SCIENTIFIC ABSTRACT BOGDANOV, G. - BOGDANOV, G. B.

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• Collection: Scientific Abstracts
• Document Number (FOIA) /ESDN (CREST): CIA-RDP86-00513R000205820008-6
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• Document Release Date: June 9, 2000
• Sequence Number: 8
• Publication Date: December 31, 1967
• Content Type: SCIENCEAB


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ARIWJPVr'GTt,'=NOV. A.; 1,111PA, Tu.
Shock abosorbers of the "Moskrich-W2"' automobile. Art. tmnsp. 36
no.U24-25 Ja 158, 1(MIR& 11:1)
1. Roakovskiy karbywatorn" sayod,
(Automobiles-Shook absorbers)

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S/076/63/037/004%)OV19
AUTHOR: Savina, M.;, Bogdanov-,:-d.,-.Potrova,_G.-L., and Yurche]?.9, G. X. /7
n,
TITLE: Catalytia 4ecorapositio f, H02 171der the cciabined acticn. oL s o,!7 uu,
land'. - the I
molyWate eiev; nts of the zinc subp
salts of
Zhurnal Sizicheskoy khiinii V, 37, DO. 4) 1936, 746-752
PERIODICAL:
:~!IEXT: :The :article exavdnes the combined effect of zinc sulfa-.e and s 0d. ium
molybdate oa-the catalytic decomposition of H202 in neutral. and acid media. Zinc
eulfatet retards the, rate. Of the decOMMOsitiOn: Of H20_9.'by sodiur, rolyhdate, the
lie
catalyltic process being the slower,:the.hiaherthe concentration of ZnS04-
'he hydro-en
eaction is of the first order,regardless~of the temberature and oP
ion and substrate conc!entration. . The activation energy is 12.8 Kcal/mole- . The
electroennductivity. under~all conditions -dipdnishes- as the decomposition Of H202
progr Iepses. The chaikgre in -the rate -of catalysis is
t the ii,.termediate pz ts~ Q.;.
detert'd ned by ~the concentra~ ion* and, na ure of -oduc- ,Mch are,
formed in the solution. New-zine pero;Komolybdates With very high decomposition
H
constants (Zr.LVo04, - nJ120 Or ZrJ,1oP4 :.2H2O2, - n 20 and ZnMmO05 * ar; 0 r Zn"'o 4
H202 - nH20) have- been isolated., ',The experimental results indicate that the re-
tarding action of thezinc ions is.due to the low equilibrium constant of zinc
card 1A

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S"; BOTVIN., N. (Vologodskaya. obl,)j LISTOPAD,.G. (Vologodskaya obl.);
SHIBAIEVS V. V028camd)j BOGDANOV G. pomoshchnik instraktora.
Profi.-LaIM'" A. ponoshchnik
X&A
instruktora, ofilylktik4 (ftybyebevskaya obl.j,- GRIMVICII, S.
NovosibirsICW obL.); 8LUFKO, A. (Urel'okaya. ASSR); LAVRFMOV.. I.
g, Vladimir) sibi.rokap
i
ReadersI letters. Pozh~delo 8 no-W9 Vq 62. (KERA 15:5)
1. Glavnyy inzh. Isoorrevalochnoy bazy,, pos.Malinovka, Kemerovskaya,
oblo (for Linev), .L
(Fire prevention)

KHRAEROV, I.; BDGDLNOV,, 0.
Impeifections of the stern tube arrangement on the motorship
*Muraiinsts.~ Mor.flot 23 nas'203 F 163. %"KM 16:2)
1. Starshiy gruppovoy inzh,-mkhanik Mmusnakogo portovogo flota
(for Khrabrov). .2, Starahiy insh. otdola tekbnichaskogo
kontro3j" Murnanokogo portovogo flota. (fot,Khrabrov).
(Mlotorships-Design and cmnstruction)

DANIIENKO, I.A.; BI~O~G ~AN_GJ_..,__kand. sellkhoz. nauk; GRIGORtYEV, Ye.P.,
red.; YELMVETSKlY., V.S., tekhn. red.
(Corn and sugar beets in swine feeding] Kukuruza i sakharnaia
svekla I kormlenii svinei. Moskva., Sellkhozizdats 1962. 229 p9
(KIRA 15:6)
L Chlen-kor'respondent Vessoyu2noy akademii sellskokhozyaystven-
~.nykh nauk im. V.I.Lenina (for Danilenko).
(Swine-Feeding) (Corn as feed) (Sugar beets as feed)

.P, .
Yc~~d.O,Ale4l,-) 6, &
SOGDANO
I
nSuChWy motrudnik.
Iffeativeness of svpplementary microelement feeding to calves.
Zhivotuovodetvo 20 no.l.-42-46 J& 158. (MM Ila)
1. Hauohno-Iseledovatel'skly institut zhivotnovodetva Isenostepi I
Pbleslya USSR.
(Calves-Feedirs and feeding stuffs) (Trace elements)

DARIL19NKO, I.A,;_3OGDLWT, G.A., imad. eel Iskokhos. nauk
Protein nutrition of swine receivirg potato-corn meat-making
rations. ZhIvotuoyodstvo 21 n0-10-00-37 0 159.
(HIM 13:2)
1. Chlen-korrespondient Toosoyusnoy akadenii sellskokhox.muk
Insid V.I.Loalm I. Ukrainakor akadouli eel IekokhoxyaystvenmVkh
muk (for' Dantleako),
(Swine-Yeeding and foods) (Potatoes as feed)
(Corn as food)

Peedhg of soma fishapecles in Usti-Kamenogorok Reservoir. Sbor.rab.
po ikht. i gidrobiol. no-2:234-244.159. (KIRA 12:11)
(Usti-Umatogorsk Reservoir-Piahes-Pood)
100*

CHABAN, A.P.;-..ANWO'
Lp_ 0~_A!
Rind of the common bullhead (Gottus gobio Idnne) in the Irtysh
Basin. Zool.zhur. 39 no,7tllO2 Jl 160. (KLU 13:7)
1. Altai Ichthyological Station of the Inatitute of Zoology, Academy
of Sciences of the Irazakh S.S.R.
(Irtyuh River-Sculpin)

BOGDANOV, G.A.
- .1 - -
Vari,%tions of the fatness factorin the White Sea herring in
1.10.wtion to the state of its sexual products. DokLAN SSSR I"
no.3t652-655 Vq 162. (MIRA 15:5)
1. Imstitut morfologii zhivotzWkh im. A.N.Seveirtsove. All SSSR.
.1 Predstavleno akademikom Ye.N.Pavlovokim.
(White Sea-Herring)

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BOODA1446-v, to A#
"A Contribution to the problem of the effect of several catalysts upon the same reaction
in homogeneous medium. I. Catalytic decomposition of hydrogen peroxyde during a sim-
ultaneous presence of the salts of molybdenum and iron." Bopdangy, Go A., and Petin., No N.
(p. 379)
SO: Journal of General Chemist (Zhurnal Obshchei Khimii) 1942, Vol 12, No 7-8.

SWD14 V
'm P C. A .
"A contribution to the problem of the effect of several catalysts upon the same reaction
in homogeneous mediun.. II. Catalysis of hydrogen peroxide in the simultaneous presence
of sodium molybdate and wolframate." Btwdanow. G. A., and Petin, N. N. (p. 390)
SO.- Journal of General Chemistry (Zhurnal Obshchei. Khimil) 1942, Vol 12, No 7-8.

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BOGDANOV9 G. A.
"Homogeneous Catalysis of H202 under the influence of the Catalyst %We
(p. 896)
SO: Journal of General ChIpip _j, (Zhurnal Obshohei Khimii)., 1941, Vol, 17, No. 5
k

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BWDANCV~ G. A,
W451,ogen Teroxide Apr 1947
tZ7:,~
Cheialstry -Comp6unds- Unstable
0 in the
"The Rogogeneous Decomposition Of % 2
Simultaneous Presence of Na2Mo04 and P62 (S04)3,
G, At Bogdan0vt 9 PP
"Zhur Fiz Xhi-" Vol XXI, no 4 *,19,4V7
Technical discussion of the effect of iemperature
on the speed of reaction, the effect of the initial
concentration of E20 an the speed of reaction)
the effect of the reiationabip, of the catalyzer
of the concentraticap the effect of the hydrogen
ion concentration upon the kinetics of catalytic
decamposItion of R202. Illustrated vith tables)
formulae, and graphs.
i
147W

dogdanov, 3. A., Docent
Doc Chen Sci
Dissert~,tion: Wlaw 112teriuls on the lbaory of Homoveneous r7atalysis in Solut 'I
0
27 April 49
Moscow Order of Lenin Chenicotechnological Inst Lnnni D. 1. Mendelaycv.
So Vecheryaya Moskva
Sum 71 .

