SCIENTIFIC ABSTRACT BAGOTSKAYA, I. A. - BAGOTSKIY, V. S.

• Document Type: CREST
• Collection: Scientific Abstracts
• Document Number (FOIA) /ESDN (CREST): CIA-RDP86-00513R000103010020-4
• Release Decision: RIF
• Original Classification: S
• Document Page Count: 100
• Document Creation Date: November 2, 2016
• Document Release Date: June 6, 2000
• Sequence Number: 20
• Publication Date: December 31, 1967
• Content Type: SCIENCEAB

S/076/63/037/001/016/029
Effect of the composition ... B144/Bls6
and adsorption, and a slow strong type in which the entire Pd
surface is~
involved and the hydrogen penetrates into the metal in a single
elementary
act. An intermediate type is possible +in (d), owing to an
increased I-
adsorpt.ion in the presence of (C4H9)4N Tests*with (a) + Hg (b),
and (d), indicated that.t~ depends-not only on the removal of H
ads from the
electrode surface but,predominantly on the-discharge of the H
ion. The
irreversibility of th6se two stages-was evident from the fact
that in (a)
vi~ th v =v ze 1/2 i~ ttpoi= 0.13, while ~tO.06. There are 7
pol dif Pol, Idif
P~gures.and-l table.
ASSOCIATION: Moskovskiy gosudarstvennyy universitet im. M. V.
Lomonosova
(Yjoscow State University imehi M. V..tLomonosov)
SUBMITTED: September 25, 1961
Card 3/3

S/62 63/149/001/020/623,
B101
%144
'AUTHORS: Sabog Ke P~ 31
T IT LE' Study of.the hydrogen overvoltage on solid and liquid
galliuml
A
in sulfuric solution
PERIODICAL:, Akademiya nauk SSSi. Doklady, v. 149, no- 1, 1963, 139
141
TEXT: The overvoltage -rLo~f hydrogen was measured on solid gallium:in
1 11 H2 SO4 and hydro gen atmosphere-at..2800, and on.liquid gallium
at 320C
.1:using a platinum..anode and 6 hydrogen reference electrode.
Results:-
the gradient of the.polarization
Is d is by 215- 30 mv less than 'Lliq;
In the
curve is the same for liquid and solid gallium, i.e., 0-095 v-
presence of traces of oxygen, solid Ga oxidizes; subsequently the
level
On liquid,
of the.polarization curve is higher and the gradient is 0.130-
layer of liquid Ga is
Ga no oxidation was observed; presumably the oxi
very r and
apidly reduced. Thecurvos 0 versus ruaro identical.for solid
liquid Gap for oxidized. solid Ga the - 66 ~. With
y are lower by about 60
:1 -increasing reduction, i~ decreases and C increases. There are 4
figures.
Card 1/2-

3/020/63/149/001/020/023

Study of the

hydrog n

..
BlOl/B144
ASSOCIATION:
Institut
elektrokhimii Akademii

nauk SSSR (Imttute of Blec i

trochemi
stry of the Academy of
Sciences
USSR)
PRESENTED:
December
6,1962t by A..N. Frum
kin, Academician'
SUBIMITTED:'
December
61 1962

-paxd: ?/2'

SABO, K.; BAGOTSKAYA, I.A.
Hydrogen overvolta~g-e on gallium as effected by the
double electric
layer and by pH of the solution. Dokl. AN SSSR 150
no.1:128-131
My 163. (KIRA 16:6)
1. Inatitut elektrokhimii AN SSSR. Predstavleno
akademikom A.N.
Frumkinym. (Overvoltage) (Elecirodes, Gallium)

KOVRAP L.D.;_BAGOTSKAYA, I.A.
-.- -.. I - ~ ~ . - . .."
Behavior of atomic hydrogen on a pure iron surface.
Zhur. fiz.
khim. 38 no.1:217-219 Ja'64. (MIRA 17:2)
1. Institut elektrokhimii AN SSSR..

SABO, K.; BAGOTSKAYA.. I A.
EXfcct of pH and o!' the electrulyte -.i
1,-idoogen
overvoltage at a galliim dropping eleitrode.
Dnkl, AN S",:';R
156 no. 2i420-423 My 164, MIRA 170)
1. Institut elektrolhimii AN

FrMEIT, A. N. ; 1ADLYA14OV6KAIII, h. 6. ; 6ii-iLk'J'Un- 1
!:~-V , X'T. -; '".1 - ...
"Electrocapillary phenomena on gallium."
report presented at 15th Mtg, Intl Comm of Electrochemical
Thermodynamics &
Kinemics, London & Cambridge, UK, 21-26 Sep 1964.
Inst of Electrochemistry, AS USSR.

