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NBSIR 76-1034

Chemical Thermodynamic

Properties of Compounds of

Sodium, Potassium and

Rubidium: An Interim

Tabulation of Selected Values

D. D. Wagman, W. H. Evans, V. B. Parker and R. H. Schumm

Physical Chemistry Division

Institute for Materials Research

National Bureau of Standards

Washington, D. C 20234

April 1976

Interim Report

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NBSIR 76-1034

CHEMICAL THERMODYNAMIC

PROPERTIES OF COMPOUNDS OF

SODIUM, POTASSIUM AND

RUBIDIUM: AN INTERIM

TABULATION OF SELECTED VALUES

D. D. Wagman, W. H. Evans, V. B. Parker and R. H. Schumm

Physical Chemistry Division

Institute for Materials Research

National Bureau of Standards

Washington, D. C. 20234

April 1976

Interim Report

Prepared for Office of Standard Reference Data, NBS

U.S. DEPARTMENT OF COMMERCE. Elliot L. Richardson. Secretary

Dr. Batty Avidiar-JoliMon. Atsistmt S^cr^tmy for Science and Technology

NATIONAL BUREAU OF STANDARDS. Ernest Ambler, Acting Director

Table of Contents

1. Introduction 1

2. Explanation of the Contents of the Tables 2

2.1 Chemical Formulae and Physical States 2

2.2 Definition of Symbols for Thermodynamic Properties 3

2.3 Conventions Regarding Pure Substances 3

2.4 Conventions Regarding Solutions 4

3. Units of Energy 6

4. Internal Consistency of the Tables 7

4.1 Uncertainties 7

4.2 Relationship to Other Tables of Thermodynamic Data 8

5. Arrangement of the Tables 8

Figure 1 Standard Order of Arrangement 11

Table A Physical State Conventions , X2

Table B Conversion factors for Units of Molecular Energy 16

Tables of Selected Value of Thermodynamic Properties 17

Compounds of Sodium

Compounds of Potassium

Compounds of Rubidium

1

Chemical Thermodynamic Properties of Compounds of Sodium, Potassium

and Rubidium: An Interim Tabulation of Selected Values

D. D. Wagman, W. H. Evans, V. B. Parker and R. H. Schumm

National Bureau of Standards

Washington, DC 20234

ABSTRACT

Selected values are given for the thermochemical properties of the

more common compounds of sodium and potassium. A more extensive set of

selections is provided for rubidium compounds. The properties included

where data are available, are enthalpy of formation at 0 K and 298.15 K

Z^f(O) and AHf(298), Gibbs energy of formation, entropy and heat

capacity at 298.15 ^f(298), S(298) and Cp(298), and the enthalpy

difference between 0 K and 298.15 K, H(298)-H(0). The values are consistent with the tables issued earlier in the NBS Technical Note

270 series.

Keywords: Enthalpy; entropy; Gibbs energy; heat capacity; potassium

compounds; rubidium compounds; sodium compounds; standard reference

data; thermochemical tables.

1 . Introduction

This is an interim report on the evaluation of chemical thermodynamic properties of compounds of three of the alkali metals. It

supplements the extensive set of selected values of chemical thermodynamic properties published as NBS Technical Note 270, parts 1-7. [l].

The values contained in this report are consistent with those in NBS

Technical Note 270 and may be combined with them to establish the

thermodynamic properties of processes.

Three tables are given here for the more common compounds of

sodium and potassium and for all rubidium compounds for which data are

aval lable

The tables contain values of the enthalpy and Gibbs energy of

formation, :XHf° and AGf°, entropy, S", and heat capacity, Cp°, all at

298.15 K (25°C), the enthalpy of formation at 0 K, ^f, and the

enthalpy difference between 0 K and 298 K, H° (298) -H° (0) . The substance

included are inorganic compounds of these elements, compounds

containing organic ligands that have one or two carbon atoms and their

aqueous solutions.

1
No values are given in these tables for metal alloys or other

solid solutions, fused salts, or for substances of undefined chemical

composi tion.

The sodium and potassium tables are incomplete. They list

properties of compounds evaluated in the course of preparing selections

for compounds already published in the NBS Technical Note 270 series

and an extensive collection of the properties of neutral electrolytes

in aqueous solution at the hypothetical standard state of unit activity.

The latter were calculated as the sum of the properties of the ions.

