SCIENTIFIC ABSTRACT VLASOV, V.A. - VLASOV, V.G.

• Document Type: CREST
• Collection: Scientific Abstracts
• Document Number (FOIA) /ESDN (CREST): CIA-RDP86-00513R001860310009-3
• Release Decision: RIF
• Original Classification: S
• Document Page Count: 100
• Document Creation Date: November 2, 2016
• Document Release Date: September 1, 2001
• Sequence Number: 9
• Publication Date: December 31, 1967
• Content Type: SCIENTIFIC ABSTRACT


RODYAKIN, IT.V.~ GARMATA, V.A.; SOFOLON, I.!.; SANDLM,,, R.A.; ARUTYUNIOV, F.A.;
; UST Tk V~S,;
- K4,50M, - IOV, UKDREYEV, A.Ye.
Quality of titanium sponge obtained with the use of various
formn of magnesium. TSvet. met. )8 no.8:64-61 Ag ,65.
(Z,ITFA 18:9)

P,, KulC I I, G; 'A ~~ it I ~ ',I A. ; Y' iN~ I Ev , A. i". ; P., LIF C I ILI K , N', "' . ; KOC IIN, ;: I - -
C, '. , j , I It 1 .- '.. .
TUUNKOV, I.P..; SHAllAl'OV, S.F. ; VOLKOVA I V.S. ; ROGALIS, Yu.,",:
llu-S911_1~- A-..,- ...
Directiono for the techniol improvement of the elactrolyqln
of zinc. TSvet. met. 38 nc.5:22-25 t~V 165. (MIRA 18:6)

VLASOTy-V.A~; ZYSIN, Yu.A.; KIRIN, I.S.; LBOVI A.A.; OSEYAYEVA,
L.I.; SELICHEMKOV, L.I.
(Yield of certain fragments in T032 Sisai-on by :14.3 Mev.
neutrons] Vykhody nekotorykh oskalkov pri delenii Th232
neitronami s energiei ll+,3 mev. Moskva, Glav. upr. po is-
pollzovaniiu atomnoi energii pri Sovete Ministrov SSSR,
1960. 11 p. (MIRA 17:4)

SEKILETOV) S.A.; VLASOV, V.A-
Electron diffraction study of phases in the system gallium -
. Kristallograftis. 8 no.6:877-883 N-D,63-
tellurium (MIRA 17:2)
1. Institut kristallografii AN SSSR i Institut fiziki i matematiki
AN Moldavskoy SSR.

Y;4ppy, Viktor Alekseyevich; YUKHNOVSKMA, S.I., red.; PETROVA,
~ 1.N.. .- K.,,-' te:khn. r- ed'.
(Gastrointestinal diseases in young children] Zhejudochno-
kishechnye zabolevaniia u detei rannego vozrasta. Moskva,
Medgiz, 1963. 18 P. (MIRA 17:4)
-,K-

VLASOV, V.A.; VOYEVODIN, Ye.N.; LBOVI A.A.; IIARTYNOVI N.P.; NIKITIN, ie.A.1
UTENKOV, G.G.
Possibility of maintaining low moisture A glove boxes. Zav-lab.
29 no.~.*"586-588 163. (MIRA 16-5)
(Rubber--Permeability)

VLASOV, V.A., prof.
History of the origin of pediatric journals in the U.S.S.R.
Pediatriia la no.4:3-8 Ify 162. (MIRA 15:5)
(prDIATRICS-'PERIODICAIS)

MOROZOV, N.N., J.nzh.; FOWPIUCkRA, A.I., Inzh.; 11OVINOV, A~11.,
inzh.; OV~V.D.; inzh.; TA.R.IVIENIXG, N.A.p red.
[Mfuiual on safety unginearing, industrial lWgiene, lubcr
protection, and fire prevention on state atO. collective
farms] Spravochnik inzhenera po tekhnike bezopasnosti,
proizvodstvennol canitarit, okhrane truda i poz1harnoi okh-
rane sovk-hoza i kolkhoza. Mosk-va, Rossellkhozizdat, 1965.
288 p. (MIRA 18,10)

VIASOV,V.D., in~.hener
ftzwtrl~~
Group switchgear vith
1 no.4:22-23 Ag '55.
automatic adjusters. Svetotekhnika
(MISA 8:9)
1. Tyazhpromelektroproyekt
(Electric switchgear)

VLAWY, V.D., Inshener.
Reingorced concrete poles for electric networks and street
lighting. Svetotakhnika, 2 no-1:25-26 ja 156. (MLRA 9:3)
1. Tyashpromelektroproyakt.
(Blectric lines--Poles) (�treet lighting)
*k.

GOIRSKIY, Lev Ivanovich- VUSOV, V.D., retsenzent; XWORRING, G.M., red.;
SWOLEVA, Ye.M*
(Electric apparatus and appliances
Elektrokonstruktaii promyshlennykh
energ.izd-vo, 1959. 255 P.
(Electric apparatus
in industrial
predpriiatii.
enterprises]
Moskva, Goo.
(MIRA 12:12)
and appliances)

VIASOVY V. F.
How to calculate opti- dimens-"ons for the lots of natal-cutting
tools. MaBhinoetroitell no.10:24 C 162.
(MIRA 15:10)
(Metal-cutting tools)

VLASOVP V.F.; TIMAN A.F.
< P
Relation for integrals of moduli of trigonometric polynomials. Dokl.
AN SSSR 138 no.6.-1263-1265 je 161; (MM 2-4:6)
1. Prodstavleno. akademikom S.N.Bernshteynom.
(Polynomials) (Integrals)

YLASOV, Viktor Fodorovich- Prinimal ucha3tiye OVCIIINNIKOV, N.I.,
cTo-ts.,JZYTPOV, N.M.,, prof.,, retsenzent; ITSKHOKII Ya.S.,
prof., nauchrqy red.; LILICIONOV, G.Ye.,, tekhn. red.
[Course in radio engineering] Kurs radiotekhniki. Moskva Gos
energ. izd-vo, 1962. 927 p. (Radio) (MIRA 15:3~

S/021/62/000/004/004/012
D299/D302
AUTHOR: Vlasov, V.P.
TITLE: On approximation processes of periodic functions by
trigonometric polynomials
PERIODICAL: Akademiya nauk b-krRSR. Dopovidi, no. 4, *1962, 438-442
TEXT: An asymptotic formula is derived for Lebesgue's function,
which is approximated by trigonometric polynomials. let
~Ll n
Kn (X) == Y, ~V' cos kx 0
2 +
be a sequence of even trigonometric polynomials with real coeffi-
cients, and Pn(x) - a sequence of functions of bounded variation on
Irg 1r]9 for which Var pn(x) 1 . Each continuous 21r -periodic
function is made to correspond with a sequence of trigonometric po-
lynomials
Card 1/3

S/021/62/000/004/004/012
On approximation processes of D299/D302
I---- 1 1 22T
T, Y; X; 1; - Y, f (f') S K. (x + u -dQ,, (u),
r 0 (2)
(n = 1, 2,3~_)
where r>2n+].
r
Various well-knovm.approximation-methods which involve expansion in
Pourier series or interpolation of the function f(x) at equidistant
points, are particular cases of (2), with different se uences (1)
and Pn (x). The convergence of the polynomial sequence M is rela-
ted to the behavior of the corresponding sequences of Lebesgue func-
tionst viz.: (x; 1; P) up /T (f; x; A; p)/.
Lnjr ~ 11 n,r
/f(t
The follow n, theorem holds: If the uniformly bounded oystom of
numbers A, ~n5 is convex (or concave)~ and for each positive sequen-
1C
ce En = 0(1/n), Var pn(t) = 1 0(1/.:Q9 then the asymptollic formu-
la
Card 2/3

S/021/62/000/004/004/012
On approximation process of ... D299/ '302
-I- n XV)
L., (x; s,,, (Q) I cn E n-k+ 1 +0(1), (4)

Cos 21z+ In I-L +
2 + r,~-
2 rX
71
+ r 1t (2n A- 1) n 2a (2n,
holds, where s,,,,(Q)r
2n+ 1
Mn
11
2r
provided that r/(2n + 1) .is an integer; (cp
=arg c
,
C
F 25r
~ j
n
. n
int
e dPn(t) ).
The theorem is proved on the basis of a 0
lemmat and by
use of Abel' s transform. There is 1 Soviet-bloc refer ence.
ASSOCIATION: Dnipropetrovslkyy derzhavnyy universytet (Dniprope-
travalk State University)
PRESENTED: by Academician Yu.A. Mytropollsikyy, AS UkrRSR
SUBMITTED: -September 1, 1961
Card

VIASOVI V.F.
Constructive characteristic of a certain class of functions.
DqkI. AN SSSR 142 no.4s773-775 F 162. (MA 15s2)
1. Dnepropetro-iskiy gosudarstvennyy universitet im. 300-
Idtiya vossoyedineniya U~-rainysi Rosiiyey. Predotavleno akademikom
S.N.Vernzhteyndm** (Functions, Continuous)

VLASOVp V*F, , dotsent
Calculating the economic efficiency of the reconditioning of
worn-out cutting tools, Vestomashinostr. 43 no.2t82-83
F 163. (Metal-cutting tools) (MIRA 16:3)

VELIKANOV, K.M.; VLASOV, V.F.
Method for calculating the economic efficiency of substituting the
machine tooling of parts with a hot stamping. Trudy LIP no.227:
87-96 163. (MIRA 17:4)

VLASOV, V.F.
Determining the economic effici6ney of metal-cutting tool
reconditioning. Trudy LIP no.227:125-127 163.
Methodology-for calculating theoptimal lot size for metal-cutting
tools manufactured in machinery plants. Ibid.:128~-132
MORA 17:4)

ZVYAGINTSEV, A.F.; IVANOV, Yu.N.; KAZAKOV, V.E.; OSTETSENKO, A.M.;
SOLO14)VICH, M.Ya.; KORZH, V.I.; DASHKEVICH, A.A.; Prinizali
uchastiye: LIPTSER, S.Kh.; RYZHIKOV, A.F.; STALINOU.ITSKIY,
V.N.; LEVENETS, L.Ye.; MOGILA, V.A.; KOVAL', A.A.; VIASOV, V.F.;
ROSHCHINy A.G.; RAYKOp V.P.-) KORNIY-ENKO, V.G.;
Investigating the possibility of
electric locomotive wheels with
proizv. 5 no.11:11-14 N 163.
manufacturing all-rolled
existing equipment. Kuz.-shtam.
(MIRA 17.

