A 111 Ob SQD111

NBSIR 74-535

A Selected and Annotated Bibliography

of Compilations of Data Relevant to

Biochemical Thermodynamics

G. T. Armstrong, G. R. Janes, and R. N. Goldberg

Thermochemistry Section

Physical Chemistry Division

Institute for Materials Research

National Bureau of Standards

Washington, D. C. 20234

July 1974

Final

NtST

PUBLICATIONS

OC JEPARTMENT OF COMMERCE

0 slAL BUREAU OF STANDARDS

NBSIR 74-535

A SELECTED AND ANNOTATED BIBLIOGRAPHY

OF COMPILATIONS OF DATA RELEVANT TO

BIOCHEMICAL THERMODYNAMICS

G. T. Armstrong, G. R. Janes, and R. N. Goldberg

Thermochemistry Section

Physical Chemistry Division

Institute for Materials Research

National Bureau of Standards

Washington, D. C. 20234

July 1974

Final

U. S. DEPARTMENT OF COMMERCE, Frederick B. Dent. Secretary

NATIONAL BUREAU OF STANDARDS, Richard W. Roberts, Director

Table of Contents

page

Introduction 1

Bibliography 3

Author Index. 62

Subject Index 64

Introduction

There is an increasing demand by workers in the biological and

biochemical sciences for thermochemical data. However, even the

location in the literature of an existing piece of data may present

a problem due to the sheer bulk of the existing scientific literature.

This is aggravated somewhat by the fact that much of the pertinent

data is relevant not only to biochemistry, but also to other disciplines

such as classical solution chemistry, electrochemistry, and thermochemistry.

As part of the program of the Thermochemistry Section at the National

Bureau of Standards, it was felt that it would be useful to survey the

existing sources of compiled thermochemical data and to prepare a

bibliography selected from this literature on the basis of its relevance

to biochemistry. This bibliography should serve to assist in the

location of desired information where it is available pending the

appearance of comprehensive reviews and compilations of data specific

to biochemistry. .

The bibliography is listed in alphabetical order by leading author.

A brief discription of the contents of each item is given to permit the

reader to select those references which will most directly apply to his

own needs. Some of the compilations were prepared specifically for use

in biological sciences; other were prepared for a more general thermoi dynamic audience, but also contain substantial amounts of data valuable

in the biological sciences; still others are of very general interest and

contain some, but comparatively limited amounts of data specific to

biological processes. These three degrees of relevance are indicated

by the Roman numerals I, II, and III, respectively.

1
This report was put together partly to place in the hands of interested

scientists some information which we think will be useful—derived from our

efforts in a slightly different direction. The real goal of this work is to

provide a survey upon which to base judgments as to the adequacy of existing

compilations, recommendations for compilation and evaluation of information

not included, and suggestions for areas requiring new experimental work.

In accord with the above goal the report is intended to be fairly

complete with respect to category I and category II, but makes no attempt

at completeness in category III.

The alphabetical subject index that follows the main section of this

bibliography gives an indication of thermodynamic properties, physical

or chemical processes, classes of substances, and in a few cases individual

substances for which information is to be found in the bibliography. It is

not practical to give an exhaustive index to the contents of the individual

references; hence the absence of a piece of information in the index does

not necessarily mean its absence in the references. This is particularly

true with respect to particular substances, which the reader should assume

are not listed except by chance of title or abstract. However, the

index is provided to steer the reader to some appropriate bibliographical

entries. The index together with the annotations in the bibliography

should allow the reader to select some appropriate sources of information.

This bibliography was instigated by J. T. Edsall, I. Wadso*, W. P.

Jencks, and P. Privalov of the joint IUPAC, IUB, IUPAB joint Subcommittee

on Thermodynamics for the Biological Sciences, to whom acknowledgement

is given for suggestions and encouragement.

2
Armstrong, G. T., Domalski, E. S., Furukawa, G. T., Reilly, M. L.

,

Wilhoit, R. C. and others.

A Survey of Thermodynamic Properties of the Compounds of the Elements

CHNOPS - A Series of Eighteen Reports

(National Bureau of Standards Reports No. 8521, 8595, 8641, 8906,

8992, 9043, 9089, 9374, 9449, 9501, 9553, 9607, 9883, 9968, 10070, and

10291, published during the years 1964 to 1970, U.S. Department of

Commerce, Washington, DC 20234).

This series of reports is a survey of the thermodynamic properties of

selected compounds of biological importance containing the elements

carbon, hydrogen, nitrogen, oxygen, phosphorous, and sulfur. Included

in these reports are heat capacity data; heats and free energies of

formation; vapor pressure data; tables of thermodynamic functions;

Gibbs energies, entropies and enthalpies of solution and dilution; and

thermodynamic properties of mixed solvent systems. References to

sources of data in the literature are included.
Alberty, R. A. I

Standard Gibbs Free Energy, Enthalpy, and Entropy Changes as a Function

of pH, and pMg for Several Reactions Involving Adenosine Phosphates

(Journal of Biological Chemistry, 244 , 3290 (1969))

The standard Gibbs energy, enthalpy, and entropy changes for the hydrolysis

of adenosine-5 1 -triphosphate to adenosine-3 '-diphosphate are computed as

a function of pH and magnesium ion concentration. A critical evaluation

of the relevant literature data is included.

4
Ashcroft, S. J. and Mortimer, C. T. II

Thermochemistry of Transition Metal Complexes

(Academic Press , London, New York, 1970)

This book surveys the literature to 1968 on energy changes for processes

involving transition metal complexes including both organic and inorganic

ligands . A critical review of the thermochemica 1 data for over 1500

systems of complexes is given. Comparable data from various sources are

shown in juxtaposition. Values of AH, AG, and AS for various stages

of complex formation are usually listed for processes in aqueous

solution. .jfl^

0

, ZGj°; -IS^

0 for crystalline complex substances are given

where available. In many instances correlations of the data for various

metals with a single ligand, and for various related complexes of a

given metal, are given graphically or by means of bond-energy estimates

based in the data.

5
Benson, S. W. Ill

Thermochemica 1 Kinetics

Methods for the Estimation of Thermochemical Data and Rate Parameters

(John Wiley and Sons, Inc., New York, London, Sydney, 1968)

This monograph gives tables of necessary data and descriptions of methods

of their use for calculating AH^, Cp, and S, at 25°C for gas phase molecules and radicals and for extrapolating them to higher temperatures.

The procedures can be applied to hydrocarbons, oxygen- containing compounds,

nitrogon-containing compounds, haloalkanes, organo-sulfur compounds, and

organo-metallic compounds; and deal principally with organic compounds.

6
Benson, S. W. , Cruickshank, F. R. , Golden, D. M. , Haugen, G. R.

,

O'Neal, H. E., Rogers, A. S., Shaw, R. , and Walsh, R. Ill

Additivity rules for the estimation of thermochemica 1 properties.

(Chem. Rev. 69, 279-324 (1969))

This lengthy technical article gives procedures for calculating the

properties AH^°, S°, Cp°, for organic compounds in the gas phase.

Parameters for calculating Cp are given for temperatures from 300 to

1500 K at intervals. The availability of Cp at T allows calculation of

AHj; 0 and S° at the same temperatures. The necessary constants for

making the calculations are given for individual chemical groupings in

some 38 tables. Many classes of functional groups and molecular conformations are included. Examples are given comparing calculated and

observed values. Agreements of 1 kcal mol ^ or less in AH^ 0 and 1 cal

mol ^ or less in Cp° and S° are generally found.

7
Bondi, A. iiJPhysical Properties of Molecular Cyrstals, Liquids, and Glasses

(John Wiley and Sons, Inc., New York, London, Sydney, 1968)

This monograph is designed for the use of chemical engineers to estimate

physical properties needed in design calculations, as well as of physical

chemists and synthetic chemists who need to understand the relationship

between structure and physical properties. Correlations of several kinds

are described in the text. These are then restated as methods for estimation

of the properties.

Substances considered include non-polar and polar gases, non-polar and

polar liquids, associated liquids, crystalline solids, glasses, polymers,

and polymer melts, as well as others. Procedures given include many

variants, depending upon the properties given as initial information.

Among the properties for which procedures are given are: density, heat

capacity, enthalpy, entropy, enthalpy and entropy of fusion, enthalpy of

sublimation and vapor pressure, cubical thermal expansion coefficient,

bulk modulus, Young's modulus, compressibility, thermal conductivity,

rotational diffusion constant, relaxation times, mass diffusion, viscosity, and others.

8
Brown, H. D. (editor) I

Biochemical Microcalorimetry

(Academic Press , New York, London, 1969 ,

This book contains seventeen articles on subjects concerning heat measurements and their relationship to biology and biochemistry. Several of

the articles contain tabulations of data:

Title of Article Author (s)

Thermodynamic Properties of Biochemical R. C. Wilhoit

Substances

This review includes several tables: (1) Selected values of thermodynamic properties (AHf°, £Gf°, S°, and Cp°) for ^120 important

biochemical species or compounds; (2) Enthalpies and Gibbs energies of

formation of adenosine phosphoric acid species relative to H2ADP-I at

25°C; (3) AH° and £G° for six important biochemical processes; and

(4) Partial molal properties (L2, L^, C2, and C^) of glucose,

glycerol, glycine, and urea at 25°C.

Chemical Structure and Reactions of Carbohydrates S. Ono and K. Takahashi

This article has a table of enthalpies of isomerization of eleven car- bohydrates and a table giving enthalpies of hydrolysis of a-1,4 and

a-1,6 glucosidic linkages in several glucosides at 25°C.

