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NBS TECHNICAL NOTE 270-7

REFERENCE

Selected Values of

Chemical Thermodynamic

Properties

U.S.

DEPARTMENTOF

COMMERCENational

|— QC— of

100 is

ho.Z70-7

Tables for the Lanthanide

(Rare Earth) Elements

(Elements 62 through 76 in the

Standard Order of Arrangement)

NATIONAL BUREAU OF STANDARDS

The National Bureau of Standards' was established by an act of Congress March 3,

1901. The Bureau's overall goal is to strengthen and advance the Nation's science andtechnology and facilitate their effective application for public benefit. To this end, theBureau conducts research and provides: (1) a basis for the Nation's physical mea.sure-

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iATIOHAL B'JF.E?.0 CF STU^IBAHIIS

^'^^ Selected Values of Chemical Thermodynamic

p7JoProperties

Q^ , Tables for the Lanthanide (Rare Earth) Elements

(Elements 62 through 76 in the Standard Order

of Arrangement)

R. H. Schumm, D. D. Wagman, S. Bailey,

W. H. Evans, and V. B. Parker

Physical Chemistry Division

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.

\ /

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

NATIONAL BUREAU OF STANDARDS, Richard W. Roberts, D/recfor

Issued April 1973

National Bureau of Standards Technical Note 270-7

Nat. Bur. Stand. (U.S.), Tech. Note 270-7, 93 pages (April 1973)

CODEN: NBTNAE

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

(Order by SD Catalog No. C13.46:270-7).

Price $1.25 domestic postpaid or $1.00 G.P.O. Bookstore

Abstract

Contains tables of values for the standard heats and Gibbs (free)

energies of formation, entropies and enthalpies at 298.15 K and

heats of formation at K for compounds of the rare- earth elements

(the lanthanides; lutetium through lanthanum; elements 62 through

76 in the Standard Order of Arrangement). These tables are a

continuation of the comprehensive revision of NBS Circular 5 00.

Key words: Cerium compounds; dysprosium compounds; enthalpy;

entropy; erbium compounds; europium compounds; gadolinium

compounds ; Gibbs energy of formation; holium compounds; lanthanides;

lanthanum compounds; lutetium compounds; neodymium compounds;

praseodymium compounds; promethium; rare- earth elememts;

samarium compounds; terbium coinpounds; thulium compounds;

ytterbium compounds.

Ill

PREFACE

Technical Note ZlO-7 is the seventh part of a series of Notes

containing the tables of numerical 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 the compounds of 15 elements, numbered 62 through

76 in the Standard Order of Arrangement. In addition there is an

Appendix which contains a list of all the corrections and misprints

which have been detected in the previous Notes of this Series.

The continued encouragement and support of the Office of

Standard Reference Data of the National Bureau of Standards is

gratefully acknowledged.

IV

Contents

Preface iv

Introduction vii

Standard Order of Arrangements of the Elements^ Figure 1 . . xi

Table A. Conversion Factors for Units of Molecular Energy . xii

Table 62 Lutetium 1

Table 63 Ytterbium 4

Table 64 Thulium 9

Table 65 Erbium 13

Table 66 Holmium 16

Table 67 Dysprosium 21

Table 68 Terbium 25

Table 69 Gadolinium 29

Table 70 Europium ...» 33

Table 71 Samarium 37

Table 72 Promethium 42

Table 73 Neodymium 43

Table 74 Praseodymium 48

Table 75 Cerium 53

Table 76 Lanthanum 60

Appendix 69

Index of Contents c 73

SELECTED VALUES OF CHEMICAL THERMODYNAMIC PROPERTIES

INTRODUCTION

Substances and Properties Included in the Tables

The tables contain values where known of the enthalpy and Gibbs

energy of formation, enthalpy, entropy and heat capacity at 298.15 K(ZS^C), and the enthalpy of formation at K, for all inorganic substances

and 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 carbon

atoms

.

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

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

composition.

Physical States

The physical state of each substance is indicated in the column

headed "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 298.15 K.