L 35883-66 - MIT(I Y:
kk: XP6010775
SOURCE; CODE:
UTHOR: Vlasov, V.
UR/0l46/66/oo9/ooi1oo9o1oo96
ademy im,_ gklL (Leningradskaya
ORG: Leningrad Mlitary Eudneering Ac qzha,
F y
voyennaya inzhenernaya krasnomamennays, akademJya)
TITLE: Discrete smoothing devices
SOURCE: IVUZ. Priborostroyenlye, Y. 9, no. 1, 1966, 90-96
TOPIC TAGS: signal noise separation, signal interference
ABSTRACT: The smoothing of a stationary random noise n(t) by a discrete smoothex
(DS) is theoreticalfy analyzed: the rms error in reproduction of a random stationary
desirable signal m(t) and the required dynamic accuracy of reproduction of a regular
1YV signal x(t) at discrete time moments
are specified. The general DS structuri
(see figure) comprises: D(z) is the
transfer function of DS digital'circuit;
W(s) is the extrapolator's transfer
Card 1/2
- UD G: h 2 -

L 35883-66
ACC NR- AP6010775
function; W (a) is the transfer function of the DS continuous part. The mechanism
a
of w-transform. and the concept of absolute pseudo -frequency x- w' are used
i To
which permits utilization of continuous-DS methods of analysis. Smoothing of
(a) discrete white noise, (b) random noir4e having limited spectral dens#y,
(c) irregular tossing (rolling or pitching) type random noise, and W harmonic noise
is considered. - Orig. art. has: 3 figures and 48 formulas.
SUB CODE: 09 SUBM DATE: 17Feb65 ORIG REF: 003
Card 2/2

VLI.SOV, V.F,; KIMANER, V.Ya., inzh., rotnenzant
(Economics of matal-cutting-tool production] Ekonomika
inatrumentallnogo proizvodetva. Moskvap Mashinostroenie,
1965. 135 p. (mim 18:3)

GONOROVSKlY, I.S.; ITSHOKI, Ya--~-y doktor toklm. nauk) prof.,
retsenzent; VLASOV, V.P., kand. tekhri. nauk, dotn.)
retsenzent; kand. tekhr, nau~j dotz.,
retsenzent; ZABOLOTS'KlY, N.G., red.
(Radio circuits and signals] Hadiotekhnichenkle tsepi i
signaly. -tzd.2., ispr. Moskva, Sovetskoe radio, 1964.
694 P. (MIRA 17-.11)

GONOROVSKIY, I.S.; 1TSIHOKI, Ya.S., do]--tor telchn. nauk, prof.,
retsenzent; VLASOV, V.F., kand. tekhn. nauk, dots.,
retsenzent; LAPIS, A.11., kand. tekhn. nauk, dots.,
retsenzent; ZABOLOTSKIY, N.G., red.
[Radio circuits and signals) Radiotekhnicheskie tsepi i sig-
naly. Moskva, Sovetskoe radio, 1963. 694 p. (MIRA 17:5)

USSR/Cbemistry - Oxides, Reduction -i 51
"Reduction of Metal Oxides With Solid Carbon,"
1P. V. Gel'd, V. G. Vlasov, N. N. Serebrennikov,
Ural.Polytech Inst imeni S. M. Kirov, Sverdlovsk
"Dak Ak Nauk SSSR" Vol L=111I, No 4,, pp 6937696
Expts for reducing chromium oxide and manganous
ox-ide vith graphite' in vacuum installation corrob-
cr~ate existing viewpoint that reducing process
consists of, 2 stages, and rate of process is detd
by 2d, slow stage, i.e., gasification of carbon
with carbon dioxide. Disproves assumption that
process is direct reaction between, oxide and
i84T8
USSR/Chemistry - Oxides, Reduction 1 Jun.51:
(Contd)
.tarbon without intermediate, formation of carbon
monoxide. Submitted by Acad S. 1. Vol If kovich,
Apr 51.
164T8

GELID) P. V., V. G., STETREE-Q-717111,0"'., N. 1%
CEL'Dt P. V.1 kiuso-'4' '-'. G., S!qUW;ER::'1jIK0VY I.T. N.
Carbons
Interaction of oxides and.their comnounds with solid carbon. Zhur.
prik-1. khim. 25, no. 2, 1952.
9. Monthl List of Russian Accessions, Library of Congress, August 1952 3*ja, Uncl.

VIASOV, V.G., kand.tokhn.nauk, dots..- LISNTAK, S.S., kRnd.tel,.bn.nauk
-." -;4,,f6 f cfarcoal. Iz7 '779.
Ki s of iron oxide reductinn b7 means o
ucheb. zav.: chern. mAt. no-7:45-52 Jl '58. (MIRA li:10)
1. Urallskiy politelchnichookiy inatitut. -
(Iron oxides) (Oxidation-reduc,il'61'ranction) Wharcoal)

VLASOV, V.G., dotio., kand.takhn.nauk; LISNYAK, S.S., kand.takhn.nauk
Kinetics of Fai0h and YeO reduction by solid carbon. Izv.vys.ucheb-zaT#;
(MIRA 11:11)
chern.mat. no.9:45-50 S '58.
1. Urallskiy politakhnicbeskiy institut.
.1 (Iron oxides) (Reduction, Chemical) (Carbon)

5W
AUTHOaS: Vlanov, V. G., Kozlov, V. A. SO'1/76-.72-11-23/32
TITLE: Dissociation Kinetics of Manganese Oxides (Kinetika dis-
sotsiatsii okislov margantsa)
PERIODICAL: Zhurnal fizicheskoy khimii, 1958, Vol 32, Nr 11, pp 2608-2613
(USSR)
.ABSTRACT: Investigations of the subject mentioned in the title are of
special interest as the dissociation processes are applied in
metallurgy, and moreover, they are characteristic examples of
topochemical reactions. Besides the investigations of the dis-
sociation kinetirs the authors also determined the dissociation
pressures of MnO 2 and Mn 203' MnO2 was used in a form which
according to the terminology by Ye. Ya. Rode (Ref 5) is called
the P-modification of MnO 2* The experiments ..,ere carried out
in a high-vacuum plant on a quartz spring balance. The dis-
sociation kinetics of MnO 2 was investigated at 600-6500C and
that of Lin203 at 400-5500C. The function of the dissociation
Card 1/3 pressure of MnO 2 versus the temperature is expressed by the

SOV/76-32-11-23/32
Dissociation Kinetics of.141rangan-ese Oxides
equation Ig P 6602 + 8.21, and that for Mn 0 by
02 T 2 3
lg P - 11040 + 8-57. It was found that the dissociation
0 2 T
of both "ides at lower temperatures (4000 or 6000, respective-
ly) takes place in the beginning at a constant velocity (g--kt).
The velocity of the process in this period is determined by
the separation of the oxygen from the o*de surface. In the
further course of the reaction this oxygen sep ation,is
slowed down and the diffusion resistance of tT layer of the
reaction products is increased. At Mjgher tempELratures the dis-
sociation processes take place accorling to-the diffusion
2
equation (g =kt), which fact is explai-niaby an increase in
the diffusion resistance mentioned above,-Jfhe character of the
dissociation processes changes on its t:ransition into the range
where there are solid solutions, arrd' the equation
ln a = kt
a-9
Card 2/3 becomes valid. The activation energies were determined.

. . SOV/76-32 -I 1 -231132
Dissociation Kinetics of Manganese Oxides
There are 2 figures, 3 tables, and 6 references, 3 of which
are Soviet.
ASSOCIATION: Urallskiy politekhnicheskiy institut im.-S. M. Kirova, Sverd-
lovsk (Ural Polytechnical Institute imeni S. It . Kirov,
Sverdlovsk)
SUBMITTED: May 29, 1957
Card 3/3

5(2)
SOV/80.-32-3-10/43
AUTHORSs Kozlov, V.A.9 Vlasov, V.G9
TITLEt The Kinetics of the Reduction of Manganese Oxides by Solid Carbon
(Kinetika vosstanovien-'ya okislov margantsa tverdym uglerodom)
PERIODICAL; Zhurnal prikladnoy khimii, 1959, Vol XXXII9 Nr 39 PP 523-531
(USSR)
ABSTRACT: The reduction of the manganese oxides I!nO->, Mn20 and Mn304 by
means of charcoal at relati7ely low 'V-emperature Is studied here.
Figiire 2 shows that the reduction of XnO at 400 - 5500C Pro-
ceeds only to Mn20 but at '500 and 55006 the reduction is auto-
catalytic. The relu'ction of Mn2 03 and Mn304 proceeds to manga-
nous oxide. The reduction rate decreases with the elimination
of oxygen. If the contact- between the reactants is very close,
e.g., if they are mixed and ground together, the reduction rate
increases sharply (Figure 5). The activation energy increases
with the transition from the higher to the lower oxide (Table 3).
It is evident that the reduction process has a diffusion cliarac-
ter wh!ch is affirmed by the equation g2 = Xr, where g is the
degree of oxygen elimination, Tthe time since the beginning of
Card 1/2 the experiment and K a ~;onstant. At the transition into the