, P,
I A 17CT18

18DT15

USSR/Chemistry,- Hydrogen Peroxide Mar 51
"Theory of the Combined Action of Catalysts in
Solution, I," G. A. Bogdanov, Moscow
"Zhur Fiz Khim" Vol XXV., No 3, pp 323-331
Studied kinetics of homogeneous catalysis of
decompn of H202by K Cr 0 t Na2WO4 and K2Cr2O
+ Na2MoO4. These c9; "7
;3sj ineffective separat,61y
are effective catalysts together. In cases of
both cottinations of catalysts, formatfon of
combined intermediate perox1dic product was indi
cated and kinetic eq was derived on this basis.
185T9
'USSR/Chemistry Hydrogen Peroxide kar 51
(Coutd)
exams in both cases Confirmed pres-
intermediate products whose rate of for-
,.n!~tlon detd character of kinetic curves.

19 U80fChemistry - Hydrogen Peroxide mar 51
TbA of the Combined Action of Catalysts'Ju
ory ,
661ttion: 11. The Role of Intermediate Prod-
ulatnl~;.on the Basis of the Catalysis of H..,Op With
Cb**i and Molybdenum Salts,," G. A. Bogaanov,
Moscow
Fiz Khim" Vol XXV, No 3, PP 3327340
Studied in detail kinetics of decompa of H,
u~ftr'action of combined catalysts N 202
a2moo4+
(both ineffective catalysts separately)
iu:.,a7c14 medium. Using kinetic curves of reaction
iW,taking Into account acidity of soln, concn
6im/dzemistry Hydrogen Peroxide Mar 51:,
(Contd)
of J:itftlysts. and %0 preliminary treatmenVof
diecusse ormation of isolated inter-
Ote pro -,(active.vith to-
ducts CuWOg respect
~i'_"d CVV65 (slj6tly'active) neither
6~slj known in,:.Ii.t.

UM/Chemixtry ftdrogen'Peroxide Dec 5
"Theory of the Combined Action of Catalysts in
Solution. IV.. Kinetics of the Catalysis of
U202 in the Presence of AgN03 + N`2WO4," G. A.
Boglanov, A. 1. Pastukhova, Moscow
"Zhur Fiz, Mae Vol MIV, No 12, pp 1450-1454
Found that decompu of B202 :Ls catalyzed by AgN03
+ Na2WO4 in acid an& neutral soln, but not by
AgW03 alone' Catalysis is accomplished by sol,
of AA formed at eertain conen of Ag and by yel-
low intermediate product (isolated for 1st time
and found to'be Ag2W,06). A92W06 after 'J" at
197T25

USSR/Chemistry Rydrogen Peroxide Nor 52.
"The Role of Intermediate Products in Catalysis
by Means of a Deposit)" 0- A. Bogdanov and T.T.
Berkengeym
"Zhur -Piz Khim" Val 26, No 11, pp 1659-1663
Investigated the joint action of barium chloride
and sodium tungstate in'the form of a deposit
Ca -the decompn of H2 0;?. Determined that the
P~ kLnetic course of the catalytic reaction is
very complex: at a relatively high initial conen
of the substrate there was a zero-order reactionp:
then a quite abrupt, decrease in tbe. rate, a zero
order reaction, and a slowing down of ~-Ufte rate at
tbe~' end Of the expt; at a relatively jor,~. initiai
cmcn of the substrate, there was a very abrupt
de=ease of the rate, a zero-order reaction, and
41 slowing. dOwn Of the rate at the end of the'proal!*
ess. This cha in the order of the reaction
brIngs v-1th it also an um ctedly abrupt decreased
In the vol and a change in the color of the depoiit':
~MeL authors surmise that the observed effects axv.~
tmsed by the formation of bertain intermediate.
cci[Pds of different properties and compa. IAs
giult Of this work, they isolated hitherto unknown:
.b&riUM Pertungstates, established their campn, a. nd
ftveloped a methcd for obtaining them.
24=13...

BOGDAKOV, G. A.
heAisitry,,~'m4eroxidic- Compounds Oct. 53
,,"Investigation ofa Catalytic Process Occurring in
-161'ation and Iselation'of aNew Intermediate Product
0~ A. B6gdanovC'l. I. Pastukhova
Zhur
Piz Khim, Vol 2T,, No 10, PP 1556-63.
Investigatedthe combined action of nickel sulfate and
wolframate on the process-of decompn of hydrogen
peroxide und.er.various.conditions. On the basis.of the
date, obtainea,.concluded that a new compd, i.e. nickel
must exist., Prepared I by two differ-
ent methods and investigated itsproperties.
272T14:

C 6- &) /V C,
C&tOgOX7: USSR Physical Chemistry - Kinetics. Combustion.
Explosives. Topochemistr7. Cat&lYSi5- B-9
Abs Jour: Referat Zhur-W-1ya, No 9, 1957, 2M7
Author : Bogdan G. A., fttrova G. L.
Inst il -not givea---
Title Homogenous Utalysix of H 0 by Sodium, ChromLte and New Peroxide
pounds
Com
Orig Pub: Zh. fiz. khimii, 1955, 29, No 1, 84-94
Abstract: Rate of decomposition of H,,,O;,(V) At 150, and concentrations 0.00125
M H.SOt and 0-005 M N&,CrOo, cOnfO=z to thO 2ad order and does not
depend on initial concentration of H,,O.,. At 250 and constant initial
concentratioas of H.,O.Xand Na CrO , v increases in proportion to the
concentration of HACI and ae- i1i order of the reaction changes to
2nd order. At 5-150 & apparent energy of activation E = 31.0 kcal/
mole, at above 250 v does not depend on temperature and E - 0. On
the basis of kinetic data the authors had predicted, as intermediate
products of the reaction, peroxide compounds (different in the case
Card 1/2 -T-

---------------------- ~- ------ ------------------
Pqr i_~ o c, D t4 o V .14
L)
Category: USSR B 9
Abs Jour: Zh--Kh, No 3, 1957, 7526
Author: Bogdanov, G. A. , Berkengeym, T. 1. , and Sherbinin, V. A.
Inst Not given
Title Additional Materials on the Theory of the Joint Action of Cata-
lysts in Solution. I. Intermediate Products of the Decomposition
of H2 02 Catalyzed by Calcium and Molybdenum Salts
Orig Pub: Zh,. Fiz. Khimii, 1956, Vol 30, No 4, 889-895
Abstract: The gasometric method (G. A. Bogdanov, Zh. fiz. khimii, 1950,
Vol 24, 1450; 195 1, Vol 25, 323) has been applied to the investi-
gation of the homogeneous catalytic decomposition of 14ZOZ using
a mixture of CaC12 and Na2M004. The rate of decomposition vs.
H 07 concentration curve passes through a maximurn independently
2 ,
of the temperature and the H ion concentration. The shape of the
Card 1/2 MOSCOW A1)14)L,*'Ov1_ 8TeO- Al'i 0-- 1, 1,,,

Category: USSR B-9
Abs Jour: Zh--Kh, No 3, 1957, 7526
kinetic curves remains unchanged in the absence of CaCl2but
a sharp increase is observed in the reaction rates. The authors
explain the relationships observed by the formation of two inter-
mediate substances of varying peroxide oxygen content. Two
salts with the following compositions have been isolated from
the reaction mixture: Ca.Mo 20 13' 9H.0 and CaMoO8, nH.O.
Card : 2/2 -9-

P ~W~2 MUMM RAPROm-

Kir-p-Its -4~! j
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BOGDANOV, G. A., Cand Agr Sci. - (diss) "Effecti of trace elements
(cobalt, copperj and manganeae) upon growths development and meta-
l
boliam in calves of the Rod Steppe br
,;od.' Khar'kov, 19,r,8. 19 pp
(Min of Agriculture USSR, Khartkov Vet Inst)* 200 copies (KL, 15-58,
117)

~Country :
Cat%,ory :
Abs. Jour : RF~f Mw,' tol-7 "o 161 195,01 74046
Author - bogdanov, G. it.
7""6
Inatitut.
Title) The -r~fectl~voner~-sof Addittcr~uil Yicro-:Aemeat
ree-dillp of Calves.
ar I f6 Pub. ZhivodPov-odistvoj 10153) No 11 42-Irr"',
Abstract
Card:
Tibe live we-Ight of 3-month old younf~ bu-Ils of
the 2r,(: CTOU~ (addi',-ional J.'ceding with cobalt
chlor~dc-%I wai by 13.6 kg larger *and that of
C,
the 3rCI group (addi~,ional -L~c'--ding v-1tL- cobalt
chloride, coppev sulfnte, -ir-X --aarganqse S'tl-'L-
fvte) vmts bv 18.6 k- larger than in til-le con-
trol group at
the agc-. of 12 months the curreg-poridiav figuresi
rere ='d 51- ke'. At Vie -093-0f 3-~I- months
celvec of the 3rO gronp w~.-tlizad 12,79 'parceritl
more. of the nitrogen, rhich they took in, 15.641
1/2