Although selections will be needed for the properties of many more

compounds of sodium and potassium, the selections given here should be

sufficient for solution of a wide range of thermochemical problems.

The rubidium table is the complete set of selections now planned

for inclusion in NBS Technical Note 270. It was prepared late in 1975.

There may be a few revisions and additions based on newly reported data.

Users of these three tables are invited to comment on the selections,

suggest substances for which values of properties are needed, correct

errors and bring new measurements to our attention. All of these will

help us improve the final tables.

2 . Explanation of the contents of the tables

The following material, adapted from NBS Technical Note 270,

provides definitions and conventions used in the tables.

2 . 1 Chemical Formulae and Physical States

The tables were reproduced from computer printout in which only

capital (upper case) letters are available. Normal one-line chemical

formulae are used, with the following modifications:

Subscripts (counts of atoms) and superscripts (charge) are printed on line: NA202 = Na202, NA+ = Na+.

The digit "1" appears wherever necessary to separate the

symbols of two chemical elements: NA1N103 = NaN03

The centered dot, used in hydrates and minerals, is shown

as a colon: NA1V104:2H20 = NaV04-2H20.

The physical state of the substance is appended to the chemical

formula in parentheses: NAIOIH(C) = NaOH, crystalline. The

abbreviations most commonly used to denote physical states are listed in

Table A. Any other notations are explained in comments within the

tables. o
2.2 Definition of Symbols for Thermocheml cal Properties

The headings used In the tables and their meanings are:

DHO - AHf5, standard heat of formation at 0 K;

DH298 = AHf*, standard heat of formation at 298.15 K;

DG298 = AGf°, standard Gibbs energy (formerly free energy), G,

of formation at 298.15 K;

H298-HO - H2go-HQ, enthalpy, H, of the compound In the indicated

state at 298.15 K referred to its value at 0 K. If the indicated

state at 298 K is gas, the corresponding state at 0 K is the

hypothetical ideal gas; if the state at 298 K is solid or liquid,

the corresponding state at 0 K Is the thermodynamically stable

crystalline solid, unless otherwise specifically indicated.

S298 = S", standard entropy, S, at 298.15 K;

C298 '= Cp° ; specific heat at constant pressure at 298.15 K.

The Gibbs free energy is related to the other quantities by:

G = H-TS, where T is the thermodynamic temperature. The enthalpy is

related to the internal energy, E, by: H = E + PV, where P = pressure

and V = volume.

All values refer to one mole of substance for the formula given.

2 . 3 Conventions Regarding Pure Substances'

The values of the thermodynamic properties of the pure substances

given in these tables are for the substances in their standard states.

These standard states are defined as follows:

For a pure solid or liquid, the standard state at any temperature

Is the substance in the condensed phase under a pressure of one atmosphere.

For a gas the standard state at any temperature is the hypothetical

Ideal gas at unit fugacity, in which state the enthalpy is that of the

real gas at the same temperature and at zero pressure.

The phase of a substance Is indicated in parentheses at the end

of the chemical formula. See section 2.1.

The values of Z^f° and ^f° given in the tables represent the

change in the appropriate thermodynamic quantity when one mole

of the substance in its standard state is formed, isothermally

at the indicated temperature, from the elements, each in its appropriate

standard reference state. The standard reference state at 25^0 for

each element except phosphorus has been chosen to be the standard state

that is thermodynamically stable at 25''C and at one atmosphere pressure.

3
For phosphorus the standard reference state Is the crystalline white

form; the more stable forms have not been well characterized thermochemically. The same reference states have been maintained for the

elements at 0 K except for the liquid elements bromine and mercury

for which the reference states have been chosen as the stable

crystalline forms. The standard reference states for the elements are indicated in the tables by the fact that the values of zXHf and Z^f** are exactly zero.

The values of S° represent the virtual or "thermal" entropy of

the substance in the standard state at 298.15 K, omitting contributions

from nuclear spins. Isotope mixing effects, etc.. are also excluded

except in the case of the hydrogen-deuterium (^H- H) system. Where

data have been available only for a particular isotope, they have been

corrected when possible to the normal isotopic composition.

