SCIENTIFIC ABSTRACT SMIRNOV, M.V. - SMIRNOV, M.V.

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• Publication Date: December 31, 1967
• Content Type: SCIENTIFIC ABSTRACT

5W SOY/20-121-4-31/54
AUTHORS: Smirnov, M. V., Ivanovskiy, L. Ye., Loginov, 1-1. A.
TITLE: The Equilibrium Potentials of Titanium in Chloride Melts
(Ravnovesnyye potentsialy titana v khloridnykh rasplavakh)
PERIODICAL: Doklady Akademii nauk SSSR, 1958, Vol 121, Nr 4, pp 685-6aa
(USSR)
ABSTRACT: The authors measured the equilibrium potentials in pure argon
in a hermetically closed wide test tube of quartz. On the
bottom of this tube there was an eutectic mixture of lithium
chloride and potassium chloride. An electrode of titanium
iodide was fastened to a molybdenum feeder and it was immersed
in a salt melt of the same composition. The potential of the
titanium electrode was measured with respect to a lead elec-
trode. The results of the measurements, (with respect to a
chlorine electrode of comparison) are given in a diagram
which demonstrates the dependence of the electromotive force
on the temperature for various given concentrations of the
titanium in the electrolyte. The experimental points agree
well with straight lines. Another diagram shows the isothermal
Card 1/3 lines deduced from the above-mentioned results for 700, 800,

SOV2o-121-4-31/'54
The Equilibrium Potentials of Titanium in Chloride Melts
900, and 1000 0K. The equilibrium potential of the metallic
titanium electrode in chloride melis which contain less than
6 weight % of titanium depends on its molar concentration
in the electrolyte according to the following thermodynamical
equation: E = E0 2,3 RT/2F) lg [Ti 2+
Ti/ti2+ + ( I -
This shows that such melts contain ions of divalent titanium
and behave as ideal solutions. The quanti y E 0
Ti/Ti2+ may
be found from the above-mentioned experimental data,
E0i/Tj2+ = (-2,371 + 6,09.10-4T)V is obtained with respect
T
to the chlorine electrode. For the calculation of the
isobaric potential for the composition of the liquid titanium
dichloride from the elements the equation
A z = (-109 36o + 27,03 T) cal/mol TiCl 2 may be used. There
are 4 figures and 12 references, 3 of which are Soviet.
Card 2/3

SOV2o-I 21-4-31/54
The Equilibrium Potentials of Titanium in Chloride Melts
ASSOC19RION: Laboratoriya elektrokhimii Urallskogo filiala Akademii nauk
SSSR
(Laboratory of Electrochemistry of the Ural Branch,,AS USSR)
PRESENTED: April 11, 1958, by A. N. Frumkin, Academician
SUBMITTED: March 25, 1958
Card 3/3

Swirnav, 1,%V., and L.Ye. D.,anorvskiy (Institute o-f' Chemistry, Urals Branch,
Academy of Sciences USSR). Electrolysis of a Ghloride Bath With Titanium
Monoxide Anodes, p. 100. Titan i yego splavy. vyp. II: Metallurgiya titana
(Titanium and Its Alloys. No. 2: Metallurgy of Titanium) Moscow, Izd-vo kN
SSSR, 1959. 179 p.
This collection ofpapers doals with sources of titanium; production of
titanituii dioxide, metallic titanium, and titanium sheet; slag coiaposition;
determination of titanium content in slags; and othtr rolated matters. The
sources of titanium discussed are the co7anplex sillimanite orals of the hy-akhtin-
skoye Deposit (Buryatakaya ASSR) and certain aluminum ores of Eastern Siberia.
One pap4!r explains the advantages of using ilmenite titanium slags for the pro-
duction of titanium dioxide ky the sulfuric acid method. Production of metallic
titanium by thermal reduction processes (hydrogen, magnesium, and carbon rcduc-
tion) is the subject of several pz:Lpenrs, while other papers are conctrned with the
electrolytic production of titanium. Other subjects dealt with are interaction
of titanium with water vapor and with hydrogen and the determination of titanium
in slags.