Country : UISSR
CatcSory : Farm Animals, Q-2
Cattle.
Jibs, Jour : Ref Zhur-Biol., No V, 19589 74046
Author
Institut, t
Titlo
Or ii~ A.Iub.
Abstract percent ;aore of 0.1g~isted altrogen; at the age
of J.0-11 nonth!;., corresponOln-ly 6 14 nd r7,6
verc,c)nt more than contro'ls. AdViho~al feed'n~"I
with cobLlt ch"lorlde ar-gi-awited aduptEvtion of
~6's (by 2,10-1,90 Percent) and of P (by 4,93-
8,27 percent) Jurin..' lactation, as, well as pos
lactctioii Deriods, Durinr, the course o-f* the
entire -axperiment the complex of microelerjent
salts auoiiented tho iitllizatioi-i of Cle. (by 4,32
-6,43 per"cent).
card: 2/2

AUTHORS: Bogdanov, Go A.p Petrovaj Go Lo 76-32-4-2/43
TITLE: An Anomalous Case of Catalysis in the Liquid PhaseI( Anomalinyy
aluchay kataliza v zhidkoy fazeI)
PERIODICAL: Zhurnal Fizicheskoy Khimii, 1956, Vol. 32, Nr 4,
PP- 746 - 755 (USSR)
ABSTRACT: This paper treats the joint effect of sodium chromate with
nickeloulphate.on the catalytic process of the decomposition
of hydrogen peroxide in solution. As the experimental part
quoted shows, the determination was accomplished by means
of a volumetric method described earlier. The experiments
showed the catalytic velocity independant of the initial con-
centration of the hydrogen peroxide, while determination under
various temperatures and constant nickel sulphate content
showed that the catalytic effect of nickel sulphate rises with
the temperature. Determination of the effect of the concentra-
tion of nickel sulphate (0005 to 0-05M) at 150C led to the
conclusion that an increase of concentration caused only a
minor increase of reaction, that is only 1.2 times, so that the
Card 1/3 concentration is not in linear proportion to the velocity of

76-32-4-2/43
An Anomalous Case of Catalysis in the Liquid Phase
oatalysation. Investigation into the influence of the con-
centration of sodium-chromate on the velocity of catalysis
conducted for this reason yielded interesting and unexpected
results. The concentration of sodium chromate was changed
in an interval of O.ooo625 to 0-058o6 M at 25cC and it was
observed that the reaction velocity rises proportionally to
the square root of the catalyst concentration, reaching a maxi-
mum at oNa2CrO - O.oo25 M and then sharply declining to
CNa2Cro4 , O.o M, fromm where it rises again to a final maxi-
mum, so that the function has two maxima. Another interesting
observation showed that in a ratio of HiSO 4: Na2Cro4 an in-
crease of the quantity of nickel sulphate caused a decrease in
the catalytic properties of the nickel sulphate, while it rose
with an increase of the quantity of sodium chromate, reaching
Card 2/3 a maximal effect at cNi/o Cr '2 1. InvestiGation on theInfluence

An Anomalous Case of Catalysis in the Liquid Phase 76-32-4-2/43
of temperature on the velocity of reaction at c H+ a O.oo125 M1
Ocr 0-005 Mi cNi - 0.01 M, aR 202 a 0-15 M and temperatures
of 5 750C showed that the influence of te-mperature on the
velocity of reaction does not, in the ease presented, follow
van't Hoff's rule, the formula seems to be identical with
Ye. I. Shpitallskiylov which is, however, not applicable. Single
determination and a diagram of the change of activation energy
with the temperature showed that the activation energy de-
creases at first, pausing through a minimum at about 350C and
rising to a maximum at about 638C. It is indicated in conclu-
sion that the second report will cover the influence of
H'1- - ions, of electro-conduction properties and cryoseopy of
the solutions, as well as an examination of intermediate pro-
ducts of catalysis. There are 7 figures, 3 tables and 9 refer-
encessanof which are Soviet (including 1 tranalation)o
SUBMITTED: March 31, 1956
AVAILABLE: Library of Congress
Card 3/3 1. Sodium chromate--Cata3,vtic properties 2. Nickel sulfate--Catalytic
properties 3. Hydrogen peroxide--Decomposition 4. Hydrogen peroxidE
--Catalysis

AUTHORS: Bogdanov, 0. A., Petrova, G. L. SOV176-32-6-2146
'..W ... WWWAWWW
TITLE: An Anomalous Case of Catalysis In the Liquid Phase. II,
(Anomallnyy sluchay kataliza v zhidkoy faze. III
PERIODICAL: Zhurnal fizicheskoy khimiA, 1958, Vol. 32, Nr 6~ pp. 1205-121o
(U,;SR)
ABSTRACT: As a continuation of a previous paper, the influence~of hydro-
gen Ions on the velocity of catalysisp the electric con-
ductivity and the cryoscopio nature of solutions of catalysts
Na2CrO and NJ *!30 in the catalytic decomposition of hydro-
gen pe oxide iveri investigated. Special experiments were
concerned with the intermediate products. The investigations
of H+-ions was investitated at cone
of the influence OWra-
tionut0of sulfuric acid of from 6,25-10- to 50,00-11/1 mol/liter,
at 15 0 and ecr , 0,005, ONi' 0901~ 0 1190 2 =0917 mo iter.
It was found that at o H+< 0Cr the velocity 6f catalysis in-
creases as the concentration of the H+-ions, the kinetic
Card 1/3 curves corresponding to a reaction of first order. If cH +> 0Cr

An Anomalous Case of Catalysis in the Liquid Phase. II
SOV/76-32-6-2/46
t4e velocity of reaction decreases with an increase of the
H -concentration. The kinetic curves show a maximum. This
second type of reaction is considered to be due to the forma-
tion of perchromic acids. In connection with the experiments
by Ye. 1. Sh.pitallskiy tests with oallum chromate were con-
ducted by R. V. Xolobkovaq showing an analogy with sodium
chromate. The investigations of electric conductivity and of
the freezing point of the solutions conducted with a solu-
tion of Na Cr 0 NiSO and an addition of hydrogen peroxide
showed thai a~ 1he, addition of the substrate the electric,
conductivity drops sharply. This is explained by the forma-
tion of an active (unstable) and of an inactive (stable)
intermediate product. The process of complex formation and-
of decomposition, respectively, is divided into several macro
stages* Experiments with the freezing point showed that a
stabilization can be reached,for several days, according to
the complex modifications. The decrease of the freezing
0
temperature takes place only after heating to from 70-80
which fact substantiat as the effect of the complexes. It
may be seen from the experimental resu"te of the separation
Card 2/3 of the complexes of thr! int'ermediateI"~OT' ducts, that NiCrO
p 5

SOV/76-32-6-2/46
On Anomalous Case of Catalysis in the Liquid Phase. 11
is present.as an-individual substance and not as an incidental
mixture of NiOrO' and NiCrO 6 in the decomposition of the
latter. There art 3 figures and 6 references, which are
Soviet.
ASSOCIATIONt Moskovskiy aviatsionnyy tekhnologioheskiy institut
(Moscow Institute of Aviation Technology)
SUBMITTED: March 3, 1956
1. Hydrogen peroxide--Decomposition 2. Catalysis-Velocity
3. Catalysts--Performance 4. Hydrogen ions-Chemical effects
Card 3/3

AUTHORS': Shcherbinin, V. A., Bogdan.ov, G. A. sov/76-32-6-10/46
Aw"WAW
010t~
TITLM: -1
'Aipplementary I)F?ta Concerning the Theory of the Joint Action
of Catalysts in Solutions (.Dopo1nitel'nyye naterialy k teorii
sovme.4-tnogo deystviya katnlizatorov v- ra,741vore) TI.The Y'knetics
of the Cathlytic 'jsecompo--itiort cf H.-Arogen "i~roxide by the
Joint 4ctiovi of 1,1Erontium anti Molybdenum !halts (M. Einetika
kataliticheskogo rn:-1ozheniya perckivJ vodoroda sovrreptnym
deystviyom soley strontaiya i atollbd(7~nuN
PERIODICAL; Zhurnal fJzichei3kcy khiraii, 1958, Vol~ ~2~ N- 6, pp-!24~2-1261
(U-jou)
ABSTRACT: The influence of sodium moltdate and of strontium chloride
was Investigated In a neutral, an acid and an alkaline nedium
thp ~!I-ctric cont I ti-vity
.Yith a simultanceus mensurLment of dw:
of the solutions. Reference is made of the papers by A.
Shilov et al. fRef 2) and by L. j'%- Rikola-vev (Ref 3), The
kinetics of the nrccess vas. inveoti%ated -ccording to 'the
amount of oxygen stparating per unit time, On the strength
of the evidence obtained it is believed that in this case
of a true catalysis the theory of the formation of inter-
Card 1/4 mediates is valid. The shape of the kinetic curves leads to

