (1971)

and G. E. Herberich, R. H. Jackson, and D. J. Miller, J. Chem.

Soc. (A) 1966 , 336 were examined and the data used to calculate

the thermodynamic properties.
23. The spectroscopic data of K. 0. Christe^ C. J. Schack and

E. C. Curtis^ Inorg. Chem. 10, 1589 (1971) were used.

24. Thermal Constants of Substances (Termichesky Konstanty

Veshchestv), Vol. IV, V. P. Glushko, Editor, Moscow (1970).

25. The combustion data of A. T. Hu and G. C. Sinke, J. Chem.

Thermodynamics 1, 507-513 (1969) were used to derive AHf°

298.15 K values for CCl, , CHCl^, and CHoCl^ in the liquid state.

4 3^ 2 2

26. The vaporization data of D. L. Hildenbrand and R. A. McDonald,

J. Phys. Chem. 63, 1521-1522 (1959) were used.

27. The combustion data of R. A. Fletcher and G. Pilcher, Trans.

Faraday Soc. 67, 3191-3201 (1971) were used to calculate

AHf° [CH^CKg)].

28. J. Chao, A. S. Rodgers, R. C. Wilhoit, and B. J. Zwolinski,

J. Phys. & Chem. Ref. Data 3^ 141-162 (1974) provide a recent

evaluation of the thermodynamic properties of CH^CCl^

.

29. Based on data in H. Okabe and M. Lenzi, J. Chem. Phys. 47,

5241 (1967) and in J. Masanet, A. Gilles and C. Vermeil,

J. Photochemistry 2, ^17 (1974/75).

30. Parker, V. B., Wagman, D. D., and Garvin, D. , NBSIR 75-968.

Selected thermochemical data compatible with the CODATA

recommendations, January 1976.

31. Value for heat of formation derived from equilibrium studies

reported by H. Imagawa, Denki Kagaku j^, 271 (1951).

100
32. JANAF Thermochemical Tables Supplement No. 48, June 1977.

33. Heat of formation value based on data in H. D. Knauth, H. Martin

and W. Stockmann, Z. Naturforsch. 29A, 200 (1974).

34. Wagman, D.D. Private communication.

101
Bond Dissociation Energies, at 0 K

Calculated from heats of formation in the accompanying table

Reaction kJ/mol kcal/mol Note

02 ^ 20

03

-> O2 + 0

H2 -> 2H

HO ^ H + 0

HO^ ^ HO + 0

-> H + 0^

H^O ^ HO + H

H^O^ ^ 2H0

493. 59±0.4

101.4±2.

1

432.00±0.04

423.8±2.