Definition of Symbols

The symbols used in these tables are defined as follows: P =

pressure; V = volumie; T = absolute temperature; E = intrinsic or

internal energy; S = entropy; H = E + PV = enthalpy (heat content);

G = H - TS = Gibbs energy (formierly the ^ree energy); C = (dH/dT)-., =

heat capacity at constant pressure.

VI

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

(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 substance

in 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 thermodynamic 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 25 "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 liqmd 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 Hi" 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 K. If the indicated standardstate 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, \anless 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 exceptin the case of the hydrogen-deuterium ( H- H) system. Where data havebeen available only for a particular isotope, they have been correctedwhen possible to the normal isotopic composition.

The values of the enthalpies of formation of gaseous ionic speciesare computed on the convention that the value of AHf ° for the electronis zero. Conversions between and 298.15 K are calculated usingthe value of H2Q8-Hq = 1. 481 kcal per mole of electrons, and assumingthat the values of H2Q0-H0 for the ionized and vui-ionized molecules are

the same.

VII

Conventions Regarding Solutions

Solutions in water are designated as aqueous (aq); other solventsare 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 non-dissociated solute in aqueous solution

is taken as the hypothetical ideal solution of unit molality, which has beendesignated as "std. state, m = 1". For strong electrolytes in aqueoussolution the conventional standard state is the ideal solution of unit

activity (unit mean molality). For nonaqueous solutions the standardstate of the solute is the hypothetical ideal solution of unit molefraction of solute (std. state, X2 = 1).

The value of IHl" given the tables for a solute in its standardstate 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 elennents

comprising the solute, each in its standard reference state, and the

appropriate total number of moles of solvent. In this representation

the value of AHf° 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 thermodynainic properties tabulated for the

individual ions in aqueous solution are based on the usual conventionthat the values of AHf°, AGf°, 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 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 "\in-ionized" is used. For an ionic species the properties tabulated

refer to that undissociated ion. By adopting the above convention with

respect to aqueous H , it follows that the thermodynamic relation A Gf°

= A Hf° - T ASf° will not hold for an individual ionic species. Howeverno problem arises when neutral chemical systems are considered.

Vlll

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. 00029

cal/deg molF = 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 degO'C = 273.15 K

These 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 anda\ixiliary 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 vmiform 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 among 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.

2A. E. Cameron and E. Wichers, J. Am. Chem, Soc. 84, 4192 (1962).

IX

Furthermore the calculated value of any thermodynamic quantity for a

reaction is independent of the path chosen for the evaluation.

In Sonne cases new^er 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 uncertain-

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 ixncertainties. 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 connposition

values are frequently tabulated to more figures to make possible the

recovery of enthalpies of solution and dilution. Similarly values of

A Hfrt and AHflqo ic may be 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.

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 compound is listed \ander the element occurring latest

in the list; water of hydration is neglected. Within a given element-table will be found all of the compoonds 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.

X

STANDARD ORDER OF ARRANGEMENT

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TABLES OF SELECTED VALUES OF PROPERTIES

SERIES I

Enthalpy of Formation at 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

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fl) 2 .3 5^ ^ .3 5 ^ ^ 3 2

66

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s ^ <T> 00 r-^ CO o^ ON CO CO .—I uo

ti ^ CO <J- m ^D r^ 1-1 1 t-t t-l .-1

1 1 1 1 1 1 1

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cr cr o" 0* D-•r-t o n! to ro ra n) o o o o 60 bO