The Kinetics of the Reduction of Ranganeae Oxides by Solid Carbon
field of silid dolutions a 7,hanae takes place in the character
of interaction of oxideb with (carbon and the prooess of re-
duction may be described by the equation in a K2 .-U,
a-K
where it is the quatntil-ly of oxygen which must be eliminated'from
the reduced oxide in order to transform it completely to the
lower Lixide and RI 46 a oonetant.
There are 4 aets of gr&j:hs9 1 diagram, 3 tablesq and 15 refer-
ences, 9 of which are Soviet and 6 German.
ASSOCIATIONA Urallskiy politekhnicheskly inatitut imeni S.M. Kirova (Ural
Poly technnicF-1. inst'i tuts imeni S.M. Kirov)
SUBMITTEDs October 19, 1957
Card 2/2

h C, V/,v
PIU-SE 1 BOOK E~LPLOITATION SOV/5410
~.a,-.,hkentnkaya konforentalya po mirnomu ispol'zovaniyu atomnoy
-nergli, Tazhkent, 1959.
Trk,41v (Qrai;3actioni of the Tanlikent Conference on the Peaceful
Ufi4,~j of Atomle Enerpy) v. 2. Tachkc-nt, Izd-vo 1,11 U,-,SSlt, 1960.
L49 -,. Errata clip Inaerted. 1,500 copies printed.
AZeney: Akademiya nauk Uzbekskoy SSR.
Reonc-nz-'blc Ed.: S. V. Starodubtoov, Academician, Acatdc.,iy of
..cience3 Uzbek SSR. Editorial Board; A. A. Abdiillaycv, Can-
did-~t,:; of Phy3icz and NatbrnatIo5; D. IN, Abdur-a:3ulov, Doctor
cf ;,.*,-:d.,;al Sciences; U, A. ArIfov, Rcademlcian, Acadr-my of
S icnce3 Uzbek SSR; A. A. Borodulina, Candidate of BioloCl,,,al
V. 11. Ivashev; G. S. illcrwiiova; A. Ye. Yiv; Ye.
L,--,'Wanov, Candidate of Phy3ics and Mathematics; It. 1. Nlholt~.7c-v,
Can-iidare of J,:,~dlcal Scie.-.ceu; D. Nlizhanov, Candidate of Chu,,ical
S:-Lence.-,; A. S. Sadykov, Corre3ponding lllcmber, Acalicmy of Scicncea
US3R, Academician, Academy of Sciences Uzbek SSR; Yu. 11. Talanin,

Tranvacticna of the Ta2hkent (cont.) 301/5410
~!andft.date of Phyeics and 41.11athc-miatlcu; Ya. Kh. Turakulov, Doctor
of BloloGlcal 3-.iences. Ed. . R. 1. Khamidov; Tech. Ed. : A. G.
Babak-hanova.
PURCTOSE : The -publi---ation ifs Intended for scientific itcrkera and
enployed in enteripriEes where radioactive ivotcpes
anJ nuclear radiation are used fcr re.zearch In choW.cal, goo-
jcgicalr and technological fields.
RAGE: 7hi_~ collection of 133 articlea rcpre~nnts the second
xilure of the Craneastlon3 of the '.a=hkent Conference on the
Fl~a-_eful Use!3 of Atomic Energy. T-ae individuaI arti-les deal
w-It'a 1, wide range of proble-ma :Ln the field of nuclr-a?, radiation,
in-iluding: productIcn and chevIcal analy~ls ef radica.-tive
lzotcpes; inventigation of the k1neties of chemical reactions
by rreans* of izotcpes; application, of spectral analy,3i.,3 for the
manufacturing of radioactive pre,,,aratlono; radloa-.tive methods
f-:~r determining the content of elemento In the rocka; and an
analysis of methods for obtaining pure substances. Certain
Card 2/20

Tranaaetions of the Taohkent (Cont.) SOV15410
Instruments used, such az automatic ro:Sulator3, flowmetera,
level giuocn, and hibli-sonaltivity ramma-rolaya, are deacribed.
No p'er3'1=li1.ios are mentioned. Rurorcnces follow Individual
artIcle5.
TABLE OF CONTENTS.
RADIOACTIVE 1301).7011ES AND NUCLEAR RADIATION
IIT F11011MMI11,0 AIM GEOLOGY
Lobanov, Ye. 'N.' (Inatitut yadernoy fiziki UzSSR - Institute o. f
Nuclear Phy'sics AS UzSSR]. Application of Radioactive Isotopes
and "Tuclear Radiation in Vzbelci3tan 7
Taksar, 1,31., and V. A. Yanrushkovakiy [Institut fiziki M La-tv
SSR - InGtituto of Physics AS Latvian 33R]. Problems of the
2ypi-Ification of Automatic-Control Apparatus Based on tfie Ui;e of
Radioactivo Isotopes 9
Card 3/20

Transactions of the Tashkent (Cont.) SOV/5410
Yhruf7hchev, V. G., A. S. Lapllin, U. 'La. MarSulin, S. P1. Stopanov,
L. I' Bclcnlkiy, T. V. Bromberg, and V. 0. Ivliyev. C Mnintry of
al,,
1
14~ h USSR]. Industrial Gavana-Plant for Sterilization of Nedical
11ateriala 170
Khrushchev, "~. G., B. A. Rubin, L. V. Metlitrkiy, A. 1. Rytov,
lei. 11. Gaysin, U Ya 1,11argulls, V. S. Grammatikati, 0. Vlasov
and A. V. Petrol. blinistr-1 of Yealth USSR). Garnma-Ylant for
Ocntinuous Irradiation of Potatoes 182
YrGkoflyev, N. S. (Institixt elronoraiki All SSSR - Institute of
Esonomica AS USSR]. Economic Efficiency of the Use of Htgh-
Capacity Gamma-Plants In the Light and Food Industry 192
Abdullayev, A. A., Ye. M. Lobanov, A. F Novikov, and A. A.
Yhaydapov (Institute of Huclear Pnysi;s AS UzSSRI, Une of
a 1-Mltichannel Scintillation Gamma-Spectrometer for the Analysis
of Rock Specimens 199
Card 10/20

S/148/60/000/007/001/015
A161/AO29
AUTHORS: Vlasov, V.G., and Lebedev, A.G.
TITLE: Dissociation of Uranium Trioxide
PERIODICAL: Izvestiya vysshikh uchebnykh zavedeniy - Chernaya metallur-
giya, 1960, Nr 7, pp 5-9
TEXT: Dissociation of UO has been studied in a 10-4 Hg vacuum to in-
vestigate the kinetics ana the mechanism of the process. UO was prepared
by a method described in Ref 4 by heating UO -2H 0 for 3 h9urs in an
oxygen flow at 3500C and for 1 hour at 400 C- 4The2orange-red UO could
easily be rubbed to fine powder and pressed into 1.4-1.5 g briquhs.
Dissociation was studied by the decreasing weight of trioxide on spring
scales. The vacuum installation had been previously described /Ref 2/.
The process started at 4200C. Complete dissociation into UO, took place
at 5500C in 1 hour and could not be obtained at lower temperatures
(curves, Pigure 1). The dependence of the dissociation rate on the
dissociation degree was stated (curves, Pigure 2). As can be seen, the
Card 1/3

3/14 60/000/007/001/0-,5
Dissociation of Uranium Trioxide A161 YA029
dissociation process rate was constant in the beginning, expressed by the
formula: g = kt where g is dissociation in %, t - time in minutes after
start of experiment, k - the proportionality coefficient, until a 42~_
dissociation was reached and solid phases of the summary composition
UO remained in the reaction space, where the separation of oxy en
ab?'all y
p I dropped to a new constant level of 9 = 0.091t + 17 90 (2
At 500 C, decomposition progressed somewhat differently (Formulae 3 and 4).
At 5500 it was constant until a 65%-separation of oxygen from trioxide
was attained at a rate of 9 = 4.65t + 40-9 (5). If the reaction
proceeded further, the rate dropped to
19 T 0-101- __9 ~0.0606t. (6)
The constant reaction rate in the beginning may be explained by a high
number of defective spots caused by crushing before briquetting, and by
the beginning of the dissociation on these spots, where oxygen was re-
moved from the surface by chance law. Later the active centers dis-
appeared. The abrupt change in the rate after the 42% dissociation point
at 5400C can be explained on the basis of the structural diagram of the
U - 0 system /Ref 3/. According to this diagram the dissociation of UO 3
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Dissociation of Uranium Trioxide A161/AO29
in the beginning proceeds without producing a now solid phase in
connection with the existence of the region of s8lid solutions, the
oxygen content of which is only reduced. At 500 C,higher temperature
caused a faster disappearance of active centers and apparent growth of
diffusion resistance in the layer of the forming reaotion products. At
5500C dissociation can be described by equation (6). The apparent
activation energy in the beginning stage (to 3q- oxygen separation) has
been calculated as 37.2 kcal/mol, which well agrees with the reaction
heat effect value of 6UO 3t;e2U 08 + 02 determined by Brewer /Ref 5/ to be
35 kcal/mol and confirms oPion of S.Z. Roginskiy /Ref 6/ that the
activation tinergy of the majority of topochemical reactions,in conditions
far from eqv.ilibrium is approximately equal to the heat effect. There
are 2 figures and 6 references: 5 are Soviet and 1 English.
ASSOCIATION: Urallskiy pdlitekhnicheakiy institut (11ral Polytechnic
Institute)
SUBMITTEDs JulY 14, 1959
Card 3/3

YOROSHIII, Ye.M.; VLASOV, V.G.
Spectrographia study of phenol acids. Part lt Hydrom4boncoic acids.
Zhur. ob. khim, 30 n6.90004-3011 S 160. (MIRA 13:9)
1. KMrlkovskiy farmatsevtichookiy inatitut.
(Benzoic acid-Spectra)