The values of the enthalpies of formation of gaseous ionic species are computed on the convention that the value of Z^f° for the electron

is zero. Conversions between 0 and 298.15 K are calculated using the

value of ^293-110 = 1.481 kcal per mole of electrons, and assuming that

the values of H2g3-HQ for the ionized and un-ionized molecules are

the same

2 .4 Convention Regarding Solutions

For all dissolved substances the composition of the solvent is

indicated in parentheses following the chemical formula. Except in

special cases, discussed below, the number of moles of the solvent

associated with one mole of solute is stated explicitly. See section

2.1 and Table A for the conventions used.-

In some cases the concentration of the solute can not be

specified. These are indicated as "AU" (aqueous, unspecified) for

water solutions and by "U" for non-aqueous and mixed media. In all

these cases the solution may be assumed to be "dilute".

4
The standard state for a non-dissociated solute in aqueous

solution is taken as the hypothetical ideal solution of unit molality,

which has been designated as "std. state, m = 1", For strong

electrolytes in aqueous solution the conventional standard state is

the ideal solution of unit activity (unit mean molality). For nonaqueous solutions the standard state of the solute is the hypothetical

Ideal solution of unit mole fraction of solute (std. state, X2 = 1).

The designation "A" is used for strong electrolytes in the standard

state and "AO" for undissociated species in water solution. In nonaqueous media the standard state defined above is indicated by

appending "X" to the formula of the solvent. The convention "std.

state, m = 1" is used only rarely for non-aqueous media. For it, an

"M" is appended to the formula of the solvent.

The value of AHf for a solute in its standard state is equal

to the apparent molal enthalpy of formation of the substance in the

infinitely dilute real solution, since the enthalpy of dilution of an ideal solution is zero. At this dilution the partial molal

enthalpy is equal to the apparent molal quantity. At concentrations

other than the standard state, the value of ZiHf'' represents the

apparent enthalpy of the reaction of formation of the solution from

the elements comprising the solute, each in its standard reference

state, and the appropriate total number of moles of solvent. In

this representation the value of ZlsHf** for the solvent is not required.

The experimental value for a heat of dilution is obtained directly as the difference between the two values of /^f° at the corresponding

concentrations. At finite concentrations the partial molal enthalpy

of formation differs from the apparent enthalpy.

The values of the thermodynamic properties tabulated for the

individual ions in aqueous solution are based on the usually convention

that the values of AHf°, , S° and Cp° for H+ (aq, std. state, m

= 1) are zero. The properties of a neutral electrolyte in aqueous

solution in the standard state are equal to the algebraic sum of these

values for the appropriate kinds and numbers of individual ions assumed

to constitute the molecule of the given electrolyte. For an ionic

species e.g., HS04~, the properties tabulated refer to that undissociated

ion, i.e. they are not equal to the sum of those for its constituent

ions. By adopting the above convention with respect to aqueous H"*", it follows that the thermodynamic relation mf° = AHf*-T(Z^f° + n-0.5S°

(Ho)) holds for individual ionic species, with n equal to the algebraic

value of the charge. For neutral electrolytes (and gaseous ions)

the normal consistency relationship applies. See section 4.

5
3 . Unit of Energy and Fundamental Constants

All of the energy values given in these tables are expressed in

terms of the thermochemical calorie. This unit, defined as equal to

4.1840 joules, is generally accepted for the presentation of chemical

thermodynamic data. Values reported in other units have been converted

to calories by means of the conversion factors for molecular energy

given in Table B.

The following values of the fundamental physical constants have

been used in these calculations:

R = gas constant = 8.3143 ± 0.0012 J/deg mol = 1.98717 ± 0.00029

cal/deg mol

F = Faraday constant = 96487.0 ± 1.6 coulombs/mol = 23060.9 ± 0.4

cal/volt equivalent

Z = Nhc = 11.96258 ± 0.00107 J/cm"^ mol = 2.85912 ± 0.00026 cal/cm"!

mol

C2 = second radiation constant = hc/k = 1.43879 ± 0.00015 cm deg

O'C = 273.15 K

These constants are consistent with those given in the Table of General

Physical Constants, recommended by the National Academy of SciencesNational Research Council [2].

These values differ slightly from those recommended by CODATA

[3] in 1973. However, adoption of the CODATA recommendations would

change the values in the present tables by far less than their

uncertainties (see section 4.1). Thus the present values may be said

to be consistent with the 1973 set of fundamental constants. The

formula weights in the tables have been calculated from the molecular

formula using the 1961 Table of Relative Atomic Weights based on the

atomic mass of ^^C = 12 exactly [4]. Values are given to four decimals

places for convenience in the computer processing. Use of the more

recent atomic weights [8] would produce only insignificant changes

in the tabulated thermodynamic values.

