SCIENTIFIC ABSTRACT SHCHUKAREV, S.A. - SHCHUKAREV, S.A.

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• Collection: Scientific Abstracts
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• Release Decision: RIF
• Original Classification: S
• Document Page Count: 100
• Document Creation Date: November 2, 2016
• Document Release Date: August 23, 2000
• Sequence Number: 10
• Publication Date: December 31, 1967
• Content Type: SCIENTIFIC ABSTRACT

ANDIRM7, S.D.; SHCHUXAREV, S.A.; BALICHEVA, T.G.
Vibrational spectra of the water of crystallization in the
single crystals NiSO4 -7420, HiSO4 -6H2O and CaS04 -2H20 in
the region of the fundamental frequency for the valence
vibrations of O-H. Zhur. struk. khim. 1 no.2:183-188 Jl-Ag 160.
(L!R~ 13:9)
1. IAninGradskiy gosudarstvenny7 universitet im. A.A.Zhdanova
(Nickel sulfate--Spectra) kCalcium sulfate--Spectra)
(Crystallization, Water of-Spectra)

5 (2); 5 (4) SOV/78-5-1-2/45
AUTHORS. Shchukarev, S. A. ,Oranska a, M. A., Tolmacheva, T. A.;
~Td_._- S
TITLE: Therms,1Disso cia tion of Vanadium Dichloride
PERIODICAL: Zhurnal neorganicheskoy khimil, 1960, Vol 5, Nr 1, PP 8 - 11
(USSR)
ABSTRACT: Publications give different data for the formation enthalpy AH
of VC1 2' The authors report on their indirect determination of
AH by investigation of the equilibrium of VC1 2 reduction by
0 0 0
means of H at 750c, 775 , 800 , and 825 , The method is describ
ed in references 9,10. The experiments lasted for 100-200 hours
Table I shows the values of the dissociation pressure of VC1,.
I
Figure I shows the linear dependence of 19 PC12 on T. The com-
puted values of the formation enthalpy AH and of the absolute
entropy,6S are shown in table 2. The value found for AH is in
good agreement with that assumed by the U.S.A. Bureau of
Card 1/2 Standards. Figure 2 and table 3 show the opposite behavior of

SWHUKAREV, S.A.; KOK071H, G.A.
Determination of the heat of formation of tungsten hexabromide.
Zhur.neorg.khim. 5 no.2:507 F l6o. (NIR& 13:6)
(Tungsten bromide) (Heat of formation)

S/078/6 0/005/008/002/0 18
3004i/BO52
AUTHORS: Shchukarev,--S-. A., Novikov, G. I., Vasillkova, I. V
Suvorov, A. V., An Shaxupin, B. N.,
Bayev, A. K.
~i 'YI
TITLE; The Therm Properties of Chlorides and Oxychlorides
!I odynamic
of Tyaasten and to enum.
V1
PERIODICAL: Zhurnal neorganicheskoy khimii, 1960, Vol. 5, No. 8,
pp. 1650-1654
TEXT: By applying various methods,, the authors wanted to check the
formation heats, formation entropiesl,.and formation enthalpies in the case
of Mo- and W chlorides, published in western papers (Refs. 1, 2). They
investigated: WC1 6;' Mocl 59 WOC1 45P Mocl 4' WO2Cl2 (obtained by a successive
chlorination of WO 3 and MoO 3by means of CC1 4~ moo 2Cl.2(obtained by the
reaction between MoO 2 and Cl 2); MOC139 WC1 49 WCi5(by the reduction of
Mocl 5 and WG16 by means of H 2)... and MoCl 21 WC12 (obtained by dispropor-
Card 1/3

The Thermodynamic Propertie13 ~;f Chiorides S/078/60/005/008/002/018
and Oxychlorides of Tungsten and Molybdenum B000052
tion of MoCl 3 and WC1 4, and MOOC14 ). Two calorimetric methods were applied:
1) Comparison of the heat of solution of the investigated substance to the
heat of solution of a substance whose heat of formation is known (Table 1).
2) Combustion in ox3rgen (Table 2). Furthermoreq the vaporization, depoly-
merization, dissociation, and disproportionation processes taking place in
a state of equilibrium, were spectrophotometrically and tensimetrically
investigated (Tables 3, 4). The enthalpies of formation, and partly also
the standard entropies of formation were calculated from the experimental
data. In Tables 5 (Mo compounds) and 6 (W compounds) they are compared
with the data given in Ref. 2 which were adopted almost unchanged by the
US Nationa-11 Bureau of Standards (Ref. 9). The values determined by the
authors are 1.4 - 1.7 times as high. Therefore, the dependence of the
free energy of formation of temperature is different alt-ogether6 This is 0
graphically represented in Fig. 1 (comparison of determined &H and 6 P
for tungsten compounds9 with the data of the National Bureau of Standards),
and Fig. 2 (comparison of the 4H of Cr. Ito, and W chloridesq with
% form
the data of the National Bureau of Standards). There are 2 figures,
6 tables, and 9 references; 6 Soviet. 2 US, and I Dutch.
Card 2/3

The Thermodynamic Proper-4,JeF )f Ch-',,-rides S/078'60/'005/008/002/018
and Oxychlorides of llluri6st3., ~w.,,4pidenum B0047BU52
ASSOCIATION: Leningradskiy gosudarstvennyy universitet Khimicheskiy
fakulltet
(Leningrad State University Department of Chemistry) -
SUBMITTED: May 6, 1959
Card 3/3

SHCHUKAHEV. S.A.; KOLBlN, N.I.; RTABOV, A.N.
Ruthenium tribromide. Zhm-. neorg. khim. 5 no.8:1900-1901 Ag 160.
(MIBA 13:9)
1. Leningradskiy gosudarstvewWy universitet, Kafedra neorg-ani-
cheskoy khimii.
(Ruthenium bromide)

S/078/60/005/009/0-9/040/yX
BO-7/BO58
AUTHORS: Shchukarev, 3 A and Ryabov, A N
TITLE: Heat of Formation of Ruthenium DioxLde
PERIODICAL: Zhurnal neorganicheskoy kh-im,.,,, 1960, Vol. '5, No. 9,
PP: 193-, - '933
TEXT: The heat of formation of RuO 2 was determined by calorimetric
measurempnts All experiments were conducted at 250 C and a pressure
of 710 atm. The heat of formation amounts to -73t I kcal/mole
Cnly RuO 2 and metallic ruthenium were detected by X-ray examinations
(determined according to Chugayev by means of thiourea) in the
combustion products of ruthenium. The formar-:on of R-jO in the
combusticn products Tas not ascertained The dat-a by Rerry and M"hn
on the heat of formation of RuO 2 (-59.5 kcal/mole) must be described
Card 11/2

Heat ef Formation --f
Ruthenium. Dioxide
S/078 160100~~,1000'1/0' -~' /0'~O/'U.
P-0 I 77B0 j a
as being wr~,ng The f-ree ~-nergv for the formation ~f R--O, is given as
FL~ 60 6 kcal/molt~ Thet-t~ ae 11 tablo and A. references:
A, formation RlAO-
Soviet and 1 German
ASSOCIATION: Ten-:ngradskly gosudars'vennyy unlverslet
A, - Ll
Kafedra neorganicheskoy khimii
(Leningrad State University, Chair of Inorganic
k- Ee r- ~is t r ~y
SUBMUTTED: June 25, 19~0'
Car.~

S/078/0'()/005/009/040/040/XX
B017/BO58
AUTHORS- Shchukarev, (i,. I-G-r-a-nskaya , MT1 (Deceased),
Shemvakina. T- S,
TITLE-
PERIODICAL!
Determination of the Formation Enthalpy of Niobium Penta-
chloride
Zhurnal neorganicheskoy khimii, 1960j Vol, 5. No 9.
pp. 2135 2.36
TEXT. The formation enthalpy of NbC11, was determined by calorimetric
measurE-ments Niobium pentachloride was prepared by chlorination of 0
nio-bium pentoxi-de with carbon tetrachloride in sealed ampoules at 300 C,
The spectroscopir analyses of the samples are given in Table 1- The
formation enthalpy of ni-obium pentachloride was as-,ertained by determining
thp heat effect of the hydrolysis of niobium pentachloride according to
equation NbCl 1; - 5/2 H 20 - 112 Nb 205 4 5HC1. The results of this
a q
determinal-ion ar- given in Table 2 The heat effect of the hydrolysis was
Card 112

Determination of the Formation Enthalpy of S/078/60/005/009/040/040/XX
Niobium Pentachloridp B017/BO58
measured in the isothermic calorimeter at 25 0C A mean value of
.165,59 + 0-45)kcal/mo-I was calculated for AH. The formation enthalpy of
Yliobiiiin pentachloride amounts to -( '93 .7 0.7)kcal/mo I . This value
agrees well with that mentioned by Schafer (Ref.. 1)., There are 2 tables
and 5 referenceQ-4 I Soviet, 2 US, and 2 German.
SUBMITTEDz March 31, !960
Card 212