-q/080/60/033/04/OZ/045
AUTERORSt Vlazoy V.O.. Kozlov. V.A.
A
T.'L=s The Interaction of Uranium Trioxide With Aolid Carbon)-i
PMODICAL: ZhurnO prWadnoy khimii, 1960, Vol 33, Nr 4, pp 76o - 765
TEXTs The rate of the process of direct reduction of uranium trioxide was in-
vestigated. Uranium trioxide was obtained by heating uranium peroxide for 6 hours in
an oxygen flao at 40000. The reducing agents were birch charcoal and sugar charcoal
with a carbon con'tent of ~9.99%. The investigation was carried out in a high-vacuum
installaticn with continuous control of the weight loss of the sample by means of
sprin
.g scales. Feduction by birch charcoal was studied within the temperature range
350 4000C, and by.sugar charcoal within the range 450 - 5300C. Birch charcoal proved
to be the more active reducing agent. The activation eneM of the reftation process
in the case of birch charcoal was 43 kcal/mole and in the case of suga~'oharcoal
65 kcal/mole. The gaseous phase formed during reduction consisted only of carbon dioxide.
The authors try to explain the mechanism of accelerating the reaction of carbon monoxide
regeneration, which is the slowest stage In the process of direct reduction of uraitium
trioxIde. There are: 4 graphs and 16 references, 10 of wh1ch are Soviet and 6 Oexman.
SUMO-. August 24, 1959
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B004/B054
AUTHORS: Vlasov, V. G. and Strekalovskiy, V. N,
TITLE: Interaction Between Hydrogen and Uranium Trioxide
PERIODICAL: Doklady Akademii nauk SSSR, 1960, Vol. 134, No. 6.
pp. 1384-1366
TEXT: The authors give a report on their investigation of the reducticn
of uranium trioxide by hydrogen in the temperature range from 300 to
5000C and at a hydrogen pressure of 50 - 400 torr. The experiments were
made in a vacuum apparatus, and the loss in weight of UO 3 was measured by
a spring balance. The experimental data are shown in diagrams; Fig, 1:
degree of reduction as a function of time at different temperatures and
P 200 torr; Fig. 2. degree of reduction as a function of time at dif--
H 2 =
ferent P and 400 0C; Fig. 3: reaction rate as.a function of the degree
of reduction at different temperatures; and Fig, 4: reaction rate as a
function of the degree of reduction at different P H2' Table I shows the
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Trioxide B004/BO54
ratio 0 : U for P H = 200 torr after two hours of heating to 350'~ 400 C,
450 0,, and 5000C~ These results are interpreted on the basis of the phase
diagram of the U - 0 system. The first horizontal sections of the curves
in Pigs, 3 and 4 correspond to the reduction of UO 3 to U3 06. Here, the
limiting stage is the reaction of hydrogen adsorbed on the oxide surface
with the oxygen of the oxide. This reaction follows equation (1):
V - kP112 . The hydrogen is rapidly adsorbed in the atomic state. As I the
H2
authors had proved in a previous paper (Ref. 1) that UO 3dissociates in
vacuo only above 430 0 C, while reduction starts alrea(brat 3500C, the latter
proceeds without previous dissociation. The curve sections in which the
reaction rate decreases with increasing degree of reduction correspond to
the continuous transition of U 30a into the phase UO 2.6+x w ith the minimum
oxygen content corresponding to 'he given temperature. The decrease in
the reaction rate is explained by a reduction of the oxygen content in
the solid phased The second horizontal sections of the curves in Figs~ 3
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Trioxide
S/020/60/134/006/022/031
B004/BO54
and 4 correspond to the reduction of UO 2.6+x to the tetragonal phase.
Here, the limiting stage is the hydrogen adsorption on the oxide surface
according to equation (2): V = k IPH2' No reduction to UO 2.00ccurred in
the temperature range investigated. The authors mention a paper by F~ F.
Vollkenshteyn (Ref. 3). There are 4 figures, 1 table, and 4 references;
3 Soviet and I Swedish.
ASSOCIATION: Ural'skiy politekhnicheskiy institut im. S. M. Kirova
(Ural Polytechnic Institute imeni S. M. Kirov)
PRESENTED: June 11, 1960, by V, I. Spitsyn, Academician
SUBMITTED: June 8, 1960
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s/i26/6i/oj.l/003/007/0l7
E3,93/E483
AUTHORS: Strekalovskly, V.N., Bessonov, Aj., Ylasov, V.G. and
Sidorenko, F.A.
TITLE- PbaAe Transformations During Reduction and Oxydation
of Uranium Oxides
PERIODICAL: Fizika metallov I metallovedeniye, 1961, Vol~ll, No.3,
pp.400-403 + I plate
TEXT; The uranium-oxygen system has lately attracted a great
deal of attention owing to the possibility of using uranium
oxides (dioxide In particular) In the manufacture of ceramic fuel
elements. However, the experimental work has been mainly
confined to studies of oxydation or thermal decomposition of
uranium oxides, and the object of the present investigation was to
study (a) the kinetics of hydrogen reduction Qf amorphous U03
and green U308 at 300 to 700%, (b) the process of oxydation of
U02 in air, oxygen and C02 at 165 to 860*C and W the phase
trannformations taking place during these reactions, The results
of the study of kinettos of the reduction process are reproduced
schematically in Fig.1, where the rate of reduction (A in
arbi.trary units) is plotted against the overall composition of the
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Phase Transformations
S/1-26/61/oil/003/007/017
E193/Elk83
resultant product, i.e. against the oxygen/uranium (O/U) ratio,
It is pointed out, in this connection, that. neither the rates
of reduction of U03 and U08, nor the energy barriers during the
crystallo-chemical transformations of these oxides are the same;
thus, for instance, hydrogen reduction Of U03 begins at 350"C, the
corresponding temperature for U08 being 450*C. In addition,
reduction of U03 at temperatures ( 5000C practically ceases when
the oxide reaches the oxide content corresponding to U02.33; at
higher temperatures, U409 and oxides -with a still lower oxygen
content are produced, The results of the kinetic studies were
correlated w1th the results of X-ray diffraction analysis of the
products of the reduction of U308, and the following conclusion*
were reached regarding the phase transformations, taking place
during the reduction process, In the initial stages ' U 08
gradually loBes its oxygen, this process continuing untii the
starting material is reduced to 46.9% (100%, reduction corresponding
to complete conversion of U03 to U02) which corresponds to the
overall composition of the product given by the formula U02.539;
at this stage, the X-ray diffraction pattern still shows the
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21220
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Phase Transformations E193/E483
lines of the U308 phase; the lattice parameters of the initial
phase have changed but no lines of a new pha3e have yet appeared;
at 62 and 69% reduction, the lines of the starting oxide are still
present in the X-ray pattern and lines of the cubic U407 phase
appeari at 75% reduction, the U308 lines completely disappear and
only the U407 lines remain; after a further decrease in the
oxygen content, the crystal structure of the oxide remains cubic
but the lattice parameter increases. Reduction of U03 takes
place in a similar manner, the crystalline U308Phase being formed
directly from the amorphous U03 which doeB not pass through the
crystalline form during this process. Ths whole reduction process
can be represented in the following mannera
Amorphous U03-"olid solution, based on U02~6 --)UO2.2_'"O2+x-
Regarding the process of oxydation of U02 in aIr or in oxygen. it
can be represented by3
U02 --4'UO2 + x--" U02.36 + O~05 --+Solid solution, based on U02.67,
The tetragonal phases (UO2~32+ 0,,Ol, U02-35, U02-371 U02~41)
whose presence can be inferred from the kinetics of the process
studied, are unstable and decompose to form U409 and U308, When
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Phase Tranaformations ... E193/E483
the oxydation reaction takes place (in air or oxygen) at
temperatures >4000C, no formation of the tatragonal phases occurs,
and the process proceeds according tos
U02'-"02 , --3P U02.25 -i~Solid solution, based on U02.67 -
Finally, it was established that U02 does not oxidize in carbon
dioxided There are 3 figures and 12 referencesi 8 Soviet and
4 non-Soviet.
ASSOCIATION: UralQskiy politekhnicheskiy institut im. S.M.Kirova
(Ural Polytechnical Institute imeni S.M.Kirov)
SUBMITTEDg July 18, 1960
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'Phase Transformations ... E193/E483
; M,.
.1 1
Fig. 1'.

24484
S/126/61/011/006/010/011
0 V't.. 7-300 E193/E483
AUTHORS: Bessonov, A.F. and Vlasov, V.G.
TITLE: Phase transformati(~~_s during oxidation of metallic
.uranium '
PERIODICAL: Fizika metallov i metallovedeniye, 1961, Vol.11, No.6,
pp-957-959
TEXT: The object of the present investigation was to study
oxidation of uranium in air and carbon dioxide. To this end,
specimens (4 x 2 x 15 mm),,were degreased, pickled in concentrated
HN03, washed in alcohol and held for 15 minutes in air at various
temperatures between 20 and*350*C, or in C02 at 400 to 9000C, after
which the surface of the specimens were examined by X-ray
diffraction. The results are reproduced-in Fig.1, showing the
X-ray diffraction pattern of the surface of uranium specimens after
(a) 8 days exposure to air at room temperature., (6) oxidation at
1000C, (8) oxidation at 2050C, (?,) oxidation at 3000C1
(3) oxidation at 3500C, (e) removal of the outer, loose, oxide
layer. An X-ray diffraction pattern of uraniuml oxidized in C02
in reproduced in the paper. The following conclusions were reached.
1) The phase transformations taking place during oxidation of
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2484
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Phase -transformations ... E193/E483
uranium in air at 265 to 4000C can be repreaented by:
UMeta--l-#aU02-*CcU02+x-*PU02-*U307-4solid solutions based on U02.67
2) The constitution diagram of the U-0 system is repeated in the
phases which constitute the consecutive oxide layers of scale,
formed on uranium in air at atmospheric pressure in the temperature
interval studied. 3) Metallic uranium, heated in C02, oxidizes to
U02 only. There are 2 figures and 8 references: 7 Soviet-bloc and
1 non-Sovlet-bloc. The reference to an English language
publication reads as follows: Blackburn P., Weissbart J.,
Gdlbransen E., J.Phys.chem., 1958, 62, 8.
ASSOCIATION: Urallskiy politekhnicheskiy institut im. S.M.Kirova
(Ural Polytechnical Institute-imeni S.M.Kirov)
..SUBMITTEDt December 15, 1960
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Phase transformations
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E193/E483