280±8

210±8

493.7±0.8

207.1±2.1

117.97±0.1

24.24±0.5

103.25±0.01

101.3±0.5

67±2

50±2

118.0±0.2

49.5±0.5

^2^2 ^ +

^ N + N

NO ^ N + 0

NO^ NO + 0

NO^ ^ NO^ + 0

N2O ^- N + NO

^ N^ + 0

N^O^ NO + NO^

N„0, ^ N0„ + N0_

z 4 / z NO^ + NO^

HNO ^ H + NO

^- NH + 0

trans-HNO^ ^ HO + NO

HNO3 HO + NO2

NH ^ H + N

350±8

941.69±0.04

627.9

300.5

205±21

474. 9±4

161.3

35. 1±0.8

53.2

89.5

203

487

202

200

343

84±2

225.07±0.01

150.1

71.83

49±5

113. 5±1

38.58

8.4±0.2

12.7

21.4

48.6

116.5

48.4

47.8

82

102
Bond Dissociation Energies, D° at 0 K

Calculated from heats of formation in the accompanying table

Reaction kJ/mol kcal/mol Note

NH^ -> H + HN 366 87.4

NH^ -> NH^ + H 448 107

CO C + 0 1071.94±0.4 256.2±0.1

CO^ -> CO + 0 525.9±0.4 125.7±0.1

CHO CO + H 70 16.7

CH^O ^ CHO + H 364 87

CH^O -> CH^ + 0 378 90.4

^ H + H2CO 93 22

CH^O^ ^ CH^O +0 237 56.8

^ CH^ + 0^ 118 28.1

CH, ^ CH^ + H 432 103.2

4 3 CH^OOH CH^O + HO 184. 44.0 ^ CH^ + HO2 276±8 66±2

CH^ONO ^ CH^ + NO2 248 59.2

CH2NO2 ^ CH^ + NO2 254 60.6

CH^ONO^ ^ CH^O + NO^ 174 41.6 ^ CH^ + NO^ 341 81.6

SO S + 0 515. 4±8 123. 2±2

SO2 ^ SO + 0 547. 3±8 130.8±2.0

SO^ ^ SO2 + 0 342. 7±4 81.9±1

Note 1. Calculated for T = 298K

10 3
r—1

I—1

.—1 I 1 H H 1 H H CO 1 1 o o o o o in o r—( o o \D r—1

CM o CM UO 00 <T X CM X X O ,—1 ,—1

CTi 1—( 1 c m

CO uO CM i CO 1 1 1—t 1 o 1 ,—1

CO o o cn o CO o o o ,—1 m 1—1

r—1

1—1 ,—1 ' E <r <r LiO X 1—1 o X X X X X X

D- CM CM CM <r

r-t r-l 1 t ,—1 H 1 I 1 CN H

CO 1 CM <r CM

cr\ o cr\ cr\

O o o CO

,—( 1—1

r—l 1—1

Csl CM CO o I—1

T—1 U X CN X X vO X o , 1 1—1

.—tr- r—1

1—1

1—t 1 w 1—1

.—f

1—1 I—1 1 1 1 H H 1 H

CM

H 00 CO

&0 1 1 1-H 1 CO <r o <r o 00 o o CO CO o o r—( o 1—1 T—{

T—l 1—1(y\ CO

CO 1—1

XXX

X r—1 ,—t ,—1 1—r ^ CM 1—I 1

,—11 H

H

H 1—1 00 OS CM O 1-1 CM CM 1—1 r-1 CM r-l CM 1 1 1 1 O O O o in O CM O o O r-l ,—1

CO ,—1\D ,—1 ^ (—1 00 ,—1

.—I ,—1 o CO CO o X X X X X • X

X

g .—I

r-l 1—1 rH .—1

mEo

1—( H

HH CO CM m CO

.—1 1—1 1 1 1 1 cn O vO O o -J- o 1—1 CO CM I—1

CO r-i o r—1r—1

rH o 1 1 o CM CM CO E O o 1-1 X X X o X

rn E

r-1 \o 00 <]• 00

.—f w

H r-l o H CM

H

CM 1 uo 1—1

CO

O vO

OO <r o ro CM I—1

CO o 1—1 r-i E I CO o <N o CO

m

O o X CM

X • X E 1—1 00 CO

-a

r-K

U} CO

H

H r-l CM 00

H I CO O ^ o 1^ o CM 1—1

CO I—1 O r-l o CO O CM o .—1 E O o X X CM - X CO

CO E

i-< r-l 00 00 o

II 1—1

CO II

11 II r-H

II 1 1—1

II E CD .-I <D 1 -P u 11 1 T—1

,—I

CO II T—1 nj 3 /

U) 3 1 CO r-l W u 1 r-H C .-1 CO 1 1 1—1 (U 1 H <1J CO \—1

00 CO E ^ 1—1 o o T—1 o 1-1 r-l CL 1 E E O E 1 1 CO

rn CO

a CO

B E C7^ 1-i E E m E CI. CM eg CM < <j -o E o to P. -u E

JJ o

1—1 f-l r-< 1-1 CO -u 1—1

CE

<<:i

oal I a. u ,-1o

s:u

1-1a.

104
105
CO

CO o

0)

CO XIoee n

CO

0)CO

CO oo

00

CO <uCO e to 4J XI

CO o

Csl

°° II CM O

CO 0)CO E CO U X

CO

<rO

00O

i-io

00

CN

4-1 CO00 QJ X CO

CO

O

CO

O

csi

CM

CN] 1^^ II u

CO a;CO B CO u X

CO

O

CO

LO

COO

COo

Cvj

O

J-) CO 01CO E CO u X

CMIo

CO Xoe

CO

B

CNJo,—(

CM\D

g

1—4 CM CO

(U X 4-1 4J c

QJ

•r-( o

•r-l (3 m

CM r—1 m ' O p, QJ •H o CO

j_l CJ o

?s ,—1

r-l c

CMg o o

CO • r^ 1 4-1 CN w-l 1 p,

}.| JJ o

cu CO r-l CO PL, CD •rl

4-1

(LI QJ ,—1 C X 3

0^ 4J 6 1 J ,—I

CO

m

,—I

,—I o o QJ

XX ^ 1

QJ QJ 3 CO CO CO vO CO CO Xi

;> CM , 1 c QJ 1 Q

4-1 CJ( o 4-1 1 )^ 4J QJ CO

<L) ?>

CO CM o

QJ 4J

CO o o 1 4-1 E g 4J

r—1 o CO 00 s X ,—1

>4-l QJ o

f\J 4.1 4-1 00

a; PPl o

cn •H r-l

c_> c

r^

g QJ

M-l 3 00 MH CO

dl o 4a o M o r-i1 g; QJ g

QJ o CJ

r-l r—1

QJ 4-1 3 1

li CO p, r—1

CO <C 1 o

,__(

Q o g

CO rH o CO

CO 1 CO }.i

g

QJ jQ

u

CO o c

,—1 U-l •H

QJ 4J , ( }.) X) 13 o o QJ QJ QJ B B ?> 4-1 CO c CO CO Ol o I—1

QJ

B E CJ 3 u o u X D. o CO X

i-i I-IH 4-1 0)

106
NBS-114A (REV. 7-73)

U.S. DEPT. OF COMM. BIBLIOGRAPHIC DATA

SHEET

1. PUBLICATION OR REPORT NO. NBS SP-5132, Gov't Accession

No.

3. Recipient's Accession No.

4, lIlLc. AINU oUDlllLr.

Reaction Rate and Photochemical Data for

Atmospheric Chemistry - 1977

5. Publication Date May 1978

6« Performing Organization Code

7. AUTHOR(S)

Robert F. Hampson, Jr., and David Garvin, Editors

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