SOV/76-32-6-lol/46
Supplementary Data Concerning the Theory of the Joint Action of Catalysts
in Solutions. 11. The Kinetics of the Catalytic Decomposition of Hydrogen
Peroxide by the Joint Action of Stront3um and Molybdenum Salts
the assumvtion that at least three intermediates are formed.
They determine the complex variation of the velocity of the
decomposition of hydrogen peroxide. The negative influence
of the strontium ions on the velocity (caused by eodil=
molybdate) is due to the difference of the kinetic and
thermodynamic properties of the intermediates, A study of the
funCti0n. Of the velocity of catalysis vercus the pH of the
medium showed that the presence of hydrcgen Ions reduce the
velocity of catalysis, and considerably change the character
of the curve. This is not the caDe in an alkaline and neutral
medium; the effect of the intermediates is explained in this
connection, With a temperature increase the minima and maxima
of the curve become more pronounced. It was observed that
the temDerature coefficient and the activation energy in an
acid medium show higher values than in a neutral medium. In
exoeriments serving for the investigation of the function of
tile velocity of catalysis versus the conditions of catalyst
Card 2/4 formation Dorotis stzontium chloride and sodium molybdate were

sov/76-32-6-lo/46
Supplementary Data Concerning the Theory of the_~oint Action of Catalysts
in Solutions. 11. The Xineti6s of the Catalytic Decom~position of Hydrogen
Peroxide by the Joint Action of Stronti"m and Molybdenum Salts
used on the one hand, and on the other hand finished strontium
molybdate was used* The investigations of electric conduc-
tivity showA that initially it decreases. Then it either
risesp or (deDendent upon the TI)H) remains constant. Alt the
end of the process it arops again. This can serve as a sub-
stantiation of-the assumption of the theory of intermediates
in homogeneous catalysis. There are 7 figuresq 1 table, and
4 references, which are Soviet.
ASSOCIATIONi Moskovskiy energetichaskiy institut
(Moscow Institute of Pol.~rer Vngineering)
SUBMITTV - January 12, 1957
Card 3/4

BOT/76-32-6-;lo/46
Supplementary Data Concerning the Theory of the Joint Action of Catalysts
in Solutions. :11. The Xinetics of the Catalytic Decomposition of'Hydrogen
Peroxide by the Joint Action of Strontium and Molybdenum Salts
1. Hydrogen Peroxide-Decomposition 2. Strontium chloride--Chemical effects
3. Molybdenum chlorides-Chemical, effects 4. Catalysts-Theory
Card 4/4 "0

AUTHORS: 0hcherbinin, V. A., Bogdunovp G. A. SOV/76-32-7-4/45
TITLE: Further Data on the Th4a~ Joint Action ot CatalyGtn
in Solution (Dopolnitellnyye materialy k teorii sovmentnogo
Oeystviya katalizatorov v rastvore).III. Strontium Purmolyb-
dates, Intermediate Productu in the Catalytic Decomposition
of H202 by Strontium and Moly bdonum Salts (III. 'Fermolibdaty
4trontsiya-promezhutochnyya produkty kataliza razlozheniya
if 202solyami stront.ciya i molibdena)
PERIODICAL: Zhurnal fizichoskoy khimii, 1958~ Vol. 329 Ur 7, PP-1466-1471
(USSR)
ABSTRACT: Three peroxide compounds were obtained by a direct synthesis
from the components representing the reaction mixture in
which the catalysis took-place. The substances were of
dark-cl xet -red and a yellow color. A fourth per-
a #ed, a brick
oxide which was obtained by the decomposition of the yellow
peroxide compound was also isolated. According to the rebulti
obtained from the analysis the first compound had the compo-.
sition SrMoO,-4H201 the necond the composition SrIl'oO 7' nH 20
Card 1/4 and the third the composition SrMoO 6-3H 20. The claret-red

C-OV/76-32"7-4/45
'i
Further Data on the Theory of the Joint Action of Catalysts in Solution.
III. Strontium Permolybdates, Intermediate Products in the Catalytic De-
composition of H 202 by Strontium and Molybdenum Salts
compound represents regular crystals of a hexaparallelo-
hedric form with a density of 3jO52-3)062, which is rather
stable at room temperature in the presence of humidity; on
a rise of temperature, in the presence of humidity and in
vacuum it converts into the yellow compound. The claret-red
peroxide is not soluble in some organic solvcnts, however,
it can wall be solved in water, For producing the substance
the yellow permolybdate is reacted with hydrogen peroxidet
by dissolving it in a 30 V,, 11 02-solution under cooling con-
ditio.,& The brick-red peroxi3e compound represents a fine
powder which dissolves well in water; it is unstable and
converts into the yellow compound. It can,also be obtained
from.the yellow permolybdate, however, with a 20-22 'If H 0 -
ow3 2
solution. The yellow permolybdate also represents a p er
with a density of 2,922-2,938, which is rather stable at
room temperature but dooomposes at higher temperature. It
is not well soluble in waterl the authors assume that a
Card 2/4 better soluble product SrMoO 5 is formed on this occasionp

SOV/76-32-7-4/45
Further Data on the Theory of the Joint Action of Catalysts in Solution.
III. Strontium Permolybdates, Intermediate Pre4ucts in the Catalytic De-
composition of R 202 by Strontium and MolybdemL Salts
which then converts-into the final decomposition product
SrkToO . The compound is obtained from a cooled 30 ~ H 20 -
solution with sodium molybdate and strontium chloride un3er
intense stirring. The experiments carried out for the in-
veotigation of the degree of the hydrolysis of.permolybdateE
showed that the hjdrolysis with the brick-red compound was
more thorough than with the two others. There are 5 tables.
ASSOCIATION: Moskovskiy energeticheskiy institut
(Moscow Institute of Power Engineering)
SUBMITTED: January 12, 1957
Card 3/4

i -- SOV/76-32-7-4/45
Further Data on the Theory of the Joint Action of Catalysts in Solution.
III. Strontium Fermolybdates, Intermediate Products in the Catalytic De-
composition of K 202 by Strontium and Molybdenum Salts
1. Catalysts--Chemioal reactions 2. Hydrogen peroxi:de--Decomposition .
3. Strontium-4hemical reactions 4. Molybdenum salts-ChendLeal reactions
Card 4/4

AUTHORS: Shcherbinint V. A., Bogdanov, G. A. SOV/76-32-9-2/46
TITLE: Further Material on the Theory of the Joint Effect of
Catalysts in Solution(Dopolnitellnyye materialy k teorii
sovmestnogo deystviya katalizatorov v rastvore) IV. The
Kinetics of Conversion of Strontium Permolybdates
(IV.Kinctika prevrashcheniy pormolibdatov strontsiya)
PERIODICAL: Zhurnal fizicheshoy khimii, 1958, Vol 32, Nr 9,
PP 1942 - 1950 (USSR)
ABSTRACT: The authors investigated the decomposition of strontium
permolybdates in aqueous solution and in the presence of
various amounts of hydrogen peroxide. The decomposition
was measured for 0,008 m. solutions of wine-red (Se.,100 8)
red (Sr1doO 7), and yellow (SrIT006) permolybdate at 150,
250, and 350 (Figs 1-3; curves 1,2, and 3); under the same
conditions but in the piwence of Na 2moo4 and SrCl 2 de-
composition curves were obtained in good agreement with
the first ones (Figs 1-3, curves 4,5, and 6); the sharp
Card 1/3 deviations in the curve for the yellow permolybdate (SrMQO 6)

Further Material on the Theory of the Joint
SOV/76-32-9-2/46
Effect of Catalysts in Solution. IV.-j!ne Ainetic~ oi~ Conversion of
Strontium Permolybdates
in figure 6 indicate that an intermediate compound, in
all probability SrMoO is being formed. The activation
energies for the deco2~osition of the wine-red and the
yellow permolybdates io given in figure 7. The conductivity
of the aquoo"s nolutions waa also determincd during
the oourse of the decompositions (Fig 8). The formation
of water and the decomposition were investigated using
a vacuum desiccator (Table). Besides the compounds already
mentioned, also calcium permolybdate (CaMo06)2 0,9 H2 0
was investigated. It was found that in the decomposition
intermediate compounds, SrMoO 6 and Sr1doO 5P ariset the
existence of which are hereby confirmed. The endproduct
is always SrV,1oO 4* The yellow permolybdates Sr1,ToO 61 CaMoOP
and SrMoO 5 are true peroxides, while the highly red-
colored permolybdates are considered to be Deroxyhydrates
of the yellow ones. There -are 8 figures, 1 table, and 8
Card 2/3 references, 8 of wihich are Soviet.