I +i
A

I-
N
M

2~8 5
G
S/126/61 Oll/oWoll/oll
410 11 E073/E335
AUTHORS: Bessonov, A.Y.I.-Borisov, B.S. a-id Vlasov, V.G.
TITLE: Investigation of the Structure of i-h-e-T-r-Imary Oxide
Film on Uranium
PERIODICAL: Fl-zika metallov i metallovedeniye, 1961, vol. il,
No. 6, pp. 959 - 960
TEXT: In ztudying the mechanism of oxidation of metals
investigation of the structure of the primary oxide film formed
in air at room temperature during the initial oxidition'period is
of great importance. For some metals the structure of the films
A.ormad during the initial period of oxidation does not differ
from those formed during later stages of oxidation. For a
.number of other metals, for instance, iron, and its alloys,
a film of a particular structure (type j-Fe 203) forms during
the initial period of oxidation. The primary oxide film is
a protective one for most metals; it Srovrs to some limit
thickness, then stops groiring and prevents further oxidation.
The kinetics of growth of the primary films depends on a
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Investigation of the Structure ... E073/E335
number of factors and so far no satisfactory theory on this
process exists. The authors carried out investigations on
uranium of 99.89r', purity which, after rolling, was annealed at
850 OC for six hours in vacuum. Plato specimens 10 X 5 x 3 Lmn
were initially ground with emery paper of varying coarseness
and lapped by a ring using high-grade alumina. After polishing
the ring was moistened with benzol or ethyl alcohol to prevent
access of air to the polished surface. Microscopic investi-
gations have shown that the surface was peppered with fine
crystals and the number and size of the crystals increased
rapidly. For determining the structure of this primary film
electron-diffraction studies were made. For removing the
scale films the specimens were etched in nitric acid for 10 min
and then washed several times in ethyl alcohol. Oxidation was
in air at room temperature for durations of 10, 30, 120 and
240 min. In the second series of experiments, the specimen,
after having been taken out of the alcohol (wet), was placed
immediately into the chamber of the electron-diffraction
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Investigation of the Structure .... E073/E335
apparatus from which the air was evacuated so that the specimen
surface interacted only vrith the air which remained in the
chamber of the electron-diffraction camera. Part of the specimens
vrere subjected to electron-diffraction investigations immediately
after polishing (without etching); back reflection pictures
wero taken. The obtained interpldne distances ifere compared
with X-ray data, obtained by the powder method for uranium
o::ides. Tlhe investigations revealed a cubic phase on uranium
o::ide with a lattic constant of a = 5A5 A for all the specimens,
Whic1h corresponds to the oxide U02' In a second series of
experimants the electron-diffraction patterns contained refloxos
from the metallic uranium in addition to lines of the phase UO 2,
This indicates that in this case the entire thickness of the
oxide film participated in the diffraction and that the primary
oxide film of uranium consists solely of the phase U02' From
the widening of the Debye lines the size of the forming UO 2
crystals could be determined, Which was about 10- 4 cm. Thus,
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Investigation of the Structure *00 E073/E335
the microscopic and electron-diffractlon investigation of
oxide films of uranium obtained on oxidation of the latter in
air at room temperature indicates that the primary film on
uranium is crystalline and cons-4--ts solely of UO 2*
(Abstractor's note: this is a complete translation.)
There are 2 Soviet references.
ASSOCIATION: Urallskiy politeklmicheakiy institut
im. S.M. Kirova (Ural Polytechnical Institute
im. S.M. Kirov)
SUBMITTED: January 13, 1961
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S/126/61/012/003/011/021
E193/E135
AUTHORS: Bessonov, A.F.9 and Vlasov, V.G.
TITLE; Concerning the mechanism of oxydation of
metallic uranium
PERIODICAL: Fizika metallov i metallovedeniye, vol.12, no.3, 1961,
403-40
TEXT., Effective measures against oxydation during the
preparation of metals or in service can be applied only if the
mechanism of this process is properly understood. Hence the
present investigation, in which the kinetics of oxydation of
uranium were studied by the gravimetric method and the
constitution of the scale formed on uranium under various
conditions was detevmlned by X-ray d�ffr-act�on, m�cvoscop�c, and
electron diffraction analyses. The experiments were carried out
on 99.8% pure uranium specimens, degreased, pickled in concentrated
HN03, and washed in ethyl alcohol. The oxydation tests were
carried out in dry air and oxygen at various temperatures and
pressures; some results are reproduced graphlically. In F:LS.1
the specific increase in weight (& m/s x 10%, mg/cm2) of uranium
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Concerning the mechanism of oxydation S/126/61/012/003/011/021
-E193/El35
heated in air is plotted against time (minutes), curves 1-6
relating to testa conducted at 250, 300, 350, 4oo, 600 and 76o Oc
respectively. The kinetics of oxydation of uranium in oxygen are
illustrated in the same manner in Fig.2, where curves 1-4 relall.'a
to results obtained at 250, 300, 350 and 400 OC. It was
established that the effect of pressure (p, mm Hg) on the rate of
oxydation (v, mg/cm2) in minutes of uranium in air at 400 OC is
described by
V = a 1 4f -P (3)
for pressures higher than 200 mm Hgj and by
v = a2 P (4)
for pressures lower than 200 mm Hg. The oxydation rate of
uranium in oxygen at 300 OC under pressures ranging from 5 to
550 mm Hg is given by v = a3 Al P
The rate of oxydation was not affected at all by forced
circulation of oxygen and only to a small extent by circulation of
air at pressures > 200 mm Hg; at p < 200 mm Hg forced
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E193/EI35
circulation of air increased the oxydation rate, this effect
becoming more pronounced at higher temperatures. The activation
energy of the process studied was 18 and 4.6 kcal/mol, when the
reaction took place in air below and above 4oo OC, respectively,
and 17 kcal/mol for oxydation in oxygen below 400 OC. The oxide
film formed on uranium in air at room temperature had a
crystalline structure and consisted exclusively of U02, The
constitution of scale formed on uranium in air at 26o-4oo OC was
determined by the present authors in an earlier investigation:
the -composition of the consecutive layers starting from metallic
titanium (Umet) is
U (met) -) a UO 2 --- ) CE UO 2+x UO2(U409 U307 -> U 308
Although the molecular volume, Uo, of uranium oxide is larger than
the atomic volume, Um, of uranium, the oxide scale formed on this
metal does not protect it from further oxydation. This is
attributed by the present authors to the coarsely-crystall-ine
nature of the oxide film formed at room temperature$ and also to
the fact that large internal stresses are set up in the oxide film
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E193/E135
owing to the large difference between the specific volumes of the
uranium oxide and uranium whose ratio varies between 1.9 and 2.6.
To determine the relative roles played in the oxydation of
uranium by the diffusion of oxygen and metal, tests were carried
out in air at 350 OC on specimens fitted with inert platinum
markers in the form of 0.02 mm thick wire; irrespective of the
duration of the test, the platinum marker remained on the surface
of the oxide scale. The results of the present investigation are
discussed in relation to various published data and it is
concluded that diffusion of oxygen through the dense triplex
QU02---)'aUO2+x7-'NPU02(U409) layer of oxides with a cubic crystal
lattice which adheres strongly to uranium, governs the kinetics of
oxydation of uranium. There are 4 figures and 15 references:
10 Soviet-bloc and 5 non-Soviet-bloc. The English language
references read as follows;
Ref.5: N.B. Pilling, R.E. Bedworth. Inst. Met., 529, Vol.29, 1923.
Ref-7: P. Blackburn, 1. Weissbart, E.I. Gulbransen. Phys. Chem.,
1958, voi.62, 8.
Ref.10: F.I. Gronvold, Inorg. Nucl. Chem., 1955, Vol-1, 357.
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concerning the mechanism of oxydation. S/126/61/012/003/011/021
E193/EJL35
ASSOCIATION: Urallskiy politekhnicheskiy institut im. S.M. Kirova
(Ural Polytechnical Institute imeni S.M. Kirov)
SUBMITTEDt February 6, 1961
Am
T
gpeH.q, NUv

BESS0140V A,V - VLASOV, V,G,
$ 0 2
Interaction of uranium metal with carbon dioxide. Piz. met. i
metalloved. 12 no.5-.775-778 N t6l. (MIRA 14:12)
1. Urallskly politekhnicheskiy #otitut imeni S.M.Korova.
Uranium-Metallography)
Mxbon dioxide)