t F.AIF rj~ C) j-~ 1 7r
r
f io 57/UYO
S
-7 v aya A
d u-le laver
I iri 1 ire re r; ;~,a I cL~ a cty
gailium electrode
;,:PSTP,~CT- The dilrerential capacity on a dropping gaiiium
electrode
was measured at ~CJC in variou3 Na,,50, , NaC101 LiCI, NaC1,
YC1, CsC1,
KI ;-nd KCNS soluLiur,6, 13,' neutral ~4~LiL solutions were
used for
iaeasure-ments at potcntials from to -1.4' volts. For measure-
,i,ent.s from -1.) to -1.1 volts the solutions were acidified
to 0.0114,
r. d - r r rr! s L~ r5 r 0 t. -1.1~ VC-1-15 t- Tr)sltive
vci~.a,-,eL they were
ac--Ji 71~
-;2
concentratinns were IN. The ej(~ctroQ~ was j,re~.ared
~c_-~,r,3in;~ to
4 p '-
-~etskava 's. Flys. Chem.,
r t i c, n YA N. rum jr V.
1A

L 16hh3-65
ACCESSION INR: APW43555
13 6 , '15 ( 1 c At nerative potentiais ccrre5j.;cndj.,,-
tc, ,reis of
cation aasorptiun, LIle aifferen~,!o.'
frora Lil to C.I. In solutions contai-,inr~ the same
Cations oaf^ dif-
ferent -tnions the differential capac4---.- curves aimc5l~
coin--i I e ~i
rr ot-F~t s c,-, r r,~:3,, r, i i v
>
t c,
c,; cf~ s3 e c L~ n 'i S Lin, Z, L.
1~1. ectric double layer. The absence of dispersion of G
i.ndlcaLed the
rroce5s of Ga dissolution, which takes place at even mort-
~,ositive
4
-- i - "he bp-veen t~~e cY,ar-e
rr,~ ,e rsi, 1 e .
density E and the potentiai 4P for Ga and ng if I LIN OV.L
U-v 4.i L
compared i F in the vicinity of-the zero chn-r-e in IN Na-SO
C = 135 and CH.. 2~-5 microfaraci/c.,n~. Further frcin
tii,~ zercj'~
c5arge the rate 5!ncrease JlnEfor Ga was reduced; it
appro.Ached E for
Thus an electric double layer of the same state as on Hg was
formed on Ga, only at a more positive potential with
repsect to the
Card 2/5

L -.6 5
CCIESSION NR: APL01-3555
zero cliarge y-i-JI;it. The Jncrease Jn C on lez5:,: riegat-*ve
V~;Iues
L I - - - ;. -
w.~js attributed not to the adsorption of 0 or OH on the Ga surface,
r- .3 r. Ca ions in the 'oundary layers, but to the
n e gat -L vE: n, -a
tiai. "I thane. B.~7-. Damaskin for participa tion in ev-aiua~"i!,g
Li,c
11 ." "Call 7-- s ourified by the ILrI,5titute.
r)t,'ained resul+s iwn wa _qk__j:qj~,q
T.&Ltals rneLricd. ,e ~.&ke tlie ofpc,rtunitv tc, tlhank AN ~35R
assoc.
a.3sJstance in cbtaininr it ." Ori~-. -art. t,,Zi 6:
ASSOCIATION : Nore
SUB14ITTED: 311-41aru4
ELENC-L : u2
SUB CODE: GC, NR REF SOV: ouu OTHER: 005
Card 3 / 5

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ta
C --, r 4 ~/'-', - -

F.i --are 2,
t
4

a r

Behavior cif a rraliium dr:iFp'-'ng el,---:!trode
hydro-en
ra'ik~j-,".ne Jn the
138 Ag 164.
I RA -.' 81
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Appearance at fre* atomic hydrogen on the mercury
1~00

cathode and the mechanism of the cathodic reduction
of tungstate. V.A.-JUguiskil and Z. A. 1(,I.t M. 1'.

Lotsinna"ir
Mowow State llniv,j. C-std. rrfsd. acad.
'
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1

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are

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dvwlilwd whirb fillpi"W1 The 01-1-trnij rowl. lbrory
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BAGOTSKIY, V. S. Cand. Chem. Sci.
Dissertation; "The Kinetics of Eydrogen Evolution on mercury."
Rfoscow Order
of Lenin State U imeni M. V. Loraonosov, 18 4un 47.
SO: Vechernyaya Moskva, Jun, 1947 (Froject #17836)

!so *sees 600*0906 ***me-
0 6 0 0 0 0 f-w-w-
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~V. .. PC -so
.00
0* A fulin
z,A. W14, wid A. N. I'minkm (blm~ 11mv., M').I.-I. 00
J. 1'4p. CArm. (V.S.S.k.) 21. 2414(1947). -41tvitua- :_Go
io I d ryci" 11 flugs. at the Cathode alrd their oxitution .00
C.A.41,
!-So
00
0 -00
:
0
so
,q
so LIO 0
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Les
AS 4. 11 A Q I At t 106K at tIfIWSTU*f CkA%S(FKAIIQ3I
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AV Q M -W r AA (U-
tv 0 It0 of a It it At wo A I Sh
It
0 0 0 0 :,is 0 0 0 0 0 0 00 0 0 0 0 0 0 0 0 0 9 0 0 0 0 a
~09 0 0 so fe 0 0 9 go 0 go 0 0 0 0 0 -s a 6 -6 ~116 s a 0-00
0 so 0 go sees 0

DokladyAkad.
Mrs-"19117); chest-trolp. (kuvqkm
Zone Ed.) 3040. 1. M.-The equat Ion of I'mmkin C.A.
ZT.:NIM) Is" be" temed by Levina ami UdnAit 40: C.A.
31.PW 42 ) an LuCU It. nPOW It to KCI sulm.
Con nd it to be valhi In I he following tom for
v-1.40D+(2RT/FXlni)+
th - (Rrip) I V. in which q is the ovrrvoltasr, i
tlw CA. and to, the Potential of the diff.- of the
eW. double layer.