Further Material on the Theory of the Joint SOV/76-32-9-2/46
Effect of Catalysts in Solution. IV. The Kinetics
of Conversion of strontium Permolybdates
ASSOCIATION, Moskovskiy energeticheskiy institut (Moscow Institute of
Power Engineering)
SUBMITTED i January 12, 1957
Card 3/3

5(43
AUTHORS: Shcherbinin, V. A.,_,Lokjapov,'~ -10-6/39
-Okk 144 " SOV/76-32
"Wn" ut- , wft~
TITLE: Purther Material on the Theory of the Joint Action of Catalysts
in Solution (DopolnitelOnyye materialy k teorii sovmestnogo
deystviya katalizatorov v rastvore) V. Catalysis of the
Conversion of Hydrogen Peroxide by a Joint Action of Sodium
Molybdate and Cobalt Chloride (V. Kataliz prevrashcheniya
perekisi vodoroda sovmestnym deystviyem molibdata natriya i
khlorida kobaltta)
PERIODICAL: Zhurnal fizicheskoy khimii, 1958, Vol 32, Nr 10, pp 2256-2265
(USSR)
ABSTRACT: The catalytic properties of cobalt in solutions, a continuation
of the hitherto carried out investigations of the homogeneous
catalysis in solution, as well as the determination of peroxide
compounds that might be present contain cobalt were the objects
of the present investigations. A graph of the decomposition
rate of the peroxide caused by cobalt chloride in the presence
of caustic soda shows that cobalt chloride has in this case a
high catalytic activity, with the increase in the concentration
Card 1/3 of the lye (with a simultaneous concentration of the cobalt

SOV/76-32-10-6/39
Further Material on the Theory of the Joint Action of Catalysts in Solution
V. Catalysis of the Conversion of Hydrogen Peroxide by a Joint Action of
Sodium Molybdate and Cobalt Chloride
salt) leading to a marked increase of the reaction velocity
and a change of the reaction order. A joint action of sodium
molybdate and cobalt chloride showed that the latter considerably
increases the catalytic activity of the former, with a maximum
obtained at a ratio of CCc : CVo = 1 : 4 and 1 : 2. A maximum
in the concentration ratio of the catalysts points to the fact
that in the catalysis intermediate products are formed. The
catalysis is homogeneous only to a certain extent. The formation
of a deposit observed in an experimental series is explained by
the hydrolysis of the cobalt chloride and a subsequent oxidation.
The experiments on the influence of the pH on the velocity of
the catalysis showed that the hydroxyl ions are completely used
up whereas the H ions are regenerated. The latter react with
the catalytically active intermediate products and decrease
their activity, and thus transform the normal catalyst into a
less active acid salt. In the joint action of cobalt chloride
and sodium molybdate the process takes place at lower activation
energies due to the formation of the catalytically active inter-
Card 2/3 mediate products. The activation energies are lowest in acid

SOV/76-32-10-6/39
Further Material on.the Theoxy.of the Joint.Action of Catalysts in Solution
V. Catalysis of the Conversion of Hydrogen Peroxide by a Joint Action of
Sodium Molybdate and.Cobalt Chloride
medium, and highest in alkaline medium, An excess substrate
hampers the catalytic process, which fact may be explained by
an action of the peroxide on the.catalytic activity of the
intermediate compounds. There are 4 figures, 4 tables, and
2.-references, 2 6f which are Soviet.
ASSOCIATION: Moskovskiy energeticheskiy institut -(Mospow Institute of Power
Engineering)
SUBMITTED: April 17, 1957
Card 3/3

5W
AUTHORS: Petrova, G. L., Bogdanov, G. A. SCV/76-32-10-15/39
TITLE: The Activating Effect of Cobalt Sulfate on the Sodium Chromate
Catalysis of H202 (Aktiviruyushcheye vli,,-aniye sullfata kobalita
na kataliz H202 khromatami natriya)
PERIODICAL: Zhurnal, fizicheskoy khimii, 1958, Vol .7.?, Nr 10, pp 2324-2332
(USSR)
ABSTRACT: The investigations mentioned in the title were carried out in
acid media; some observations on the activating effect of iron
sulfate were made for purposes of comparison. The method of the
kinetic investigations had already been described (Refs 2,3).
The catalyst solutions were added to the reaction mixture one
after the other; first CoSO 4) and after the temperature balance
had been.obtained also Na2cro 4' In all experiment's 20 ml H 202
solution and 2 ml catalyst solution each were used. The follow-
ing experimental conditions were maintained: c H202 = o,16 m
Card 1/3 CH,30 0,00125 11, cCr ' 0,005 M, c 0,01 M (used as NiSO
4 4 ~ n ~ .4

SOV/76-32-10-15/30,
The Activating Effect of Cobalt Sulfate on the Sodium Chromate Catalysis of
H 202 ccc ~ 0,01 M. An especially strong activating effect of cobalt
salt was observed at 45 and 550. The iron salts showed an even
stronger effect on the decomposition of hydrogen peroxide. Thus,
the activating effect of the salts of the elements of the side
group of iron increases with the decrease of the ordinal number
within the Mendeloyev system. The course of the kinetic reaction
of the decomposition of hydrogen peroxide is almost independent
of the initial concentration of the substrate. Robertson (Ref 5)
found that the activation of the H 20 2 decomposition in potassium
bichromate by cobalt chloride is a logarithmic function of the
amount of cobalt chloride added. No direct proportionality
between the concentration of cobalt sulfate ana the catalytic
decomposition of H 202 could be found. A comparison of the
activating effect of nickel ions and cobalt ions showed that an
increase in concentration of the cobalt salt causes a higher
reaction velocity than the nickel salt. An increase in tempera-
ture in activation with the cobalt salt (in contrast to nickel
salt) causes an increase of the temperature coefficient and of
Card 2/3 the activation energy. The influence of the H+- ion concentration

SOV/76-32-10-15/39
The Activating Effect of Cobalt Sulfate on the Sodium Chromate Catalysis of
H202
on the process must be observed at cH+~ 'Cr and CH+ >cCr-
In the former case an approximately direct proportionality
between the reaction velocity and the acid concentration may be
found. At cH+> cCr the velocity of the catalysis decreases with
the increase in the H+-ion concentration. The catalysis of 1 20 2
with Na chromate as well as nickel sulfate does not obey the
van't Hoff law (Vant-Goff) (Refs 2.3), which.fact was also
observed with cobalt sulfate at t.emperatures of Ir and 250. The
formation of intermediate complex compounds of chromium and
cobalt was proved by the method by Knorre-Illinsk-iy (Ref 7).
There.are 6 figures, 2 tables, and 7-references, 6 of which
are Sovieta
SUBMITTED: 'may 8, 1957
Card 3/ 3

5W
AUTHORS: Shcherbinin, V. A., Bogdanov, G. Av SOV/76-32-11-7/32
TITLE: Joint Action of Catalysts in Solution (sovmestuoye deyetviye
katalizatorov v rastvore) VI. Investigation of the Electric
Conductivity of Solutions During the Catal4tic Decomposition
Process of-Hydrogen Peroxide Under the Influence of Sodium
Molybd4te and Cobalt Chloride M. Issiedovaniye elektr*o-
provodnosti rastvorov v protsesse kataliticheskogo razlozheniya
perekiii--vodoroda pod-vldyaaiyem molibdata natriya i khlorida
koball-ta)
PERIODICAL: Zhurnal fizicheskoy.kh1-ii,, 1958, Yol 32, Nr_~1.1,.pp 2507-2513-
(USSR)
ABSTRACT: -The investiga-b-ions mentioned-in the title were carried out at
the same time with a study of the kinetics of the catalysis
in neutral and acid solutions. The expe-riments, were carried
cut at 250 and with c co `Mo = 0.002 gram,ion, c H 0 = 0.16
2 2
mole. The addition of H 202 to neutral sodium molybdate and
Card 1/3 cobalt chloride solutions leads to a relatively rapid formatior