S/07e 6-0/C05/01 1/0031 025
B01 1-W3060
AUT TIC ~'- "S' Shchukarev, S. A. , Apurina,
I
TITLE: lihe System '-ickel - Tellurium,
0 1960, Vol. 5, No- 11,
~:hurnai neor anicheskoy kh-im"i, 0
2410-2413
pp.
TEXT: The authors investigated the system nickel - tellurium and
checked tne earlier established ;)hase conditions ir, the interval
NiTe 1 . O-jNiTe 2.0' 1,1oreover, they for the first time otudied the region
Ili IT
~' _ ~'iTei.o* An isopiestic method, described previously (Refs. 6,7) was
applied. It is stated that the experiments took 60 hours. Experimental
results obtained at 9000C with preparations NiTe >,1.0 (Table 1) show
that in the system investi.-ated at 9000C there is a wide field of
i the composition NiTe UO
homo eneity, which extends at least fro. 1.0
NiTe 1-7 , and, possibly, even further to a higher tellurium content.
Card 112

The SY.,ti2N1 NiCkei - TellUri=
~i/078/?UO/0015/0 11,'005/025
3015/3060
In tHe interval NiTe 1.0 - NiTe 1-95 the lattice parameters (Table 2) are
dependent, as shown by the X-ray pictures, on the composition, in
a-ree.ment witii previous experimental results. Experiments with
pre-parations 'Ii - NiTe 1.0 show (Table 3) that at '11000C in the system
1rli - Te the comi~oLuids NiTe 0.62 and 11iTe 0.88 exist in a very narrow
hoimo.-eneous re-rion, as -.,;ell as the phase '.iTe 11iTe
0 o.66-o.67 - o.a2-0.83*
The authors thank Ye. V. Stro~;anov and I. I. Kozhina for their assistance
in L_ -in- the ,,-ray Pictures. There are 5 fi-,ures, 3 tables, and 11
references: 4 Soviet, z', German, and 2 US.
~,SSOCIATIO:'I: Lenin~,-radsrkiy --osudarstvennyy universitet (Leningrad State
University)
SUB.'"'T'TED: July 70, 1)5c,
Card 2/?2

SHCffUKAREV, S.A.; VASILIKOVA, I.V.; SHARUPIH, B.N.
Molybdenum halides. Part 4: Determining the eathalpy of for-
mation of molybdew- dichloride and trichloride. Vest.LGU
15 no.10:112-120 160. (KIRA 13:5)
(Molybdenum chloride) (Enthalpy)

SHCHMEM, S.A.; SMIRNOVA, Ye.K.; VASILIKOVA, I.V.; IAM, L.I.
Rathalpies of formation of tantalum pentachloride and pentabromide.
Vent. LGU 15 no.16:113-119 16o. (MIRA 13:8)
(Tantalum chloride) (Tantalum bromide)
(Rathalpy)

-Sf1qjRYKARZV, S.A.; 14LKARNITA, A.A.
Bibliography of works on the periodic law. Vest. WU 15 no.16:151-152
16o. (MIRA 13:8)
(Bibliography-Periodic law)

60
SOV/79-30-2 -1/78
AUTHORS: Shchul~.arev, S A., B-ji-4-s3va,. Z. U1. , 3a-Y-1a':--,)-.-, il. A,
TITLE: Concerning Heat of Solution of Magnesium Perchlorate riex-=-
hydrate
PERIODICAL: ZhUrnal jbshchey klhimil, 196-0, Vol. 30, Nr -2, PP 353-355(LTSSR)
ABSTRACT- Heats -of solution of Mg(C1002 611,30 for various dilutions at
250 were measured in a microcaiorimeter [described In Mishchenko,
K. P., Pronina, M. Z., et al., Zhur. priklad. khim. 27, 1003
(1954)]. Magnesium perchlorate, obtained by dissolving M.-O in
perchloric acid, was recrystallized 3-5 times and dried for 24 hr
Dver concentrated sulfuric acid (the time -of drying was determined
by f ind-ing. the maximum LH in the plDt' of LH vs -Uime) . Tables
L ani 2 list the exDer-'mental results (each is an average of n H
fDund Jn 8-9- experiments. Figure 2 gives the graphical representa-
tion along with the A F1 for zinc perchlorate hexahydrate (Shchu-
'."arev, S. A., Andreyev, S. N., et al., Zhur. obstichey khim., 29,
L)468 (Ly-)9)j. It can be seen that the limiting value for integral
heat of d-TIlution of the uiagnesium perchlorate hexahydrate equals
Card 1/-' 1.00 kcal;mole (reached at dilution ' :1
I ~ -00). Tliere are 2 figures;

C Dn,_,ern -in., _)f --t' !-!--_I~nos iivr, Pet-cjjlL,-)j-:jte 7'~1
I /7i
and 6 ri~ f'eren=', ScVi~ t BeLgi-in, -1 U.S .
U.S. references are: 3meets, Ch, A., 27, Nr 1, 51629 (11~36); Smit,
Ree--, , Hardy , J. Ain. Chem. Soc . , 54 _i-513 32) -
As S cx-, I AT I N f ? ~ I I it - -1, 1 S tt L I I v f y I I I r I II ds 'k L y 1 (1, 11 v I 111 y y
',III Lvc 1%; ~L t,f~t)
S!IBMITWED: Febl-Liar., 10, L95)
Table 1 Table 2
DiLutions Z\Fav Diluti:)ns
1/m,-) 1e) :~C,:l I/rno le)
IWO :25 )
()5 � 0
02
700 1.00 � 0.03 1 t5 .
.
2
47 � 0
02
1 500 1.0) � 0.03 1: It .
.
2
91 � 0
02
1 300 1. 17 � 0.03 1 !) .
.
3
2.1 � 0
02
1 2(Y) 1.73 � 0.03 1 8 .
.
3
42 � 0
02
1 100 1.75 � 0.03 1 7 .
.
56 - 0
3
02
1 511 1.86 1: 0.03 1:6.5 .
.
3.71 10
02
30 jm4 � ().(n .
Card 2/3

Si i
a n id
E; 10EI

10? o l M I 1!-_i '7rl 0 71-n
-,iorhe
-al
m
tn
ir
-Lc-. " he ve s
"Ies g < Zr I < c o <
ren c e s

cc, S r) I T 'I

-
scl-.,r
/r

- - - - - - - - - - -
ca

li,7

f") 3J ic,
T Lj ~21
T I-l' D

SHGEUKAREV, S.-A-;-'ORLOVA, G.M.; BORISOW., Z.U.
Heats of solution of copper Perchlorate hemahydrate in
water and aqueous solutions of perchloric acid. Zhur.ob.
khim- 30 no~7:2097-2102 JI 16o. (KIRA 13:7)
1. Leningradskiy gosudarstvemxVy universitet.
(Copper Perchlorate) (Roat of solution)
(Perchloric acid)

S/079/60/030/007/001/020
BOOI/BO63
AUTHORS:
TITLEt
Shchukarev, S. A., Morozova,
------------
The W - WS1 System
2
M. P., Dameng Kh.
PERIODICALs Zhurnal obshchey khimii, 1960, Vol- 30, No- 7, pp. 2102-2104
TEXTj Contrary to the sulfides of the 3ds elements, which are homogeneous
in a fairly wide range (Refs. 1,2,3,4,5), only little material is available
on the ranges of homogeneity of the sulfides of the 4d5s and 5d6s elements.
It was the purpose of the present paper to study the phases in the W-WS 2
system. The WSx preparations were produced by homogenizing pulverulent
mixtures of pure metallic tungsten and pure sulfur in evacuated quartz
ampoules at 8000C. Annealing took 500 h. The four preparations produced
had the composition WSO'911 WS 1.73' WS 1.989 and WS 2' In accordance with
data published in the-paper of Ref. 6, the X-ray analysis showed only the
lines of tungsten and disulfide in the whole interval W-WS 2. Moreover,
the two lattices showed no change. No homogeneous preparations were
card 1/3

The W - WS2 S y s t e*m S/079/60/030/007-1,001/920
B001/B063
obtained by annealing the tungsten-sulfur mixtures. The quantity of sulfur
was higher than is necessary for the formation of WS 20 The free sulfur
found indicates that WS2 has no range of homogeneity extending to a higher
stoichiometric sulfur content. Thus, it was found that in the W - S system
there is only the compound WS2 which has no noticeable range of homogeneity.
As compared to sulfur. tungsten is only tetravalent, whereas chromium
shows the neighboring valences 2 and 3. and forms compounds with sulfur
that are characterized by wide ranges of homogeneity. Finally, the authors
discuss several rules concerning the change in the ranges of homogeneity
of oxides and sulfides in the periodic system. It may be seen from the
accompanying table that no transfer of sulfur from the sulfide WS,.9,
to metallic tungsten is observable, which is also the case with the pair
WS 1-73 -WS 0.91- There are 1 table and 11 referencess 3 So-wiet, 5 Germang
1 Belgian, and 2 British.
Card 2/3

The W - WS2 System
S/079/60/030/007/001/020
B001/k63
ASSOCIATION: Leningradskiy gosudarstvennyy universitet (Leningrad
State University)
SUBMITTED: July 8, 1959
V-1,
Card 3/3

SHCBUKAREV, S.A~; BORISOVA, Z.U.; GUSEV, A.M.
Heat of solution of cadmium and mercury perchlorates hexahydrates.
Zhur. ob. khim. 30 no.12:3857-3859 D 16o. (MIRA 13:12)
1. Leningradakiy gosudarstvennyy universitet.
(Cadmium Perchlorate) (mercury Perchlorate)
(Heat of solution)

