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CHNICAL NOTE
270-4
Selected Values of Chemical
Thermodynamic Properties
Tables for Elements 35 Through 53 in the
Standard Order of Arrangement
*<"?£AU of*^
U.S. DEPARTMENT OF COMMERCENational Bureau of Standards
k
UNITED STATES DEPARTMENT OF COMMERCEMaurice H. Stans, Secretary
NATIONAL BUREAU OF STANDARDS • A. V. Astin, Director
NBS TECHNICAL NOTE 270-4ISSUED MAY 1969
Nat. Bur. Stand. (U.S.), Tech. Note 270-4, 152 pages (May 1969)
CODEN: NBTNA
Selected Values of Chemical Thermodynamic Properties
Tables for Elements 35 Through 53 in the
Standard Order of Arrangement
D. D. Wagman, W. H. Evans, V. B. Parker,
I. Halow, S. M. Bailey, and R. H. Schumm
Institute for Materials Research
National Bureau of Standards
Washington, D.C. 20234
NBS Technical Notes are designed to supplement the
Bureau's regular publications program. They provide a
means for making available scientific data that are of
transient or limited interest. Technical Notes may be
listed or referred to in the open literature.
For sale by the Superintendent of Documents, U.S. Government Printing Office, Washington, D.C, 20402
Price $1.25 cents.
PREFACE
Technical Note 270-4 is the fourth part of a series of Notes
containing the tables of material prepared as a revision of Series I
of National Bureau of Standards Circular 500, Selected Values of
Chemical Thermodynamic Properties, by F. D. Rossini, D. D. Wagman,
W. H. Evans, S. Levine and I. Jaffe. This Note contains data for
compounds of nineteen elements, numbered 35 through 53 in the
Standard Order of Arrangement. In addition the Appendix contains
a list of corrections for errors and nnisprints which have been
detected in the previous summary Note TN 270-3. Data for compounds
of elements numbered 1 through 34 are contained in TN 270-3.
CONTENTS
Preface ii
Intr oduc tion v
Standard Order of Arrangement x
Table 35 Mercury 1
Table 36 Copper 13
Table 37 Silver 29Table 38 Gold 39Table 39 Nickel 43
Table 40 Cobalt 54Table 41 Iron 74Table 42 Palladium 90Table 43 Rhodium 93Table 44 Ruthenium 94Table 45 Platinum 96Table 46 Iridium 103Table 47 Osmium 104Table 48 Manganese ^06Table 49 Technetium 116Table 50 Rhenium 117Table 51 Chromium 120Table 52 Molybdenum 129Table 53 Tungsten 134
Appendix 139Index 140
SELECTED VALUES OF CHEMICAL THERMODYNAMIC PROPERTIES
by
Donald D. Wagman, William H. Evans, Vivian B. Parker,Iva Halow, Sylvia M. Bailey, and Richard H„ Schiomm
INTRODUCTION
Substances and Properties Included in the Tables
The tables contain values where known of the enthalpy and Gibbsenergy of formation, enthalpy, entropy and heat capacity at 298.15°K(2 5°C), and the enthalpy of formation at 0*^K, for all inorganic substancesand organic molecules containing not more than two carbon atoms. In
some instances such as metal -organic compounds, data are given for
substances in which each organic radical contains one or two carbonatoms.
No values are given in these tables for metal alloys or other
solid solutions, fused salts, or for substances of \indefined chemicalcomposition.
Physical States
The physical state of each substance is indicated in the columnheaded "State" as crystalline solid (c), liquid (liq), glassy or amorphous(amorp), or gaseous (g). Solutions in water are listed as aqueous (aq).
For non -aqueous systems the physical state is that normal for the
indicated solvent at 298ol5°K,
Definition of Symbols
The symbols used in these tables are defined as follows: P =
pressure; V = volume; T = absolute temperature; E = intrinsic or
internal energy; S = entropy; H = E + PV = enthalpy (heat content);
G = H - TS = Gibbs energy (formerly the free energy); Cp = (dH/dT)p =
heat capacity at constant pressure.
Conventions Regarding Pure Substances
The values of the thermodynamic properties of the pure substancesgiven in these tables are for the substances in their standard states
(indicated by the superscript " on the thermodynamic symbol). Thesestandard states are defined as follows:
For a pure solid or liquid, the standard state is the substancein the condensed phase under a pressure of one atmosphere.
For a gas the standard state is the hypothetical ideal gas at unit
fugacity, in which state the enthalpy is that of the real gas at the sametemperature and at zero pressure.