WWWW'WWWWWWWWWWW _._- -~-__
990-4 be
41 6 1. 1, 11 off U it M ft' jgituamumuil
~A -S-A-JL AIj AL I A ~..j VIP A 1--A A
o0 4 4 66#4 *0
Go "oMM Ab Wr#111#6 1.9,11
00 A TIWW 91 onseWsOm peledutim at a drow"s mer-
N. Milma". ZA11F. Fit. thit". (J~
1-00
irb 7eb equation
YS 14
4C.A. 29.25W) Is valid only if the Ionic cown. C next
00 to the drop Is Independent of the d.c., i. It C - of (d
consi.), the equation I a /,(7 re-
'00 sults. to is tbo im limiting diffusion current Ui%ru bir -00
0 the riliiation of llko%rik), at is 3trittIPPIP, 4 brine ~Vnic
0
charge, F Fanday no., D diffusion cotff,, and I firne. .04
00 is 300PAP. r being the life time of a drop, and CO 1% .00
J. ;I function ilmessing Imm I at is - 0 to, e.g.. 0.W543 .1 j~
to. It. Cuives of Ike COOMtration Polarhation of
hydre Ibid. 1466-76.-The above
.,C!. V. S. B"inslill.
e
uu,
quat was cohfiknid by measuring the current I (life
t- discharge of H * as function of the polarization %vitage.
00 Thesoin.waso.33 NKci + 0.49 X 10-4or3,9 X lj)-9N
IfCI and was satil. with lit. The I wits found by sub-
tracting the cuffent in 033 N KCI (which 6 stwat for job
charging the double layer on the growing tic drop) from
'r that In the solos. conic. JICL The value of 0 was rated.
from cipts. on stationary He cathode In dfl. IICI + diL
XCI, and The valtic of D from Illsovit's equation; In 4.2 X coo
10-4 N HCI + 0.33 N KCI, D of H * was 7.9 X to -4 sq.
I cm./sisc. The r was lowered by cathodic polarization see
from, e.g. 8 we. at -0.8 v. to IM than 3 W. at - 1.5 V.
Contrary to Ilerrvnky (C.A. 32, 541) tbere is no essen- ja 00
list diffaTisce between the kinetics of It discharSt at a Poo
inationasy and that of timpping electrode. J. J. U.
V,
IN)ONO Nit Q"V off O%V It(
1 0 '71 AA I t I
U 0 AV so At 41
1W 0 0 4 1 a 3
0 00 00 00so 0000 0 sole 0 0 Le 9 000000 Do**

10 i
0 44
so A
00 0
00
so
00
go
go of
00 '3
00'0
.3
00
i ;
4
17
KbMksd MIMI-
flam as a 1AIrreary C1 V S. PA.
W.tsklt anti 1. R. Y,blk,v,%. PNi4te-fesk"I
of 1%yoleal t1hrenimtry), Y. 123, Apr.
1040. p. 413-4.11.
Obtains, experinooentally. a curve Inditatinst the
relationship of ovorvoltaxv to Ing of current den.
ill), on thp mercury cathoile In phostoWe butTer
solutions In the JAI Interval from 2.23 to 7, Wows
that the valu" fit overvoltneer at qNstloolant miTri'M
dortromity depends ion till and ion total lion conevittrot-
tion of the solution. It Is further IndleRtrit thm
the liberation of hydrqmn from slightly arid anti
neutral solutions to subject to the same regularl-
It" as In Sold solution, firsults are in agreement
with the thri-ry prolmoval by Frumloin. it "-f.
10119*0 -4V INV eke &"Inv
U 614t)) 0"K eftv
I~h - W -". 10 0-
14 W 4 ~*" a
it it 1W 0 a
0. ~MIA at ~1. '14 ~D
4 #IN
0 g 6
file
2
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roe
too 0

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t
.

ova U,
b16 omen c!irtT6dv i6z rimcury in mA.Alne 5~1

the lai6it~,= Mr t.~
Cthoee redljt~m cd 0

aad D. L. Moto;- (Al. V. 1-ma
l

Mesa -d. A
~
ow). Dobwy AL,. -~ S.S. S.R. 71

cAlbnde reAucli-n of 0 was studi--,

,-'3 -
ncuufo --tAni. C, dc,

Th. f"'o, wl

-palw=e,2 %vLth respcet tc.
the auxili.- -A-ucl ur incrt-uric

ioln " c':- -4c 7:.- -,ft(i

the
ro,---h---rfm of fl., ep. r 1,~. h-v, v and

in tas-x T~ir ne.--, -Ii.
t-I h~ rt-A~Cti.-l

SOCHEVANOVI V.G.;.PAGOTSKIY_, VS., red.;
BDGATIN, G.A., red.;
BABDCHKIN, S.N., tekhn. red.
[Galvanic cells) Gallyanichaskie elementy.
Moskva, Gos-
energoizdat, 1951. 271 p. (MIRA 16:7)
(Electric batteries)