S/05z-/6 1/00----/00 1/01-37/008
B117/B203
AUTHORS: Shchukarev, S, A.T- Savorov. A, V,
TITLE: Thermodynamic study of some :h1orine derivatives of
molybdenum and tungsten
PERIODICAL: Vestnik Leningradskogo universiteta, Seriya fiziki i
khimii, no, 1, 1961. 87-99
TEXT: The authors give results 3f therm-c-aynamic studies of com-pounds of
t,.,,,o isotope groups; MoC 1-MON IMCIO C 1,~ --- MoO, and
5 2 ~
i - WOC 14- WO2C1 2- Wo 3'
WC I They used t'neir mcmbrane- and o-Dti,:otensimetric
methods (Ref. 23: G, I- Novikov, A. V S-vorov, "Zav. lab." no. 06, 750,
1959; Ref. 24: S, A. Shchukarev. G, I, Novikov. A. V. Suvorov, ZhNKh. 1,
2433, 1956). The two apparatus use'. were 4,mDroved., For instance,
temperature was measured -.-.,ith th~ "id of a thermocolumn consisting of
three thermocou ,les an ac--ura~y of -,-,5 B,., means of an MB-01
(:-"PV-01) electron poten-7-iometer :t was Possible to kee-o the temnerature
constant for a long per, c.-- -21~) hr ) wl t~-, The same accuracy. Pressure
Cardl/6

S,, -, 5 A /6 1 1.1" 0 0 0 / 0 0 10 7 /',-; C P,
Thermodynamic study of some ch-iorinz4 !K3 3
,.-,,as meanured in the range of 1-800 mm Hg with ar. m5in (MBP) mercury mano-
meter with ari accuracy of ~0.1 mm Fig, and in the range of 800-1400 mm Hg
with a U-shaped mercury manomt-:ter with an. accuracy of tl mm Hg. With the
Use of an X~/-!9-M (FEU-- 10-M) e__e~~tron plictcmultipli-er together with a volt-
'.L
age divider it was possibie to &xtena -ons:.derabl
y the range of exactly
measureable optical densities- Ili t'-*tfie use of plane -parallel, all-soldered
optical cuvettes, the ootical deris-ity was measured %,ith the same accuracy as
the vapor -pressure (about 0 5, *:~o). The pressure of saturated and unsaturated
IJOC15 vapor was studied. Trio series of measurements were made at a chlorine
pressure of about 300 -and 400 m,'1', H9 -In e temperature range of 801-3000C.
The data averaged by the me thod of t squares correspond to the eauations.
6H, kca~lmole AS energy units
sublimation ~m'ocl 51sclid 10'3 Patm- 9,~ 1 '5,0-4 750VT 21,7-0-5 43.5 'tO.5
evaL)Oration MoCl
~ 5'53.6-3o"O 13.91"0.5 25.3+ 0.5
liqu log P
atm
5
By simultaneous solution of these equations. the melting point 2010C and
the boiling point 2706.50C are obtained, The values ietermined from the
dissociation equation (b:oCl "LICCI + 11- (C1 for the equi-
2)
gas I:f
gas
C,rd 2,16

S/054/61/000/001/007/008
Thermodynamic study of' some chlorine-, B117/B203
librium constant K p correspond to the equation log K. = 3.201 - 2779/T;
6H = 12.8 1 0.5 kcal/mole; 4S = 14~8 0..5 energy units. The data found
for the evaporation process of liquid MOOC14 correspond to the equation:
log P atm ~ 4.783 - 2552/T; AH - 11.7 0.5 kcal/mole;AS - 21.9 � 0.5 energy
units. This gives a boiling point of 250,50C,. The data determined for the
dissociation of MoOC1 according to the scheme (MOOC1 ) =(MOOC1 )+-!(Cl
4 4 3 2 2
from two series of measurements at an initial chlorine pressure of 170
and 430 mm Hg correspond to the equation% log Kp = 3.152 - 2498/T;
&H - 11-5 + 1 kcal/mole!, A.S = 14--5 1 energy unit. To investigate the
thermodynamic characteristics of' MoO 2 Cl 21 the authors studied its process
of formation from MoO 3 and chlorine according to the scheme
(Moo + (C1 (moo Cl -L(O ). Experiments showed that MoO started
31 2) 2 2 ' 2 2 3
reacting with chlorine at temperature above 50000. The results obtained
correspond to the equation; log K p = 3~112 - 2865/T; 6H = 13 � 1 kcal/nole,
AS = 14 + 1 energy units. The pressure of saturated WC1 6 vapor was studied
Card 3/6

S/'054/61/000/001/007/008
Thermodynamic study of some chlorine-, B117,/B203
at pressures of up to 900 mm Hg. The data obtained corresponded to the
following equations: (1) Sublimation 6,-WC1 6: log Patm= 7-00 - 4400/T;
AH = 20.1 t 0.3 kcal/mole; 6S = 34.3 1 0.5 energy units; (2) sublimation
P-WC1 6: log Patm= 5-983 - 3645/T; tH = 16-7 1 0.3 kcal/mole;
&S = 27.5 + 0.5 energy units; (3) evaporation WC16: log Patm= 5.222 - 3216/T;
AH = 14.7 0.5 kcal/mole: AS = 24A 1 0.5 energy units. By simultaneous
solution of these equations the temperatures of phase transformations are
obtained: T = 2310C, Tmelt =2910C. T boil = 3430C is determined by
with P = 1. In the range of unsaturated vapor, the
solving Eq. (3
dissociation of WC16occurs in two stages at the same time. The data found
correspond to the equations: (WC1 ) +-!(C1
6) = (WC15 2 2
log Kp = 6,729 5280/T; 6E = 24,2 1 O~5 kcal//molei AS = 30.8 � 0.5 energy
units; (Wcl 6) (WC14) + (C12) log Kp = 11,200 - 9333/T;
+
AH = 43 1 kcal/mo~e; AS = 51 + 0,5 energy units. This shows that the
dissociation of WC1, in the first stage is more intensive than in the
Card 4/6

Thermodynamic study of some chlorine- B!17/B203
second stage. The pressure of saturated WOCI vapor was measured up to
1340 mm Hg. The data obtained correspond to the equations: Sublimation
WOC14: log Patm = 9.743 - 4789/T: AU - 21.,7 t 0.5 kcal/mole;
f-
4S = 44.2 0.5 energy units; evaporation WOC1 41 log P atm = 4-564- 2250A;
6H = 11 1 kcal/mole; AS = 22 1 1 energy units: hence, the melting point
of 2110C and the boiling point of 22700 are obtained. For the dispropor-
tionation of WOCl 4 according to the scheme 2(WOCl 4)= (WO9C1 2) + (WC'6)'
the following thermodynamic characteristics were determined in first
approximation: log Kp - 1~41 - 2400/T; AR = 11 + lkcal/mole;
f23 = 6 t 1 energy units. In the system 'NO 2Cl 21 the simultaneous course
of three independent processes is assumed: (I) ~Wo 2C1 21 = (WO2Cl 2);
(11) 2 IWO2 C1 21 = (WOC14 ) +[W0 31 , and (III) 3fW02C121 = (WC16) + 2Lw031'
The partial pressures obtained and the respective equilibrium constants
correspond to the equations (pressure in atm): Mlog PWO2 Cl2-6.666 - 5043A:
Card 5/r'

S/054/61/000/~)01/007/008
Thermodynamic study of some chlorine,.. B117/B203
6H = 23 + 11 kcal/mole; AS = 51 1 energy units; (II) log I~Ucl - 11-547-7471/T7
+ 4
/AH = 36 - I kcal/mole; 83 = 56 1 Pnergy units; = 18-455 - 12648/T;
+ (III) log Plh'Cl6
U = 56 - 1 kcal/mole;.6S = 82 1 energy units, The simultaneous solution
of these equations shows that W02 Ci 2prevails in vapors only below 224 OC.
At higher temperatures, WOC1 4 prevails- At 3720C, the pressure of WC16
vapor equals the pressure of WO 2 0112vapor- At temper~_tures above
4000- 4500C, the dissociation processes must obviously not be neglected.
The composition oL" vapor above WO 2C12becomes even more complicated.
A. V. Tarasov assisted in the investigations of WOC1 4 and WO 2C1 2'
D~ N. Tarasenkov and A. V, Komandin are mentioned. There are 5 tables
and 26 references: 15 Soviet-bloc and 11 non-Soviet-bloc.
Card 6/6

`3
S/020/61/141/6 2 1
I C-) B'03/Bl 01
LUTHORS Shchukarev, S. A., and Semen~~v, G. A.
TITLE: Mass-spectrometric study of -~he vapor composition above~
rare-earth oxides
PERIODICAL: Akademiya nauk SSSR, Doklady, v, 141, no. 3, 1961, 6!~ r654
TEXT: The vapor composition above the oxides of all rare earth elements
(except Tu) was studied in a MW-1305 (MI-1305) mass spectrometer within
vaDorization from an iridium band. The thermocouple used in the ''.
spectrometer was gaged by means of an optical pyrometer of the 18t".type in
the Laboratoriya vysokikh temperatnr Vsesoyuznogo nauchno-issledc),~aftlfhkogo
Instituta metrologii im. Mendeleyeva (Laboratory of High Temperature-s"'of
the All-Union Scientific Research Institute of Metrology imeni
11endeleyev). It is recommended to take into account the simultaneous
formation of ions having equal mass by direct ionization of neutral
L,articles when setting out to obtain quantitative data on the ratio oil the
partial pressures of the vapor components. Such ions may also form by
dissociative ionization of heavier molecules. The authors criticise the
Card 115