The values of A Hf and AGf* given in the tables represent the changein the appropriate thermodynajnic quantity when one gram -formulaweight of the substance in its standard state is formed, isothermally at
the indicated temperature, from the elements, each in its appropriatestandard reference state. The standard reference state at Z5"C for
each element except phosphorus has been chosen to be the standardstate that is thermodynamically stable at 25 "C and at one atmospherepressure. For phosphorus the standard reference state is the crystalline
white form; the more stable forms have not been well characterizedthermochemically. The same reference states have been maintained for
the elements at "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 are indicated in the tables by the
fact that the values of A Hf " and A Gf ° are exactly zero.
The values of H^q^. -Hq represent the enthalpy difference for the
given substance between 298.15*K and CK. If the indicated standard
state at 25 "C is the gas, the corresponding state at "K is the hypo-thetical ideal gas; if the state at 25 °C is solid or liqiiid, the corres-ponding state at "K is the thermodynamically "stable^crystalline
solid, unless otherwise specifically indicated.
The values of S " represent the virtual or "thermal" entropy of the
substance in the standard state at 298.15°K, omitting contributions fromnuclear spins. Isotope mixing effects, etc. , are also excluded except
in the case of the hydrogen -deuterixim ( 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 AHf " for the electron
is zero. Conversions between and 298.15°K are calculated using
the value of H298 H, 1.481 kcal per mole of electrons, and assximing
that the values of H|Qg-H5 for the ionized and un-ionized moleciiles are
the same.
Conventions Regarding Solutions
Solutions in water are designated as aqueous (aq); other solvents
are designated by name or chemical formula. The concentration of the
solution is expressed in terms of the number of moles of solvent asso-ciated with one mole of the solute. If no concentration is indicated, the
solution is assumed to be "dilute".
The standard state for a solute in aqueous solution is taken as the
hypothetical ideal solution of unit molality (indicated as "std. state,
m = 1"). In this state the partial molal enthalpy and heat capacity of the
solute are the same as in the infinitely dilute real solution. For non-aqueous solutions the standard state of the solute is the hypothetical
ideal solution of unit mole fraction of solute ("std. state, X2 = 1").
The value of A Hf " given in the tables for a solute in its standard
state is the apparent molal enthalpy of formation of the substance in
the infinitely dilute real solution. At this dilution the partial molalenthalpy is equal to the apparent molal quantity. At concentrations
other than the standard state, the value of A Hf ° represents the apparententhalpy of the reaction of formation of the solution from the elementsconnprising the solute, each in its standard reference state, and the
appropriate total number of moles of solvent. In this representation
the value of A Hf " 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 A Hf " at the corresponding concentrations.
The values of the thermodynamic properties tabulated for the
individual ions in aqueous solution are based on the usual conventionthat the values of AHf% AGt", 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 kin^s and number of individual ions assumed to constitute
the molecule of the given electrolyte. When the undissociated species,
rather than the s\im of the ions, is meant, the notation "undissociated"or "un-Ionized" is used. For an ionic species the properties tabulated
refer to thatxindissociated ion. By adopting the above convention withrespect to aqueous H , it follows that the thermodynamic relation A Gf *
= A Hi" - T A Sf " will not hold for an individual ionic species. Howeverno problem arises when neutral chemical systems are considered.
Unit of Energy and Fundamental Constants
All of the energy values given in these tables are expressed in termsof the thermochemical calorie. This unit, defined as equal to 4.1840
joules, is generally accepted for the presentation of chemical thermo-dynamic data. Values reported in other units have been converted to
calories by means of the conversion factors for molecular energy given
in Table A.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 ± 0.00029cal/deg nnol
F = Faraday constant = 96487. + 1.6 coulombs /mol= 23060.9 ±0.4 cal/volt equivalent
Z = Nhc = 11. 96258 + 0. 00107 J/cm"^ mol = 2. 85912 -k 0. 00026 cal/cm"^ molC2 = second radiation constant = hc/k = 1.43879 ± 0.00015 cm deg
0»C = 273.15*KThese constants are consistent with those given in the Table of GeneralPhysical Constants, recommended by the National Academy of Sciences -
National Research Council . The formula weights in the tables havebeen calculated for the molecular formula given in the Formula andDescription column using the 1961 Table of Relative Atomic Weights basedon the atomic mass of ^ C = 12 exactly .
Internal Consistency of the Tables
All of the values given in these tables have been calculated fromthe original articles, using consistent values for all subsidiary andauxiliary quantities. The original data were corrected where possible
for differences in energy units, molecular weights, tennperature scales,
etc. Thus w^e 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 thermodynamicrelationships annong these properties. The quantities A Hf ", A Gf, andS° at 298. 15 "K satisfy the relation:
A Gf° = A Hf° - T ASf.