FRUMKIN, Alekeandr Naumovich, 1895-, redaktor; BAGOTSKIY,
V.S.; IOFA, Z.A.; -
KAMIOV, B.N.
(Kinetic energy in electrode proceases] Kinetika
elektrodnykh protsessov.
[Pod red. A.N.Friu*ina. Moskva] Izd-vo Monkovskogo
universiteta, 1952.
318 P. (MI-RA 6:7)
(Electrochemistry)

FRUMKIN*v As No IDFA, Z. A.
Overvoltage
N. I. Kobomev's adsorption theory of overvoltage. Zhur. fiz. khim.
26 no. 12
1952
9. Monthly List of Russian Accessions, Library of Congress, May
1953. Unclassified.

1y
Lquilibnwa potential of t~,e svs'.em~. ongc-n
h.vd---,rcn

---
slow dlj~~r~e tbeDry of Frumlin for 11
mduction (C.A. 44.
874Zrl 1-~d Th- -Pr- -( -~hr

-3
C/.,
uSsR/Chemistry Hydrogen Peroxide; Bov 53
Polarography
"Mechanism of Electrochemical Reduction of
Oxygen
;.-and Hydrogen Peroxide at a
Mercur?r,-,Electrode,"
J4. S. Bagotsk1y"2:1. Ye.
Yablokovat~koscov State U
Zhur Fiz Khim, Vol 27, No ii,pp 1663-1675
Investigated the kinetics of polarographic
reduction
of %02 and 02 (alone-or in the presence Of
H202) in
solne, of different PH. Found that the
kinetics of
reduction of 02 on acidic and alkaline
solns are diffe'-
rent" but formulated a single mechanism
whickL ex-
plaine, the behavior of 02 in both ranges.
Demon-
strated that all kinetic phenomena
observed In the
274T20
reduction of B202 can be explained by the
assump-
tion that only molecules and not ions of
H202 are
reduced.

.-,. I-,- I- . .- . . I 1
.1
"' I '. I..: % I , . , I .

~s r, ~ C -1 .- I ~_ 4 ~ - V ~~
AUTHORS:Shte;7nber 9 G IV'. (Engineer) and Bagotskiy V,S'.
(Cand.
Chem.Sc ~M-7-10/30
TITLE: Some special features of the operation of the positive
electrode in a chromic-acid cell'. (Nekotorye osobennosti
raboty polozhitellnogo elektroda elementa s khromovoy
kislotoy),.
PERIODICAL: "Vestnik Elektro"omyshle-nn sti" (Journal of the
Elect_r_1_c=..n_Tu_stryp "Vol-,2b, To""=, -1957, PPF-34-38
(USSR)'.
ABSTRAM.Galvanic cells based on the electro-chemical system
n ta C 0
'/-2 r2 7. ~2SO4/zn are still used be-cause of their
comparatively high power, 'their ability to work at low
temperatures and the possibility they afford of compact
constructiom:. During the discharge of a chromic acid cell
some phenomena are observed, the nature of which are not
yet clear. For instance, under some conditions 6f-dis-
charge the cell voltage drops in jumps of 0~.'27- 0'.3 volts
after wh 'ich the element continues to operate at normal
capacity. Under other conditions of discharge the cell
voltage suddenly falls almost to zero despite the presence
of a considerable reserve of unused active substances.
Card Both these phenomena are associated with step-wise
change
1/5 in the potential of the carbon electrode. The effect of

Some special features of the operation of the positive
electrode in a chromic-acid cell. (Cont'.) 110-7-10/30
step-wise change in the -potential of the carbon electrode
by 0.1-0".3 volts in the negative direction has been called
the "partial passivation" of the carbon, and the effect
of step-wise reduction of potential by one volt or more
is called "total pasdivation!' of the carbon. It is well
known that cathodic polarisation of metals in chromic
acid occurring at some definite current density causes a
sharp potential jump in the negative direction after which
separation of hydrogen commences. A similar potential
jump has also been observed on the carbon electrodes This
effect which is apparently analogous with."total passiva-
tion!' of the carbon is usually explained as being due to
the formation on the cathode of a screening diaphragm of
trivalent compounds.
Carbon materials may differ widely in physical-chemical
properties and it was therefore of interest to find out
whether partial passivation is a general property of
carbon electrodes or is associated with special features
of some particular types of carbon'. The investigations
Card were made on 9 types of carbon of different physical-
2/5 chemical propertiesq see Table 1~. The investigations
were

Some special features of the operation of the positive
electrode in a chromic-acid celf. (Cont..) IID-7-10/30
made by taking polarisation curves, and a number of
pbysical-chemical properties of the carbon were also de-
termined.
Fig.1 shows curves of the relationship between the poten-
tial (measured against a noimal hydrogen-electro~le) and
the current densityv. and Fig.2 shows curves of the poten-
tial as a function of time for different types of carbon,
it is seen that for all-types of carbon, at current
densities of 180-200 mA/cm4 there is a sharp ump of poten-
tial of'1 to f.'2 V in the negative direction itotal passi7-
vation). Separation of hydrogen commences after the jump'.
At lower current densities of 5-60 mA/cm2 three of the nine
types of carbon investigated displayed step-wise potential
displacement'of 0'.1-0'.3 V (partial passivation)'. The same
three types of carbon display step-wise potential reduct-
ion during polarisation at a constant current density of
5-40 MA/oM2.
Fig'.3 shows polarisation curves taken on a rotating carbon
Card electrode at different speeds of rotation'. As the speed
3/5 is increased from 0 to 1200 rpm the current density at
which