L:ass-spectrometric study
S/02 61/1,1',/003/011/021
B! 03YB1 01
assumption by Y. B. Panf-sh (Ref. 4, see below) according to which:the
inle-relation of icnic currents in the mass spectrum at an ionizing
voltage of 20 v corresponds to the interrelation of the concentrations of
the corresponding neutral molecules in the vapor. On the one hand, an
ai-bitrary choice of electron energy may result in considerable
di.ssociative ionization, and on the other, ti-.q efficiency of the ioniza-
tion of certain molecules, especially those --f the ".~02 type, may be
extrem,;ly low. The potentials of ion lotme-tion were esti-mated for all the
oxides. The scale of the ionizing voltage was Lorrected using the
ionization potentials of argon and mercury as a basis. Then the initial
sections of the curves of ionization ef-ficienzy were extrapolated from the
time of beginning formation of ion fragments -.int.; 'the ionic current peak,
since here tile current strength depends little on the electron energy.
The interrelation of "he ionic currents at the maximum efficiency,
corrected for the ratio of the effective ionization cross sections
(Ref. 6. see beloi0 corresuonds to the i,terrelation of the concentrati--ns
of the neutral .iarticles- The results a"re represented in Table 1. In
each exueriment the mia X4 I-, ta`en as unit. The
measurements -,ert~ carriei out at iciently high to at' ain
Card 2/9 .

16,/141 /003/01 1/021
~
...ass-srectrometric study 1
101
a vapor pressure of 10-5 mm H,j of tho rnp,~rient .Modif -,cat 4. -ns of
the Langrravir method were used for La 0, N."II)o '.11ith other oxides, thF.
~ 3*
I
vapor pressure was determined during, vap,-rization of
e.:IU4molar quantities of the oxide in and La 0 Above Er CA and
2 3' 2 .'
Ybl)O 35 the vapor pressure of the metals w ~z inz-asured. it was found that
the volatility of the oxides of the i-d--,- .--d'aaI elements in a high vacuum
and the composition of their vapors vaz~- widely. The stability of the
gaseous monoxides of the lanthanide ;n passing from La to Lu
compounds, shows a general tendency to This results in an
increasing ITI/110+ ratio. This regularl,.-; -~o strictly periodical: The
lattei- ratio is highest for elements lha:. rl, a valency -2 (Eu, Yb), and a
lowest sublimation enthalpy of the meta-1. These oxides are also more
volatile. Dioxide molecules (CeO.' PIO 7'.,0.,) were found to be present
in the vapors of elements having the ?4. This was also found to
be the case in check tests carried out i:. a s,,~e-,,~rcLmeter with a tunsaten
band, as the ionic currents of ir+ and ~,annat be separated in the
Ii'i-1305 instrument. On heatinF in a va C-0- dissociates untc atci~:t
Card 3/f

' )0723
S//~D;O 6! /141 /G031/c', 1/021,
Mass-spectrometric study ... 1~1 35YB1 01
- CeO
CeO
(Ref. 8, .9 below) . T., . -;ap,,r -,~f this oxide contains Cleo.
1.80
1.67
and CeO molecules. The ratio of tl~,a -atrrents CeQ_~-/CeO_+_ does not
2 2
remain constant, but increases gradua-1-1. the quantity of substance ~Dn
eases, i.e. fror,
the vaporizer band decr ".5 1.0 at the outset to
'
,:I 011~ --
0.8 : 1.0 at the end of the test ~,- \. 11~r, -pas ~cun`,
il~-age 45 v,
3
to vaporize congruently at a solid -Tia, -on of* aiooro-ximat
ceo, Formation of ions of the tcy-
6* :r cclymeric ions
not obs'erved. There are 2 figures, 1 and 6 references- 2 Soviet
and 6 non-Soviet. The three most inpcz-3!. i-~ferences to En.-lish-
lan6uage p-.jblications read as follows: R : ",'. B. Panish, J. Chem-
Ph,' rs., 34, 1079 (191601 ) ; Ref . 6: J - D. P. Stevenson, J. Am-
Chem. Soc., 78, 546 (1)56); Ref. 8: X. A. Girre-rich, H.
Holtschmidt, T. In. Nucl. Chem., 16, C'.
PRESEITITED: June 26, 1961,by A. N. T-,!rr ,- A_'ademician
s U. 2- ~': 1 T TE, 1) J 1:
Card 4/i

T~ 701A,
SHCHUKAiU,:Vp S.-A--.-; LO-A:, O~A.
,,,4kpcrt-troL;ho tome tric study of complex cobalt, bromids-a in alcohol
solutions. Zhur.neorg.kh1m. 6 no.-IAOL-808 ~D ?611.
(MIRA 14 :4)
(Cobalt compounds-Spectra)

SHCHUKAREV., S.A.; SUVOROV, A,,V,
Thermodynamic investigation of certain chloro derivatives of
molybdenum and tungsten. Vest. LGU 16 no-4:87-99 161,
(MIRA 14:3)
(Systems(Chemistry)) (Tungsten com ounds)
(Molybdenum compounds5

ISHCHUKAR.!,',V-,--S.A,j KOLBIVI, N.I,-~, RYABOV, A~N.
Anhydrous ruthenium tribrcmide. Vest. LGU 16 no,4:100--104 161.
(Ruthenium bromide) (MIRA 14:3)

SHCHUKAREV,_S.A.; K6LBIN, N.I.; RYABOV, A.N.
Ruthenium triiodide. Zhur.neorg.khim. 6 no-5:1013-1015 My
,61. (KERA 14.4)
1. Leningradskiy gosudarstvennyy universitet.
I
(1,Rrutenium iodide)
.6

SHCHUKAREV, S.A.; KOLBIN, N.I.; SEMENOV, I.N.
Preparation of osmium tribromide. Zhur.neorg.khim. 6 no-5:1246-
1247 MY 61. (KMA 14:4)
(Osmium bromide)

SHCHUKARE;V, S.A.; MDROZOVA, M.P.; STOLYAROVA, T.A.
Enthalpy of the formation of compounds of man anese with the
elements of the maln sub-group of group V. Zhur.ob.khim- 31
no.6:1773-1777 Je 161. (KMA 14:6)
1. Leningradakiy gosudarstvennyy universitet imeni A.A.Zhdanova.
(m.nganese compounds) (Enthalpy)

SHCHUKAREV,__S_.A.-,-_SUVOROVt AN.
v--
Thermodynamic study of chloro derivatives of molybdenum and tungsten.
Zhur.neorg.khim. 6 no.6:1488-1489 Je 161. (MIRA 14:11)
(Molybdenum chloride) (Tungsten chloride)

2LL420
S/.079/.61/.031/007/002/008
~z 00 D229/D305
AUTHORS: Shchukar_e_y_,__�._A._, Semenov, G.A., Ratlkovskiy, I.A.,
and'Pdrdvoshchikov, V.A.
TITLE: Determination of saturated vapor pressures of indium.
oxide
PERIODICAL: Zhurnal obshchey khimii, v. 31, no. 7, 1961,
2090 - 2092
TEXT: This is a report on determining very low saturated vapor
pressure of indium. oxide by the flow method using a radioactive
tracer - InI14 in the range of temperature from 12900 to 14900. It
is known (Ref. 1: S-V. Bleshinski , and V.F. Abramova, Khimiya in-
diyao Izd. AN Kirgizsk SSSR, 1958~ that the ignition of In2O at
the temperature up to 12000 did not lead to a change in weigL of
indium oxide. The attempt to measure the vapor pressure of In2O3
at 10600 using the flow method was unsuccessful. In view of the
above it was decided to determine vapor pressure of In2O3 by a
Card 1/0

/h420
S/079/61,031/007/002/008
Determination of saturated ... D229/D305
flow method at much higher temperatures (12900-14900) with air as a
carrier gas suppressing the dissociation of indium oxide. Air was
found to be satisfactory, as it is proved (Ref. 1: Op-cit.) that
indium nitride if formed, burned up in the air, forming oxide. It
was assumed that indium oxide vapor is monomeric. After describing
the indium oxide preparation method, the authoisnote that its radio-
chemical purity was checked by a y-spectrometer (illustrated in
this article). The rate of flow of carrier gas at its saturation
with In2O3 vapor was determined for three temperatures: 12900, 1445'
and 14900C. The values of molar concentration at the flow rates less
than 4 ml/min were not taken into account when extrapolating for
zero rate, as they showed discrepancies. The flow rate of 5-7 ml/
min was chosen. The values of indium oxide.molar concentration ob-
tained by extrapolation for the zero rate and measured at the low
rate of 5-7 ml/min varied roughly by 8 ~o. Saturated vapor pressure
of indium oxide was measured in the temperature range of 12900 -
14900C and the dependence of the saturated vapor pressure of indium
oxide on temperature is shoun in Fig. 2. Results were taken from
Card 2/4