Physical States of Biomolecules : Calorimetric T. Ackermann

Study of Helix-Random Coil Transitions in Solution

There is a tabulation of calor imetr ical ly determined enthalpy values

accompanying conformational changes of macromolecules in solution

(26 articles).

Calorimetry of Enzyme-Catalyzed Reactions H. D. Brown

Tabulated are calorimetric enthalpy values for enzyme catalyzed

systems (21 articles).

9
Chapman, T. W. and Newman, J. Ill

A Compilation of Selected Thermodynamic and Transport Properties

of Binary Electrolytes in Aqueous Solution

(Lawrence Radiation Laboratory, UCRL-17767, Berkeley, California, 1968)

Data from the literature on the properties of sixty-one common binary

inorganic electrolytes at various temperatures are tabulated with appropriate references. The properties include the density, viscosity,

transference number, diffusion coefficient, and the activity coefficient.

10
Chris te risen, J. J. and Izatt, R. M. II

Handbook of Metal Ligand Heats and Related Thermodynamic Quantities

(Marcel Dekker, Inc., New York, 1970)

This handbook gives tabulated values of thermodynamic functions in aqueous

solution. Enthalpies are given for equilibria involving metal ions and

ligands, together with the related thermodynamic quantities, log KA AS,

and ACp, where available. The body of the book consists of a table

(192 pp) in which are summarized the published literature values up to

1969, classified according to ligand. In addition, the appropriate

reaction, the temperature, the method, and conditions of measurement of

AH are given. Both inorganic and organic ligands, and complexes of

about seventy metallic elements are given. A seven page guide to the

use of the table and indexes is given.

The table is indexed by author, by ligand formula, and by metal. An

index of synonyms and a chronological list of references are also given.

11
Clark, W. Mansfield I

Oxidation-Reduction Potentials of Organic Systems

(The Williams and Wilkins Company , Baltimore, 1960)

This 584 page monograph contains a comprehensive discussion on the

determination of the electrochemical potentials of organic systems with

emphasis both on theory and experimental practice. Included are approximately 100 tables of critically evaluated oxidation and reduction potentials

for organic and biochemical systems thru circa 1960. Included are the

quinones, phenols, anilines, porphyrins, NAD, and NADP systems, and

several others. The author has, in most cases, specified the conditions

to which the data refer.

12
Conway, B. E. II

Electr ocherr.ical Data

(Elsevier Publishing Company, New York, 1952)

This monograph is a comprehensive (359 pp) collection of data on various

aspects of pure and applied electrochemistry, relating to organic and

inorganic substances, both solid and in solution. All data are presented

in tabular form, organized into ten chapters, each introduced briefly by

the author, with references to all data sources and short explanations

of approach. A chapter on physical properties includes tables of densities

and vapor pressures of various aqueous solutions, dielectric constants

and dipole moments and other properties. Relative partial molal enthalpies

and activity and osmotic coefficients are tabulated in Chapter III, on

molecular and ionic interaction in the liquid phase, followed by a

section on transport in solutions of strong electrolytes, which includes

lists of conductance values, ionic mobilities, transference numbers and

diffusion coefficients. A chapter on dissociation constants, solubilities,

and buffer solutions also includes instructions for the preparation of

12 buffer solutions. The chapter on properties of electric double

layers contains tables of e lectrokinetic potentials and properties of

various interfaces including ones of such biological interest as the

mammalian red blood cell. The biologist would also find relevant the section

on transport and general properties of colloids and macromolecular

electrolytes, including extensive tables of mobilities for such compounds

as hemoglobins, serum albumins, and red blood cells, among others.

With the exception of the chapter on the electrochemistry of melts,

13
which deals primarily with electrochemical parameters of molten and fused

salts and various oxides, the final third of the book concerns electrode

chemistry. Chapter IX is a compilation of data on reversible electrode

processes, including listings of liquid junction potentials, half -cell

potentials, and electrochemical equivalents for certain elements.

Chapter X is titled, "Parameters of electrode kinetics" and represents

a critical selection of the available determination of the parameters

of a number of electrode reactions.

14
Cox, J. D. and Pilcher, G. II

Thermochemistry of Organic and Organometa 1 lie Compounds

(Academic Press, London, New York, 1970)

This monograph is a critical compilation of thermochemica 1 data published

since 1930. The enthalpies of formation of some 3000 substances are

listed, with estimates of error. Where enthalpies of vaporization are

known or can be reliably estimated these are listed and in these cases

the enthalpies of formation of both gaseous and condensed phases are

given. Extensive introductory material presents experimental procedures

and procedures for reduction of experimental data of the type found in

the book. Applications of thermochemical data are given, and there is

a section on methods of estimating enthalpies of formation of organic

compounds

.

15
Domalski, E. S.

Selected Values of Heats of Combustion and Heats of Formation of

Organic Compounds Containing the Elements C, H, N, 0, P, and S.

(Journal of Physical and Chemical Reference Data 1, 221-277 (1972))

Selected values of the enthalpies of combustion and enthalpies of

formation of 719 organic compounds are reported. The selected values

are augmented by commentary and original source references. The

Wiswesser Line Notation is also given for each compound. The methods

used in updating older work are described.

16
Florkin, M. and Mason, H. I

Comparative Biochemistry, Volume II

Free Energy and Biological Function

(Academic Press, New York, London, 1960)

This book contains several chapters dealing with the use of Gibbs energy

data in biochemistry. The following chapters contain references to and/or

tabulations of thermochemica 1 data:

M. R. Atkinson and R. K. Morton, "Free Energy and Biosynthesis of

Phosphates". This chapter contains a tabulation of Gibbs energies and

equilibrium constants for various metabolic processes involving phosphates. The temperature, pH, magnesium ion concentration, and

appropriate literature references are given.

L. F. Leloir, C. E. Cardini, and E. Cabib, "Utilization of Free Energy

for the Biosynthesis of Saccharides". Included in the discussion are some references to equilibrium data relevant to the biosynthesis of

saccharides

.

P. P. Cohen and G. W. Brown, Jr. , "Ammonia Metabolism and Urea Biosynthesis". In their discussion of ammonia metabolism, the authors have

used other compilations of thermodynamic data to compute Gibbs energy

changes for these processes.

17
Fox, D., Labes, M. M. , and Weissberger, A. (editors)

Physics and Chemistry of the Organic Solid State

(Interscience Publishers (Wiley), 1963)

Chapter 1. Thermodynamics of Crystals

E. F. Westrum and J. P. McCullough

In addition to discussion of thermodynamic properties of organic

substances and their measurement, this chapter (178 pp) gives tables

of entropy of fusion, and vapor pressures and a table of thermodynamic

data sources for about 800 organic compounds (798 references).

18
Hamer, W. J. and Wu, Y. C.

Osmotic Coefficients and Mean Activity Coefficients of Uni-univa lent

Electrolytes in Water at 25°C

(Journal of Chemical Reference Data, 1, 1047 (1972))

This evaluation gives values for the osmotic coefficients and mean

activity coefficients of 79 uni-univa lent electrolytes in aqueous

solution at 25°C, with values expressed on the molality scale. The

data from the literature were fitted, by statistical procedures, to

equations which express the quantities as functions of electrolyte

concentration. Literature references are given to 51 additional uniunivalent electrolytes.

19
Harned, H. S. and Owen, B. B. Ill

The Physical Chemistry of Electrolytic Solutions

(Reinhold, Publishing Corporation, New York, 1958)

This book (^ 800 pp) is a treatise on the physical chemistry of

electrolytic solutions with coverage of both equilibrium and nonequilibrium properties. The book includes tables of values of the

equivalent conductance, dissociation constants, transference numbers,

diffusion coefficients, relative apparent molal heat contents, activity

coefficients, pH values, densities, and activity coefficients for

many of the more common inorganic and organic electrolyte solutions.

20
Izatt, R. M. , Christensen, J. J., and Rytting, J. H. I

Sites and Thermodynamic Quantities Associated with Proton and Metal

Ion Interaction with Ribonucleic Acid, Deoxyribonucleic Acid, and Their

Constituent Bases, Nucleosides, and Nucleotides

(Chemical Reviews, 71, 439 (1971))

This review contains twenty-three journal pages of tables of

thermodynamic data (log K, AH, AS, and ACp) pertinent to the interaction

of protons and metal ions with the nucleic acids and their molecular

components together with the methods and experimental conditions (pH,

temperature, ionic strength) used in their determination. There are 229

references to articles in the literature.

21
Janz, G. J. Ill

Thermodynamic Properties of Organic Compounds

Estimation methods, principles, and practice (revised edition)

(Academic Press, Inc., New York, London, 1967)

This well established monograph discusses computation of thermodynamic

properties such as heat capacities, entropies, enthalpies and Gibbs

energies by statistical mechanical methods, by methods of structural

similarity, by methods of group contributions, by methods of group

equations, and by methods of generalized vibrational assignments.

The chemical properties: enthalpy of formation, and enthalpy of combustion are treated in terms of bond energies and group increments.

Some 78 tables are given of increments, group contributions, and bond

contributions as specifically needed for estimation of particular

properties

.

22
Jordan , T. Earl III

Vapor Pressure of Organic Compounds

(Intersc ience Publishers, Inc., New York, 1954)

A comprehensive compilation (266 pages) of vapor pressure data for

organic compounds. Included are tables on the hydrocarbons, alcohols,

aldehydes, esters, ketones, acids, phenols, and metal organic compounds.

Data for each compound are shown in graphical form, i.e. vapor pressure

as a function of temperature. References to the data sources in the

literature are given.