22522
S/080/61/034/001/003/020
A057A129
AUTHORS: Vlasov, V.G., and Shalaginov, V.N.
TITLEt Reduction of Uranium Trioxide by Carbon Monoxide
PERIODICALt Zhurnal Prikladnoy Khimii, 1961, Vol. 34, No. 1, pp. 20-27
TEXT: Indirect reduction of higher uranium oxides by carbon monoxide is
important in the technology of uranium metal, since uranium oxide with a
very clean surface.can be obtained. Only one note exists in literature by
D. Katz and E. Rabinowich (Ref.l: The Chemistry of Uranium, National Nu-
clear Energy.Series)o stating that uranium trioxide (but not U308) is quickly
reduced by CO at 350 C. The purpose of the present study was to determine
the reduction kinetics of uranium trioxido in CO gas. Amorphous uranium
trioxide powder, prepared by heating UO4 -nH20 in oxygen (6 hrs at 4000C) and
carbon monoxide obtained by decomposing formic acid with sulfuric acid, were
used in the experiments Investigations were carried out in a high-vacuum
apparatus (pressure 10-4 torr) containing a quartz microbalance to control
continuously the lose in weight of the uranium trioxide sample. At 2500C
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Reduction of Uranium Trioxide by Carbon Monoxide A057/A129
and 9CO = 200 torr in ~ hrs no considerable reduction of U03 by CO tiakes
place, while above 400 C the reduction is too fast to be controlled. Thus
two series of experiments were carried out - one with an initial CO pressure
(pC~) of 200 torr at temperatures from 2600-4000C to investigate the effect
of emperature, and the other series at 3000 and 4000C changing PCO from 15
to 400 torr to determine the effect of CO pressure. The obtained rate curves
~'_'or the first series are given in Fig.20 and for the second in Fig. 4,5.
Activation energies were calculated and the following results obtained:
Degree of reduction in % 6 33 6o 75
apparent activation energy
in kcal/mole 30.7 30.7 23.3 25.3
Fig.2 shows that the maximum reduction rate is observed at 20-28% of re~pc-
tion. With rising temperature a shift of the maximum towards higher deirees
of reduction is observed. The rate curves in Fig.4 and 5 indicate the de-
pendence of total reduction rate (v) on the initial pressure of CO (pCO). At
a given degree of reduction and at constant temperature v = X-p,,, where the
coefficient K is a function of the temperature and degree of re uction (Fig.
6). The results of the,present paper demonstrate that reduction of UO* by
CO occurs easily at 300*C. Since UO 3 dissociates in high vacuum above3 4200C,
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Reduction of Uranium Trioxide by Carbon Monoxide A 0 57/A1 29
dissociation cannot be an intermediate state in the indirect reduction of U03
The boot explanation of the present results can be given on the basis of the
adsorption-catalytic theory of reduction of metal oxides by G.I. Chufarov and
Ye.P. Tatiyevskaya [Ref.7t "Problemy metallurgii" ("Problems in Metallurgy")
Izd.-AN SSSR (Ed. AS USSR) (1953), or Ref.8: "Fiziko-khimiche~ekiye osnovy
domennogo proizvodstva i covremennaya praktika proizvodstva chugunall ("Phys-
ico-Chemical Principles in the Blast-Furnace Production and Modern Practice
of the Cast Iron Production") Sverdlovsk (1955)]. The different stable and
non-stable phases-of the system uranium-oxygen have to be considered simul-
taneously. G. Brauer [Ref.2: -'Rukovodstvapopmparativnoy neorganicheskoy
khimii" ("Manual of the Preparative Inorganic Chemistry") IL, M (1956)] as-
sumes that the composition of amorphous uranium trioxide can change continu-
ouoly until the formation of U02.~6. Then formation of U 30 starts. In the
present investigations reduction 1z --- * U02 92 occurred wigh constant rate,
i.e., under kinetic conditions. In"this stem there was no formation of a new
phase, hence the limiting stage is the surface reaction between carbon mon-
oxide (
,adsorbed on uranium oxide) and oxygen of the uranium oxide. This
provea the observed dependence of the total reduction rate on the initial
carbon monoxide pressure. The rate of surface roaction is independent of the
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Reduction of Uranium Trioxide by Carbon Monoxide A057/A129
degree of oxygen removal apparently due to some factors like the formation of
defect places and low diffusion resistance. With the formation of the new
phase U02.92 crystallo-chemical transformations start between the new and the
old phase, i.e., the phase boundary catalyzes the process and autocatalysis
occurs. Rate curves in Fig.3-5 decrease until UO 2.55 is formed. The latter
is the lower limit of the U 308 phase according to G. Hoekstra and S. Sie-
gel [Ref.q: Reports of the 1st International Conference on the Peaceful Uses
of Atomic Energy, in Geneve, VII,483 (1957J. In the next reduction stage the
new phase U4 0~0002;25) is formed, i.e., change in reduction degree from 45 to
75% occurst 2 + Co---+ U09 25 + C02 under kinetic conditions. Then in
step 02.25-1,0' t;2,x ~' U02, 1'.e., change in degree of reduction from 75 to
100%, oxygen is introduced into the cubic dioxide lattice according to Ref.9
and Ref.11: R. WillardBon, I.. Moody, H. Goering, J. Inorg.Nuclear Ch., 6,1,
19-33 (1958), and Ref.12s A. Arrot, I. Goldman, Phys.Rev., 108,4,948-953
(1957), disordered in the first and ordered in the second stage. The slowest
stage is the oxygen diffusion into the solid phase and herewith stage U02,2
~p U02 is a diffusion-controlled process. This statement corresponds wita
the present experimental data. Briefly, the whole investigated process oc-
curst from UO 3 to U02.92 with a rate independent of the reduction degree,
Card 4/10

-22522
S/080/61/034/001/003/020
Reduction of Uranium Trioxide by Carbon Monoxide A057A129
from U02*92 to U02.55 autocatalytioally, from U02-55 to U02.25 again with
constant rate and from U02.25 to U02 with a rate decreasing with increasing
degree of reduction. There are 6 figures and 12 references: 7 Soviet-bloc
and 5 non-Soviet-bloc.
SUBMITTED: June 15, 1960
Card 5/10

22523
S/08OJ61/034/001/004/020
A057/A129
AUTHORSt Strekalovskiy, V.N., Vlasov, V.G.
-----------
TITLE: Kinetics of Reduction of Uranium Trioxide by Hydrogen
PERIODICAL: Zhurnal Prikladnoy Khimii, 1961, Vol. 34, No. 1, PP. 32-38
TEXT: The purpose of the present investigation was to extend the knowledge
of the mechanism of indirect reduction of metal oxides, in particular of the
kinetics and mechanism of uranium trioxide reduction with hydrogen gas.
Since indirect reduction of UO is thermodynamically possible until U02 only,
the part between UO 3 and U02 01 the.uranium - oxygen phase diagram was of in-
terest. Reduction of UO to U02 is important f0 uranium production [Ref.1,
G.A. Meyerson, Atomnaya Lergiya, 7,2 129 (1959T, but literature contains
only' information on the prep~tation of U02 with particular properties [Ref.2.
D. Katz, E. Rabinowitch, Chemistry of Uranium, N.N.E.S.; Ref-3, G. Seaborg,
D. Katz, The Actinides, N.N.E.S.; Ref.4, D. Vaughan, I. Briedge, A. Allison,
C* Shirartz, Ind.Eng.Chem., 49,10,1699-1700 (1958); Ref-7, I. Maly,,H. Lands-
persky, Iaderna Energie, 4,1,9-18 (1958A and no data are given on the whole
Card 1/10

22523
S/080/61/034/001/004/020
A057/A129
Kinetics of Reduction of Uranium Trioxide by Hydrogen
mechanism and kinet-ics of this process. In the present paper experimental
results on the reduction-of U03 by hadrogen at temperatures of 350 0- 5000C and
hydrogen pressures of 50 400 torr are given. The used amorghous U03 powder
was prepared by heating UO nH20 in an oxygon otream at 350 C during 5 hre
with final heating at 4000~*for I hr. The inveatigations were carried out in
a high-vacuum circulation apparatus with a tungsten spring balance. Hydrogen
was circulating through the system con"inuouely, while temperature was re-
gulated by an electronic 0B.-Ol (EPV-01) thermoregulator and controlled by a
TTTT (PP) bridge. From the experimental data "reduction degree versus time"
curves were plotted (Fig.2_3). Two series of experiments were made: one at
temperatures from 3000-5000C and a hydrogen pressure of 200 torr, the other
at 4000C and pressures from 50 to 400 torr. The dependence of the reduction
rate on the reduction degree (Fig-4,5) indicates that in the beginning of the
process at hydrogen pressures from 100 to 400 torr the dependence of the re-
duction rate (v) on the hydrogen pressure (pH ) at constant temperature can
be expressed by v = k F, . This was also 2observed in investigations intc
Card 2/10

22"; 2 3
S/080/61/034/001/004/020
A057/A129
Kinetics of Reduction of Uranium Trioxide by Hydrogen
reaction kinetics of lead-, cadmium- and tin-oxides In hydrogen [Ref.13:
G. Bj6rling, Svensk.Kem.Tidskrift, 67,6-7,319 (1955A. The apparent activa-
tion energy for this reduction stage (first horizontal part of the curves in
Fig-4,5) was calculated with 20.8 kcal/mole. The second reduction stage re-
presents a sharp decrease in reduction rate. In this step the total compo-
sition of the solid phases does not change essentially (see Tab.1). The de-
crease in reduction rate is apparently due to the decrease in oxygen concen-
tration in the solid phase. It is possible that a simultaneous decrease of
hydrogen adsorption occurs. Hence the total rate of reduction decreases. In
the last stage of reduction the reaction rate is constant again (except the
rate curve for 5000C and p H - 200 torr) and is expressed by v = kl*Pff . At
4000 and 4500C these horizoRtal parts of reduction curves (Fig-4) corr9spond
to the reduction Of U02 6tx phase until the tetragonal phase. For this stage
(706 reduction) the activation energy is 30 kcal/mole. The composition of
reaction products (Tab.2) demonstrates that reduction did not proceed until
formatien Of U02, only at 5000C reduction went further than U409 . The reason
why on the curve for 5000C (Pig-4) reduction from UO 3 to UO 2.47 occurs with
Card 3/10

22523
S/060/61/034/001/004/020
A0571A-29
Kinetics of Reduction of Uranium Trioxide by Hydrogen
constant rate Must be explained by additional investigations. Katz and Pabi-
nowktch (Ref.2) stated that amorphous U03 crystallizes when stored for a long
time. In the present investigations amorphous U03 was stored for 1.5 years
and another sample was heated at 4000C and no crystallization was observed.
Thus in the present work amorphous UO was reduced. Dissociation of UO oc-
curs above 4300C [Ref.12: Biltz, W., 3Willer, H. Z.anorg.Chem.,163,258 ?1927)1
thus in the present investigations UO 3 did not dissociate. The obtained re-
sults indicate that reduction of amorphous UO with hydrogen until formation
of U308 is controlled by the surface reaction etween adsorbed hydrogen and
the oxygen of the oxide. Adsorption occurs with sufficient high rate, reac-
tion equllibrium is formed and the adsorption isotherm can be expressed by
a ~ kl.pyz (a = hydrogen concentration on the surface of the oxide, 1/2 means
at
th 2 hydrogen is dissociated to atoms - according to Ref.17, F.F. Vol'-
kenshteyn, Usp.fiz.nauk, 50,2,257 (1956) . P.W. Jacobs, P.S. Tompkins, Chem-
istry of the Solid State, Bullerworth,chap.7, London (1955) (Ref.18) stated
that the surface reaction is developing with a constant rate. This is in ac-
cordance with the present results, since in all cases reduction from UO 3 to
Card 4/10