24420
S/079/61/031/007/002/OCB
Det-ermination of saturated ... D229/D305
three fraenendent experiments ~rit-h prep~Lrations of different" tuotal
activity. T-'--p total determination errcr of indium oxide vapor pres-
sure consist-s of: Determination error of total activity of prepara-
tion(� 1.2 error in i,ieasuring actf-vit 6 determination
error of preparation temperature (� 0.5 ;~, error in measuring volu-
r..,,e of naszed carrier gas (� 2 5). T,e determin-.%tion error of indium
oxide va-por pressure calculated on the basis of the-se values amoants
u
to 6 ~6- Enthalpy of sublimation of iridium oxide was found to be 11-8
� 21,-cal/riol. Entropy of the process o-f sublimation :~f !n203 was cal-
culated taking the heat capacity valucs of indium oxide in the tem-
perature range of 00-1000C (Ref, 1; 01).cit.), as no value of On of
In2O3 at high temperature could be found in tech-nical literatu!re
0 - U
Caiculz_ted S0298 anounts to 42 � lKca--/Mol. degree. There are 2 ~i_
gures, 3 references: 2 Soviet-bloc and 1 non-Soviet-bloc.
ASSOCIATION: Leni--qgradskiy.gosudars~uve--qnyy universituet imeni A.A.
Zhdanova (Leningrad State University imeni A.~,'. Zhdanov)
SUBI-TMM-M 7% -June 2', la60
Card 3/4

S7.L11L I U
AUTHORS:
S/078/61/006/008/016'018
Z5516 B127/B226
Shchukarev, S. A., Semenov, G. A~, Ratlkovskiy, I. A.
TITLE: Determination of pressure of saturated gallium-oxide vapor
PERIODICAL: Zhurnal neorganicheskoy khimii, v. 6, no. 8, 1961, 1973
TEXTs The authors worked according to the flow method in an 0 4~ en atmos-
phere at 1523 - 16820C. The experiments were conducted in a platinum boat
attached to the end of a movable alundum bar. This arrangement was con-
tained in an alundum tube and fixed in a furnace with a tungsten spiral in
an alcohol atmosphere. The temperatures of the samples used were measured
with a platinum - platinum-rhodium thermocouple and a '"-1 (PP-1) poten-
tiometer with optical pyrometer. The gas production rate was measured at
1562 - 15920C. The values of the molar Ga 203 concentration obtained by
extrapolating for zero velocity, and those measured at a gas production
rate of 11 - 13 ml/min did not differ by more than 6,,. The results ob-
tained are shown in a figure, and may be written as: log 27098
T
+ 13.339 mm Hg. In the vapor phase, Ga 20 3 proved monomeric. Enthalpy and
Card 1/0

2553L S/078/0'1/006/008/016 'ole
Determination of press-Lire... B127/B 226
entropir of sublimation of gallium oxide calculated from the slopt? otC the
a
straight line: log p = f( is 1264-2kcal/mole and 49--lkcal./mole-deg.
Under standard conditions entropy and enthalpy of Ga,,,o3formation were
calculated to bp 137t6kcal/mole, 57`4kcal/mole-deg. ;nd -127i6kcal/mole,
-15�dkcal/mole-deg. There are 1 figure and 5 referencest 1 Soviet-bloc
and , non-Soviet-bloc. The two references to English-language publica-
tions read as follows- Ref. 4: E. King, A.Christensen. J. Amer. Chem.
Soc., 8-0, 1799 (1958). Ref. 5. L. Brewer. Chem. Rev., ~2, 1 (1953).
SUBMITTED: February 27, 193.61
Card 2/3

SHCHUKAREV. ~,A,_; LOBAIFEVA, O.A.; IVANOVA, M.A.; KONONO
Spectrophotometric study of complex palladium (J
aqueous solutions.. Vest.LGU 16 no-10:152-155
(Palladium compounds) (Spectrop,
M.A.
chlorides in
')l. (KM 14;5)
ometry)

2-2-00
01:
S/0- 61/006/012/01 1
B12 J110
_'UTHO-46 Shchukarev. S. A., Semenov, G.. A2, R,.- kovskiy, I., k.
TITLE: Determination of the saturated vapo, ressure of thalliam.
oxide
Ph,RIODICAL: Zhurnal neorganicheskoy khimii, v. no,. 12, 1961i 2817-2816
12EXT: The pressure of saturated Tl 203 vapor w. measured using flow in
an oxygen atmosphere. Thallic oxide was prept ad by solving the pure
metal in HNO 3and additional oxidation by mea , of bromine water; excess
bromine was removed by boiling. Thallium. hy oxide was precipitated with
ammonia and converted by boiling under watei co the crystalline form, i
T1203 was subsequently dried in a current o dry oxygen at 2500C for 4
hours. The temperature of the boat in the urnace was measured with a
Pt-PtRh thermocouple equipped with the po. rtiometer M-1 (PP-1). The
vialocity of the carrier-gas current corra,ponding tot-saturation with
TI203 vapors was measured at 670., 700 rr,- 7500C. When extrapolation to
Card 1/3

:1018-7
S/078/61/006/01211/011/011
Determination of the... B120110
zero velocity was performed, the change in molar concentration was made no
allowance for at rates of flow below 3 ml/min., since considerable devia-
tions were found to occur at these rates. A rate of flow equal zo 3 mi/min
was chosen, with maximum deviation of the extrapolated molar concentura-
tions ot' TI203from measured values being 4-,o. Experimental data o:)taincd
are illustrated in the Figure; they are described in gocd approximation
by the equations: T120 3-3pT 1203 log p -(112,196/T) + 1';~440 and
Sol gas
log p 429/T) 12,663. T1 0-, was suppose-c to be
T120 3liq _*T120 3gas 2 "1
present in the vapor in monomer form, Sublimation enthap:es of thallium
oxide calculated from tho slope of the straight line log p = f(!/T) were
~c;A L 1 kcal/mole and ~2.3 + 1 kcal/mole, respectivel slablimat-~,on
entropies 48.3 kcall'. mole.,degree and 44.9 kcal/mole.,degree,
respectively, the melting point 716 20C, the boiling Tj04 nt 11690C, the
heat of vaporiza4,i.:)n at bc-iling temperature 50.0 t- 1 kcal/ /mole, and the
heat of fusion 5 5 t I kcal/mole. There are I f-J'aure and references;
2 Soviet and 3 non-Soviet, The two references to ~_ublica-
tions rmz!ad as follows !A , B ~ F 1) unka n , J . A,~i t r -
Card 2/3

SHCHUUREVOY S,A.; AI.DFEYEV, S.N.; B-,*dJC1MTA, T.G,; ITECIL4=11, L.N.
Infrared absorption spectra of aqueous solutions of some
perchlorates in tile region of the fundamental frequency of
O-H valence oscillations. Vest L&U 16 no.16:120-124 161.
(1-11IRA 14:8)
(Perchlorates--Spectra)

44'R'Uy-'~REVJ, S.A." WISILIKOVI,,., I.V.; OMTSjtjyA '~f
T-SIT;TSIUS., V.M.; SUBBOTINA, N.A. jp M.A. [deceased];
Detennination of tlie enthalpy of Vanadium tribromide formation.
Vest LGU 16 no.16:125-129 161. (MIRA 14:8)
(Vanadium chloride)
(Enthalpy)

PERfl-L-011L , I ~ L~ -. I I IV, '- SJJ1C1'1 LIT RDI, OVA, I.V.
.--- , VASILIF
Enthalpy of vanadium ox~Tchloride formation. Vest LGU 16
no.16.,130-135 161. (MIRA 14:8)
(Vanadium chloride)
(Enthalpy)

S.A.; VAS11 'FOV,%, I.V.; 2.AY'F'jFVjk, N.D.
Stucy of molybdenum halides, determination of t1,-- entuh-alp
y 01
molyhdenum tetrabromide formation. Vest LGU 16 n0-1-2:127-129
, (I . (l,',IRA 14:11)
(Molylidenum halides) (Heat of formation)

S~4CHUKARDI, E.A.; VASIL'KOVA, 1.V.; SHAWiFIN, B.11.
Mo]yLds,num halides. Part ': Thermodynamics of L%oQ Cl and MOO- 2*
H20. Vest LGU 16 no.22: 130-134 '(1. - 1 2 ( KIRA ft 11 )
(Molybdenum halides)

SHCHUKAREVY Sergey Aleksandrovich; TOWACHEVA, T.A., otv.red.;
PIASTRO, V.D., red.; ZHUKOVA, Ye.G.,, tekhn.red.
[Lectures on the general chemistry course) Lektsii po obshchemu
kursu khimii. Leningrad, Izd-vo Leningr.univ. Vol.l. 1962.
405 P. (MMA 15:5)
(Chemistry--Study and teaching)

S/620/62/145/001/016/018
B145/B101
Shchu'arev, S. A., Semenov, G. A., and Frantseva, K. Ye.
De ',4 nation of the saturation vapor piles~ub6~of h1obium
dioxide
1, 1962, 119 - 121
~Aademiya nauk SSSR. Dok1adyq v. 145, no.
T Z'X T T.-,,e sacurallion vapor pressure of niobium dioxide was measured in
1~,58 - 21220K using a variant of Knudsen's* effusion method (see
:1. P'nipps, C. 7J. Sears, 0. C. Simpson, Manhattan Project, Div. IV, 14b,'
T;io Trans ur anium Elements , N . Y., 19499 P. 704, and An. N. Nesmeyanov,
energiya, 3, 227 (1957)), and the heat of sublimation and the
dis5oc 14--ttion energy of C-;-tseous NbO2were calculated from the results. Die 4/
cyL,ndrical effusion chamber was of forged molybdenum (diameter'of the
ratio betaeen the areas of the material to be
e ~usio-i ooening: 0.308 mm,
L US' 1; heating by electron b6mbard~
aporized and -~'ie e~f !on openIng = 500 :
-.e t; aztainabie vacuum: 1 .1o-5 mm Rg; 21000K). The oxide has the com-
-tion NbO and was tagged with Nb95. The'values mee;sured satis-
'?.0 S 2.008
1/2