SOV/76-32-11-7/32
Joint Action of Catalysts in Solution, VI. Investigation of the Electric
Conductivity of Solutions During the Catalytic Decomposition Process of
Hydrogen Peroxide Under the Influenee of Sodium Molybdate and Cobalt Chloride
of poroxide compounds that are apparently carriers as the
electric conductivity of.the solution considerably decreases.
During the process of catalysis the electric conductivity
remains constant all the time, then'it abruptly increases
(complete decomposition of E 202) but does not reach the
initial value. The increase of the-electric conductivity at
-the -and of the -reaction reaches. a higher -value in acid.
solutions-than in alkaline solutions. Two factors exert an
influence on this stage-...a) The regeueration-of the R+ ions
of the:-peroxy c.caapl&.x_campoun&s_.forme&.aE
(by the decomposition
intermedi,at-e-produats , b) The. acid, conaiderab-ly-hindars the
)
formation of cobalt oxides. At pH-> 7 the electric conductivit3
depends only to a small epent on the OH- ion-concentration
(ak/8o OH M 0). It is assumed that first sodium permolybdates
-aTe formed from the sodium molybdate.and hydrogen.peroxide.
These permolybdates then react in an exchange reaction with
cobalt chloride and are transformed into cobalt molybdate. The
Card 2/3 concept of the role played by the OH- and H+ ions in the

SOV/7 -32-11-7
Joint Action of Catalysts in Solution. VI. Investigation of the Electric
Conductivity of Solutions During the Catalytic Decomposition Process of
Hydrogen Peroxide Under the Influence of Sodium Mo.lybdate and Cobalt Chloride
catalysis-as given on the basis of the data from the reaction
kinetics (Ref 1) is proved:-The OR7 ions irreversibly and the
H+ ions reversibly take part in the formation of the inter-
mediate products of the catalysis. An abnormally big increase
of the electric conductivity of solutions with.a concentration
of CH2so4 > 0.001 M was observed on..the addition of hydrogen
peroxide* There are 4 figures and 5 Soviet ref9rences.
ASSOCIATION: Moskovskiy energeticheskiy.institut (Moscow Institute of Power
Engineering)
SUBMITTED: April 17, 1957
Card 3/3

5M
AUTHORS: Shcherbinin, V. A.,. Bo lanov, G. A L_~ sov/76-32-12-102
TITLE: The Joint A~tion of Catalysts in Solution (Sovmestnoye deyst-
viye katalizatorov v rastvore) VII. Cobalt Peroxides as
Intermediate Products in the Catalytic Dissociation of
Hydrogen Peroxide by Sodium Molybdate and Cobalt Chloride
(VII. Perekisnyye soyedineniya kobal'ta - promezhutochnyye
produkty kataliza razlozheniya perekini vodoroda deystviyem
molibdata natriya i khlorida kobal'ta)
PERIODICAL: Zhurnal fizicheskoy khimii, 1958, Vol 32, Nr 12,
pp 2761 - 2766 (USSR)
ABSTRACT: Black cobalt permolybdate was produced the effect of which
on hydrogen peroxide is analogous, according-to the kinetic
curve, to that of sodium molybdate and cobalt chloride.
Because of the instability of the permolybdate it could only
be produced at temperatures between -400 and -450 C. The
permolybdate is a colloid, showing the Tyndall-effect and
coagulating if bases or potassium chloride are added. Accord-
ing to the varying cobalt content of the compound these are
Card 1/2 closely related compounds which pans over into one another

The Joint Action of Catalyate in Solution. VII. Cobalt SOV/76-32-12-16/32
Peroxides as Intermediate Products in the Catalytic Dissociation of Hydro-
gen Peroxide by Sodium Uolybdate and Cobalt Chloride
through intermediate products. The production of cobalt
peroxide was also carried out at low temperatures (~250
to -350 C), resulting in a green CoO 2 compound with
bivalent cobalt being icomeric with the black cobalt
dioxide Co02 (with tetravalent cobalt). Tho researchers
of N. N. . Semenov's school: V. V. Voyevodskiy, N. N.
Emanuellpand N. I. Kobozev advocated the theory that the
intermediate p7oducts result in chain reactions. There
are 3 tables an." 3 referencesp 2 of which are Soviet.
ASSOCIATION: Moskovskiy energeticheskiy institut (Moscow Power-
Engineering Institute)
SUBMITTED: April 17, 1957
Card 2/2

5(2) SOY/156-59-2-11/48
AUTHORS: Bogdanov, G, A., Prokhorova, I. K.
TITLE: The Homogeneous Catalysis of H 202 Caused by the Salts
and New Strontium Pertungstates (Gomogennyy
WO
+ SrCl
Na.
2
2
4
+ SrCl 2 1 novyye pervollframaty
iataliz H
0
solyami Na2WO
2
2
4
strontsiya)
PERIODICAL: Nauchny ye doklady vysshey shkoly. Khimiya i khimicheskaya
tekhnologiya, 1959P Nr 2f pp 264-267 (USSR)
ABSTRACT: The catalyeia mentioned in the title is reversible and homo-
geneous. The curves of figure 1 show the effect of the stron-
tium ion upon the deoomposition of hydrogen peroxide: 1) The
addition of SrCl 2 reduces the velocity with increasing con-
centration of Sr2+-ions; 2) in the case of increasing con-
centration of SrCl 2 the maximum of the curves becomes flatter.
Herefrom the conclusion is drawn that in the course of Cats-
lyais intermediate products fDrm, i.e. strontium pertungstates
of different composition. The activation energy E and the
temperature coefficient y were not constant in neutral medium
but were dependent on the concentration and temperature:
Card 1/2 dE/do - dj/dc 1, 0 and dE/dT - dy/dT < 0. In acid mediump

SOV./156-59-2-11/48
The Homogeneous Catalysis of H 202 Caused by the Salts Na 2W04 + SrCl2 and
New Strontium Pertungstates
however, dE/do = dy/de - 0. The electric conductivity was
measured in alkaline, acid and neutral medium (Pig 27 Table 1).
Also from these measurements it was possible to draw conclu-
sions to the formation of intermediate compounds. The latter
were also found in isolated state and as strontium pertungstates
of different oomposition: SrWO 6'3H20' SrW06 .2H20' SrWO8-3H2oP
SrWO8 .2H20. They decompose readily under separation of oxygen.
Their heats of decomposition and the specifio weights (Table 2)
were determined for the purpose of proving their individualism.
There are 2 figures, 2 tables, and 4 Soviet references.
?WSENM BYt Kafedra obehohe i neorganicheskoy khimii Moskovskogo tekstill-
nogo instituta ~Chair of General and inorganic Chemistry,
Moscow Textile Institute)
SUBMITTED: June 20, 1958
Card 2/2

5(2) SOI/78-4-2-4/40
AUTHORS: ''Shcherbinin,.Vo A.g.Bogdanov, G. A.
TITLE: The Permolybdates of Strontium,- Calcium, and. Cobalt
(Permolibd.aty strentdyaq kalltsiya i kobal'ta)
PERIODICAL. Zhurnal neorE;anichaskoy khimii, 1959,.Vol 4, Nr 2j
pp 260-271 (USSR)
ABSTACT,.- New permolybdates of strontiump calciumg and cobalt were
produced-and their composition, solubility, transformation
mechanism'in water,,-and the electric conductivity of their
aqueous solutions were investigated..,Four permolybdates of
strontium were producedz SrMoO864H 20 (Vordeaux-red),
SrMoO (red), SrMo .3H20 (yellow), and SrMoO nH 20
7'4H20 06 5*
(Oream-_cOlored)~ Thesyntheses of these compounds are de-
scribed.in detail. The examination'of the properties showed
that only SrMoO 6 and SrMoO5 are real peroxideev whereas the
coMpoUudB,SrMoO,,*4H 0 and SrMoO 0 are perhydrates of
2 1 7*4H2
these real peroxides. The pqrhydree forms are as follows:
Card1 1/3 SrMo06. 2H20*2H202 and SrMo06'H 20 2' 3H20. The transformation

SOY/78-4-2-4/40
The Parmolybdates..of Strontium# Calciumi and Cobalt
velocity of the permolybdates in water and the electric
conductivity of the respective solutions were investigated.
The electric conductivity of yellow permolybdate shows a
,sudden increaa6 at the-beginning of the process, reaches a
maximum, and,finally decreases. The electric conductivity
of red and bordeaux-red permolybdate is constant at the
beginning, increase"s some time later, reaches a maximum and
then decreases. The dehydration of strontium permolybdates
by.phosphorous pentoxide at 190 and 200 was investi-ated-
the results are shown in the !,igures 2, 3, and 4. The calcium
permolybdAtes (CaMoO 6)2 0.9H20 and GaMoO 8* nH 20 were also
produced..The compound (Camoo 6)2 0.9H20 is insoluble in organic
solvents but easily soluble.in water. The red permolybdate
CaMoO,.nH 20 is a finely crystalline powder, soluble in water
and several organic solvents. At room temperature the-com-
pound turnsinto yellow permolybdate (Camoo 6)20'9H20 while
oxygen becomes free. Red calcium permolybdate was used for
Card 2/3 the production of yellow permolybdate. CaMoO 6 is the real