A129
K~netics of Reduction of Uranium Trioxide by Hydrogen
U308-occurred at constant rate. There are 5 figures,.2 tables, and 18 re-
ferences: 9 Soviet-bloc and,q non-Soviet-bloc.
SUBMITTED: April 7, 1960
Figure 21
Dependence of the degree of reduction
on time at different t6mperatures
(PH = 200 torr)
2
A - degree of reduciion in %
B - time in min (vaAid also
for Fig 3)
Card 5/10
20. .70 40

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F-fra 2 Cf alkal,' th., kinetics
of ursridum I-r-isl-Ad6 wilth :arblun monoxide. Kin. i
(M-ERA J-7s:8)
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TITLE! Invesiti9dtion
based on_2012Lglyrene
aly. 'VYP-
atory i stsintillyats.-materi
1 Cl-rED SOUPCE: sb. sts1ntij_lY
1963, 85-90
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3. Khark
scintillation efficiency, _,icin-
TCipIC TAGS: plastic scintI-.Ilator,.
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lator aging, polystyrene, Organ-3-
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(pS):by different factors, Such
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order to develop
-Card 1/3
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ACCESSION MR i AR50056_`~l
ture of PS, it st,-xdy was made of the stability of PS in time. The
-PS we-re prepared by poiymerizat4.o- 4:~f styrene with additive's of PPP
(21Y.) and POPOP (0.06% at T - 200, 1-70, 140, 1251 and durationa (t)
of 100, 70, 50, 32, 24, 16, and 8 hours. Standard samples 16 i=
n IJ I -un e t e r u)1 r-,, m ]h I -_, h, w e r e t r2ene relative scirL.tillation
e f f i e r M -1 r-. ~'_ UIi r, C , r C a:~ FEQ-29
plotting the indicest the samples -were stored under different condi-
tions: without exposure to light at T 0, 20-25, - 40, 60--7'0*,
natural elimination at T = 70', and also at increased humidity.
years, wJ th them S Ple
1-The observations wei~e carried out kior 1.5-2.51 am
Inspected visually and measured every six months. It was established
that it is necessarv to ensure minimum content of the residual mono-
mer in the PS. The best PS were those manufactured at T = 170-1800
and t 32 I-iours, for blocks 20 mm in diameter (t increases w:,;.th
efficiency during .2.5
-and--:- al-Ero-Under- don-
1 'Y~daks# in the, e 6f I Cj eit t
r
2/1

AUTHORSt Strekalovskiyt V.N., Vlasov, V.G.
TITLEt Reduction of U 308 by Hydrogen
3/080/61/034/001/005/*020
A057/A12q
PERIODICAL: Zhurnal Prikladnoy Khimii, 1961, Vol. 34, No. 1, PP. 38-43
TEXTs The present work is a kinetic study of the reduction of U 0 by hydro-
0
gen gas at 450 _7000C and hydrogen pressures of 20-400 torr. Reluchion of
U 0 in hydrogen is used in uranium technology, and for the preparation of
U82800 or U40 Kinetics and mechanism of this process were studied insuf-
ficiently unt?i noir. The opinion of some American investigators (Ref.2t
D. Katz and E. Rabinowitch, ~!he Chemistry of Uranium, N.N.E.S., Div. VIII,
v-5) that the reduetion of U308 in hydrogen occurs in two steps contradicts
the modern view on the mechanism of indirect reduction of metal oxides. A
recent publication by S. Andorson and J.C. Clayton [Ref.6t J.Inorg.Nuclear
Chem.,7,4 (1958)] on reduction of U409 is of interest, but it contains only
data concerning the last stage of reduction from U308 to U02. The present
Card 1/8

Reduction of U308 by Hydrogen
5~1034/001/005/020
S/060761
A057A129
investigation was made in a high-vacuum-circulation apparatus (evacuated to
10-4 torr) incorporating a recording vacuum balance. The investigated
"green" U 0 was obtained by heating U03 (specific surface area 4.1 m 1g) at
6000C. Tgeerate oT the reduction process was controlled by the weight de-
crease of the U308 sample (weighing approximately 0.25 g). All experiments
were carried to complete ceasing of reduction in a time period between 2.5
to 375 min. Typical rate curves for the effect of temperature and reduction
rate are given in Fig.1 and 2 [Abstracte?s note: in Fig.1 erroneously 50 mm
Eg is printed instead of 200, and in Fig.2 200 mm Hg instead of 50 mm HGI
while the ef'ect of hydrogen pressure is demonstrated in Fig-3 (in the fig,-
ur~s A -reduction rate in 76 reduced per min, B = total composition of the
solid product of reduction, and C w degree of reduction in ~). Reduction
occurs with relatively constant rate at 200 torr hydrogen pressure and below
6000C (Fig.1). At 6000C and 05000C reduction rate is constant until solid
UO is formed, and at 450 C until formation of U02,~2. After this the
ra~ A5 aeoreases until U02 15 is formed, then a relativ y constant rate re-
mains until the product ; the composition U02 -U02.28 is formed. The rate
curve for 6500C is in the beginning somewhat dl~ferent from the last-mention-
ed curvas. Rate curves in Fig.2 start with a characteristic increase in the
Card 2/8

Z-2524
S/OBOJ61/034/001/005/020
Reduction of U 0 by Hydrogen A057/A129
3 8
reduction rate, but are otherwise similar to those at 200 torr hydrogen pres-
sure. The rate curve for the reduction at 6000C and 400 torr hydrogen pres-
sure (Fig.3) is unique starting with maximum rate and decreasing continuous-
ly until zero. The following values of apparent activation energy were cal-
culatedt
hydrogen pressure in torr 200 50
degree of reduction in % 10 40 15 40
activation energy in kcal/mole 21-4 20.6 17.4 15.2
In the discussion the authors point out that there is no unique opinion about
the nature of solid solutions in the uranium - oxygen system (see R. Rundle
et al.,Ref.11i J.Am4hem.Soo., 70,99-105 (1948) and H. Hering and P. Perio,
Ref.12: Bull.Soc.Ohim.France, 351-357 952) which consider UO as lower
limit of the chase UO while F. Gr~nlvold, and H. Haraldsen 2.agf.8 : Na-
2 6tx1 p
ture, 162,69 f1948) an& H.R. Hoekstra and S. Siegel, Ref.13s Reports of
the Ist International Conference of the Peaceful Use of Atomic Energy, Geneve
(1955) suggest U02 56 as limit) as well as concerning the limit of solubility
orming non-stoichiometz
of oxygen in U02'f* -ic UO +X [see D. Vaughan R Wil-
lardson, Ref.141 Preprint Nucl. Energy a.Sci.Wf.s.a., 13,15 (19'58)). Cor-
responding to A.A. Baykov s principle of sequence of chemical reactions [Ref.
15: Metallurg, 3,5 (1956;1 the present authors consider the following scheme
Card 3/8

z2524
S/080/61/034/001/005/020
Reduction of U30a by Hydrogen A057/A129
of phase transition valuable for T>65000C:
U308 )'1U02.6-ix--P U409 *U02+x 0 U02 (where x - m6 - 0.14)
The first step occurs under kinetic conditions and is controlled by the sur-
face reaction between adsorbed hydrogen and the oxygen of the oxide. During
reduction the crystal lattice is disordered and new active centers formed (by
chain mechanism), which increase the surface reaction rate, Simultaneously
oxygen concentration in the surface layer of the oxide dacreases and inhibits
the surface reaction. The beginning of the reduction is controlled by the
formation of active centers, thus reduction rate increases with degree of re-
duction. Herewith the increase in the reduction rate (Fig.2) at the beginning
can be explained, while at hydrogen pressures of 200 torr (Pig.1) this step
is so fast that it cannot be observed experimentally. When both above-men-
tioned factors are in equilibrium the reduction process has a constant rate.
The continuous decrease in reaction rate at the end of the reduction stage of
the phase U02 3�, (successive transition into the phase U02.6-xmtx ) can be
explained by de fact that the number of newly formed active cen ets is limit-
ed, while the concentration of oxygen in the condensed phase decrease with
the progress of the reduction process. In literature U02.6�x is considered
to be the lower phase limit and in the present experiments the reduction rate
Card 4/8

22q24
S/080/61/034/001/005/024D
Reduction of U 0 by Hydrc~gen' A057/A129
3 8
stopped to decrease with.the oxide U02.45' This difference can be explain-
ed by the fact that the reduction process did not occur-in single zones.
The second horizontal part of the.rate curves.in Fig-1-3 corresponds to the
phase iraneitio"n Of U02.6-xmax__"'U409. If f&mation of U409 is due to a
well-regulatedland formation Uf U023-xmax. to a non-regulated introduction
of oxygen into the cubic lattice of uranium oxide (see Ref.13) there should
be no great change in the crystal lattice, and oxygen evolution should occur
successively. This is ,the reason that in this step the reduction rate de-
creases.continuously with the progress of the process. Apparently this step
occurs under diffusion conditions, controlled by the diffusion of oxygen to-
wards the place where the-reaction occurs. There are 3 figures and 16 re-
ferences: 9 Soviet'-bloc and 7 non-Soviet-bloc.
SUBMITTED: May 10,'1960
Card 5/6