S/020/62/145/001/016/018
De Iler.-..14:lation of the saturation B145/B101
-IOU- P = -30300/T + 12-42 mm
12 eq u a z; i o n -Deat of sublimationt
1 ~5 2 From the pWblished values of F 0 - Ho VT and of
T 298
0 0
.:0 H for condensed and gaseous NbO the sublimation enthalpy 6 H
2 3, 8 0 2' 0
-.s ca culated as 141 + 0.4 kcal/mole. The dissociation energy of gaseous,
.N'b 0 - '= published data for the heat of sublimation of metallic -
2' ccda"L'Ited I
~-nd t'-e heat of atomization, worked out as 14-9 � 0.1 ev. There are
'r'Cures and 11 tab'e. The most important English-language referencesare.
:.'arE7rave, -2-roc. a' the Symposium on High Temperature - a Tool for
t`-e Future, 3arkeley, California, 1956; Physicochemical Measurements at
TP_11~peratures, Ed. Bockris, White, Mackenzie, Butterworths Sci. Publ.j
L. Brewer, G. Rosenblatt, Chem. Rev., 61
3 257 (1961).
T 0": 'eningradskiy gosudarstvennyy universitet im. A. A. Zhdanova!
(Leningrad State University imeni A. A. Zhdanov)
P R S 2 _"" 2ED :,:arch 3, 1962, by A. N. Terenin, Academician
Pebr,.isry 27, 1062
Card 212

S/05~/62/000/002/011/012
B117 B101
A Ul 7 10 it Shchukarev, S. A., Kurbanov, A. R.
TITLE: Thermodynamic investigation of some tantalum chlorides
Leningrad. Universitet. Vestnik. Seriya fiziki i khimii,
no. 2, 1962, 144 - 151
T 7 ' ~'l
Z-J.: The pressure of saturated and unsaturated tantalum pentachloride
vapors between 425 and 10200K and the thermal stability of tantalum tetra-
chloride were investigated. TaCl was produced by direct chlorination of.
5
metallic tantalum with chlorine at 300 - 3500C. TaCl 4 was obtained by
reduction of TaCl with metallic aluminum and sheet tantalum. Sublima-
5
tion and evanoration of TaCl 5 were studied at 425 - 5300K- It was found
"or 'the sublimation: 6H - 22.7 kcal mole, AS = 45.2 entropy units (eou.),
for the evaporation: 6H - 14.9 kcaltle, AS - 29.3 e.u. A, melting
temoerature of 2160C and a boiling temperature of 2350C were determined-
-Prom the equations for sublimation and evaporation. The difference in
Card 1/2

Thermodynamic investigation of...
S/054/62/000/002/011/012
B117/B101
enthalpy and entropy of these two processes was used to ca-lculate heat
and entropy of melting of TaCl 5; 6H - 7.8 kcal/mole, LS - 15.9 e.u. Foro.
the dissociation accordina to the reaction (TaCl )
(TaC1 +1/2 C1
0 5 gas 4 gas 20
the followin- was found. 6H 33-55 kcal/mole, As - 31-3 e.u. For the 1:
0
very sl o-.-. disproportion (32 36 hr) of TaCl 4 according to
21,'LaCl'o rTaC1 + (TaC1 AH - 27.0 kcal/mole,
- ii~ solid- L 31 solid 5 gas
AS e.u. 'When measuring the pressure of gaseous TaCl over solid
5
3-; in the absence of [TaCl 4) at 4500C, the conproportion reaction
`aCl + (TaCl 2(TaCl was observed. In this case,
3,1solid 5 gas 4 gas
sH = 33.1 kcal/mole and AS - 32.3 e.u. were determined. Enthalpy and
entropy of sublimation of TaCl 4 were calculated from the disproportion
and conproportion processest AH - 30.2 kcal/mole, AS - 46.4 e.u. The
results show a satisfactory agreement with published data. There are
2 figures and 2 tables.
%;--"~ITTLD. July 7, 1961
Card 2/2

SHCHUKAREV, S.A.; ANDREYEV, S.N,,; BURKOV, K.A.
-
Complex formation in the syBtem NiG12 - HG1 - H20. Dokl.AN SSSR
144 no.2:371-373 Vq 162. (MA 15:5)
1. Leningradskiy gosudarstvey?nyy universitet im. A.A.Zhdanova.
Predstavleno akademikom I.I.qhernyayevyme
(Nickel chlorides) (Hydrochloric acid) (Complex compounds)

c-z/078/62/007/003/004/019
B110/B138
AUTHORS: Shchukarev, S. A., Semenov, G. A.,.Ratikovskiy, I. A.
T IT 1, E: Determination of the saturated vapor pressure of metallic
thallium
P;-:RIODT('AL: Shurnal neorganicheskoy khimii, v. 7, no. 3, 1962, 469 - 471
T7IvIT: The saturated vapor pressure of thallium was measured with T1 204 0
using Knudsen's method. 10 - 15 measurements at temperatures up to 1200 C
and residual pressure of about 1o-5 mm Hg were made with a differential
all-metal apparatus. A quartz effusion chamber was placed in a quartz
furnace heated by a NITo spiral. The e.m. f . of me of the chromel/alumel thermo-
couples was measured on a TfF-1(PP-1) potentiometer, and an -DTIF!~-OI(EPV-01)
thermoregulator for the other. The effusion opening evaporating surface
ratio was 1:1000. The apparatus was calibrated against saturated Ag-metal
2 2 2j - M,
vapor. p [17-153ITq st (r + h )]/AtI str . yTT where p = vapor pressure
of the mixture of stable isotopes in question, mm Hg; A = area of effusion
2
opening, cm ; t = time of target exposure, sec; I T = radioactivity of
Card 1/3

S/078/62/007/003/004/019
Determination of the saturated ... B110/B138
condensate deposited on target, imp/min;, qst = Weight of initial radio-
active substance in the sample, g; radius of collimator, cm; h = distance
between effusion chamber and collimator, cm; T = temperature of effusion
chamber, OK; ivi = molecular weight of the vapor of the substance examined.
An. r1(-1(MS-1) mass spectrometer was used to determine the composition of
Tl vapor during evaporation from an open surface, at an ionization voltage
of 50-60 v, and an emissi6n current of 1.2 ma. T11, T12+, Tl 0+, 0+, and
+ + 2 + 2
Tl 2ions were found in a ratio of 100:10:2:1:1. The Tl 20 and T1 2 currents--'
decreased rapidly with time, but their ratio remained constant and
temperature-independent. T1 0+, 0+, and Tl+ are probably the result of the
2 2 2
dissociation of oxide films forming on the surface. This is in good agree-
ment with mass-spectrometer examinations of Ga and In evaporation. Like
Ga and In (Me2/Me = 10-3), Tl vapor is also assumed to have a monomer
204
structure. T1 metal with T1
was reduced for 4-5 hrs in H 2 current at
2500C, and vacuum heated for 3-4 hrs at 4 7000C. Temperature dependence
Card 2/3

S/07 62/007/003/004/01'
Peterminntion of the saturated... B1 1 OYB1 3.8
of pre:,sure: log p = -8708 T + 7-3697 (2) Heat and entropy of thallium
evaporation for log p = f(1 T) and the temperature range 701-0740K were
found to be ~9-6 _+ 0.5 kcal~g-atom and 20.9 + 0-5 kcal/g-atom'degree. The
boilin.- temperature of Tl, calculated by (2) was 19390K, and the correspond-
ing evaporation heat was 40.5 kcal/g-atom. There are 2 figures, 1 table,
and 6 references: 3 Soviet and 3 non-Soviet. The two references to
English-language publications read as follows: F. F. Golemann, A. Egerton.
Trans. Roy. Soc. (London), 234A, 177 (1935); S. Antkiv, V. H. Dibeler. J.
Chem. Phys., 21, 1890 (19537-
SUBMITTED: April 24, 1961
Card 3/3

S102 02/14-4/003/029/030
0 2, 3: Sh~~'-_,,-karev, S. Andre-ev, S. N., and Balicheva, T. G.
T 1 V-4brational spec-zra of perchloric acid -in the liquid and
,:,;azeous state
!.r.~-_demiya nauk SSSI.R. Doklady, v. 144, no 1062, GO6-0,C6
3,
'--"he 7-,ate of ~;he GH bond in nerchloric-L-cid molecules in the gas
h z- s e, al-_hydrcus 11clo 41 and solid 11,03-0 4. 1.2 0 was studied in the
r,~. on of fi;ndamental-tone valence f'requency vibrations of OH. The
rez::eCtIve "fibrational s--.:ect--a were investigated using, the recording
znfrared s1~acizometer (IKS-14) and the noarecording infrared
formed using L'J/
Ms-6) (Fi~:-. 1). Calibra-~ion was perk
ITCI, T_:3r, CG, CU
the rotation vibratilon spectra of NH 3 __4' and C 6U
aesul-~S: Gaseous HC10 is raonorieric in the same way as a 0.001~
4
solution of HC10 4 ='L C C 1 4* (2) ~-.'ha line-shift of anhydrous HC10 4 amounting
to 170 cra_ 1 J_s accounted for by the H bords which have an energy amounting
Card 1/~! 7