Some special features of the operation of the,~ositive
electrode in a chromic-acid cell'. (Cont'.) 1 -7-10/30
total passivation commences increases threefold'.
In order to studv the influence of the solution composi-
tiony potential/time curves were determined with constant
current density on the cathode in solutions with different
concentrations of chromic and s-alphuric acids, trivalent
chromium and salt. Fig'.4 shows curves taken on solutions
with different concentrations of chromic acid with con-
stant total solution acidity'. On the basis of the.experi-
mental data that was obtained it may be concluded that the
effect of total passivation. of carbon is caused by definite
concentration changes in the layer of solution adjacent to
the electrode. The removal of these concentration changes
also removes total passivation of the carbon which demon-
strates the absence of an insoluble diaphragm of chromium
salts at the carbon surface under conditions of total
passivation:.
The effect of partial passivation is not associated with
changes in concentration near the electrode'. Partial
Card passivation is a general property not only of carbon
4/5 electrodes, but of inert metal electrodes in general

Some special features of the operation of the ositive
electrode in a chromic-acid cell'. (Cont.) 11t-7-10/30
(platinum and gold) in chromic acid:. Partial passivation
depends on the nature of the carbon, the composition of
the solution and preliminary polarisation of the electrode.
Change in the composition of the solution or preliminary
treatment of the carbon can vary both the electrode poten-
tial before and after partial passivation, and the time to
the commencement of partial passivation ,. Data on the
influence of mixing, the composition of the solution and
preliminary treatment of the carbon on partial passiva-
tion show that this effect is not associated with the
deposition of chromium compounds of low solubilityf, Par-
tial passivation is caused by change in the state of sur-
face of the carbon under the influence of the process of
Card reduction of chromic acid.
5/5 There are 4 figures, 9 references, 1 of which is Slavic'.
ASSOCIATION: NIEEI'.
AVAILABLE:

i r 5 x, y
AUTHORS: Shteynberg, G. V., Bagotskiy, V.S., 20-3-41/59
TITLE; Certain Features in the Catholic Reduction of Chromic
Acid on a
Carbon Electrode (Nekotoryye osobennosti katodnogo
vomkanovleniya
khromovoy kisloty na ugollnom elektrode)
PERIODICAL: Doklady Akademii nauk SSSR, 1957, Vol- 115, Nr 3,
PP- 568-571,
(USSR)
ABSTRACT: In the case of cathodic polarization of a carbon - or
any other in-
ert electrode - in a solution of chromic acid a sudden check of
the
reaction 9f reduction of the chromic acid anion Cr207 +14 R+ +
+ 6e -4 2cr+++ + 7H20 is often observed. This check is
accompanied
by a instantaneous shift of the potential to the negative,which
is
followed by a reaction of hydrogen separation (a complete
inacti-
vation of the electrode). Apart from this phenomenon, in some
in-
stances a small shift of a few tenths of a Volt have been
observed
in the case of densities, where the potential of hydrogen
separa-
tion has not been reached. The complete inactivation of inert
elec-
trodes in solutions of chromic acid was the object of investiga-
tions of several authors. In the paper under consideration the
in-
fluence of a series of factors (composition of the solution, of
stirring and of the treatment of the electrode) on the partial
in-
activation of the carbon electrode was studied. From the figures
it can be seen, that the potential of the upper and lower niveau
Card 1/3 of the curve, corresponding to the active and
partially inactive

20-3-41/59
Certain Features in the Cathodic Reduction of Chromic Acid on a
Carbon Electrode.
condition of the electrode, as well as the duration of the
active
state are dependent on the composition of the solution. The in-
fluence of identical components of the solution on the
potentiil
of the active state and on that of the partially inactivated
elec-
trode is differing. In particular the effect of an addition of
an
indifferent salt to a highly concentrated solution is falling
in-
to the eyes. The salt instantaneously shifts the potential of
the
partially inactivated electrode to the negative, whereas the
poten-'
tial of the active electrode is very little affected. An
introduc-
tion of three-valent chromium, even in1high concentration has
practically no influence on the partial inactivation. An
addition
of chromiumsulfate in high concentrations, however, shifts the
po-
tentiil of a partially inactivated electrode. This is
apparently
not connected with the presence of three-valent chromium. A
simi-
lar shift also takes place in highly concentrated solutions of
sul-
phuric acid and chromium acid. These effects detailed here are
to
be considered as a check of the electrochemicil reaction and
not
as a change in their nature. The experimantal results obtained
here
contradict the conception, that the check is produced by the
for-
mation of a diaphragm consisting of compounds with small
solubility
Card 2/3 of the three-valent chromium. It is probable, that
the partial in-