S/080/61/034/008/005/018
D204/D305
AUTHORS.- Vlasov, V.G. and Lebedyev, A.G.
TITLE: The dissociation kinetics of uranium oxides
PERIODICAL: Zhurnal prikladnoy khimii, v. 34, no. 8, 1961,
1739-1744
TEXT: The present work was undertaken because of the lack of in-
formation on the kinetics and mechanism of the dissociation pro-
cesses of uranium oxides, Knowledge of these would be of interest
for technological. processes, based on the dissociation of oxides
as well as being examples of a topochemical process. Specifically,
U03 and L1308 were investigated- U03 was prepared by heating U04-
nH20 in a stream of 02 for 3 hours at 3500C, followed by I hour at
400OC; the resulting product was finely ground and pelletized U 0
was prepared by heating t~ 11 1
in 0 OUOOH~o in air for I hour at 8000C and en
2 for I hour at 900 C: this product was pulverized ~nd used in
a poiMery form, Dissociation processes were followed by continuous-
ly recording the loss of weight of the heated oxides by means of a
Card 1/4

'L ~ ~ L _'
S/080/61/034/008/005/018
The dissociation kinetics... D204/D305
spring balance. The initial rate of dissociation was determined by
the angle of the tangent to the curve of oxygen removal plotted
against time. The apparent activation energy was calculated from
Arrenius' equation. Results: U03 dissociates at a convenient rate
at 450-6500C, while complete conversion into U308 was reached only
at 5500C and above. At 4500C, U03 dissociates at a constant rate,
following the equation. g -a 0.168 t (g - degree of dissociation,
t time elapsed from the onset of the desired temp. min). At
g 42%. the rate diminishes abruptly and then becomes constant, as
shown by equation: g a 0.091t + 17.90. At 5000C, the initial rate
follows equation ~ a t 1 9 and after g = 30% dissociation is expres-
sed by (g - 30) - 15.3 (t - 21). At 53000 the expression is g
4.65t + 40.9 until g = 65% and thereafter Ig 10_0_1~zg - 0.0608.
The influence Of 02 at various part. pressures, on the rate of dis-
sociation of U03 was investigated and found to be represented by
equation: v - A - kP02 , where A and k are constants at a given
temperature. The apparent energy of activation, calculated from
Card 2/4

J
3/08 61/034/008/005/018
The dissociation kinetics- D204yrj3O5
g 307* was 37.2 Kcals/mole. U~08 at 7000C dissociates at a con-
stant rate, following the equation. g = 0.03 t, 4~t 8000C the cor-
responding expression is Ig - k t, (a - degree of dissociation,
a - g 1
corresponding to the conversion U30,,, --PUC)2~6 -,, ot a mi,.-dmunl
oxygen content, i.e,. U02.55); a is 1-1,9-,", and valuer. of Icl. at 800,
900 and 100001~ a-j~e 3,08-10-3, and 1,97-LO-2 respectivelv- Beyond
a m 18',; dissociation proceeds at a constant rate and is represented
by., g = k2(t - 1:0) - 18, where to 'is ttle time required for reaching
g - 18"n and k2 - a constant at a given temperature, v')lues of 1'2
and to are given below-..
temp. toi,'" 1000 900 800
k2 0.1 0,06 0,04
to (min) 70 165 330
There are 3 figures and 10 references. 7 --,oviet-bloc arnd 3 non-60v-
iet-bloc., The references, to the publications read
as follows. V, Gronvol,-Ii, J, Tnorg. Nucl, ;iiem- 1, 351' (195.5 , 'Zhe
Card 3/4

/080/61/034/008/005/018
The dissociation kinetics., ~j20411)305
Transuranium 11-lements, Oart If, Papers 6,, 40 to 22, 80, 6'61, New-
York - Toronto - !,ondon (1949).
SUBMITTi-A) October 3, 1960
Card 4/4

0
AUTHORS:
TITLE:
Beusonovil A. F., Vlasov, V. G.
339932-
s/14 4/vw/VV4/002/003
AOO6/A101
Kinetics of uranium oxidation with air, oxygen and carbon dioxide
PERIODICAL: Izvestiya vysshikh uchebnykh zavedeniy, Tsvetnaya metallurgiya,
no. 4, 1962,- 137 - 142
TEXT: Oxidation of uranium metal was studied in aggressive gas media at
various temperatures aiA~ pressures of the oxidizing gas, for the purpose of ob-
taining kinetic characteristics and revealing the mechanism of t 'he process. Com-
mIercially pure uranium:.j4etal plates (2.5xl.5xl.5 mm) were oxidized in a high-vac-
u4m device. The true ratp of the oxidation process was granhically determined from
tITe inclination angle of'-,the tangent to the"oxidation-degree-versus-time" curve,
The apparent activation;-~nergy was calculated with the aid of the Arrhenius equa-
tibn. The average composition of the oxidation product was determined by calculat-
ing the increase in weight of the specimen during oxidation and the loss in weight
during reduction with hydrogen. It was found that the oxidation process in all the
given ag~resslve media obeys the tempora17 linear law; the rate of the process is
proportional to the square root from air and oxygen pressure. The possible mechbn-
ism of the uranium oxidation is analyzed with the aid of Soviet and foreign
Card 1/2

S/1 49/6L/000/004/002~00 3
Kinetics of uranium oxidation with air,... A006/A101
sources (Ref. 9: P. Chiotti, H. Klepfer, R. White. Trans.Amer..So'c.Metals, 51, 772
(1959)). It was found that the diffusion oi jxygen atoms through a dense layer of
uranium dioxide was the decisive limiting stage. There are 4 figures.
ASSOCIATION: Urallskiy polite*khnicheskiy institut (Ural Polytechnic Institute)
SUEMITTED: July 25, 1960
Card 2/2

S/149/62/000/005/004/C,08
Aoo6/Alol
AUTHORS: Vlasov, V. G., Bessonov, A. F.
TITLE: Oxidation of uranium dioxide
PERIODICAL: Izvestiya vysshikh uchebnykh zavedeniy, Tsvetnaya metallurgiya,
no. 5, 1962, 113 - 122
MIT: Since the opinions of scientists differ on the mechanism of the
oxidation process of uranium dioxide, the gathering of experimental data in this
field is imperative. The authors studied kinetics of uranium dioxide oxidation
in different gas media and investigated simultaneously the effect of the admix-
ture of alkali metal carbonates and Th03, ZrO2 and T102 oxides upon the kinetic
characteristics of the oxidation process. Kinetics of oxidation with air oxygen
was studied within a range of 165 to 8000C, at 2.5 - 600 mm Hg atmospheric p'res-
sure. The results are shown in Graph (2). Determined values of the apparent ac-
tivation energy at different oxidation degrees range from 34.6 kcal/mole at 28%
oxidation to 39.4 kcal/mole at 90% oxidation. Kinetic characteristics of U02
oxidation,*with pure oxygen were investigated in a range of 125 to 3300C and
Card 1/6

Oxidation of uraniim dioxide
S/14q/62/OGO/005/GC4/CC8
Aoo6/A101
pO2 = 100 mm Hg. The following schemes of phase transformations are proposed-
U02. Oil _--` U02+xmax -t' U02.25 - U02) .36+0.05 -7 U02.6 -xmax ---;O'UO2.67 for the 260 to
3900C range, and U02. oil --> UO,-> for the 400 to
.+x max ---~ U02.25 -il U02.6-xmax --~IUO2.67
8000C range. The effect of different admixtures upon the process Is given in
Figures 5 and 6. Due to the liberation of considerable amounts of heat In oxida-
tion Of U02 to U3081 local overheating occurs in the solid phases, enta:11ing a
sharp increase in the process rate on these spots, so that several phase transi-
tiorfs take place. This explains the jumplike evolution of the process in the
150 - 2000C range. The inhibiting effect of K2CO admixtures on U02 oxidation
at 1850C is apparently due.to the fact that at tPs temperature the migration of
potassium ions from the carbonate crystal lattice into that Of U02 is little
probable. Simultaneously the admixture is in a close contact with U02 and screEm
a portion of its surface. As a result, the surface for oxygen adsorption from
the gaseous phase is reduced and the total rate of the oxidation process de-
creases. At 33000. the accelerating effect of alkali metal carbonates appears on
those stages where a substantial reconstruction of the crystal lattice takes
place. Apparently the catalytic effect of carbonates consists in the fact that
Card 2/6

Oxidation of uranium dioxide
sl 14 q/62/oco/oo5/or,,4/bc-8
Aoo6/Aloi
their particles,are crystallization centers of a new phase which eliminates the
induction period. There are 6 figures.
ASSOCIATION: Ural'skiy politekhnicheskiy institut (Ural Polytechnic Institute)
SUB14ITTED: April 22, 1961
Card 3/6

Ox-idation'of uranium dioxide
Figure 2.
Card 4/6
s/14q/62/OoA/oO5/oo4/or,8
Aoo6/Aloi
Isotherms of U02 oxidation with air oxygen (at constant 200 mm llg air
pressure)
rb
- ---------
1
jjj
M
. . . . ...

Oxidation of uranium dioxide
.5/149/62/000/005/004/008
A0061AI01
Figure 5. Isotherms Of U02 oxidation with air oxygen at 1850C (1 and 2) and at
3300C (3 - 6) without admixtures (2 and 3) and with admixtures of
K2CO3 (1 and ll~ Na?C03 (5); L12CO3 (6).
V)
cd
2p
Z3
0 '%
0
4a
0
4J
2'13
Card 5/6

S/149/62/OOO/(Yj5/004/008
Oxidation of uranium dioxide Aoo6/Alol
Figure 06. Isotherms of U02 oxidation with air oxygen at 330OC-without admix-
ture (1) and with admixture of ThO2 (2); Zr02 (3) and T102 (4)
,7.67
91
cd
X;
2,A 9
0
2.44
.CA" 4
"i~ Z.27
olz~
.H.% [z
+3
(d
43,
0
X
0
Card 616
IN