oXI

Wi-i .-1

cII II

rt B B

4-> C

01 4) 24-1 J-l -g

II II m t^ II cc E E " " EmW u

c4-> o

(0

nj ra to 3m 4J 4J ^ "^ +J (3

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CM CO O CO O O CM CO

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(4 ^ ^ ^ ^ ^ ^ ^ ^ 2 2 ^ ^

67

APPENDIX

Errata for Technical Notes 270-3, llQ-k, 270-5, and 270-6

TN Page

3 22 HFCliq) ^Hf°gg = -71.65 kcal/mol

X denotes undetermined residualentropy

3 26 HCl in 150H2O(aq) ^298 = -39.710 kcal/mol

3 32 HBr(g) AHfJ = -6.826 kcal/mol

3 41 I Cl', std. state. ^298 = -32.9 kcal/mol

m=l(aq) Z^f = -27.8 kcal/mol

S" = 52.9 cal/deg mol

3 43 S(g) mf° = 56.951 kcal/mol

s" = 40.084 cal/deg mol

3 48 H2S"^(g) ^5 = 237.0 kcal/mol

H2S2(liq) ^298 = -4.33 kcal/mol

H2S2(g) = 3.71 kcal/mol

H^S^Cliq) = -3.57 kcal/mol

H2-S3(g) = 7.29 kcal/mol

H2S^(liq) = -2.99 kcal/mol

^284(8) = 10.57 kcal/mol

H2S3(liq) = -2.49 kcal/mol

H2S3(g) = 13.84 kcal/mol

H2Sg(liq) = -1.99 kcal/mol

3 56 Se(g) H°-H° = 1.4815 kcal/mol

S** = 42.21 cal/deg mol

Cp^ - 4.978 cal/deg mol

3 61 N(g) Z^Gf° = 108.886 kcal/mol

S« = 36.613 cal/deg mol

3 85 PH„, std. state. ^298 = -2.27 kcal/mol

in=l(aq) ^f° = 6.05 kcal/mol

S" = 28.7 cal/deg mol

69

TN

3

Page

85

86

87

89

91

97

132

196

208

231

APPENDIX

Errata (Cont.)

+PH. , std. state,

in=l(aq)

H PO "_, std. state,

in=l(aq)

H PO in 0.75H2O(aq)

PH. OH, std state,

in=l(aq)

t£.V

tGV

.AHf298

22.0 kcal/mol

-270.17 kcal/mol

-304.35 kcal/mol

AHf° = -70.59 kcal/mol

ZCf° = -50.64 kcal/mol

S° = 45.4 cal/deg mol

H.P^O^ in 500H-0 should be in 150H^O4 2 7 2 2

PN(g) AHfQ

AsCl^Cliq)

AsCl^Cg)

ZNGf

298

298

^5AHf

298

298

= 8. kcal/mol

7.76 kcal/mol

2.47 kcal/mol

= -62.0 kcal/mol

= 51.7 c:>l/deg mol

= -62.12 kcal/mol

= -62.5 kcal/mol

= -59.5 kcal/mol

C2H glycollate ion ^^^298 " "155.9 kcal/mol

std. state, m=l(aq)

B (amorp) X denotes undetermined residualentropy

Al (c) ; the third, fourth and fifth lines should read;

P

k

298

TeCSeO^)^ should be TY^iSQ.0^

^

AHf^gg = -391. kcal/mol

= -397. kcal/mol

(Delete value for ^^\^^Mf°^o = -395. kcal/mol

Tl2Se(c)

TlOCH^Cc)

formula weight = 487.70

AHf° - = -39.7 kcal/molzyb

70

4

4

4

4

4

4

APPENDIX

Errata (Cont.)

TN Page

3 233 ZnO«2ZnO •2H2 0(c) ^298 = -368.6 kcal/mol

ZnO'2ZnO • 3H2 0(c) ^298 = -438.6 kcal/mol

3 234 ZnF^Cc) ASf -170.5 kcal/mol

3 244 ZnAs2(c)

Zn^As^ (c)

^298 =

^l98=

-10.0 kcal/mol

-7.7 kcal/mol

3 248 CdF , std. state. ^298 = -177.14 kcal/mol

in=l(aq)

4 3 Hgl(g) ^0 =

^298 =

^^298 =

32.9 kcal/mol

31.64 kcal/mol

21.14 kcal/mol

14

16

57

59

60

62

CuC 12(c) Cp< 17.18 cal/deg mol

Cu„(OH) CI should be CuCl •3Cu(0H)<,, formula weight 427.110

CoBr in 1000H20(aq) AEIf° g = -71.6 kcal/mol

[Co(NH3)g]3+

std.

state, m=l(aq)

[Co(NH2)g]N^^"^, std.

state, m=l(aq)

,3+.