20-3-41/59
Certain Features in the Cathodic Reduction of Chromic Acid on a
Carbon Electrode.
activation is connected with a modification of the state of the
oxyde layers on the surface of the electrode. Several facts
in favour of the concept, that some forms of the surface oxydes
correspond to the active condition of the electrode. They
vanish
during the cathodic polarisation and reappear during the soft
ano-
die polarization of the carbon. The phenomenon of partial
inact-i-
vation of the carbon-electrode can be explained as a
modificati':~.,
of the electrochemical mechamism of the reaction of
ion-reduction
of the 6-valent chromium into three valent chromium. This
transi-
tion takes place because of the modification of the oxyde
layers
on the electrode sueface. Phenomena of the same qualitative
cha-
racter were observed on inert platimum and gold electrodes.
There
are three figures.
ASSOCIATION: State Union Scientific Research Oarbon Electrode
Institute.
(Gosudarstvennyy soyuznyy nauchno-issleauvatellskiy elemento-
elektrougollnyy institut)
PRESENTED BY:Frumkin, A. N., Academii:iia, Feb. 32, 1957
SUBMITTEDs FebruarY 5, 1957
AVAILABIEs Library of Congress
Card 3/3

I BAGOTSKIY, V.S., Imnd.khim.nauk
- -
Progress in the field of electric power production from chemical
action. Khim. nauka i prom. 3 no.4:448-454 158. (MIRA 11:10)
(1lectric power production from chemical action)

50) PHASE I BOOK EXPLOITATION SOV/2216
54veshchanlye po elektrokhlmll. 4th,
Moscow. 19%. ril
Trudy... s Isborr.11c] (Transactions of
the Fourth Conference an Elect-
rochomistry; Collection or Articles)
Moscow, Izd-vo AN SOSE.'
1959. 89 P.
Errata 02 Ip Inserted. 2,500 Copies
printed.
Sponsoring Agencyt Akadomlya nauk SSSR.
Otdolonlye khlmicheakikh
nauic.
Iditorial Boardt A.M. Prumkin (Reap, Ed.)
Academician, O.A. Yesin,
Yroressor) S.I. Zhdanov (Ramp.
Secretary), B.M. Kabanov Pro-
rossor, 3.1. Zhdanov (Reap. Secretary)l
B.N. Kabanov. ?;;ftsllor,
Ta. M. Xclatyrkin, Doctor of Chemical
sciences; V.V. Losev, P.D.
WkOVt3eTo PrOfea3Orj Z.A. Soloy-yeval
V.V. Stender. Professor-.
and G.K. FlorlanovIch; Ed. of Publishing
House: N.C. Yagcrov.
Twch. Id.i T.A. Prusakova.
PURPOZEt This book Is Intended for
chemical and :Ieotrlcal angl-
neers. physicists, metallurgists and
researcher in tereated in
Various aspects of electrochemistry.
OVERAGE: The book contains 127 of the 138
reports presented at
the Fourth Conference on Electrochemistry
sponsored by the Depart-
Rant of, Chqmlcsl Sciences ar4 the
Institute of Physical Chemistry
Academy of Sciences, USSR. The collection
pertains to different
branches of electrochemical kinetic$,
double layer theories and
galvanic processes In metal
e2ectrodepoeltOn and Industrial elect-
7
rolysio. Abridged discussions are given
At the and or each dIvI-
*ion. The maJority of reports not
Included here have been
published In periodical literature- No
personalities are mentioned.
References are given at the end of most
of the article@.
Z&4-,t-.- !-
4, y, S.A. , J~O._Zjjj=%tzkiy (Deceased),
and 1_4_Bogdanova.
Anodic Behavior of Manganese and Its
Alloys Z3
(Dnepropetrovskly
khIm1ko-tekhnolog1cheskIY ln#tl'ut
Imeni F.E. Dzerzhin3kogo; Inatitut khImil
AN KaZSSR - Dnepro-
petrovsk institute of Chemical Technology
Imeni P. r. Drer-
VhInsk17, Institute of Chemistry, Academy
of Sciences, Kaz-
SSR). Electrlode Processes at a Lead
Anode and Its Corrosion
During the Electrolysis of Sulfuric Acid
Solutions 729
Discussion IF. P. Tsyb and contributing
authors) 732
PART IX. CHEMICAL SOURCES OF CURRENT 735
Electrode Processes In Mew Electrochemical
Card 2964
Sources of Current 737
Easpv yn. B., z. a. yampOl -skaya, and
BX_"banOV.
Lead
Su1T1LtW--Tr--hO_M09ftt've ?'a%* Ot W T44
Battery
d V 1. Bartlenko. Mechanism of the W65
or lffLci.."'n _Zge-7mterial of the
Positive
ey in e-jE~
Electrode of a Lead Battery T48
XrIxAlA.P_0Yq_1--Y- - 8. S. Vaymberg, and
IL X. Kabanov.
Znv#&t1i8tj"g & LaAC-rr=jde- E lect rode
i-Or P6t'e_MtIWI Drop 757
and oxygen Evolution
Ary%~~qya,__T_A, (Vp0boyu~ny7
nauchno-Inaledovatol'oklY
inatitut Istochnikov toka-All-Union
Scientific Research
Institute of Electric rover Sources),
Growth Of Zinc -
D*ndrltea in Some Swelling Polymers .62
plerov, V. X. (Gor1kovskly
politekhnichoskLY lnstLtut laenI
card 'J0/34