23
Joshi, R. M. and Zwolinski, B. J. II

Vinyl Polymerization, Volume 1, Part I, edited by G. E. Ham

(Marcel Dekker, Inc., New York, 1967)

Chapter 8: Heats of Polymerization and their Structural and

Mechanistic Implications

The authors discuss experimental methods used to measure and derive

heats of polymerization. A listing of experimental data on heats of

polymerization is provided for 81 organic polymerization reactions.

Other tables give heats of formation, heats of vaporization, entropies,

Gibbs energies, equilibrium constants, rate constants and activation

energies at 25°C for a variety of polymerization processes. A discussion

of the structural influence upon the heat of polymerization is also

given. At the end of the chapter, 164 references are cited.

24
Kortum, G. , Vogel, W. , and Andrussow, K. II

Dissociation Constants of Organic Acids in Aqueous Solution

(Butterworths, London, 1961)

This book is a compilation of 1056 dissociation constants of organic

acids in aqueous solution, presented in tabular form. Introductory

and explanatory remarks are in both German and English. Remarks in the

Table are in German. Part I is a critical discussion of techniques for

measurement of dissociation constants by conductance, electrometric,

catalytic and optical methods. Each method is classified and coded in

Part II, on use of the table, where methods of calculation and corrections

for solvent and for hydrolysis of salts in conductivity measurements are

also coded, for reference in the table. The Table itself is arranged by

acid class including: aliphatic and alicyclic carboxylic acids, aromatic

carboxylic acids, phenolic acids, and other acids and special classes.

The Table gives the name, chemical formula, and thermodynamic dissociation

constant K of each acid, the temperature (°C) of measurement, the range of

concentration over which the measurements were made, code for the method

of measurement, calculation procedure, and any corrections made, a

critical evaluation of the quality of the measurement, and the source

reference. All data were drawn from the literature, covering the

period between 1927 and 1956, and are referenced in a classified reference

list. A compound index is provided.

25
Krebs, H. A. and Romberg, H. L. , with appendix by K. Burton I

Energy Transformations in Living Matter

(Springer-Verlag, Berlin, 1957)

The main part of this monograph surveys the various biochemical pathways

by which living systems utilize energy. In the Appendix are (1) Tables

of Gibbs energies of formation of ninety-eight compounds of biological

importance, (2) Gibbs energies and electrochemical potentials of important

biological oxidation-reduction reactions, and (3) Gibbs energy changes

accompanying the processes of glycolysis and alcoholic fermentation,

the tricarboxylic acid cycle, and of hydrolysis. The source of data

is given for each entry.

26
Lange, E. Ill

Heats of Dilution of Dilute Solutions of Strong and Weak Electrolytes

in "The Structure of Electrolytic Solutions" (W. J. Hamer, editor)

(John Wiley and Sons, Inc., New York, 1959)

A discussion of the theoretical interpretation and calculation of heats

of dilution of electrolytes of various charge types with some information

on non-electrolytes and weak electrolytes. Data from the literature are

presented in graphical form. Included are data for eighteen inorganic

electrolytes and seven inorganic non-electrolytes. Data refer to 25°C.

27
Larson, J. W. and Hepler, L. G. II

Heats and Entropies of Ionization

in Solute-Solvent Interactions, J. F. Coetzee and C. D. Ritchie (editors)

(Marce 1-Dekker , New York and London, 1969)

This chapter is a detailed review and evaluation of the enthalpies,

Gibbs energies, entropies, and heat capacity changes accompanying

ionization of aqueous acids. Included are eleven tables of data on

various types of acids, including the carboxylic acids, phenols, anilinium

ions, ammonium ions, the amino acids, barbituric acids, and several

inorganic acids. The authors also discuss the interpretation of the data

in terms of molecular considerations. The tabulated data refer to 25°C

and standard state conditions. There are 224 references.

28
Latimer, W. M. II

The Oxidation States of the Elements and their Potentials in Aqueous Solution

Second edition

(Englewood Cliffs, New Jersey: Prentice-Hall, Inc., 1959)

Although orginally published in 1938 the second edition copyrighted in

1952, still stands as a comprehensive (392 pp) and useful text for the

worker interested in a summary of existing data on energy levels of the

elements in their various oxidation states. Written in narrative form,

organized into 23 chapters with 4 appendices and an author and subject

index, the text is augmented by numerous graphs, charts, formulae, and

solved methematical problems. For each element the enthalpies of

formation, Gibbs energies of formation and entropies have been tabulated

for important compounds. A preliminary chapter discusses general methods

by which the Gibbs energy data have been obtained, and gives references

to more detailed treatments. A second chapter is devoted to values for

the ionization potentials and the electron affinities of the elements,

and their relationship to the oxidation-reduction potentials of the

elements and their compounds in their standard states. The remainder of

the text is devoted to a systematic review of each element. For each

element is given a brief introductory passage, noting number of valence

electrons and electronic states., f ollowed by more detailed discussions of

oxidation states, E° values for relevant couples, and useful potential

diagrams of potentials in acid and base solution. For quick reference,

approximately 400 oxidation-reduction couples are listed in Appendix I,

with the couples arranged in order to decreasing E° values, and divided

into those in acid solutions, and those in basic. Appendix II includes

a list of activity coefficients for 77 strong electrolytes, and Appendix

29
Ill is a discussion of methods by which estimates of entropy values we

made, where necessary. A group of study problems in Appendix IV is

meant to be particularly useful to the student and/or instructor, who

might wish to use the book in conjunction with a course.

30
Linke, W. F.

Solubilities: Inorganic and Metal-Organic Compounds- -A Compilation of

Solubility Data from the Periodical Literature. Volume I: A-Ir,

Volume II: K-Z

(Volume I: D. Van Nostrand Co., Princeton, New Jersey, 1958;

Volume II: American Chemical Society, Washington, DC, 1965).

These two volumes (total of 3401 pages) are comprehensive compilations

of unevaluated solubility data for inorganic and metal-inorganic compounds. Both aqueous and non-aqueous solvent systems are included.

References are given to the data sources.

31
Long, Cyril (editor) I

Biochemists Handbook

(D. Van Nostrand Co., Princeton, New Jersey, 1961)

This reference book contains several tables of thermochemical data:

"pH and Acid-Base Equilibria" S. P. Datta and A. K. Grzybowski

This chapter contains a discussion of pH scales and the electrometric

measurement of pH, tables of assigned pH values for various buffered

solutions, and tables ( ^600 entries) of thermodynamic acid dissociation

constants of weak organic acids (some as a function of temperature).

"Free Energy Data and Oxidation-Reduction Potentials" K. Burton

This chapter contains some revisions and additions to Burton's earlier

tables (see, in this bibliography, the book by Krebs and Romberg).

32
Meites, L. (Editor) II

Handbook of Analytical Chemistry

(McGraw-Hill Book Co., New York, 1963)

This treatise on analytical chemistry contains several useful tabulations

of the rmochemical data. Several of these tabulations are taken directly

from other sources cited in this bibliography and are not included below:

Title of Section Author (s)

Equilibrium Constants of Proton- V. E. Bowers and

transfer Reactions in Water R. G. Bates

Tabulated are pK values at 15, 25, and 35 °C for ^200 organic and

inorganic acids; no literature references are given.

Formal Equilibrium Constants of Protontransfer Reactions at Finite Ionic Strength L. Meites

This section contains a tabulation of pK values at 25 °C for a selected

series of vL50 acids, and bases. This data was taken from Bjerrum,

Schwarzenbach, and Sillen, "Stability Constants of Metal Complexes",

part I, Chemical Society, London, 1957. Also given are tables of

acid dissociation data pertinent to ethanol-water and methanol-water

mixtures

.

Formation Constants of Metal Complexes D. A. Aikens and

C. N. Reilley

Tabulated are log K values for the binding of the more common inorganic

metal ions to 55 ligands. AH and AS values are also given for four

ligands. Literature references are given.

33
Merrill, A. L. and Watt, B. K. I

(a) Energy Value of Foods; Basis and Derivation

Agriculture Handbook No. 74, 1955.

(b) (Watt, B. K. and Merrill, A. L.)

Composition of Foods; Raw, Processed, Prepared

Agriculture Handbook No. 8, revised, 1963

(U.S. Government Printing Office, Washington, DC 20402)

This pair of monographs provides numerous composition and energy values

for food and foodstuff ingredients. It should be noted, of course, that

the Calorie used in food energy values is 1 kcal as used in thermochemistry.

In Agriculture Handbook No. 74, Part I gives a discussion of the sources

of food energy in terms of organic compound class, and of the experimental determination of heats of combustion. Parts II, III, and IV

apply the data to physiological processes. An appendix gives

composition and heat of combustion of foods. Tables 1-5 and table 24

give heats of combustion of specific food items or component substances.

Care should be used in taking values from the numerous tables, as correction

factors have sometimes been applied to adjust for physiological processes.

These adjustments are indicated by footnotes. In Agriculture Handbook

No. 8, Appendix A is of particular interest as it gives notes on energy

values and nutrients, including (adjusted) heats of combustion of many

foods and food ingredients.

34
Miller, D. G. Ill

Application of Irreversible Thermodynamics to Electrolyte Solutions.

I. Determination of Ionic Transport Coefficients for Isothermal

Vector Transport Processes in Binary Electrolyte Systems. II. Ionic

Coefficients Jly for Isothermal Vector Transport Processes in Ternary

Systems

.

(Journal of Physical Chemistry, 70, 2639 (1966); 71, 616 (1967)).