SOV/78-4-2-4/40
The Permolybdatea of Strontium, Calaiumt and Cobalt
peroicidet the crystalline product (CaMoo 6)2 O.9H20 is the
perhydrato.'of.~l,iiia'oompound. The corr6ot formula is
(CaM006-4H2O)2*H.O2 * The cobalt permolybdatee to2(XO06)3
and C02(XQ0 021 and cobalt peroxide were produced and their
properties described. In cobalt parmolybdates cobalt is tri
and tstravalent. This.valency change of cobalt in6reases the
difficulty of colorimetria determinations, The permolybdates
of cobalt are unstable at-room temperaturep practically in-
soluble in aestonep.ether, and earbon tetrachlorider, easily
soluble and decomposable in water, while oxygen is separated.
The solutions are'oolloidal and, on the effect of potassium
chloridey~alkali or direct ourrentp coagulable. Cobalt per-
oxideCoo 2 is'a green powder whichp on heatingy turns black
while. oxygen is separated. There are 5 figures, 4 tables,
'and 14.ref6ranoes, 7 of which are Soviet,
ASSOCIATION: Moskovski;y energeticheskiy institut (Moscow Power Engineering
Institute)
SUBMITTED: November 22, 1957
Card 3/3

5(2) sov/63-4-3-29/31
ALTMORS - Proldhorova, I.K., Bogdanov, G.A.
----------------------
'TITLE: The Homogeneous Catalysis of H202 by the Salts Na2~ 04 71- SrC12
PERIODICAL: Khimicheskaya nauka i promyshlennostl, 1959, Vol 4, Nr 3,
pp 413-414 (USSR)
ABST-RACF2:-- It, has been shown that SrC12 does not catalyze the decomposition pro-
cess of H202* whereas N~~N decomposes hydrogen peroxide. The ad-
dition of SFCl2 to NaL W04 decreases the reaction rate considerably.
The-reaction rate is Krectly proportional to the concentration of
OH-.ions. In the temperature interval of 25 - 450C.the-reaction rate
changes appreciably which is explained by the formation of intermediate
products. The relative concentration of the intermediate peroxide pro-
ducts is a function of the substrate and the temperature. The change
of electric conductivity as well as the rate of catalysis is determined
by the intermediate complexes. For ixplaining all phenomena, it is
necessary-to assume the formation of at least 3 complexes.
Card 1/2 There are 5 Soviet references'.

,The Homogeneous Catalysis of H202 by the Salto Na 2W04 SrC12 sov/63-4-3-29/31
I ASSOCIATION::, Moskovskiy tekstilinyy institut (Moscow Textile Institute)
Suplarnm I November 3, 1958
Card 2/2

BOGDANOV, &oA.; XOROTCHENKO, N.A.
Calcium peroxytungstates. Part 1. Zhur.ob.khim. 31 no.9:2812-2817
s 61. . (MIRA 14: 9)
1. 14oskovskiy tekstilInyy institut.
(Calcium tungstate)

BOODANOV, G.A.; KOROTCHEUKO, N.A.
..............
Calcium peroxytungstates. Part 2. Zhur.ob.khim. 31 na.9:2817-2823
s 61. (MIRA 14: 9)
1. Moskovskiy tekstillnyy institut.
(Calciur. tungstate)
s

,BOGDANOV G.A.; KOROTCHENKO, N.A. (Moskva)
datalytic decomposition of H 0 imder the effect of Ni (CH)2
Zhur. fiz. khim. 35 uo.7:161'f~f.621 J'l 161. (MIRA 14.-'7)
(Hydrogen peroxide) (Nickel hydroxide)
M

BOGDANOV, G.A.; PE7ROVA, G.L.1 MINAYEV, A.I. (Moskva)
CalciuD perozychromates and the machaniom of the catalytic
decomposition of H202 by chromateo. Zhur,fiz.khim. 35 no. 8:173.6-
1717 Ag 161. (MM 14:8)
L Moskovskiy goeudaretvennyy univorsitet imeni M.V, Lomonooova
i Moskovskiy tekstilInyy institut.,
(Caloium chromate)
(Hydrogen peroxide)

PROKHOROVA, ~G.A.~Moscow)
Strontium pertungstates. Part 1. Zhur.fiz.khim. 35 no.10:2177-
2181 0 161. (HIRA 14:11)
(Strontium tungstate)

BOGDANGVt-G.A.; PROKHCF-ROVA, I.K.
Kinetics of decomposition of peroxo salts in solution. Zhur.
fiz. khim. 36 no.9tl932-1937 S 162. (MIRA l7t6)
1. Tekstilfnyy institut, Moskva.

SAVINA, M.V.; BOGDANOV, G.A.; PM.,,)VA, C.L.; YURCIIENKO, G.K. (Moscow)
g a' whalaw-w
Catalytic decomposition of H2Q_) under the combined action of
sodium molybdate and salts of the zinn -qubgroup. Part 1.
Zhur. fiz. khim. 37 no.4:746-752 Ap 10. (MIRA 17:7)
1, Moskovskiy tekstilinyy institut.

~ACCESSION 'NR; AP4044742 S/0153/64/007/003/006/0410
AUTHMI, S: Bogdanov , G.A.,* Semenoia, B. G.; Cherny*rhev, A. S.
'TITL'E: Catalytic decomposition of hydrogen peroxide in the presence
of NiSO 4 and Na3~_1004
.SOURCE: IVUZ. Khimlya i khimicheskaya tekhnologiya, v. 7, no.
1964, 406-410
'POPIC TAGS: hydr__& lde2latalytic decomrosition, reacition
ro ezll
_ p~t~
kin,-_-tics, energy of activation, entropy
conEtanf. nickel peroxomolybdate, synthesis, nicrkeL aulfa~,e cantairl-
ing catalyst,, sodium molybdate containinv, c.=_~t q, sl~
-Z
of t-_
ABSIRACT- Thek.kinetics were studied
0" F~'02 in neutral and acid soluticns
6-1tw,dtaneously resent. The reaction ,ias first-L 0rder, irnd4endent
of temperature T15-55C) or acidity of the solution (energy of
activation = 14.4-14.9 kcal/mol, alnost independent of a al-
tho he catalytic process
',~gh increased acidity retarded t amew t).
Clar 11Z.

Z16187-65
ACUSSION. NR: AP4044742:..
-the ature -o t e intermediate produrt.,; was the sa-me
r-gardless of temperature and pH. The entrouv of activation and the
equilibriumi constant of the intervrediate com~iex was calculated; the
decomposition of the latter was a monomolecular procens. If the
coitcentration of the NISO4 was much greater than that of the Na2Mo04
the order of the reaction was higter, apprDachi--g 3,~cc-nd of-dar. The
nic-kel ions can either accelerate (at the start of the reaction) the
action of the Na.)4oO,. or retard it (as the H 0 concentration de-
2
creased). it wa~ as'Alumed that nickel perof
as inter-mediate products. For confirmation, tl,.~
Ni.Mooz.nfl 0 and the unstable NJ14oC, nE 0 NUL'r-
we r e, 9 L
mt es,ze~'. Orig. art. has: i f1gure anc.
ASSOCIATIO14: Moskovskiy tekstillnyl:y institut, Kafedra obshchey i
peorganicheakoy khimil (Mo,5cow Textile jn,~titute. De-
______partment of General a~.id inorganic Cherliqti7~1',
,I K -
SUUCTITED: 02Ju.Loz ENCL: 00
SUB CCDE: 1C, GG N11 IMF SOV : 007 OTHER: GOO
Cant 2/2.