5(4) ?HAZE I BOOK EXPLOITATION SOV/2216
Soveahchanlye p0 elaktrokbimli, 4th, Moseo-, 2956.
Trudy... ; Itborn'ki (Transactions of the Fourth Conference on Elect
rochemistry; Collection or Articles) Moico., lzd-vo AN SSE,"
1959, 868 P. Errata slip Inserted. 2,500 copies printed,
Sponsoring Agencyt Akedemlya nauk SSSR. Otdal.nlye k1siml-crieskikh
nauk.
Editorial Boardi A.W. PruMkls (Reap. Ed. ) Academician, O.A. Y
Profeaaorl 3.1. ZhdanoV (Reap. Secretary), B.S. Xabano~.
ressor. 3.1. Zhdanov (Reap. Secretary)l B.N. Kabanov,
Ya. M. Kolotyrkl-n. Doctor or Chemical Sciences; V.V. 1,03-. P
Lukovtaev, Professor; Z.A. Solov1y,1vai V.V. Stender, P.~f~jao-
and O,M..FlorIanovich;k.Rd of Publishing House; N.G. Yegorcv;
rech. Ed : T. A. PIruna va:
PURPOSE: This book Is intended for chemical and electrical eng---
nee", physicists. metallurgists and researchers intertated in
.~..s aspects of electrochemistry.
,E.
OVV
-RAr
T c book Contains 127 of the 2118 reports
hh onrerence on E -vsent:dDe
the Fourt prby th
C laenctrochem--stry sponsored a;art
ment of Chemical Sciences d the Institute of Physical Chem,
at
AcAd:my or Sciences, USSR, The collection pertains to dirr'r.'4'!7^
bran hes or electrochemical kinetics, double
gal vanic Processed In metal elbctrodepositan layer theories 4,d
'01y and industrial elect-
Ab.-Idg.d discussions are given at the end of each 41,4-
alon-~h. Jor-Ity of reports not included here have been
publis hed In"period icaIliterature. No personalities are mentioned,
References are given at the and or moat or the article,.
-fl-lla-11- A-K-. I
ranrlr-Academy o-r"S`c1c7E-.ie3, USSR). Cathodic Processes During_
the Preelpitettlon or Thorlum Fro. Fused Electrolytes 340
--9-U-1-1 I I T , and ALV PPzhIn3kaya (Ocauda.-stvennyy nauchno-
,,~rl iz --
1;~O~aiel 14kiy n't Zlt't t3vctnyth, netlllo~~'tate Sole-
3ea rch Institute of Nonferrous Metals). Mchar.13m of
R uc tion of Galena From Suspensions In need Mixtures of
R
:d
Magnesium and Sodium Chlorides at I Llquld-Lead Catloda 152
Panchanko, I.D.(Institut obahchey I neorganicheakoy krzimil AN
--U3SH--Z6At1tut* of General and Inorganic Chemistry. Academy
of Sciences, UkrSSR)jusEquatlon for a Polarographic Wave at
Solid Electrodes In ed Salts 355
'chmqyk -.1i,G. (Aviatalonnyy Inatitut Kuybyshev-Av%&tlon Inati-
to , Kuybyshev). Some Problems or the Polarograpky of Fused
Etulactralytes 358
Vaysburd, S. Ye., and V.L. Meyfeta (Cosudarstvennyy Inatitu,
Card 15/34
P- proy.1tirov.nlyu predpriyatly nikelevoy promyshlennovtl-
S'. te Institute for the Planning or Enterprises of the
Nickel Industry). DOCC-P03itl0r) VOltage and Properties of
Slags Used in Nonferrous Metallurgy ~62
DlOcus"10n IV.P. M35hovets and contributing authoral 365
PART V. THE ELECTRODE POSITION OF -TTALS '69
-,Ajah .,- R--
r
Iftyalcal Institute 01- the Bulgarian Academj of- Science"
Spiral Growth and Overvoltage During the Elect rocry3tal I jZat4
.on
of Silver 371
U..?Iil,and B.E C.Qn,~!%.y (U.S.A.). D.t.
nation or Faraday 1-mpeciance a~-Solid i ictrodta and Ph'e!..
Which Determine Rate During the Electro4epoaltlon of Copper 380
-Vargramyan, .4.T. Nonhomosenalty of an Electrode Surface and
Card 16/ 34
the Kechanlam of the Electrooepo3itlon of Xetals 395
Polukarov, Yu, X. , and K,M, Gorbunova (Institute of Physical.
Chemistry, Academy of Sciencea,USSR). Some Theo~rirnl

Cher-Ical form of -the notion of matter. Part 1: Daterminaticn
nf t'-re chemical form of the zot_'on of mattcr. Filos. vop.
f-z.i no. 1:73-82 159. (',U-PL 14:2)
(Motion) (Chemical affinity) (riatter)

SMIRNOV, M.Y.; IVANOVSKIY, L-Te.
Electrolysis of the chloridizing bath with anodes of titanium
oxide. Titan i ego splavy no.2:100-102 '59.
(MIBA 13:6)
1. Institut khimii Urallskogo filiala AN 33SR.
(Titanium--31actrometallurgy)

5W
AUTHORSi Smirnov, M. V., Yushina, L. D. SOV/62-59-2-10/,61-.