-SHGHUKAREV) S.A.; ANDREYEVy S.N.; BALIGPEVAy T.G.
Infrared spectra of perchloric acid and its solutions in the region
of 3700 - 2300 cml. Vest. LGT 17 no.4:128-134 162. (MM 15:3)
(Perchloric acid-spectra)

SHCHIUKAREV, S.A.; VASILIKOVA, I.V.,- KOROLIKOV, D.V.; NIKOLISKIY, S.S.
Thermodynamic study of molybdenum dibromide. Vest. LGU 17 no.4.,
148-1,40 162. (MM 150)
(Molybdenum bronides-Thermal propertiei)

S/lj3/62/005/005/001/011
E071/E133
AU I i it -1:.3 11. c I I i I ka r #, vSellieflov, G.A. , and Frantseva, K.Ye.
T 1,1 1 1. A ir-iss spoctromc-tric mtmly of' the evaporation of NbO
("A L: Jvvo.-4t i.ya vysshikh tichel-Inyl-Ai zavedeniy, Khimiya i
10, 1 'Ili chf-skaYa tc1(hI-1-()KiYa, v.5, r,0.5, 1962, b91-693
~Jiohitim monoxiao ror tlie investigation was obtained by
the i-q-thiction of purp niobinm jpf!ntoxirl(? (99.961,.) in dry hydrogen.
A 11-1--n (if Nhu wa--i placed oil a I migsten or iridium strip in the
o1 IC S011 ri, C 0 1~71 WiISS 3 , I I The
. [-1 3 0 ( 1- 305).
was 111-nsurpil with a cctlihrnted tmigsten-rhenium thermo-
collplv to tile -strip. Th,~ pr-.-iviicc~ in the vapour of the
ttlHol'illy, ioll-5 wit-s C!5 till) li~~Iled: N, h ~- ,N h C) 'and Nl)O,j4. In order
to :t~t, ri,itie the origiti of' ioms. the potential o~ their
appeal-WIC' evalliated by plottins thq- df!pelldence of ionic
cill't-vilt "11)(" against the pot-Iltial. This was evaluated as
J(I.j -V. completo allsonce of ,%hI, inl).-i at an ionising potential of
1,i V indicatod that were formed (hie to dissociation-
i () D L!-~ it ( 1 o TI .Thus tlxer(,- two typi-!, of' ions corresponding to the
noitLral. muleciiles present III th,, vapolti- Nbo 2 atid Nbo.
Card 1/2

PqHWITV,j-_ S. A.; SEMENOV, G. A.
Evaporation of hafnium dioxide. Izv. vys. ucheb, zav.; khim.
i khim. tekh. 5 n0.5:845 '62. (MIRA 16:1)
1. Leningradskiy gosudarstvennyy universitet imeni A. A.
Zhdanova, kafedra neorganicheakoy khimii.
(Rafnium oxides) (Evaporation)

S/076/62/007/006/001/024
R12-4 /
.,/ B1 36
A NIT H 01; 1 A., Smirriova, Ye. K., VasilIkova, I. V.,
,Ior~Tv
T-TTL-: Formation -enthalpy of' niobium pentabromide and oxytribromide
P H 1 C,1A L Zhurnal neorganichpsk-cy khimii, v. 7
no. 6, 1962, 1213-1215
T:,'K'17: This was determined from their measured hydrolysis enthalpies
for a newly d~.-veloped method of separating niobium and tantalum by
.Clractionating their bromine compoun-is. ?IbBr free from oxybromide was
5
produced by making niobium pentoxide react with CBr in sealed ampoules
5 .
evacuated with a forepump. A mixture of Nb 0 NbOBr , and unreacted CB
0 2 51 3 r4
was obtained by 15-20 hr heating at 200 C. The ampoule was cooled, the
gaseous reaction products were removed, the ampoule -as sealed again and
heated "or 8-10 hr at 360-3800C. The reaction products CO, COBr,,, and Br 2
were drawn off with a forepump at 70 0 C. The resulting NIbBr 5 was purified
Card 112

S'/078/62/007/006/0011/024
Formf-ttion erithalpy of niobium ... B 12 4 /B 1 'j ~,
f r o'-' ~: b 20~' by dULIcle subli-nation in vacuo. NbOBr3~as produced by
oxidation~'of Nb-Rr- at 1'50-1600C and bromination of 14b 0 with CBr at
0 j 2 5 4
1) "1 - 20 The heat released durinE. hydrolysis of the bromides was
(jet,~rfljijj*?tj calorim.-trically at 260C to be 68. 7 + 0.9 kcal/mole (NIbRr 5)
and 3114-8 -~ 0-6 kcal/moic. (NbOBr,). The enthalpies calculated on the basis
of nublished data were: 'L11, -135.2 + 1.2 kcal/mole and
lqbBr,
1'0 D
179.3 � 1.0 kcal./mole. There are 3 tables. The three most
ICO Fir3
important English-language references are: K. M. Alexander, F. Faibrother,
J. Chem. Soc. (London), p. 223 0949); P. Fairbrother, A. H. Cowley,
Scott, J. of the Less. Common Mietals, 1, 206 (11059); G. Z. Humpley,
J. Amer. Chem. 30c. 76, 978 (1954).
UK..ITTED: july i4, 196,
Card 21

S/07 62/007/006/002/024
B1 24%3138
5 6henulwareliq S. A., Smirnova, Ye. K., Shemyakina, T. S.,
_7Y_ 1-1 1 ~Ij -1 1 ~11 I
llydrolvsis and formation enthalpy of niobium oxytrichloride
hi;rn;i] nf-_,(_)rt-,3nichesIroy khi:;)ii, v. 7, no. 6, 1962, 1216-1218
t~nthalpy of NboUl- was determined from the heat
0
re!Qased dtlrinC its hydrolysis. N b 0 11 1was produced at 650-700 C by
chlorination :)I' ;b2 05 in a dry chlorine flow saturated with M 4 vapor, and
purif.ed from small amounts of NbC1 5 by vacuum sublimation. After removing
14L the oxychloride was sublimed, a -ray powder being left behind. The
--I Ci 51 o
same powder was obtained by heating oxytrichloride in a sealed ampoule
previously stored in moist air. X-ray patterns and chemical analyses
revealed a chemical substance of the composition Nb 4 09cl2 formed during
hydrolysis of ',"113OC13at 350-5500C. The mean heat of hydrolysis of the
Card '1112

S/07-9/621007/00610021024
Eydir,.)-',~ysis zinu for-ation enthalpy ... B124/Bj38
oxytrichlor-ide sas found to be --,5.e' + 0-5 kcal/mole on the basis of
mer--curements made at 250'" 0
with an isothermal calorimeter. The formation
e2ithalry cal:,ulated From published data for NbOCI 3 was L H996 212.2
+ '-cal/;mole. This value is in good agreement with the formation
entha-loy of solid Nb('-)Cl,, calculated by H. Schqfer and F. Kahlenberg from
the heats of a solution of NbOCI 3 in hydrochloric and hydrofluoric acids
(-210.2 kcal/mole). There are I figure and 3 tables. The two English-
lang-uaGe references are: Selected Values of Chemical Thermodynamic
7iasir-ington, 1952; G. Z. Ha-mrray, J. Amer. Chem. Sac. 76,
9715 (1954).
jU1Y 14, 1961
C,ari 2/2

SRCHUKARKV, SoA ; TOLNIACHEVA, T.A.; TSINTSIU~, V.1C
Dismutation of vanadium tribromide at high temperatures.
7 no,,7.150~--1508 Jl *62.
(Vanadium brckmtde)
I
Zhur.nedrgkhirn.
(MIRA 16;3) *

SRGIIUKM~Us S.A,,; VASIL'KUVA, 1,,v.; Pi~IWILOVA, I.L.; CHEiU'IYKH., L-V.
r Enthalpy of vanadium trichloride formation, Zhurneorg.khim, 7 Uo.7:
1509-151-1 J1 262. (MIRA 16 *,3)
(Vanadium chloride) (Heat of formation)

1,110BUCOW", FROD G.-F.
Ellthalr7 -~f the fomat-,oo ot ~:al-,ium roz,-)po,.,nd.- vith element-S of
t1le. main Fsubgrciap o---' tl2e IVII~ gioup. Zhur.ob.khim. 32 no.?.2069~-
OMIRA 15~7)
j
I.. Le ni%f rail sk-ly gesudarst-vennyy universitet.
(Gall:A,.im compounds) (Heat of formation)

G -Rant , kovs-k- a'. Y I.".
-id thal-
0 7 v" cj,_ C)-- ai
1962,
y 77
~esc. r...ez-ais in
z c -at i
y
0 C) Ow.-I ua-
-il 0-1s ~c-ns was used -0 detelmine t ric r
V,-,. e_-:*_Csocia-*L-ion ~onizatioTL).
C. -a c r.-,_ltals via chlorides a-Lid
C LL,~.L- - j- L
c,'_it- ai=i zroM. Indi,,iai oxalate by decounos-Ltidn
-.3 o- ~'-is o-`dc s*--o,,-7ed o-,i-y the lines of
LLI L
d o f va)ors o~-' 'a-
s-3ecrr~
3 ,03 (at 1150