50, 2) BOV/2o-128-3-39/58
AUTHORS. Mendzheritskiy, E. A. ,
TITLE: Equilibrium Conditions an a Zina.Electrode
in-Alkaline-Solutions
Saturated With Zincate
PERIODICAL: Doklady Akademii nauk SSSR, 1959, Vol 128, Nr 3,
PP 575-577
(USSR)
ABSTRACT; In spite of many investigations, the t pe of
s-olid-and.prod-
ucts (whether zinc hydroxide or -oxide~.for_me4..An__itor1r4n
the solutions mentioned in. the title- on-the-zinc-alecirDde
has not been precisely determined (Ref 0-The.corivera.ion
of primarily separated modifications of zinc hydroxidea in
stable forms causes an "aging".of the zinaate solutiona.by
impoverishment in zinc ions. A publication Burvey.shows
(Refs 2-5), that individual investigators diaagree w1th
respect to the value of the free energy of the~stablest
9-modifioation of zino hydroxide. To determine. this.problem
more precisely, the authors measured the eleciromotiveL.force
(emf) of the chain; Znp ZnOoaq(KOH'+ zincate)HgO, Hg at dif-
ferent alkali concentrations. In the case of formation of
zinc oxide on the discharge of such an element, the electro-
Card 1/-S motive force (emf) must be independent of the
concentration
/_7

SOV12o- 128-3-39/,58
Equilibrium Co4ditions on a Mnc Electrode in Alkaline
Solutions Saturated
With Zincate
of the alkaline solution according to the equation
Zn + HgO - ZnO + Hg (1). If, hovever, zinc hydroxide is
formed (2), the emf of the chain is bound to decrease with
the increasing alkali concentration since the water activity
falls. Principal attention in these experiments was paid
to the maximum approximation to the state of equilibrium.
In preliminary experiments it was found that the omf of iner-
curic-oxide elements is fully stabilizad 2-3 months after
the preparation, and remains practically unchanged during
the subsequent 9 months and more. A partial additional charge
with an elimination of 10-15% capacity of the element great-
ly accelerates the stabilizing process of the emf. Heret the
solution is particularly saturated with zincatew and the
solid phase falls out. Figure 1 shows the dependence, found
in this way, of the emf on the alkali concentration in the
KOH-solutions saturated with potassium zincate betpeen 0.6
and 12-5 n. It shows that the emf is constant between 0.6 and
1.5 n, and amounts to about 1-344 volts. This value
approximate-
Card 21a ly corresponds to the data of reference 2 for F_ Qn
/Y (OH)2'

SOVJ20-128-3-39/58
Equilibrium Conditions on a*Zino Electrode in Alkalifte.Solutiona_
Aaturat~d
With Zincate
Prom the amf value of 1.353 volts in-higher-concentrated solu-
ti8ns, the value of th8 free energy of the zinc oxide at
25 follows, i.e. A F ZnO - -76.4 + 0.1 kcal.-The difforenoe
of this value by 0.35 kcal as compared with V. Latimer
(Ref 4) 9 is essential since it yields a vdl:ue- of the free.
energy 'of the transition of-the-zina-hydromide-4nta-zine..
oxide AF - v0.5 kcal instead. of -0-15 kaal-The-sigrx-of
this new value is undoubted,- and gives_pr_oQf._of.a_high thermo-
dynamic resistance of the zinc-oxide-in.dilifted solutions
(at a water activity - 1). The-above conaluaion-sta-ting
that, under equilibrium conditionst,zinc-oxidei.not zinc
hydroxide, is formed, is also confirmed by.othem.exparimantal
results. The temperature coefficient of the emf measured
amounts to 0 4 + 500C + 0-00004 volt/degree. There.ara 1
figure and 8 references, 3 of which are Soviet.
ASSOCIATION: Vsesoyuznyy nauchno-iseledovatellskiy institut
istochnikov
toka (All-Union Scientific Research Institute of Scurcei of
Card 3 CurrentY it.

S/02 60/132/03/42/066
,57 A310 0 B004YB007
AUTHORS: Popova, T. skiyj
Kabanov, B. N.
TITLE: Anodic Passivation of Zinc in Alkaline Solutions
-
A
1
PERIODICAL; Doklady Akademii nauk SSSR, 1960p Vol- 132, No. 3,
pp. 639-642
TEXT; It was the aim of this paper to investigate the influence
exerted
by the adsorption of oxygen and by the formation of an oxide film
upon
the passivation of zinc. The anodic behavior of Zn was investigated
in
KOH by means of osoilloscopic; recording of the potential - time
curve
y(t) at constant current density i on a rotating disk electrode.
"Pass
=itn was determined (Qpass is the amount of electricity necessary
for
passivation, t n is the time up to pa8sivation). Fig. 1 shows the
diagrar~
1/qpass - f(i). At mean current densities there is a linear
dependence
between 1/Qpass and i. In the case of i being low, Qpass becomes
dependent
on the rate of stirring, and in the case of a very low i and a high
rate
Card 1/3