TITLE; Equilibrium Potentials of Metals in Molten Electrolytes
(Ravnovesnyye potentsialy metallov v rasplavlennykh
elektrolitakh) Communication 1. Equilibrium Potentials of
Thorium in Chloride Melts (Soobahcheniye 1. Ravnoveanyye
potentsialy toriya v khloridnykh rasplavakh)
PERIODICAL: Izvestiya Akademii nauk SSSR. Otdeleniye khimicheskikh nauk,
1959, Nr 2, pp 251-258 (USSR)
ABSTRACT: In the present paper the authors present the determination
results of equilibrium potentials of thorium in equimolar
mixture of sodium- and potassium chlorides both with and
without thorium-chloride addition. The equilibrium potential
of thorium. in chloride melts which contained in the initial
was measured in the temperature
state 0.14 up to 78% ThCl
4
range of 680 - 8250 (Fig 2). In order to determine the change
of the electromotive force with the varying concentration
of ThCl2 in the melt, isothermal lines were drawn (Fig 3).
The molten mixtures of sodium- and potassium chloride with
Card 1/3 thorium dichloride behave in all concentrations of ThCl 2 like

Eauilibrium. Potentials of Metals in Molten SOV/62-59-2-10/40
Electrolytes. Communication 1. Equilibrium Potentials
of Thorium in Chloride Melts
ideal solutions. A dependence of the equilibrium potential
of thorium on temperature and concentration was found.
According to experimen-l"al data the oxidation-reduction
potential of thorium in chloride melts as well as the equili-
brium constant of the reaction was calculated:
Th 4+(melt) + Th:i--42Th 2+ (melt).
In the temperature range of 680 - 825 0 the equilibrium constant
varies from 510 up to 0.91. According to the temperature
dependence of the electromotive force of galvanic elements
with the melt containing thorium dichloride the quantities
of the decomposition voltage of the molten ThCl, and the
r_
variation of the isobaric potential for the following reac-
tions were calculated:
Th(solid) + C1 2(gaseous) ThC 12 (liquid
and ThC1 (liquid) + Th(solid) 2ThCl quid)
4 2(14
The stationary potential of thorium. in the equimolar mix"ure
Card 2/3 KC1 + NaCl at 700 - 8420 was determined (Fig-4). There are

Equilibrium Potentials of Metals in Molten SOV/62 - 5 9-2 -1 Of/.
Electrolytes. Commuflication 1. Equilibrium Potentials
of Thorium in Chloride Melts
4 figures and 12 references, 9 of which are Soviet.
ASSOCIATION: Urallskiy filial Akademii nauk SSSR (Ural Branch of the
Academy of Sciences, USSR)
SUBMITTED: March 18, 1957
Card 3/3

5-'2), 5W
LUTHORS. Tsiovkina, L. A., Smirnov, M. V, SOV/78-4-1-301/48
TITLE: The Influence of the Nature of Cations and Anions on the
Solubility oil Titanium Tetrachloride in Salt Malts
(Vliyaniye prirody kationov i anionov na rastvorimost'
tetrakhlorida titana v solevykh rasplavakh)
PERIODICAL: Zhurnal neorganicheskoy khimii, 1959, Vol 4, Nr 1, PP 158-162
(USSR)
ABSTRACT: The solubility of titanium tetrachloride in melts of LiCl,
KC1, CsCl, NaCl-KC1, and an equimolar mixture of NaCl-KC1
with additions of 10, 15, and 20 wt.% NaF was examined at
650 - 8000. The dependence of the solubility of TiCl 4 on
the nature of the cations in the melt shows a solubility
increase in the direction from LiCl to CaCl. The solubility
increase is caused by the formation of complex anions. The
complex forming process is indicated by the following reactions:
TiCl 4gas +C1 Melt ~-tTiCl 5melt'
2-
Card 1/2 TiCl 5melt +C1 melt TiCl 6melt'