6
4 . Internal Consistency of the Tables

All of the values given in these tables have been calculated from

the original articles, using consistent values for all subsidiary and

auxiliary quantities. The original data were corrected where possible

for differences in energy units, molecular weights, temperature scales,

etc. Thus we have sought to maintain a uniform scale of energies for

all the substances in the tables. In addition the tabulated values of

the properties of a substance satisfy all the known physical and

thermodynamic relationships among these properties. The quantities

^f*, /^f° , and S° at 298.15 K satisfy the relation:

Z^f* = AHf° - T ^f*.

to the precision given. The special case of solutions is discussed

in section 2.4. Furthermore the calculated value of any thermodynamic

quantity for a reaction is independent of the path chosen for the

evaluation.

In some cases newer data may have become available on certain

substances after the values were selected for these tables. Because

of the need to maintain the internal consistency of the tables, it is

not always possible to incorporate these newer data into the tables

without a detailed analysis of the effect of such a change. Unless

great care is used, relatively signi ficant. errors in calculated values

of Z^H* or for specific reactions may result from the introduction

of such data. See section 4.2.

4 . 1 Uncertainti es

The uncertainty in any value in the tables depends on the

uncertainties of all the determinations in the total chain of reactions

used to establish the value.

In general, when uncertainties are not stated explicitly certain

rules have been followed with respect to the number of significant figures

recorded. Values are tabulated such that the overall uncertainty

lies between 2 and 20 units of the last figure. On the other hand,

values are given so that the experimental data from which they are derived may be recovered with an accuracy equal to that of the original

quantities. Thus the number of significant figures for any one value

in the tables need not represent the absolute accuracy of that value.

For solutions of varying composition, values are frequently tabulated

to more figures to make possible the recovery of enthalpies of solution

and dilution. Similarly values of /^fg and ^f^gg.lS given to

different numbers of significant figures. In this instance the

quantity with the lesser number of figures is used to represent the

uncertainty estimate. The larger number of figures is used for the other

quantity to retain the significance of the temperature correction term.

7
The remarks above apply directly to the tables on sodium and

potassium compounds. For rubidium uncertainties are stated explicitly

immediately below the value of each property. (The form is +-0.05,

where +- means ±)

4.2 Relationship to Other Tables of Thermodynamic Properties

The chemical thermodynamic properties in the present table may

be combined with those published in NBS Technical Note 270 [l] in

order to calculate the change in a property for a process , However

we recommend against these values being combined with those in any

other tabulation or with a property reported in an original research

paper. In particular, we warn against indiscriminate combination with

the CODATA Key Values for Thermodynamics [5-7].

There are several reasons for avoiding the combination of

thermochemical data from more than one table. The most important is

that different large-scale tables use different thermochemical

properties of formation for substances that are ubiquitous in

thermochemical measurements. Outstanding examples are the common

inorganic acids and their ions. Another reason is that the groups

preparing different tables may have relied on different measurements

as the basis for selecting property values.

It is difficult to predict a priori how a change in one selected

formation property would affect values assigned to other substances

because of the way these are linked by complex networks. In general,

it may be expected that the advantage of internal consistency of a table will be lost if values from several sources are combined and

that experimental measurements may be reproduced poorly.

No general, simple algorithm can be suggested for overcoming

this problem. If it becomes necessary to extend a table of data

to substances other than those tabulated, the user is advised to consult

the group that prepared the table about the procedure that he plans

to use

5 . Arrangement of the Tables

The compounds in the tables are entered according tq the Standard

Order of Arrangement, (see Figure 1), by the principle of latest

position. In this scheme, a compound is listed under the element

occurring latest in the list; water of hydration is neglected. Within

a given element -table will be found all of the compounds of that element

with elements occurring earlier in the order; the arrangement within

a table follows the same ordering.

8
The selections for rubidium compounds were made late in 1975 by

W. H. Evans. Those for sodium and potassium have been made by all of

us and by former members of the Chemical Thermodynamics Data Center

during the past decade. The extensive collection of properties of

electrolytes in aqueous solution was prepared by R. H. Schumm. The

tables have been printed using computer programs that are modifications

of ones developed by Dr. J. B. Pedley, University of Sussex, Brighton,

England, for the CATCH System of Thermochemical Tables.