These papers derive equations relating fundamental isothermal transport

coefficients (J^j's) to experimentally measurable quantities for electrolytes in a neutral solvent. ^i j

' s f°r tne most common aqueous ionic

solutions are calculated from critically reviewed data.

35
Millero, F. J. Ill

The Partial Molal Volumes of Electrolytes in Aqueous Solutions.

Compilation of the Partial Molal Volumes of Electrolytes at Infinite

Dilution, V° , and the Apparent Molal Volume Concentration Dependence

Constants, S* and b , at Various Temperatures.

Water and Aqueous Solutions, R. A. Home (editor)

(Wiley-Interscience , New York, 1972)

Two chapters in this book are concerned with the measurement and interpretation of partial molal volumes and their concentration and temperature dependences. Included are tables of the partial molal volumes

of the common inorganic and organic electrolytes (^200 systems) as

well as values of the partial molal volumes of the more common inorganic

and organic ions (^100 species). The data refer to temperatures from

0 to 200°C.

36
Mishchenko, K. P. and Poltoratzkii, G. M.

Aspects of the Thermodynamics and Structure of Aqueous and Non-aqueous

Electrolyte Solutions

(Izd. "Khimia", Leningrad, 1968) (In Russian)

This 350 p. monograph contains extensive discussions and correlations

(theoretical and empirical) of existing experimental data on enthalpies,

Gibbs energies, and entropies, of solution and ionization of inorganic

acids, bases, and salts in water and selected organic solvents. Heat

capacities, enthalpies, Gibbs energies, and entropies of the substances

and their ions in solution are also discussed. Extensive use is made

of diagrams relating observed properties to periodic groupings of the

elements. The monograph contains numerous small tables of properties

of limited groups of substances. A summary compilation of selected

values of thermodynamic properties occupies 43 pages, giving AHf,

Z^Gf, S and Cp of pure and dissolved inorganic substances in their

standard states at 25°C, selected enthalpies of solution at 25°C,

enthalpies of dilution of common acids, bases, and salts at 25°C, and

heat contents and partial molar heat capacities for selected salts vs.

concentration and temperature in water, methanol, ethanol, and a few

other organic solvents.

37
Parker, V. B. Ill

Thermal Properties of Aqueous Uhi-univalent Electrolytes

(NSPvDS NBS 2, U.S. Government Printing Office, 1965)

This short (41 pp) monograph is a review of the heat-capacity, enthalpy

of solution, and enthalpy-of-dilution data on simple 1-1 electrolytes,

organic and inorganic, in dilute, aqueous solutions. From the critical

analysis of this data, tables of selected "best" values of apparent

heat capacities, and enthalpies of dilution are given, as well as

selected values of the enthalpies of solution to the infinitely dilute

solution. Also included is a review of data on the enthalpies of

neutralization of monobasic acids which has led to a selected "best"

value for the enthalpies of ionization of water. Data on each parameter

are introduced with a discussion of methods employed in reducing the

data to a standard form and are listed by compound, in the order: acids,

ammonium and amine salts, silver salts, and salts of the alkali metals.

For each compound are listed the various investigations, with the

temperature and range of concentrations measured. Graphs of molal

heat capacity and molal enthalpy as functions of concentration are also

included, for aqueous solutions of many of the compounds discussed.

In addition, there is an abb reviated listing, by compound, of review

and compilation papers on the thermal properties of the aqueous uniunivalent electrolytes. These and other references are also listed

alphabetically in a separate reference section with 652 entries. The

chosen "best" values for each parameter and compound are arranged in a

series of 21 tables, for T = 25°C.

38
Pauling, L. Ill

The Nature of the Chemical Bond, 3rd edition

(Cornell University Press, Ithaca, New York, 1960)

This well established monograph provides general information about the

nature of chemical bonding in (principally) inorganic compounds which

is fundamentally very important for the estimation of enthalpies of formation, but not always easily applied.

39
Perrin, D. D. II

Dissociation Constants of Inorganic Acids and Bases in Aqueous Solution

(Butterworths, London, 1969).

This short (163 pp) monograph is a compilation of dissociation constants

of 217 inorganic acids and bases. The classes of compounds include not

only conventional acids and bases, but also hydrated metal ions and free

radicals, such as hydroxyl, the only criterion being gain or loss of a

proton or hydroxyl ion. The data are organized into a single table

listing 217 compounds, preceeded by a brief introduction to the use of

the table, and a section on methods of measurement and calculation.

The methods are classified as conductome trie , e lectrometric , optical,

or other. Elements and compounds are listed in decreasing extent of

protonation. pK values are, wherever possible, obtained by extrapolation

to ionic strength 1=0. The table also gives tha temperature of each

measurement, remarks as to ionic strength, concentration, and any other

factors relating to pK, coded references to method of measurement, the

procedure used in evaluating the constants and any corrections taken

into consideration, and the literature references. There are

approximately 1100 references listed alphabetically by author.

40
Perrin, D. D. II

Dissociation Constants of Organic Bases in Aqueous Solution

(Butterworths , London, 1965)

Published in the same series as the book by Kortum, Vogel, and Andrussow,

this book tabulates values of dissociation constants for organic bases

in aqueous solution. The bases are arranged under the headings aliphatic,

alicyclic, aromatic, heterocyclic, natural products, dyes and indicators,

substances lacking a basic nitrogen atom, and miscellaneous. Accompanying

the data entry for each base is the temperature, method of measurement,

formula, assessment of the measurement, and the appropriate reference.

There are 3790 data entries in this book.

41
Phillips, R. C, George, P., and Rutman, R. J. I

Thermodynamic Data for the Hydrolysis of Adenosine Triphosphate as a Function of pH, Mg^+ Ion Concentration, and Ionic Strength

(Journal of Biological Chemistry, 244 , 3330 (1969))

This article deals with the computation of the Gibbs energy change for

the hydrolysis of adenosine-5 1 -triphosphate to adenosine-5 1 -diphosphate

as a function of magnesium ion concentration, pH, and ionic strength.

A critical evaluation of the existing data pertinent to this computation

is included. References to 24 papers are given.

42
Reid, Robert C, and Sherwood, T. K. Ill

The Properties of Gases and Liquids, their Estimation and Correlation,

2nd edition

(McGraw Hill Book Co., New York, etc., 1966)

This lengthy monograph follows the procedure of discussing various methods

available for calculating or estimating particular properties of particular

materials, and then provides recommendations for action with respect to

each kind of property. Included in the book are procedures for making

estimates of critical constants, normal boiling temperatures, LennardJones-potential parameters, compressibility factors and equations of

state, liquid molal volumes and densities, and vapor pressures. Estimates

of enthalpies of vaporization, and of ideal-gas heat capacities, enthalpies

and Gibbs energies of formation are treated. For real fluids variations

of enthalpy, entropy, internal energy, and heat capacity with pressure

are treated. Some methods are given for estimating the properties of

fluid mixtures. Surface tension and the transport properties—viscosity,

diffusion coefficient and thermal c onduc t ivity--are discussed. Numerous

tables present comparisons of observed and calculated properties.

43
Robinson, R. A. and Stokes, R. H.

Electrolyte Solutions, The Measurement and Interpretation of Conductance

Chemical Potential and Diffusion in Solution of Simple Electrolytes,

second edition (revised)

(Butterworths, London, 1965)

In this, the revised second edition of a monograph first published in

1955, the authors have approached their subject in terms of those

fundamentals which distinguish or characterize aqueous organic and

inorganic electrolyte solutions. Included in the text is a discussion

of properties of ionizing solvents (ie . water), and electrolytic conductivities and transport numbers. The measurement and theoretical interpretation of chemical potentials are treated in some depth, as is the

theory of diffusion, emphasizing conductance and diffusion, in relation

to viscosity in concentrated solutions, and methods of measurement of

diffusion coefficients. The final third of the text deals primarily

with characteristics of specific electrolyte solutions, including weak

and mixed electrolytes, and strong acids, and includes an extensive

(98 pp) appendix of approximately 75 tables of osmotic and activity

coefficients, standard cell potentials (E°) in various organic

solvents, ionic radii, and ionization constants of organic acids in

aqueous solution, among others. The narrative is heavily supplemented

with graphs, tables, equations, and an occasional derivation, all

referenced at the end of each of the 15 chapters.

44
Rossini, F. D., Pitzer, K. S., Arnett, R. L. , Brown, R. M. , and

Pimentel, G. C.

Selected Values of Physical and Thermodynamic Properties of Hydrocarb

and Related Compounds

(Carnegie Press, Pittsburgh, Pennsylvania, 1953)

This monograph resulted from the work of American Petroleum Institute

(API) Research Project 44. Values are given for 40-odd physical and

thermodynamic properties of several hundred hydrocarbons in metric

and U.S. Customary units. The data in most instances represent

selected values from careful studies, many of which were done in

connection with the same API Research Project. Experimental data are

supplemented by theoretical calculations or empirical correlations.

References to the source data and a bibliography are given. The

data in many instances are identical to those in NBS Circular C461,

listed below.

45
Rossini, F. D. , Pitzer, K. S., Taylor, W. J., Ebert, J. P., II

Kilpatrick, J. E., Beckett, C. W. , Williams, M. D., and Werner, H. C.

Selected Values of Properties of Hydrocarbons

National Bureau of Standards Circular C461 (1947)

(U.S. Government Printing Office, Washington, DC)

This monograph was prepared as part of the work of the American Petroleum

Institute (API) Research Project 44. Values are given for some 36

physical and thermodynamic properties of several hundred hydrocarbons

in metric and in U.S. Customary units. The data in most instances

represent values found from careful studies, many of which were done

in connection with the same API Research Project. Experimental data

are supplemented by theoretical calculations or empirical correlations.