The Influence of the Nature of Cations and Anions SOV/78-4-1-30/48
on the Solubility of Titanium Tetrachloride in Salt Melts
The dependence of.the solubility.of titanium tetrachloride
in the melt of NaCl-KC1(1:1) on the temperature and the
dependence of the solubility of the NaF concentration was
investigated. In melts with fluorine ions the solubility of
TiCl4 incred6e6~witli the formation of titanium fluorine com-
2- 2-
plex TiF6 w The complex ion TiF6 has a higher temperature
stability than the ion Tici 2- There are 6 figures and 13
6 *
references, 1 of which is Soviet,
SUBMITTED: October 28, 1957
Card 2/2

05871
5(2) SOV/78-4-11-24/50
AUTHORS: Smirnov, M, V,, Chukreyev, N. Ya.
TITLEt The Behavior of Beryllium in Fused Salt Baths in the Presence
of Metallic Beryllium
PERIODICAL: Zhurnal neorganicheskoy khimii, 1959, Vol 4, Nr 11,
pp 2536 - 2543 (USSR)
ABSTRACT: Alkaline- earth metals are dissolved in their chlorides under
the formation of subohlorides. The authors found also for
berylliuii (Ref 3) that the Be + ion is present in chloride
melts in addition to the Be2+ ion. In order to confirm this re-
sult, the reaction of metallic Be in alkali-chloride melts is
investigated here within the temperature range 351-600.0. The
reaction Be2++Be=2Be+ is measured by variation of the.redox
potential of a-molybdenum electrode. t6 redox potential varied
by 1.3 v, and thus allowed for the determination of the smallest
Be+ quantities. To make sure whether this was rq4lly a varia-
tion ~f the redox potential of the molybdenum electr ode, the
authors compared the potentials of the molybdenum electrode
and the~beryllium electrode with those of a-chlorine electrode
Card 1/3 (Table 1). The Be electrode had a constant potential of -2.44 Y

05871
The Behavior of Beryllium in Fused Salt Baths in SOV/78-4-11-24/50
the Presence of Metallic Beryllium
Card 2/3
whereas the potential of the Mo electrode dropped from -1.13 7
to - 1.82 v. Figure 1 shows the course of the redox potential
during the experiments which were extended to 30 h. The
potentials of the Mo and Be electrode could not be fully com-
pensated because the sarface of the latter was passivated. The
weight loss of the Be anode was measured for the purpose of
determininp the equilibrium constant of the reaction
Be2++Be--,-' 2 Be+. The scheme of figure 2 shows the apparatus
used. A eutectic LiCl-KC1 melt served as electrolyte, the anode
and cathode space were separated by a BeO pot, and the cathode
was made of molybdenum wire. Results of 20 experiments are
listed in table 2. As the Be anode corrodes in addition to
the anodic diesolution of Be, the authors determined the disso-
lution rate of Be in chloride melts at the same experimental
temperatures (Fig 3). The results corrected in consideration
of the corrosion of Be in chloride melts and the equilibrium
constant calculated for the experimental temperatures are listed
in table 3. Figure 4 shows the temperature dependence of the
equilibrium constant which satisfies the empirical equation

5W SOV/20-127-5-37/58
AUTHdRS: Smirnov, M. V., Chukreyev, N. Ya.
7 -------------------- -_
TITLE- The Redox Potential of the System Be + /Be ++ in a Melt of A.2141i
Metal Chlorides
PERIODICAL: Doklady Akademii nauk SSSR, 19599 Vol 127, Nr 5, pp 1066-1069
(USSR)
ABSTRACT: In preceding papers (Refs 1,2) the authors found that in
chloride melts which are in contact with metallic beryllium-,
besides Be++- also Be+-ions are contained. There follows the
determination of Eo +9 E0 -t-+, and 0 the basis
Be/Be Be/Be %9+/.Be++ On
of the corresponding thermodynamic equations for the equilibrium
potentials of Be and its mono- and bivalent ionsg and the de-
termination of the redox potential of the system Be+/Be++ in
salt melts. Measurement of the equilibrium potential was car-
ried out in a temperature interval 380-9400 in a measuring cell,
which is shown by figure 1. As an electrolyte, an eutectic melt
of LiCl and KC1 in argon atmosphere was used. Figure 2 shows
the-variation of the electromotive force of the cell
Be jBeCl 29 LiCl,KClj Gi 2C with temperature. The isothermal
Card 1/2 line of the equilibrium potential of the beryllium electrode