7-
ACCESSION NFL: AP5008914
AVMR: B~o ~da ~q _Kolobkova, R. V.; Petrova, G. L.
TITLE: Catalytic decompp6ition' of hydrogen peroxide' ~y sodiu-m tunzstate tccnther
with the salts of elements ofthe zinc 6ubgroup
SOURCE: Zhut-nal fizicheskoy khimli, v. 39, no.
TOPIC TAGS: hydrogen p*roxida, sodium tungstate, zinc sulfate. cadn-lLu-i
Mel-cul ~~( Ciitratc, peroxide decompositio-., ri~jox
A PBS T R.~ 'Ihe article describes the resz;lts cill th~
i. peruxi~je in ioluLiorl in the preser-ce of
6; c,? e
r ',,;.-~WO, +-ZnSC,,; Na2W04 +- CdS04 Na;WCI~
r,t- :t:)ds an-- e~ectrlca'l conduc~~v-.'V
compof 1Lon 01 h2l-j- by sodium tungstate is app rec I a-!
ar,6 Hi ions, The rate constaots were czlcula,,ed fc-:
the c, talytic reaction. Curves of redox ?( tentiair
which Indicate the formation of no less thin, three
in ag; eement with the kinetic data and
invo 1., ing i1g' or H92 dical-cha:.n procesbe~- A.
ions, ra
C.,d 1~ 2

L 4.1690-65
AMISSIOR NR: AP5008914
takt; place, and intermediate compounds are formed. Orig. art. has: 5 figures,
1 ti,ble and 7 formulas.
ASSOCiAnON: Moskovekiy tekatil'nyy institut (Kdsccrw Textile institutel_
SUMUTMD: I4Feb64 ENCL: 00 SUB CCVX: IC
NO IW ~Ov; 009 07M.- 002
OD
Cori _2/2

L 9737-66 3a(X)/NF(t.)/kWT(b) IJP(c) JD1JG
ACC NR: APS027169 SOURCE CODE- UR/0076/65/039/010/2359/2364
AUTHOR: Turcbenko, G.K. Nuzenko, L. A.
ORG: Moscow Textile Institute (Moskovs1dy tekstIl1nyY Institut)
TITLE: Study of sodium peroxooxyvanadates
SOURCE- Zhurnal fizichoskoy khimfl, Y. 39, no. 10, 1965, 2359-2374
TOPIC TAGS: vanadate', peroxide, vanadium .compound
f
ABSTRACT: The met6s of preparation of sodium peroxooxyvanadates, Which are Inter-
mediates In the catalysis of.hydrogen peroxide by sodium vanadate, were -elaborated, and
the compounds were Isolated. Their composition,was determined to be NaV04, NaV04-
HP2, and NaV04- 3HP ; the latter two have, not been described before. NaV04 Is a true
peroxide with a fairly s~%re inner coordination apbere. The decompositioa of sbdlum mon- 1
oporoxovanadate in solution is bomegeneousand occur's via an inner-sphere recombination
without being accompanied by radical-ebain lirocesses. The dependence of the decompositiod
rate on the concentration obeys an equation Mat Is close to first-order. The molar con-
ductance of aqueous NaVIO solutions changes anomalously with dilution; 0stwald's and
4
UDC 541.128 + 541.124/.128
Card 1/2

WGDASOVO G.A.) n-RCHENY-Op G.K.-, MUNK09 L.A. (Pcetow)
Thf-'Ory of OAtftlysla In solutions Part 1. /'bvr,, fiz, khl'm. '18
no.5il.229-1231, Xy. 164, On's 18,12)

13-23,64
-,,~,djjjm pera. L.1 O-Z 39
jF-IM, 181~2)
~luLqr-jttod April 4,,
.or

4_`Y14-00- - WTkd,'/M'1Am/'/M'rknJ
ACC NRi AP6005512 (A) SOURCE CODE: UR/0256/661000/001/0043/0047
AWHOR: Bogdanov, G. A. (Major)
ORG: none
TITLX: Target interception at low altitudes
SOURCE: Vestnik protivovozdushnoy oborony, no. 1, 1966, 43-47
TOPIC TAGS: pilot training, target discrimination, target seeker, jet fighter air-
craft 191trooener
ABSTRACT: The problem of training iet interceptor pilots tq,~-p6rform more effectively
at low altitudes is discussed. The author stresses t-he neq4'.:fbr pilots to have a
sound knowledge of the fuel consumption rate at low altit#,deil,the effects of the high
er air density on pilot and aircraft, the problem of spot's t'r-agets while maintain-
ing safe altitude and speed$ and the problem of distinguishing true targets on the
aircraft radar screen. Possible disruption of air-groundo",air-air radar coamunication
is also discussed. Orig. art. has: 2 photographs.
SUB CODE: 01,15/ SUBM DATE: none
af

UVAROV, I.P.; PARSHUTKIN, Yu.A.; BALASHOV, N.N.; BDGD&NOv,,_~q,A.; -MMDZGIN, B.S.;
NEMCHENKO, A.G.; YUDIGNICH, Yu.D.j KIFRIANOf,'_LI.
Vapor-PhAdf pyrolysis of wood-tar oils. Gidroliz. i lesokhim.
prom. 14 *80-6 161. (MMA 16:32)
1. TSentrallnyy nauchno-issladovatellskiy lesokhimicheskiy institut
(for Uvarov, Parshutkin, Balashov, Bogdanov). 2. Voe-Boyuznyy
nauchno-iseledovatellskiy institut po pererabotke i ispoll-
zovaniyu topliva (for Bezmozgin,,'IIemohenko, Yudkevich).
3. Leningradskaya lesotekhnicheskaya akademiya im. S.M. Kiravei
(for Kiprianov).

ROGDANOV. G.B. [Bohdanov,, H.B.) (Kiyev); SMETSKIV, 3.10 [Senetalkyi,
T-7-7(Kiyev)
Gas discharge counter in an impulse magnetron. Avtomatyka 8
no.6:78-80 163. (MIRA 17:8)

BOGDANOV, G.A.; ZIMINA, V.V.
Automatic weight proportioning equipment. Ogneupory 30 no.3.*15-36
'65. OMIRA 18--5)
1. Boravicbskiy konbinat ogn6uporov*

BOGDANOV, G. B.
Cand Tech Sci - (diss) "Study of the properties of ferrites as
thermoreSiBtOrS." Kievq 1961. 13 pp; (Ministry of Higher and
Secondary Specialist Education Ukrainian SSR, Kiev Order of Lenin
Polytechnic Inst); number of copies not given; price not given;
(KLI 7-61 sup, 232)

229o6
s/ioq/6i/oo6/oo4/O21/O25
+Z310 629,0Y) n4o/n63
AUTHORs Bogdanovt G.B.
TITLE: The possibility of employing fer~ites for the absolute
measurement of microwave power
PERIODICAL: Radiotekhnika i elektronika, Vol.6, No.4, 1961,
pp. 663-667
TEXT: The purpose of this note is to determine the properties
of manganese ferrite an a ferromagnetic semiconductor thermistor
for the absolute measurement of microwave power in well-known
bridge circuits. The basis of this proposal is the dependence of
ferrite electrical resistance on temperature and the strong
heating (above 100 OC) of a ferrite sample through absorption of
microwave power at ferromagnetic resonance# in principle the
difference between the ferromagnetic semiconductor thermistor and
the ordinary semiconductor thermistor is that the former interacts
almost exclusively with the magnetic microwave field, while the
latter, with the electric field. The advantages of the ferrite
are that electrical breakdown between particles cannot take place
in the interior of the sample and, with suitable installation,
Card 1/2

22906
s/iog/61/oo6/004/021/025
El4o/E163
The possibility of employing ferrites for the absolute measurement
of microwave power
the ferrite does not reduce the electrical stability of the
microwave system. The use of a magnetic bias field permits wide
variation of the power level measured. Finally, the fact that
with increased temperature the Curie point is approached, makes
the ferrite "self-protecting". Acknowledgements are expressed
to Ya.A. Monosov and V.I. Pronenko for discussion of the paper.
There are 4 figures and 4 Soviet references.
SUBMITTED: September 29, 196o
Card 2/2

3 7h 09
S/142/62/005/001/002/012
E192/E382
AUTHORS: Bokrinskaya, A.A. and
TITLE: Ferrite thermoresistors (dynainic characteristics)
PERIODICAL: Izvestiya vysshikh uchebnykh zavedeniy,
Radiotoldinika, v. 5, no. 1, 1962, 26 - 36
TEXT: The characteristics of non-magnetized ferrite
temperature-dependent resistors (FTR) are investigated by using
the earlier motl-iod proposed for thermistors (Ref. 2
A.A. Bohrinskaya - Dinamicheskiye kharakteristiki termistorov
(Dynamic chliracteristics of thermistors) pub. by Kiyev Order of
Lenin Polytechnical Institute, 1956, 21). First, the static
charactGristics are given and an exaniple of such a characteristic
is shown in Fig. 1. This gives the resistance of various types
of FTR as a function of temperature 0% - The first three curves
refer to manganese ferrites, while curves 4 and 5 are for
Mg-Mn materials. With regard to the dynamic operation of FTR,
this refers primarily to their work in AC circuits, where the
principal characteristic of the ferrite is its resistance-
temperature dependence, Ri =VZ(a). The thermal balance in a
Card 1/#

S/142/62/005/001/002/012
Ferrite thermoresistors B192/B382
FTR can be described by:
d
C - + H G = R (t) (1)
dt
where C and H represent the differential thermal capacitance
and the differential dissipation constant of the resistor, while
0- = 8 00 where kt_4:-0is the temperature of.the surrounding
meditwi and is the temperature difference on the FTR. The
equation is analyzed under the assumption that the resistor
operates under conditions such that the load is much greater
than R;~ secondly, the temperature of th'e resistor is
uniform and C and H are independent of temperature. It is
also assumed, that the resistance
as a function of temperature is in the form
R(19) = A/&11 where n > 0 and A is a constant. Eq. (1)
Card 2/5