References to the source data and a bibliography are given. The data •

in many instances are identical to those in the Carnegie Press publication

by Rossini et al listed above.

46
Rossini, F. D. , Wagman, D. D. , Evans, W. H. , Levine, S., and Jaffe I. II

Selected Values of Chemical Thermodynamic Properties

National Bureau of Standards Circular 500 (1952)

(U.S. Government Printing Office, Washington, DC 20402)

This was for many years the most comprehensive authoritative compilation

of thermochemical data at 298.15 K for inorganic substances. All inorganic

substances and organic substances containing two carbon atoms or fewer

per molecule are included if thermodynamic data exist for calculating

one of the properties tabulated. Properties tabulated in Part I are

£H

f °,, AHf

° 9g , AJ

f

° 9g , log K

f , S°

9g

, and C

p

° 9g

. Properties tabulated

in Part II are temperature, pressure, enthalpy change, entropy change

and heat capacity change for the phase changes: transition, fusion, and

vaporization. The data from original sources were critically evaluated

by competent thermochemis ts and best values selected for the functions

tabulated, maintaining internal consistency by the relationship:

^f298

= ^f298 ~ ^^298'

^e sources °^ data for each data item are

listed and a bibliography is included. Some information in this book

can still not be found readily elsewhere as the revision is not yet

complete. Also, see Wagman et a_l in this bibliography.

47
Schafer, D. and Lax, E. (editors) II

Land olt-Borns te in

Zahlenwerte und Fuctionen aus Physik, Chemie, Astronomie,

Geophysik, und Technik, Sechste Auflage

Eigenschaften der Materie in Ihren Aggregatzustanden

4 Teil, Kalorische Zustandgrossen

(Spring-Verlag, Berlin, Gottingten, Neidelberg, 1961)

This most recent issue of thermodynamic information of the LandoltBornstein series gives thermal properties: molar heat capacity, entropy,

enthalpy, enthalpy of formation, Gibbs energy of formation, in the standard

state, and enthalpies of phase changes for many organic and inorganic

substances in SI units. The dependence of thermal functions and heat

capacity upon temperature is given for many substances. Some other

thermodynamic quantities are given. Extensive tables are given of group

contributions to enthalpy of formation and the Gibbs energy of

formation of organic substances (gases) in kcal mol ^ and kJ mol .

Many of the heat capacity data are presented in diagrams.

48
Sillen, L. G. and Martell, A. E. II

Stability Constants of Metal Ion Complexes, Section I: Inorganic

Ligands, Section II: Organic Ligands, second edition

(Special Publication No. 17, The Chemical Society, London, England,

1964 and Supplement No. 1, Special Publication No. 25, 1971)

With the publication of this second edition of Stability Constants, the

Chemical Society combined two previously separate volumes into one, twopart volume (754 pages), the first covering constants of inorganic

ligands, the second, organic ligands. Both sections include all data

published up to the end of 1960 and some from 1961-63; the scope of the

inorganic section has been extended to cover redox equilibria and the

extraction of inorganic ligands into non-aqueous solvents. The data

are organized into two separate tables, each table summarizing the data

for the association of one particular ligand with all the metallic ions

which have been studied in conjunction with it. Method of measurement,

composition, and temperature of the media to which the data refer, are

given for each ligand-metal pair. Acid dissociation constants of the

ligands are recorded by including the hydrogen ion as one of the cations

with which the ligands associate. Redox equilibria are represented

by including the electron as a ligand, and hydrolysis of metallic ions

is described by regarding the hydroxyl ion as one of the ligands.

The arrangement of material is now more uniform than in the two parts

of the first edition, but there remain minor differences of presentation

between the inorganic and the organic section. In the inorganic table,

80 ligands are ordered according to group in the periodic system; metal

ions are arranged within each inorganic ligand table, in the same order.

In the organic section, the ligands (1028) are in order of their

49
empirical formulae, and the metallic ions in the alphabetical order of their

international symbols. Methods of measurement are highly variable, with

42 separate methods alphabetized and coded in the introduction; medium

is usually aqueous. Equilibrium constants are given in both tables.

The organic section includes consecutive or stepwise constants, K,

whenever possible, and cumulative or gross constants, Bn , if they are

the only quantities determined, or if the sequence of stepwise constants

is incomplete. The inorganic table includes equilibrium constants for

consecutive and cumulative reactions, solubility constants, acid

constants and base constants. Certain special constants are also

given; e.g. Kp - equilibria involving a gas. Both tables give enthalpy

and entropy changes, and symbols relating to the references which are

listed at the end of each table. Each of the metals, inorganic, ligands

and organic ligands are indexed alphabetically, with appropriate table

number, at the end of the book.

This supplement to the second edition of "Stability Constants of Metalion Complexes" is a review of pertinent literature published between

the completion of the 1964 Tables and the end of 1968, including also

some data published before the completion of the 1964 Tables, but omitted

from them. In the organic part, a change of policy has been initiated;

rather than being omitted, results seeming incomplete or of dubious

validity are now included in the tables, with critical comments. The

section "How to use the tables" has been brought up to date; a few

methods have been added. Limits of error are now sometimes given.

A new feature of the organic section is a Functional Group Index,

covering also the 1964 Tables, and a table of 34 macromolecular organic

ligands, including albumin, DNA, RNA, and insulin.

50
Sober, H. A. (editor) I

Handbook of Biochemistry - Selected Data for Molecular Biology

(The Chemical Rubber Co., Cleveland, 1968) (See also 2nd edition, 19 70)

This compendium contains the following twenty-three tables of thermochemical data. The same tables, some containing additional information are

in the second edition (indicated in parentheses).

Tab le Author or Source

Coefficients of Solubility Equations From "The Chemistry of the Amino

of Certain Amino Acids in Water Acids and Proteins", C.L.A.

Schmidt (editor), Charles C.

Thomas Co., Springfield, IL.

Solubility data for 34 amino acids are fit to equations giving the

solubility as a function of temperature.

Heat Capacities, Absolute Entropies, and J. 0. Hutchens

Entropies of Formation of Amino Acids and

and Related Compounds

Cp°, S°, and Z^S° at 25°C are tabulated for 28 amino acids, 3 peptides,

4 proteins, and 3 related substances.

Heats of Combustion, Enthalpy and Free J. 0. Hutchens

Energy of Formation of Amino Acids and

Related Compounds

Enthalpies of combustion and formation and Gibbs energies of formation

at 25°C are tabulated for 45 amino acids and related compounds.

Solubilities of Amino Acids in Water at J. 0. Hutchens and

Various Temperatures E. P. Kirby Hade, Jr.

The solubilities of 18 amino acids are tabulated at four different

temperatures from 1 to 40°C.

Heats of Solution of Amino Acids in J. 0. Hutchens

Aqueous Solution at 25°C

The heats of solution for 37 amino acids at 25°C are tabulated

Free Energies of Solution and Standard J. 0. Hutchens

Free Energies of Formation of Amino Acids

in Aqueous Solution at 25°C.

Gibbs energies of solution and formation at 25°C are given for 18

amino acids.

51
Activities of Amino Acids and

Peptides at 25°C

J. 0. Hutchens

Molal activity coefficients at 25°C are tabulated as a function of

molality for 14 amino acids.

Solubility of Fatty Acids in Water from K. S. Markley, "Fatty

Acids-Part I", 2nd edition,

Interscience , New York (1960)

The solubilities of 13 fatty acids in water at five temperatures

from 0 to 60°C are tabulated.

Approximate Solubilities of Water in from K. S. Markley, "Fatty

Saturated Fatty Acids at Various Acids-Part I", 2nd edition,

Temperatures Interscience, New York (1960)

The approximate solubilities of water in thirteen saturated fatty acids

at various temperatures is given.

Solubilities of Simple Saturated from K. S. Markley, "Fatty

Triglycerides Acids-Part I", 2nd edition,

Interscience, New York (1960)

Tabulated are solubilities of five saturated triglycerides in various

non-aqueous solvents and at a variety of temperatures.

Solubilities of Mixed Triacid Triglycer- from K. S. Markley, "Fatty

ides at 25°C Acids-Part I", 2nd edition,

Interscience, New York (1960)

Oxidation-Reduction Potentials, Absor- P. A. Loach

bance Bandsand Molar Absorbance of

Compounds Used in Biochemical Studies

Oxidation- reduction potentials at ambient temperatures for an assortment

of 253 couples frequently encountered in biochemical studies are tabulated

with appropriate references.

Oxidation-Reduction Potentials of R. W. Henderson and T. C. Morton

Hemoproteins and Metalloporphyrins

Tabulated are oxidation-reduction potentials for 241 (282) hemoproteins

and metalloporphyrins at assorted temperatures.

52
Heats of Proton Ionization and

Related Thermodynamic Quantities

R. M. Izatt and J. J. Christensen

This section is an extensive tabulation of enthalpy and entropy changes

and pK values for organic and biochemical systems with 323 (418) references to

the literature.

Ca lorime trie AH Values Accompanying G. C. Krescheck

Conformational Changes of Macromolecules

in Solution

Tabulated are AH values accompanying the conformation changes of 25

macromolecular systems.

Free Energies of Hydrolysis and W. P. Jencks

Decarb oxylation

A discussion is given of standard states appropriate to biochemical

thermodynamics. Tabulated are Gibbs energies of hydrolysis of esters of acetic

acids and related compounds , of thiol esters , amides, phosphates, and

of glycolysis (and of decarboxylation).