Anodic Paasivation of Zinc in Alkaline Solutions S/020
60/132/03/42/066
B004 3007
of stirring, no passivation occurs. From these results as well
as from
the anodic polarization curve (Fig. 2), the curve of the
increase of the
potential after 60-min passivation and after switching off the
anode
current (Fig. 3) as well as from the dependence of the
dissolution rate
of the passivated electrode on the speed of rotation (Fig-
4)-the authors
draw the following conclusions: The dissolution of zinc
depends on the
dissolution rate of the zinc oxide (and peroxide). As
passivation occurs
already at potentials (-1.1 to -1.0 v), which are more
negative than the
reduction potential of the zinc peroxide in the oxide film,
passivation is
primarily based on a change in the concentration of KOH and
the zincate
retarding dissolution in the liquid layer near the electrode.
The forma-
tion of the oxide film is a secondary process. There are 4
figures and 7
references: 4 Soviet, 2 German, and 1 Indian.
ASSOCIATION: Institut elektrokhimii Akademii nauk SSSR
(Institute of
Electrochemistry of the Academy of Sciences, USSR)
PRESENTED: January 25, 1960, by A. 1. Frumkin, Academician
Card 2/3

.Anodic Passivation of Zinc in Alkaline Solutions
S/020/60/132/03/42/066 ~z
B004/BO07
SUBMITTED: January 11, 1960
Card 3/3

WHE) A.I.; ASTAKHOV, I.I.; NIKITINA, Z.Ya.; REZNIK, I.F.;
Change of the structure of a negative electrode in a
oilver-zino
storage cell in operation. Zhuro-prikl.khim. 34
no.10:2254-2260
0 161. (MIU 34:12)
1, Institutelektrokbi-44 AN SSSA i Voesoyuznyy
nauchno-isoledovateliskiy
inotitut istochnikoir toka,
(Electrodes)
I

1OFAJ, Z,-A.; KOIU~EV, L.V.; BAGOTSKIY, V.S.
Hydrogen overvoltage on a zinc electrode In
alkaline
solutions. Effect of the concentraticn of a
potassium
hydroxide solution. Zhur. fiz. khim. 35
no.7:1571-1577 J1.
161. (MIRA 34:7)
1. Moskovskiy gosudarstvennyy universitet im.
M.V.Lomonosova
i Vsesoyuznyy nauchno-issledovatellskiy institut,
istochnikov
toka.
(Hydrogen) (Overvoltage)

OSHE~ A.I.; BAGOTSKII., V.S.
Mechanism of the cathodic reduction of zinc oxide
phase layers
on a zinc electrode. Zhur. fiz. khim. 35
no*7:1641-1642 Jl
161. (MIRA 14:7)
1. Inatitut elektrokhimii AN SSSR.
- (Zinc oxide) (Reduction., Electrolytic)

S/030/62/000/007/002/004
1048/1248
AUTHORS: Bagotakiy, V.S., Doctor of Technical Sciences, and
A;aRkin, A.N. , Acdemician
TITLE. The problem of direct conversion of chemical energy
into electrical Cen~rgjj
PERIODICAL: Akademi-i--nauk.SSSR, Vestnik. no. 7, 1962, 19-32
TEXT. This reyiews the history and the state of development
up to 1960 of fuel cells and other electrochemical current gene-
rators. Their operations Eire briefly discussed, the emphasis
being on weig
C, ht vs. -,Do,.Ner output considerations. The use of fuel--
cblls is preferrea fb 'r long times of operation (20 hrs and
over),*
but conventional storage batteries (e.g., lead or Ag-Zn accdumu-
Card 1/2

S/030/62/000/007/002/004
The problem of direct .... 1048/1248
lators) are superior for short-time uses. Although available
luel c6lls have a weight of 35-70 kg./];_-w. output, cells
weighing
15-20 kg.";, . could be developed the lowest possible limit being
/.-w
6-10 kg./kw. 2uture applications envisaged are in city transport,
for military purposes (due to quietness and absenoe of smoke),
and
in Artificial earth satelites and spacerockets. A Scientific
Council for Puel Calls, associated with the USSR Academy of
Scien-
ces, has been set up in the USSR. The article is based mainly on
VIestern Sources. There are 4 figures.
Card 2/2

S/076/62/036/007/003/010
B101/B138
AUTH023: Popova, T. I., Bagotskiy, V. S., and Kabanov, B. N.
(Moscow)
TITLE: Anodic passivation of zinc in alkali. !. Measurements
at
constant current densities
PERIODICAL: Zhurnal 'Lizicheskoy khimii, V. 36, no. 7, 1962,
1432 -1438
T:: X T :The -,~otential-time curves for rotating zinc anodes
were oscillo-
,--'r,'11)hicnllv recorded in 0.1 - 1 N KOH at 60 - 5000 rpm,
200C, and current
densities, i, of uP to 340 ma/cM2. The curve 1/.,4 ' showed
three sections
2 pass.
BeMeen 10 and 200 iriia/cm, the total amount of el.ectricity
required for
Dassivation rises lineirly with i, and is not affected by
changes in the
becomes independent of i and
race of stirring; at i -\ 200 ma/cm2, Qpass
z-anches a 1�.-..itin,- value vhich is independent of the
stirring rate but
diminishes with decreasing alkali concentration; at.i