SOV/20-127-5-37/58
The Redox Pot ential of the System Be'/Be" in a Melt of Alkali Metal
Chlorides
(E - lg [~e3 , Fig 3) calculated an the basis of the experimental
dat&,-. confirms that the melt contains Be*-ions, the concentration
of which decreases with increasing temperature. Table 1 shows
the results of calculation for melts with different beryllium
content in the temperature interval 700 - 12000K. Figure 4
shows the temperature dependence for 0 'o
qe/Be-~ and EBe/Be-"'
Empirical equations are written down for this temperature de-
pendence, and the constants of the thermodynamic equation for
the redox potential of the system Be-*/Be++ are calculated.
There are 4 figures, 1 table, and 3 Soviet referenceso
ASSOCIATION: Institut elektrokhimii Urallskogo filiala Akademii nauk SSSR
(Institute of Electrochemistry of the Ural Branch of,the
Academy of Sciences, USSR)
PRESENTED: April 13, 1959 by A. N. Frumkin, Academician
SUBMITTED* April 13, 1959
Card 2/2

S/631/60/000/001/001/014
B101/B147
AUTHOR: Smirnov, M. V.
TITLE: Residual currents and cathodic current yield in the electrolysis
of salt melts
SOURCE: Elektrokhimiya rasplavlennykh solevykh i tverdykh elektrolitov,
no. 1, ig6o, 3-6
TEXT: Previous studies on the electrodeposition V Be (ZhFKh, 12, 2174,
1958), Th (Izv. AN SSSR, OKhN, 1285, 1956), Ti (Izv. Sibirskogo otd.
AN SSSR, 1960), Zr and Hf have shown that a charge reversal of ions to
subions occurs: Me Z+ + ne = Me(i-n)+ . The metai deposition sets in as
soon as the concentration of these ions in the electrolyte layer close to
the cathode corresponds to the equilibrium between them and the salt melt.
The charge reversal produces a residual current. The cathodic potential
y is given by 9 = E 0 (z-n)+/, z+ + (RT/nF)lntnFD (z-n)+ [Me Z+ 1/61
Me e me
Card 1/3

S/631/60/000/001/001/014
Residual currents and cathodic... B100147
- D (z-n)+ /D z+19 where Eo (z-n)+/, z+ is a constant of the thermo-
Me me Me e
dynamical equation of the redox potential, D Me z+1DMe(z-n)+ are the
diffusion constants of the ions in the melt, 6 is the thickness of the
diffusion layer on the cathode, [Me Z+1 is the molar part concentration of
the metal ion with ordinary valence in the melt. The residual current
caused by the cathodic charge reversal can now be written as
ires = nFD (z-n )+[Mez+]/6 texp[(nF/RT)((p - Bo (z-n)+/,,z+)] +D (z-n)+/D
Me Me Me mez+
ires reaches a limit when the deposition of the metal begins
(P = equ = const), The ratio of the molar part concentration of the ions
Fie
remains also constant: [Me(z-n)+ I,/- ez+] (z-n)/z = K. If no metal is
IM S
lost by side reactions on the cathode the current yield is given by
I = 1 - 'res /i. If the accumulation of ions of low valency is prevented by
Card 2/3

BARABOSHKIN, A.N.; SMIRNOV, M.V.
Time necessary to attain a steady state in electrolysis with
a constant current intensity. Trudy Inst.elektrokhim.UFUl
SSSR no.lt7-16 160. (NUM 15:2)
(Salts)
,(Electrolysis)

S/631/60/000/001/002/044
B101/B147
AUTHORS: Komarov, V.' Ye., S V., Barabo8hkin, A. N,
TITLE: Equilibrium potentials of zirconium in a fused equimolar
mixture of sodium chloride and potassium chloride
SOURCE: Elektrokhimiya rasplavlennykh solevykh i tverdykh
elektrolitov, no. 1, 1960, 1-f-22
TEXT: Measurements were made at 687-9780C in an equimolar NaCl + KC1 melt,
with 0,16-6.8 To by weight of Zr in an argon atmosphere in order to
determine the temperature coefficient of the equilibrium potentials of Zr
with respect to the chlorine electrode and to clarify the effect of
cations on this coefficient, The emf between Zr and Cl was found to be
Ll - 2,56o - 3.62-10-4T 0.005 v for 0.16 % by weight of Zr;
F, 2 =2,587 - 4-72-10-4T 0.002 v for 1.24 % by weight of Zr;
F-3= 2.6oo - 5-43-10-4T 0.003 v for 6,8 % by weight of Zr. Taking into
account the thermo-emf between the carbon current lead to the chlorine
Card 1/4