Ionization Constants of Acids and Bases W. P. Jencks and J. Regenstein

Given is an extensive tabulation of pK values for ionization of several

hundred acids and bases with 116 (117) references to the literature.

Measurement of pH R. G. Bates

Buffer Solutions R. G. Bates

pH values have been assigned to several important buffer systems.

Properties of Some New Buffers for Good, Winget, Winter, Connolly,

Biological Research Izawa, and Singh, Biochemistry,

5, 472 (1966)

Tabulated are pK values with temperature coefficients and metal-buffer

binding constants for several buffers useful for biological research.

53
Stephen, H. and Stephen, T. II

Solubilities of Inorganic and Organic Compounds (in five volumes)

(Pergammon Press, Oxford, 1963)

This series of five volumes (circa 5500 pages) is a selection from

the literature of data on the solubilities of elements, inorganic

compounds, and organic compounds in binary, ternary, and multi-component

systems. References are given to sources of data in the literature.

The data are unevaluated.

54
Stull, D. R. , Westrum, E. F., and Sinke, G. C. II

The Chemical Thermodynamics of Organic Compounds

(John Wiley and Sons, Inc., New York, London, Sydney, Toronto, 1969)

This monograph is divided into three parts. The first part gives

theoretical basis and principles of thermodynamics and then.. ochemis try

,

some experimental and computational methods used, and some applications

to industrial problems. The second part gives thermal and thermochemica

1

properties in the ideal gas state from 298 to 1000 K. In this section,

the sources of data are listed and discussed and standardized tables are

presented for 918 organic compounds. Values of Cp°, S°, - (G - H°gg)/T,

H° - H°

98 , AHf

°, Z£

f

°, and log Kp are given at 100 K intervals. In

the third section are listed selected values of enthalpy of formation,

entropy, and consistent values of £G^° and log Kp of organic compounds

at 298 K. In excess of 4000 compounds are listed. A very few inorganic

compounds are also found in this book. A chapter very briefly discusses

methods of estimating thermodynamic quantities.

55
Tatevskii, V. M. } Benderskii, V. A., and Yarovoi, S. S. Ill

Rules and Methods for Calculating the Physico-chemical Properties

of Paraf;:inic Hydrocarbons

(Translated from the Russian by M. F. Mullins and edited by B. P. Mullins)

(Pergamon Press, New York, Oxford, London, Paris, 1961)

This monograph is a summary and a consolidation of the results of some

years of work by Tatevskii and others, extending and elaborating some

procedures introduced by Rossini and others. It suffers from ambiguity

of statement which is somewhat distracting, but the methods presented in

it have been attracting increasing attention recently. Properties calculated include: molar volume, molar refraction, vapor pressure,

enthalpy of formation from atoms or elements, Gibbs energy of formation,

and enthalpy of combustion. Three different methods are used. Tables

of constants and illustrations of the accuracy of the methods are given.

56
Wagman, D. D., Evans, W. H. , Parker, V. B., and (in various individual II

parts) Halow, I., Bailey, S. M. , Schumm, R. H. , Churney , K. L.

Selected Values of Chemical Thermodynamic Properties

National Bureau of Standards Technical Note 270, October 1965 (and

continuing)

(U.S. Government Printing Office, Washington, DC 20402)

This technical note is a revision of NBS Circular 500 Part I (see above)

and is issued in parts as segments of the work relating to selected

sequences of elements are completed. The following parts had been

issued as of 1974.

270-1 Tables for the first twenty-three elements in the standard

order of arrangement

270-2 Tables for elements 24-32 —elements in the standard order

of arrangement

270-3 Tables for the first thirty-four elements in the standard

order of arrangement. This table includes thermochemica

1

data for compounds containing one or two carbon atoms.

270-4 Tables for elements 35-53 in the standard order of arrangement.

270-5 Tables for elements 54-61 in the standard order of arrangement.

270-6 Tables for the alkaline earth elements, elements 92-97 in

the standard order of arrangement.

270-7 Tables for the Lanthanide (Rare Earth) elements, elements 62

through 76 in the standard order of arrangement.

The remaining elements will be covered in two or three additional parts

to appear over a period of about two years. Documentation and references

have not yet been issued.

This is the most comprehensive recent compilation in English of critically

evaluated them ochemical data at 298.15 K for inorganic substances. All
inorganic substances and organic substances containing two carbon atoms

or fewer per molecule are included if thermodynamic data exist for calculating any of the properties tabulated. The coverage when complete will

be approximately 12,000 substances. Properties tabulated are AH °, AH °

, ^298' H

298.15~ H

0' S 298' Cp298.15* The data fr °m ori § inal sou *"ces have

been critically evaluated by competent thermochemists and best values

selected for the functions tabulated, maintaining internal consistency by

the relationships £G

f

° 9g

= AH

f

° 9g

- TASj29g , and AH^g - AH

f

° =

E(H298 " H

0

) *

58
Westrum, E. F. (editor)

Bulletin of Thermodynamics and Thermochemistry

(University of Michigan, Ann Arbor, Michigan)

The 16th annual issue appeared in 1973. The Bulletin is a current

awareness bibliography of articles that pertain to thermodynamics and

thermochemistry. The Bulletin is presently divided into sections on

inorganic systems, organic systems, organic systems (mixtures), and,

since 1971, biological and macromolecular systems. Also included

are sections on work in progress at various laboratories, substanceproperty indexes, and bibliographies on books of interest to thermodynamicists. No data values are given.

59
Wilhoit, R. C. and Zwolinski, B. J.

Handbook on Vapor Pressures and Heats of Vaporization of Hydrocarbons

and Related Compounds (API 44 - TRC)

(Thermodynamics Research Center, Texas A and M Research Foundation,

College Station, Texas, 1971)

This handbook gives subject data on 680 hydrocarbons, 95 sulfur compound

and water from 0 to 150°C. It is indexed by compound name, and by boili

point

.

60
Wu, Y. C. and Hamer, W. J. Ill

Electrochemical Data. Part XIV. Osmotic Coefficients and Mean Activity

Coefficients of a Series of Uni-Bivalent and Bi-Univalent Electrolytes

in Aqueous Solutions at 25°C. Part XVT. Osmotic Coefficients and Mean

Activity Coefficients of a Number of Uni-Trivalent and Tri-Univalent Electrolytes in Aqueous Solution at 25°C.

(National Bureau of Standards Reports No. 10052 and 10088, U.S. Department

of Commerce, 1969).

These reports give values for the osmotic and mean activity coefficients

of uni-bivalent , bi-univalent , uni- trivalent , and tri-univa lent electrolytes in aqueous solution at 25°C. In each case, the values tabulated

are those calculated by fitting the literature data to the equation for

the excess Gibbs energy, and represents the best fit to the experimental

data. Literature references are included.

61
nULL1U 1. TnlllUC Hp yA

A p k p T"m An n T 9 Doma Islci. , E, S. 3, 16

riXtveilo A "1 VpriQ ^ 5 o • 33 Fhprt T P 46

A 1 fiPTfv R A A b VuLlG j »i • 11* 47 57

r\llU.L LlootJw IV « or FI r> y\c in M 1 7

3 1 8

nLA mtit.pftL L P T j IV e J_i » Fur r Ul ukLin. awclw aa , fl1 > • T1. •

-\

Ac-hrrnft- 9 T S Clo nr P 42

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46 uaUc , Jx • J X Ron H

p

tqV t i V A 56 ncixtjw , x 57

Rpn c on ^ 1J 6 7 UnctuicL amo v TaT , w • .Jo X19y 61 , V) X R on rM A p. nciLiicci, u o o*

Bowers V. 33 Haiippn C R 7 Brown H D 9 HpnHpfcnn UC11UCJ.QUL1 P UT j 1A.» w # 52

Brown, G. W. 17 QCLJ1CL , J_i « * ' i C VJ Brown, R. M. 45 nun-iitirio , j« vj

«

3SIX Burton K 26 32 XX11 9 1 , z x

,

Cabib, E. 17 i- j6 aw ct , o • S 3

fprrl ini r F 1 7 X / Jarre, x. /, 7

PnPTiTnpn v>ll apuiail y TJ. * WVY 0 Ton -7 C T •j an z , \j • j . 9 9

rhi*T V I U—LOcjfpncipri LCUOCII T T

j « ft XXy<CXj.J-J 11 ? 1 S3 Tonfl/C! T.T P .9 J Cbtir'npv K T, 57 joraan, i. tj. 9 Clark W M x1 z9 JOSul, K« rl. 9/, Z4

Cohen P 0 i 7 MipauriCK, j. c.

.

to/l A

frinnnl 1 v T NT S 3 Romberg, H. L. 9 £ ZD

Conwav B F 1X 3. J tvorLuin, (.7. 9 >; Z J UOX , J . JJ . 15 Krebs, H. A. 26

Crulckshank, F. R. 7 Krescheck, G. C. 53

Datta, S. P. 32 Labes, M. M. 18

62
page

Lange, E. 27

Larson, J. W. 28

Latimer, W. M. 29

Lax, E. 48

Leloir, L. F. 17

Levine, S. 47

Linke, W. F. 31

Loach, P. A. 52

Long, C. 32

Markley, K. S. 52

Martell, A. E. 49

Mason, H. 17

McCullough, J. P. 18

Meites 33

Merrill, A. L. 34

Miller, D. G. 35

Millero, F. J. 36

Mischenko, K. P. 37

Mortimer, C. T. 5

Morton, T. C. 17, 52

Newman , J

.