ASf°

AGf°

= -37.6 kcal/mol

= 35. eu cal/deg mol

42.9 kcal/mol

60. cal/deg mol

[Co(NH3)^(H20)2]""(aq) AHf°gg = -244.2 kcal/mol

= -125.5 kcal/mol

S° =107 cal/deg mol

Z^f° = -117.4 kcal/mol

S* = 140. cal/deg mol

[Co(NH3)g](N03)3, (c) ^f<

std. state^ m=l(aq)

63 [Co(NH3)^Cl2] cis(aq) ^^293 = -160.5 kcal/mol

trans (aq) ^298^ -162.3 kcal/mol

[Co(NH^),Cl^]Cl cis(c) AHf° _ = -209.1 kcal/mol

trans (c) AEIf° _= -209.7 kcal/molZyo

cis(aq) ^^f^Qo = -200.5 kcal/mol

trans(aq) AHf° _=-202.3 kcal/molZyo

71

APPENDIX

Errata (Cont.)

TN Page

4 63 [Co(NR^) ]C1^ std. Z^Gf° = -131.7 kcal/mol

state, tn=l(aq) S° = 75. cal/deg mol

4 63 [CoCNH^) (H20)2]Cl2(c) ^^298 " "366^9 kcal/mol

in lO^OOOF^O (aq) AHf°gg = -364.1 kcal/mol

4 64 [Co(NH„),](C10, )^(c) AGf° = -53.0 kcal/mol

S° = 147. cal/deg mol

std. state, m=I(aq) Z^f° = -43.8 kcal/mol

S" = 166. cal/deg mol

4 65 [Co(NH„)^]Br„ (aq) Z£f° = -112.2 kcal/molJ D J

Std. state, m=l S° = 94. cal/deg mol

4 66 [Co(NH2)g]l3 (aq) Z^° = -74.6 kcal/mol

std. state, m=l S° = 113. cal/deg mol

4 67 [Co(NH„),]SO,'^ ASf° = -220.2 kcal/molJO HStd. state, m=l(aq) S° = 57. cal/deg mol

4 68 Co(HCO ) should be Co(HCO )

4 70 [Co(NH3) C^O ]"''(aq) -^£298 " "298.0 kcal/mol

4 98 PtS(c) ^298"^0 " ^'^^^ kcal/mol

m£^ = -19.020 kcal/mol

4 99 PtTe2(c)^298""o

" ^'^^^ kcal/mol

S* = 28.92 cal/deg mol

Cp" = 18.03

4 108 Mnl2-4H20(c) ^^298 " '^^^'^ kcal/mol

4 113 MnC20^(c) ^^^298 " "2^5.9 kcal/mol

MnC20 .2H20(c) ^^298 " "389.2 kcal/mol

S° = 48. cal/deg mol

MnC20 •3H20(c) ^^^298 " "'^59.1 kcal/mol

5 2 ^10^8^" ^^^' ^^^^®^ "^^298 ="^^^^' kcal/mol

in=l(aq) S" = 53. cal/deg mol

H V^^O^g"^" std. state, ^£398 =-1846. kcal/mol

m=l(aq)