S/631/60/000/001/002/014
Equilibrium potentials of zirconium in... B101/B147
electrode and the molybdenum lead to the zirconium electrode, the following
equilibrium potentials 4are obtained: El . -2.552 + 3.45410- 4T v;
E 2 979 - 4.55,10- T vy- E = -2,592 + 5.26-10-4T v, Owing to the
2 . 4+ 2+3
71~a-"Iion 7r + Zr 2Zr (1) the isothermal lines are not 1--near-
mc- it, melt
At low Zr concentrations, the equilibrium constant of this reaction is
-,,en by* K X) 2lz-rl/x, where x = molar part of the Zr ions-
7- x ~- molar part of the Zr 2+ ions, and [Zrj = total concentration of Zr,
The average vale-noy of Zr at (Zrj = 5~83~10- 4 is approximately 2. Fo,-7*
)-:Jr, ~2 .36 at 10000K and 2.26 at 12000K.
'. j - 2-46'110 It is 2
Wo -7-!2.3 kcalimo~le was found in an LiCl - KCI melt, whereas
Z-
LCI-2
AHO amounts to -1-,7.7 kcal/mole for the NaCi + KC1 melt, This
7rCI
2+-
d'~ffere-n~-e is due to the interaction of Zr with chlorine ions in ~-.h=
1--ard 2/4

S/631/60/000/001/002/014
Equilibrium potentials of zirconium in... B101/B147
Assuming a latent heat of fusion of ZrCl4 equal to 9.0 kcal/molej the
heat of formation of ZrCl 2- ions in the melt is found to be -16 kcal/mole.
6
A paper of L S, blorozov, D, Ya. Toptygin (Izv: AN SSSR, OKhN, 1920,
1959) is mentioned. There are 4 figures, 1 table, and 10 references:
6 Soviet and 4 non-Soviet. The four references to English-language
publications read as follows: E. M~ Larsen, J. J. Leddy, J. Am, Chem.
Soc,, 78, 5983, 1956; P. Gross, C~ Hayman, D. L. Levi, Trans. Farad. SO--i
~J, 1285, 1957; A- A. Palko, A. D. Ryon, D. V1_ Kuhn, J. Phys, Chem, 62,
319, 1958; L, Jang, R. G, Hudson, Trans, Metallurg, Soc- AIME, 215,
589, 1959.
Card 4/4

S/631/60/000/001/003/014
Thermodynamics of formation of the B140/BIIO
&>O. the greater part of titanium is bound to the fluorine complex, with
,8~(O, to the chlorine complex, TiO 2 '- C electrodej were produced from
pure TiO 2 for the experiment. TiO 2 was mixed with concentrated, aqueous
glucose solution., The mixture was evaporated and -the residue p--,iverJ zed-
Cylindrical electrodes were molded from the powder and heated at 8000C with
Pxclu3-~cn of air, The Pyrolysis of glucose yielded carbon formJng a
homogeneous mixture with the oxide An analysis of the electrode? yi.elded
52~79/-o T! an,! -,64% C- The following reaction prooeeeded on -his
elpc~rod,~~ T-iO2 4 C - 3e ---~Ti Ti saturaticr, in the electrolytic
Layer near the .cathode gijres a constant, potent,,-al, At first, an
r-QUiMC.i.e,;u1ar HaCl and M m-i-xture was used as eiec-trolyte- 0,1110% by
weight NaF 'gas added in a second series of experiments With higher NaF
content; the TiO C electrode was destroyed The melt was sublect-d -~o
red;.:~~eij pressare for 1 hr, and the gaz rc-cm fialed w-ith C02> and CO to fzor-
a cxjgen a,,--iv1-,ty in the sy:5'em T,ie elec,rode was
Card 2/4

s/631/60/000/001/003/014
Ther ~odjnLinics oi forzation of the ... P1 40/ B1 10
,aZ = -27 190 - 27-513 (1.694 + log EIF J).T+550 cal/g-ion;
AH = -27.2 kcal/g-ion; 53 = 27-513 (1.694-+ log EV'j). AS changes its
J~
_F 2,07-10- 3. For a lower concentration, 6S