10

Ono, S. 9

O'Neal, H. E. 7 Owen, B. B. 20

Parker, V. B. 38. 57

Pauling, L. 39

Perrin, D. D. 40. 41

Phillips, R. G. 42

Pilcher, G. 15

Pimentel, G. C. 45

Pitzer, K. S. 45,46

Poltoratzkii, G. M. 37

Regenstein, J. 53

Reid, R. C. 43

Reilly, C. N. 33

page

Reilly, M. L. 33

Robinson, R. A. 44

Rogers, A. S. 7 Rossini, F. D. 45 ,46 ,47

Rutman, R. J. 42

Rytting, J. H. 21

Schafer, D. 48

Schmidt, C. L. A. 51

Schumm, R. H. 57

Shaw, R. 7 Sherwood, T. K. 43

Sillen, L. G. 49

Singh, R. M. M. 53

Sinke, G. H. 55

Sober, H. A. 51

Stephen, H. 54

Stephen, T. 54

Stokes, R. H. 44

Stull, D. R. 55

Takahashi, K. 9

Tatevskn, V. M. 56

Taylor, W. J. 46

Vogel, W. 25

Wagman, D. D. 47,57

Walsh, R. 7 Watt, B. K. 34

Weissberger, A. 18

Werner, H. C. 46

Westrum, E. F. 18,55,59

Wilhoit, R. C. 3,9,60

Williams, M. D. 46

Winget, G. D. 53

Winter, W. 53

Wu, Y. C. 19,61

Yarovoi, S. S. 56

Zwolinski, B. J. 24,60

63
Subject Index

Subject Page

acetic acid esters

hydrolysis

acid constants

see also equilibrium constants

acids, inorganic

ionization

thermodynamics in water and

nonaqueous solvents

neutralization enthalpies

dissociation constants

acids, organic

vapor pressures

dissociation constants

ionization

hydrolysis of esters

decarboxvlation

5 3

50

28, 33

37

38

40, 49, 53

23

25, 32, 33, 49, 5 3 28

53

53

acids, strong

activation energies

polymerization

activity coefficients

inorganic electrolytes

organic electrolytes

strong electrolytes

amino acids

peptides

uni-polvvalent electrolytes

adenosine-5 1 -diphosphate

adenosine-5 ' -triphosphate

albumin

alcohols

vapor pressures

Gibbs energy changes

aldehydes

vapor pressures

44

24

10, 13, 19, 20, 44

13, 19, 20, 44

29, 44

52

52

61

4, 9, 42

4, 9 , 12

13, 50

23

26

23

alicyclic organic bases

dissociation constants 41

64
Subject Page

aliphatic organic bases

dissociation constants 41

alkali metal salts

thermodynamics of solutions 38

amides

hydrolysis 5 3

amino acids

ionization thermodynamics 28

solubilities 51

heat capacities, entropies 51

entropies and enthalpies of formation 51

enthalpies of combustion 51

enthalpies of solution 51

Gibbs energy of formation 51

Gibbs energy of solution 51

Gibbs energy of formation in solution 51

activities 51

ammonia

metabolism 17

ammonium ions

acid ionization thermodynamics 28

thermodynamics 38

anilines

redox potentials 12

anilinum ions

acid ionization thermodynamics 28

aqueous electrolytes 10, 37

aromatic organic bases

dissociation constants 41

barbituric acids

ionization thermodynamics 2 8

base constants 50

see also equilibrium constants

bases

see also acids

inorganic

organic

thermodynamics in aqueous and non

solvents

binary systems

solubilities in 54

33, 37, 40, 53

33, 41, 53

-aqueous

37

65
Subject Page

binding constants (see also equilibrium constants)

metal-buffer complexes

biochemical pathways

biosynthesis

Gibbs energy changes

boiling point

estimation

organic compounds

bond energy

buffer solutions

carbohydrates

isomerization and hydrolysis

carboxylic acids (see acids, organic)

chemical potential

aqueous electrolytes

C,H,N,0,P,S compounds

colloids

transport properties

combustion energy

complexes } metal-ligand

organic ligands

inorganic ligands

compressibility s estimation

conductance

aqueous electrolytes

conductivity, thermal

estimation

consecutive reactions

equilibria in

correlations of thermodynamic data

creatine

heat capacity, entropy, entropy of formation

enthalpy of combustion and formation

Gibbs energy of formation

53

26

17

43

60

5, 6, 22, 39

13, 32, 53

44

3, 16

13

3, 15, 16, 34

5, 11, 49

5, 11, 49

8, 43

13, 20, 44

8, 43

49

4, 5, 6, 7, 8, 24,

43, 45, 46

51

51

51

51

66
Subject Page

creatine 51

heat capacity, entropy 51

entropy of formation 51

enthalpy of combustion and formation 51

Gibbs energy of formation 51

critical constants, estimation 4 3

density

estimation 8, 43

inorganic electrolytes 10, 13, 20

organic electrolytes 20

deoxyribonucleic acid 21, 50

dielectric constants

aqueous electrolyte solutions 13

solvents 13

diffusion constants

estimation 8, 43

inorganic electrolytes 10, 13, 20, 44

organic electrolytes 13, 20, 44

dilution, enthalpy of 26

dipole moments 13

dissociation constants

aqueous electrolytes

organic acids, aqueous

inorganic acids and bases

organic bases

ligands

dyes and indicators bases

dissociation constants 41

electrochemical data 13

oxidation-reduction potentials 12

electrochemical potentials

biological oxidation-re duct ion reactions 26 vs pH 29

in organic solvents 44

electrode processes 14

13, 20

25, 32

40

41

49

67
Subject Page

electrolytes

aqueous and non-aqueous

uni-univalent

uni-polyvalent

molar volumes

irreversible thermodynamics

equilibrium constants of

Gibbs energies, enthalpies, heat capacities,

and entropies

dilution of

oxidation-reduction potentials

solubilities

10, 13, 20, 44

37

19, 38

61

36

35

5, 11, 21, 25, 26, 28,

32, 33, 40, 41, 49, 51

5, 11, 21, 26, 28, 47,

27, 57

12, 26, 29, 49

31, 51, 54

electron affinities

of elements 29

elements

solubilities

thermodynamic properties

energy transformations in living matter

energy values of foods

54

57

26

34

enthalpy

estimation

partial molal

apparent molal

enthalpies of salts, acids and bases vs.

T and concentration in water, and organic

solvents

hydrocarbons

inorganic compounds

organic compounds

enthalpy change

of phase changes

of fusion, estimation

of formation

of dilution

of complex formation

of sublimination

of vaporization

of combustion

of protonation of nucleic acids,

nucleotides and nucleosides

of polymerization

of ionization

of vaporization

of vaporization, estimation

of formation, estimation

68

8, 22

13

20

37

45, 46

47, 48, 57

47, 48, 55, 57

3, 4, 5, 9

47, 48

8

3, 5, 6, 7, 9, 15,

16, 22, 24, 29, 37,

45, 46, 47, 48, 51, 55,

3, 27, 38, 47, 57

11, 21

8

15, 24, 45, 46, 47, 60

16, 22, 34, 45, 46, 51

21

24

28, 37, 38, 53

15

43

43, 48, 56
Subject Page

enthalpy change (continued)

conformational change of macromolecules 53

of combustion (estimation) 56

entropy 3, 6, 7, 9

estimation 6, 7, 8, 22, 30

inorganic substances, various oxidation states 29

dissolved acids, salts, bases in water and

non-aqueous solvents 37

hydrocarbons 45, 46

inorganic compounds 47, 48, 57

organic compounds 47, 48, 55, 5 7 amino acids and related compounds 51

entropy change 4, 5

of fusion 18

of fusion, estimates 8

of formation 5, 51

of dilution 3

of solution 3, 37

of complex formation 11, 21

of protonation of nucleic acids,

nucleotides, and nucleosides 21

of polymerization 24

of ionization 28, 37, 53

enzyme catalyzed reactions 9, 26, 51

equation of state

estimation of 43

equilibrium constants

metal ion-ligand 11, 21, 33

protonation of nucleic acids, nucleotides,

and nucleosides 21

of polymerization 24

acid-base 32

proton transfer reactions 33

of formation 47, 57, 55

esters

vapor pressures 23

Gibbs energies of hydrolysis 53

estimates, bond energy 5,6, 7

estimation, properties (various kinds) 8, 15, 22, 30,

43, 55, 56

ethanol as solvent

thermodynamic properties of acids, bases

salts in 37

69
Subject Page

ethanol-water mixtures

acid dissociation in 33

expansion coefficient, thermal

estimation

fatty acids

solub ilities 52

fermentation

Gibbs energy change

food and foodstuff ingredients

composition and energy values

free energy - see Gibbs energy

gases

thermodynamic functions

polar properties, estimation

non-polar, properties estimation

Gibbs energy - see also chemical potential

estimation

biological systems

hydrocarbons

organic compounds

Gibbs energy change

of formation

of dilution

of solution

phosphates hydrolysis

metabolic processes

biosynthesis of saccharides

urea biosynthesis

ammonia metabolism

of polymerization

biological oxidation-reduction reactions

tricarboxylic acid cycle

fermentation

glycolysis

of ionization

of formation (estimation)