72

INDEX OF CONTENTS

ChemicalSynabol

Ag

Al

Ar

As

At

Au

B

Ba

Be

Bi

Br

C

Ca

Cd

Ce

CI

Co

Cr

Cu

Dy

Er

Eu

F

Fe

Ga

Gd

Ge

H

Element Table Volvime -

Number Page Number

Silver 37 4- 29

Alumimam 29 3-207

Argon 5 3- 17

Arsenic 20 3- 95

Astatine 13 3- 42

Gold 38 4- 39

Boron 28 3-196

Barium 96 6- 78

Beryllium 92 6- 1

Bismuth 22 3-103

Bromine 11 3- 31

Carbon 23 3-106

Calciiom 94 6- 30

Cadmivim 34 3-248

Cerium 75 7- 53

Chlorine 10 3- 24

Cobalt 40 4- 54

Chromium 51 4-120

Copper 36 4- 13

Dysprosium 67 7- 21

Erbium 6,5 7- 13

Europivim 70 7- 33

Fluorine 9 3- 21

Iron 41 4- 74

Gallium 30 3-218

Gadolinium 69 7- 29

Germanium 25 3-177

Hydr ogen 2 3- 12

73

ChemicalSymbol

He

Hf

Hg

Ho

I

In

Ir

Kr

La

Lu

Mg

Mn

Mo

N

Nb

Nd

Ne

Ni

O

Os

P

Pb

Pd

PmPo

Pr

Pt

Ra

Element Table Volume -

Number Page Number

Helium 3 3- 15

Hafnium 59 5- 22

Mercury 35 4- 1

Holmium 66 7- 16

Iodine 12 3- 36

Indium 31 3-223

Iridium 46 4-103

Krypton 6 3- 18

Lanthanum 76 7- 60

Lutetium 62 7- 1

Magnesium 93 6- 9

Manganese 48 4-106

Molybden\im 52 4-129

Nitrogen 18 3- 61

Niobium 55 5- 6

Neodymium 73 7- 43

Neon 4 3- 16

Nickel 39 4- 43

Oxygen 1 3- 11

Osmixom 47 4-104

Phosphorus 19 3- 84

Lead 27 3-187

Palladium 42 4- 90

Promethium 72 7- 42

Polonium 17 3- 60

Praseodymium 74 7- 48

Platinum 45 4- 96

Radium 97 6-103

74

ChemicalSymbol

Re

Rh

Rn

Ru

S

Sb

Sc

Se

Si

Sm

Sn

Sr

Ta

Tb

Tc

Te

Ti

Tl

Tm

V

WXe

Y

Yb

Zn

Zr

Element Table Volume -

Number Page Number

Rhenium 50 4-117

Rhodium 43 4- 93

Radon 8 3- 20

Ruthenium 44 4- 94

Sulfur 14 3- 43

Antimony- 21 3- 99

Scandium 60 5- 24

Selenium 15 3- 56

Silicon 24 3-171

Samarium 71 7- 37

Tin 26 3-181

Strontium 95 6- 57

Tantalum 56 5- 10

Terbi\im 68 7- 25

Technetixom 49 4-116

Telluriiim 16 3- 58

Titanium 57 5- 12

Thallivim 32 3-227

Thulium 64 7- 9

Vanadiiom 54 5- 1

Tungsten 53 4-134

Xenon 7 3- 19

Yttrium 61 5- 28

Ytterbium 63 7- 4

Zinc 33 3-233

Zirconium 58 5- 18

* U. S. GOVERNMENT PRINXrNG OFFICE : 1 973—51 1 .325/241

75

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U.S. DEPT. OF COMM.BIBLIOGRAPHIC DATA

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NBS-TN-270-73. Recipient's Accession No.

4. TITLE AND SUBTITLESelected Values of Chemical Thermodynamic PropertiesTables for the Lanthanide (Rare Earth) Elements(Elements 6Z through 76 in the Standard Order of Arrangement)

5. Publication Date

April 1973

6. Performing Organization Code

7. AUTHOR(S) R. H. Schumm, D. D. Wagman, S. Bailey,W. H. Evans, and V. B. Parker

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Contains tables of values for the standard heats and Gibbs (free)

energies of formation, entropies and enthalpies at 298.15 K and heatsof formation at K for compounds of the rare-earth elements ( thelanthanides ; lutetium through lanthanum; elements 62 through 76 in theStandard Order of Arrangement). These tables are a continuation of

the comprehensive revision of NBS Circular 500.

Keywords: Cerium compounds; dysprosium compounds; enthalpy;entropy; erbium compounds; europium compounds; gadolinium compounds;Gibbs energy of formation; holium compounds; lanthanides; lanthanumcompounds; lutetium compounds; neodymium compounds; praseodymiumcompounds; promethium compounds; rare-earth elements; samariumcompounds; terbium compounds; thulium compounds; ytterbium compounds,

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