"5

9
References

1. Wagman, D. D. et al., NBS Technical Note 270-3 (1968), 270-4

(1969) , 270-5 (1971), Parker, V. B. et al, NBS Technical Note

270-6 (1971), Schumm, R. H. et al, NBS Technical Note 270-7

(1973).

2. NBS Technical News Bulletin, October 1963.

3. CODATA Task Group on Fundamental Constants, CODATA Bulletin

No. 11 (December 1973).

4. Cameron, A. E., and Wichers, E., J. Am. Chem. Soc. 84, 4192 (1962).

5. CODATA Task Group on Key Values for Thermodynamics, CODATA

Bulletin No. 17 (January 1976).

6. Idem, CODATA Special Report No. 3 (September 1975).

7. Parker, V. B., Wagman, D. D. and Garvin, D., NBS Interagency

Report, NBSIR 75-968 (January 1976).

8. Commission on Atomic Weights of lUPAC, Pure Appl. Chem. 21_, 577

(1970) .

10
STANDARD ORDER OF ARRANGEMENT
TABLE A ; Physical State Conventions

The following conventions are used to designate the physical

state of a substance. These apply to the attached table and to the

NBS Thermochemical Data Bank. This information appears in a

parenthetical expression appended to the molecular formula. Some of

the explanations imply a thermochemical value, particularly those

for solutions. These normally are used in describing enthalpy

measurements.

Basic Svmbols Explanation

(G) Gaseous, e.g., in HICL(G) for HCi(g)

(GS) Gaseous reference standard state for an element,

e.g., 02(GS) for O^Cg)

(C) Crystalline, e.g., in N1H4CL(C) for NH^Ci(c)

(CS) Crystalline reference standard state for an

element, e.g., in RB(CS) for Rb(c)

(L) Liquid, e.g., in H20(L) for H^OCi)

(IS) Liquid reference standard state for an element,

e.g., in BR2(LS) for ^v^ii)

(AM) Amorphous

(GL) Glassy

(A) Hypothetical standard state of the ideal aqueous

solution at unit activity. For a neutral electrolyte

the value of a property is equal to the algebraic

sum of the values for the ions assumed to constitute

the molecule of the electrolyte, e.g.HC£(A) =

H+(A) + C£-(A). For an ionic species this

notation is commonly used to refer to the

undlssoclated ton as written, e.g. HSO^(A)

12
Explnnatton

Hypothetical standard state of the ideal aqueous

solution at unit activity of the undissociated

(non-ionized) species, e.g. HF(AO), HF^'CAO).

May also be used whenever the designation (A)

could be ambiguous. Note that the descriptions

HSO, "(A) and HSO,"(AO) are equivalent, but

that HF(A) and HF(AO) are not.

(AU) Aqueous solution of undefined, but usually

dilute, concentration, e.g. XeO- (AU)

The symbols used above occasionally are modified by numbers

to distinguish two substances in the same state that have the same

molecular weight, as for isomers,: (AU2), (C3) . They are also used

in combination with descriptive material, e.g. (C:HE), (C:AL) etc.

to mean "crystalline, hexagonal", "crystalline, alpha form" etc.

Special notations for substances in solutions

The notations for the "state" of a substance in solution may

combine a definition of the system, e.g. UCJi in 220 moles of water,

and a specification of the thermochemi cal property associated with it.

Usually the thermochemi cal property is the apparent integral enthalpy

or free energy of formation or an absolute entropy, i.e. the formation

properties of the solvent are not included. If a partial molal property

Is tabulated the notation D: ("D" for "differential") occurs as the

first term in the state bracket. The notations given below illustrate

the differences for Integral and differential (partial molal) properties,

and extrapolated values. Examples are given for aqueous, mixed, and

non-aqueous solvents.

13
Symbol

H1CL(200H20)

H1CL(D:200H20) and

H2O(D:HlCI/f200H2O)

Explanation

An aqueous solution of specified composition, e.g.

one mole of HCi in 200 moles H2O. The value of

represents the apparent integral enthalpy

of formation.