/-,C -'/~32/03.5/007/001/013
z: 5 '21 were chczrac-
~yr
Of to
-C cui:rcalcs correspondLL&
~)Y t-',c cc currents
'uenci-, 0.,7 L-
t 0 C inte-LIS' ties).
to %~ac, very feeble curre-at
c, n(-, to r. 3
is o-)servecl. ~ollowins scheme of decom-
C. 0 1, 0 + 0
"U -
2 27
3 0. S 0 1d !.:.:)o solid + 1,1203solid + 02;
(5) 0 -z-e>
gas
1~20sclid 0-) (7) 1- + There are
So-,-4d solid "'gas
:
-urc - h ng
I- - s and 1 ab I c .The most imDortant of tLtie:"ZIIglisL -la uage
I-Oforenccs- reads as follows: 1. 2,n-Lkiv and V. Dibeler, J. chem.
21, 1-390 (1953).
ay 23, 1961

3/08 62/035/007/002/013
D267 X307
_;hchu'_.-.arcv, V-sillicova, !.V. and Shalulcukhinal
_ysis O~~ 4-,Ic ci-I'lorination of ntOlYD-
c anal
t-C ~dseous ME Ixture of chlorine with sul-
t.1
::- L
Ld-2s
C
_~__Oy -,jo. 7, 1962,
Or OF Clo With SUl-
-dates a-~7d
CLIC~:_ L-LolyLD
'-,c chlorides,
out 160
--Ilatc the pro-
o d. c Sof the c:orra
f
there-
s of entha-
-Is 01. c.*k'G-_'-I. v
_1101-T ProbabIQ refi-i-3-
e %,'C_.-e ca-CU-1atcd e ja val 293
eS b~:O G and.
sche-,.ies Deu-2e- Ca~'OC; 4
3030--: for &12 pOS,~ I 4t
(or -.)ure C12)
:o the GrIe -haml at--d 012 2 0 3- 2
Z7Z d-

VGCG/62/035/007/002/013
T I - 1 c C) c !I, n C. D267/D307
on ot*.-~2r. Mcr't tirle analysis
_.' ~ , L ob, `o most ?.robable
.1 c rll_,_vV._
o
s"n o~..Tad
c 8charme_5 anr~ - I -he with the zai.%.-ture
"I- -1-ith sv.) -lo-rid-es -s mora adva-i~-ac-,co-us than c,-ilo-.i-,.iaticL
o- '-.L, . -phur _.._ - - ~ C) ) 11
- -i ~-,- C3~ 'a 10 h P_ ThQre f.2 1 flHigrure a-,d -nbla.
L
_7D

I
SACHUKAR-V, S.A. (L,-n-inevad); 'LWhEITYL, A.-k. 1~--rdngrad)
EvoLution of the rapresentations of secow.&-r7 od c
. peri icity. Vop.
Lit. est. i tekh. no.13.76-79 162. (%~kmu 16-15)
(Periodic table)

,5fiGff-U"-j~-v, S.A. (Lonirgrad)
From ray reminiscelices. of N.S. Kurnakov. Vop. ist. est. i tekh.
no.13:105-106 162. (MM 16:5)
(Kurnakov., Nikolai Semenovich, 1861-1941)

S/07 6 2/00 7 /00910051/00 7
B144Y3101
AUTHORS: Shchukarev, S. A.j__Smi'rnova, Ye. K., Shemyakina, T. S.
TITLE: Thermographic study of the systems NbOC1 3 - NaCl and
NbOCl 3 - KC1
PERIODICi~L: Zhurnal neorganiaheskoy khimii, v. 7, no. Q, 1962, 221 -2219
7
TEXT: The thermograme of NbOC1 3 purified from NbCl 5 and mixed with NaCl
"Cl were tal-en at 3 0 -
r K 0 9000C. Conclusions from tl!.-.- resulting
o
constituti on diagrams: 1) In the NbOCl 3 - KC1 system two compounds are
formed: MOU (NbOC1 .:KC1; 50 mole-% KC1) melting congruently at 440OC;
KC1) melting incongruently, eutectics
K2NbOCl 5 (NbOCl3-2KC1; 66.7 mole-',*
Pt 388 and 422 OC, peritectic at 4860C, monotectic transition at 5460C.
2) In the NbOCl 3 -' NaCl system only the one compound,
NaNbOCl 4 (NbOC1 3 *ITaCl; 50 mole-/. NaGl), is formed melting congruently at
430 OC9 eutectics at 380 and 410bC, monotectic transition at 7600c,
Card 1/2

S/07a/62/007/009/005/007
Thermographic study of the zyetems ... B144/B101
the formation of minute amounts of NbC15 and of further oxychlori-des is
assumed. Demixing was observed in both systems. There are 2 figures.
SUBMITTED: July ill 1961
V/
Card 2/2

SHCHUKAREV.,, S.A.; KURBANOV, A.R.
Thermodynamic study of some tantalum chlorides. Vest.LGU 17
no.lo.-144,151 162. OURA 15:5)
(Tantalum chlorides--Thermal properties)

IN - . T.S. ; S,.1R,,'GVA , Ye.K. ; SH-CPK~Py-v -IS -A-
Enthalpy of the formation of double compounds of niobium
oxy-trichloride with NaGI and KC1. Vest. LGU 17 no.16:2.55-157
162. (MIRA-
(1-Tiobium compounds) (Enthalpy)

SHCHUKAREV, S.A.; STROGANOV, Ye.V.; ANDREYKV, S.N.; PURVINSKIY, O.F.
GryNtal structure of the crystal hydrates of transition metal
salts. Structure of CoI2.6H20. Zhur.strukt.khim. 4 no.1:63-66
ja-F 163. (MIRA 16:2)
1,- Teningradskiy gosudarstvpnnyy universitet.
(Cobalt iodides) ((crystallography)

S)FICHUKATTV, 5.A.; PERFILOVA, I.L.
Interaction of vanadium trichloride with sodium, potassium, and
rubidium cftlorides. Zhur.neorg.khim. 8 no.9:2106-2108 S 163.
(MIRA 16:10)

SITCHUKAREV, S.A.; SMIRNOVA, Ye.K.; VASILIKOVA, I.V.
, 7--'. " - ~ - -
Ther!rographic analysis of the system RIbCl - CbOClj and CsCl -
116jul, Vest. LGU. 18 no.16-.132-133 163. ~ (MIRA 16:11)

3HCHUKARDI, S.A., Frof., otv. red.; FIASTRO, V.D., red.
[Chemistry of the rare elements] Khjlriia redkikh elementlov.
Lehingrad, Izd-vo Leningr. univ., 1964. 160 p.
(IMP-A 17: 5)
1. Leningrad. Un-i-iersitet.

SHCHUKAREV, S.A.; KOKOVIN, G.A.
Determination of the heats of formation of W02 Br2 and WOBr 4'
Zhur. neorg. khim. 9 no.7:1565-1569 Jl 164.
(MIRA 17:9)
1. Leningradskiy gosudarstvennyy universitet i Institut
neorganicheskoy khimii Sibirskogo otdeleniya AN SSSR.

A , "

SHCHUKAREV, S.A.; SMIRNOVA, Ye.K.; VASILIKOVA, I.V.; KOTOVA, M.S.
Enthalpy of formation of sod-Jum and potassim chlorotanta-
lates. Vest. LGU 18 no.22:174-176 163. (NIRA 17:1)

1!14 v
khl

KURBANOV, A.R.; SUVOROV, A.V.; SHCHUKAREkV, S.A.; NOVIKOV, G.I.
Thermodynamics of tantalum chloridas. Zhur. neorg. khim.
no.3:520-525 Mr 164. (MIRA 17:3)

SHCHUKAREV, S.A.; SHFMAKINA, T.S.; S~URNOVAJ, Ye.K.
Compounds of niobium oxy-trichlorides with sodium and
potassium chlorides. Zhur. neorg. khim. 9 no-3:547-549
Mr 164. WIRA 17:3)

I I .. . I ~

.. S7-:Cl'tTkAP.T-V, S.,'.; TC1!.',Ar.*-l:ET,, T.!-.; SLAIMITISKAYA, G.M.
Thermal dissociation of platinum -iodidps. Zhur. neorg. khLn.
9 no.11:2501-2506 N 164 ("'Em isa)
1. Leningradokiy gosu('rtrs-t7-v-wnyj universitet- imeni Zhdanova,
Kafeira neorganichesPof khimii.

.SHC-'HLTFA,'Zl, S.A.~ TOUTIAMONA, T.A~j PAZUHllIA, Yu,,-T.
Dissociation pressure of palladiwa iodide. Miurz. eo---R. khim
1.1 no.11.,25017-2510 N '64 VEM 18'.1)
1. Leningradskly gosudarstwenny-
y imi-,ersltat, Ka-fedra nrz-
or.aan * clie-qr'-.ry khim-.1.

C) A.
f. on .,~r~n t%,n,-z3 c (j:, j v ;.-a -lar.i-,,m bromides. 'hur.
(14I,%~ 18:2)
,7,)--i;,i:;rstvennTv universitet, kafedra neorganichE-
skoy khimii.