NBS Technical News Bulletin, October 1963.
'A. E. Cameron and E. Wichers, J. Am. Chem, Soc. 84, 4192 (1962).
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. Becauseof 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 significant errors in calculated values of A H" or A G"for specific reactions may result from the introduction of such data.
Uncertainties
The uncertainty in any value in the tables depends on the vmcertain-
ties of all the determinations in the total chain of reactions used to
establish the value.
A discussion of the uncertainties will be included in the final
publication of these tables in the National Standard Reference DataSystem. However we have followed certain rules with respect to
significant figures to indicate these uncertainties. Values are tabulated
in general 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 numberof significant figures for any one value in the tables need not representthe absolute accuracy of that value. For solutions of varying compositionvalues are frequently tabulated to more figures to make possible the
recovery of enthalpies of solution and dilution. Similarly values of
A HfQ and AHf^og ir may be given to different niombers 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.
Arrangement of the Tables
The compounds in the tables are entered according to the StandardOrder of Arrangement, (see Figure 1), by the principle of latest position.
In this scheme, a compoimd 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 elementsoccurring earlier in the order; the arrangement within a table follows
the same ordering. An exception occurs in the carbon tables (Table 23),
which is divided into subgroups consisting of all compounds with onecarbon atom, then all with two carbon atoms, etc.
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SERIES I
Enthalpy of Formation at CKEnthalpy of Formation at 298. 15°K
Gibbs Energy of Formation at 298. IS^K
Enthalpy at 298. 15°K
Entropy at 298. 15 "K
Heat Capacity at 298. 15°K
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Errata for Te chnical Note 270-3
Page 22 HF(liq) AH^°gg = -71.65 kcal/mol
Page 32 HBr(g) AH^ = -6.826 kcal/mol
Page 43 s(g) AGf = 56.951 kcal/mol
S° = 40.084 cal/deg mol
Page 48 H2S+(g^ AHfQ = 237.0 kcal/mol
Page 56 Se(g) H° - H° = 1.4815 kcal/mol
S° = 42.21 cal/deg/mol
Cp° = 4.978 cal/deg/mol
Page 61 N(g) AG£° = 108.886 kcal/mol
S° = 36.613 cal/deg mol
Page 86 H2PO4" (aq) AGf ° = -270.17 kcal/mol
Page 231 Tlzl 5603)3 instead of Te (8603)3
TlzSe formula weight = 487.70
Page 234 ZnFzCc) AGf° = -170.5 kcal/mol
139
INDEX OF CONTENTS
ChemicalSymbol
AgAl
ArAsAt
AuBBi
BrCCdCI
CoCrCuFFeGaGeHHeHgI
In
Ir
KrMnNNeNi
OOsPPbPdPoPtRe
Element
Silver
AluminunnArgonArsenicAstatine
GoldBoronBismut hBromineCarbonCadmiumChlorine
Cobalt
ChromiumCopperFluorineIron
GalliumGermaniumHydrogenHeliumMercuryIodine
IndiumIridiumKryptonManganeseNitrogenNeonNickel
OxygenOsmiumPhosphorusLeadPalladiiim
PoloniumPlatinumRhenium
Table Volume-Number Page Number
37 4- 2929 3-2075 3- 17
20 3- 9513 3- 4238 4- 3928 3-196ZZ 3-10311 3- 31
23 3-10634 3-24810 3- 2440 4- 5451 4-12036 4- 13
9 3- 21
41 4- 74
30 3-21825 3-1772 3- 12
3 3- 15
35 4- 1
12 3- 3631 3-22346 4-1036 3- 18
48 4-10618 3- 61
4 3- 16
39 4- 43
1 3- 11
47 4-10419 3- 8427 3-18742 4- 9017 3- 6045 4- 9650 4-117
140
ChemicalSymbol
RhRnRuS
Sb
SeSi
SnTcTeTl
WXeZn
Element Table Volume -
Number Page Number
Rhodium 43 4- 93
Radon 8 3- 20
Ruthenium 44 4- 94
Sulfur 14 3- 43
Antimony 21 3- 99Selenium 15 3- 56
Silicon 24 3-171
Tin 26 3-181
Technetium 49 4-116Telluriunn 16 3- 58
Thallium 32 3-227Tungsten 53 4-134Xenon 7 3- 19
Zinc 33 3-233
Compounds are located in the Table for the element (in the compound)having the highest Table number.
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