These represent the partial molal (enthalpy) of

formation of the substance in a solution of

specified concentration, e.g. the partial molal

enthalpy of formation of HCi and H^O respectively,

in a solution consisting of 1 mole HC£ and 200

moles H2O

U1CL4(H1CL104+50H20) This describes a solute dissolved in a mixed solvent,

e.g. one mole of UCi^ in a mixture of 1 mole of

HCjCO^ and 50 moles H2O. The value of Z^Hf represents

the apparent integral enthalpy of formation of

the substance, UCj^^, in the medium.

This represents a solute at an unspecified but

usually dilute concentration in a solvent mixture

of fixed composition.

U1CIA(H1CL104+

50H2O :AU)

14
Symbol Explanation

U1CIA(L(H1CL) :AU)

RB1I(C1H3C1N:S)

RB1I(C1H3C1N: U)

RB1I(1000C1H3C1N)

Specifies the partial molal (enthalpy) of foirmation

of a substance in a mixed medium, e.g. the enthalpy

of formation of 1 mole of UCX^ in a large amount

of a solution containing UCJL^, HNO^ and H^O in

the molar ratios 1:1:50.

Specifies a thermochemical value extrapolated

from those in a particular type of solution, e.g.

the integral (enthalpy) of formation of UCi.^ at

an unspecified concentration in water solution

obtained by extrapolation from values in solutions

containing HCj^ at varying concentrations.

Ideal solution of a substance (Rbl) in a nonaqueous solvent (CH^CN), the substance being in

the standard state of unit activity on the molal

scale unless otherwise indicated. (In some early

entries in the Data Bank these are written

ambiguously as (C1H3C1N)).

Solution of a substance (Rbl) in a non-aqueous

solvent (CH^CN) at an unspecified concentration.

This is analogous to (AU)

Solution of a substance (Rbl) in a non-aqueous solvent

at a specified concentration.

15
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16
TABLES OF SELECTED VALUES OF THERMODYNAMIC PROPERTIES

Enthalpy of Formation at 0 K

Enthalpy of Formation at 298.15 K

Gibbs Energy of Formation at 298.15 K

Enthalpy at 298.15 K

Entropy at 298.15 K

Heat Capacity at 298.15 K

17

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NBS-I14A (REV 7-7))

U S. DEPT. OF COMM. BIBLIOGRAPHIC DATA

SHEET

1. IMIhl.K A riON OK KI' POK 1 No. NBSIR 76-1034

2. Gov't Ac ( f s s 1 on No.

3. Recipient's Accession No.

4. rn I.I- AND suH'rn i.i- CHEMICAL THERMODYNAMIC PROPERTIES OF COMPOUNDS OF SODIUM,

POTASSIUM AND RUBIDIUM: AN INTERIM TABULATION OF

SELECTED VALUES

5. Publication Date April 1976

6. Performing Organization Code

D. D. Wagman, W. H. Evans, V. B. Parker and R. H. Schumm

8. Performing Organ. Report No. NBSIR 76-1034

9. PF.RI-ORMlNCi ORGANIZATION NAMK AND ADDRKSS

NATIONAL BUREAU OF STANDARDS

DEPARTMENT OF COMMERCE

WASHINGTON, D.C. 20234

10. Project/Task/Work Unit No. 3165151

11. Contract/Grant No.

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

National Bureau of Standards

Department of Commerce

Washington, DC 20234

13. Type of Report & Period Covered

Interim

14. Sponsoring Agency Code

15. SUPPl.l-MKNTARY NOTKS

16. AHST KAC 1 (A 200-word or less (actual summary of most si^idcant information. If document includes a significant

bi bl io^raphy or literature survey, mention it here.) Selected values are given for the thermochemica 1 properties of the more common

compounds of sodium and potassium. A more extensive set of selections is provided

for rubidium compounds. The properties included, where data are available, are enthalpy of formation at 0 K and 298.15 K, ZXHf(O) and AHf(298), Gibbs energy of

formation, entropy and heat capacity at 298.15 K, AGf(298), S(298) and Cp(298)

and the enthalpy difference between 0 K and 298.15 K, H(298)-H(0). The values are consistent with the tables issued earlier in the NBS Technical Note 270 series.

17. KI;Y WORDS (six to twelve entries; alphabetical order, i apitalize only the first letter of the first key word unless a proper name, separated by semicolons) -Enthalpy ; entropy; Gibbs energy; heat capacity; potassium

compounds; rubidium compounds; sodium compounds; standard reference data; thermochemical tables

.

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