of hydrolysis

of decarboxylation

26

34

55

8, 43

8, 43

22

32

45, 46

55

3,

3,

45

51

3,

3,

4,

17

17

17

17

24

26

26

26

26

28

43

53

53

5, 9

5, 9, 26, 29, 37,

, 46, 47, 48,

, 55, 57

37

37, 51

17, 42

, 26, 32

32

, 37

, 48, 56

70
Subject Page

glasses - see solids

glucose

partial molal properties 9

glucosides

hydrolysis 9

glycerol

partial molal properties 9

glycine

partial molal properties 9

glycolysis 26

glycosides

hydrolysis 5 3

group contributions 6, 7, 22, 48

half-cell potentials 13

halogen compounds, organic 6

heat capacity 9

C,H,N,0,P,S compounds 3 estimation 6, 7, 8, 22, 43

dissolved acids, salts, bases in water

and non-aqueous solvents 37

uni-univalent electrolytes 38

hydrocarbons 45, 46

inorganic compounds 47, 48, 5 7 organic compounds 47, 48, 55, 57

amino acids and related compounds 51

heat capacity change

of complex formation 11, 21

of protonation of nucleic acids, nucleotides,

and nucleosides 21

of ionization 28

heat content - see enthalpy

heat of formation - see enthalpy changes of formation

helix-random coil transition 9

hemoglobin

mobility 13

71
Subject Page

hemoproteins

oxidation-reduction potentials

heterocyclic organic bases

dissociation constants

hydrocarbons

hydrogen ion concentration

hydrolysis

of ATP, ADP

metal ion hydrates

hydroxyl ion

as a ligand

index, substance-property

indicator bases

dissociation constants

inorganic

ligands - see ligands

electrolytes

inorganic compounds

oxidation states thermodynamics

solubilities

thermodynamic properties

current awareness bibliography

chemical bonding

inorganic ligands - see ligands

instability constants - see equilibrium constants

insulin

interface potentials

intermolecular forces

estimation

ionic strength, effects

ionic transport coefficients

ionization

aqueous acids

52

41

6, 23, 45, 56,

4, 17

4, 9, 26

42

49

40, 49

59

41

10, 13, 29, 36

44, 47, 57

13

29

31, 54

47, 48, 57

59

39

50

13

43

21, 33, 42

35

28, 33

72
Subject Page

ionization constants

organic acids 44

acids and bases 5 3

ionization potentials

elements 29

irreversible thermodynamics 35

isomerization

carbohydrates 9

ketones

vapor pressures 23

Kp - equilibria involving gases 50

Lennard-Jones potential - see intermolecular forces

ligands 5, 11, 33, 49

liquids

properties estimation 8, 4 3

liquid-junction potentials 13

macromolecules

helix-random coil transitions 9 transport properties 13

as ligands 50

current awareness bibliography 59

magnesium ion (effects) 4, 17, 42

metabolic processes 26

metal complexes 5, 6, 11, 33, 49

hydrated ions 40

with nucleic acids, nucleotides, and

nucleosides 21

with buffers 53

metalloporphyrir.s

oxidation-reduction potentials 52

metal-organic compounds

solubilities 31

thermodynamic properties 6, 15, 23

73
Subject Page

methanol as solvent

thermodynamic properties of salts, acids,

and bases in 37

methanol-water mixtures

acid dissociation in 33

mixed electrolytes 44

mixed solvent systems 3, 33

mixtures, fluid

estimation of properties 43

current awareness bibliography 59

mobilities

ionic 13

proteins 13

modulus

bulk, estimation 8

Young's, estimation 8

molar volume - see volume

multi-component systems

solubilities in 54

NAD

redox potentials 12

NADP

redox potentials 12

natural product bases

dissociation constants 41

nitrogen compounds, organic 6 non-aqueous solvents

solubilities in 3]

electrolytes In 37

metal-lig&nd complexes in

non-polar gases - see gases

74
Subject Page

nucleic acids 50

nucleosides 21

nucleotides 21

nutrients - see foods

organic bases

dissociation constants 41

organic compounds 6, 7, 13, 15,

18, 22, 24, 25

48, 55

C2 or C 1 47, 57

solubilities 53

current awareness bibliography 59

organic electrolytes

molar volumes 36

thermodynamic quant itites 38

properties 44

organic ligands - see ligands

organo-metallic compounds - see metal-organic compounds

osmotic coefficients

inorganic electrolytes 13, 19, 44

organic electrolytes 13, 19, 44

uni-polyvalent electrolytes 61

oxidation-reduction potentials

organic systems 12

compounds of the elements 29

biological systems 26, 32

metal-ligand complexes 49

selected 52

hemoproteins and metalloporphyrins 52

oxygen compounds, organic 6

partial molar volumes - see volume

peptides

heat capacities, entropies 51

enthalpy of combustion and formation 51

Gibbs energy of formation 51

activities in aqueous solution 51

75
Subject Page

PH

effects on reactions

effect on oxidation-reduction potentials

acid-base equilibria

ATP hydrolysis

of buffers

4, 17, 21

29

32

42

53

phenols

redox potentials

vapor pressures

acid dissociation constands, aqueous

ionization thermodynamics

12

23

25

28

phosphates

Gibbs energy and biosynthesis

hydrolysis

17

53

physiological energy use 34

pK values

acids and bases

buf fers

33, 40, 53

53

polar gases - see gases

polymers

properties estimation

polymerization processes 24

porphyrins

redox potentials 12

potential diagrams (emf)

elements and compounds 29

pressure, effect of

on enthalpy, entropy, internal energy,

heat capacity, estimation 43

proteins

heat capacities, entropies 51

proton transfer reactions

equilibrium constants 33

qumones

redox potentials

12

12

rate constants

polymerization 24

76
Subject Page

red cells

mobilities 13

redox potentials - see oxidation-reduction potentials

refraction, molar

estimation 56

relaxation time

estimation 8

ribonucleic acid 21, 50

saccharides

biosynthesis and Gibbs energy 17

salts

thermodynamic properties in water, methanol,

ethanol and other organic solvents 37

thermodynamic properties of uni-univalent

in solution 38

serum albumin

mobility 13

silver salts

thermodynamic properties of solutions 38

solids

crystalline, properties estimation 8

glasses, properties estimation 8

solubilities 13, 31

amino acids 51

fatty acids in water 52

water in fatty acids 52

triglycerides 52

elements, inorganic compounds, organic

compounds 54

solubility constants - see also equilibrium 50

constants

stability constants - see also equilibrium constants,

binding constants

metal-ion complexes 49

statistical mechanics 22

structure, relation to physical properties 8, 22

77
Subject Page

sulfur compounds, organic 6, 60

surface tension

estimation 4 3

ternary systems

solubilities in 54

thermodynamic functions of temperature 7 C,H,N,0,P,S compounds 3 organic compounds 18, 48, 55

hydrocarbons 45 , 46

inorganic substances 48

amino acids and related compounds 51

thiol esters

hydrolysis 5 3

transference number

inorganic electrolytes 10, 13, 20

organic electrolytes 13, 20

transition metal complexes - see metal complexes

transition temperatures

inorganic substances 47

organic compounds and 47

transport coefficients, ionic 34, 35, 44

tricarboxylic acid cycle

Gibbs energy changes 26

triglycerides

solubilities 52

urea 51

partial molal properties 9

biosynthesis 17

enthalpy of formation and combustion 51

Gibbs energy of formation 51

vapor pressure

C,H,N,0,P,S compounds

estimation

aqueous electrolyte solutions

organic compounds

water

38, 43, 56

13

3, 18, 2.3,

60

78
Subject Page

vibrational assignments (estimation method) 22

viscosity

estimation 8, A3

inorganic electrolytes 10

volumes, molar

aqueous ions and electrolytes 36

liquids, estimation A3

hydrocarbons, estimation 56

water

vapor pressure and enthalpy of vaporization 60

Wiswesser Line Notation

organic compounds 16

79
NBS-1 14A (REV. 7-73)

U.S. DEPT. OF COMM. BIBLIOGRAPHIC DATA

SHEET

1. PUBLICATION OR REPORT NO. NBSIR 74-535

2. Gov't Accession

No.

3. Recipient's Accession No.

A4. "FIT"! 111LCPT AINU 4Mn jUD <I 1 RTFTI 1 1 1 P A Selected and Annotated Bibliography of Compilations

of Data Relevant to Biochemical Thermodynamics

5. Publication Date July 1974

6» Performing Organization Code

7. AUTHOR(S)

G. To Armstrong, G. R. Janes, and R. N. Goldberg

8. Performing Organ. Report No. NBSIR 74-535

9. PERFORMING ORGANIZATION NAME AND ADDRESS

NATIONAL BUREAU OF STANDARDS

DEPARTMENT OF COMMERCE

fiAjrilMu 1 Un, U.V..

10. Project/Task/Work Unit No. 3160118

11. Contract/Grant No.

12. Sponsoring Organization Name and Complete Address (Street, City, State, ZIP)

Same as No. 9

13. Type of Report & Period

v." (j v err C LI Final

14. Sponsoring Agency Code

15. SUPPLEMENTARY NOTES

16. ABSTRACT (A 200-word or less (actual summary ol most significant information. If document includes a significant

bibliography or literature survey, mention it here.)

' • •• CT!

This report is a selected and annotated bibliography of sources of

data compilations relevant to biochemical thermodynamics. Included

in the annotations are brief descriptions of the type of thermodynamic

properties tabulated, the class of materials dealt with, and the degree

of completeness of the compilations.

17. KEY WORDS (six to twelve entries; alphabetical order; capitalize only the first letter of the first key word unless a proper name; separated by semicolons)

Bibliography; biochemistry; biology; data compilations; thermochemistry;

thermodynamics.

18. AVAILABILITY Unlimited 19. SECURITY CLASS 21. NO. OF PAGES

(THIS REPORT)

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