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AE-192 UDC 541.15:547.53

CN O LJJ Radiolysis of Aqueous Benzene Solutions in the Presence of Inorganic .

H. Christensen

AKTIEBOLAGET ATOMENERGI STOCKHOLM, SWEDEN 1965

AE-192

RADIO LYSIS OF AQUEOUS BENZENE SOLUTIONS IN THE PRE- SENCE OF INORGANIC OXIDES

Hilbert C . Christensen

Abstract

Aqueous 0.1 N alkaline solutions of benzene have been irradiated with Co y-rays in the presence of various inorganic oxides. The ad- dition to the solution of silica gel, (ll) and (lll) oxide did not increa.se the yield of phenol. When chromium(lll) oxide gel, oxide or dioxide were added, we obtained a 9 - 1 3 per cent increase, and the addition of dioxide and dioxide caused a 31 and 39 per cent increase3 respectively. The-in- crease of the phenol yield was related to the energy absorbed by the solid, and G r values defined in this way were calculated as follows:

G a 4 j = 3 7 G = 6 4 and G 8 The ZnO -° S-iO3 ' ' UOS ' ThO3 = *°- ific surface areas of the oxides were determined and the possibility that the increase of the phenol yield may be dependent on this quan- tity is discussed.

Printed and distributed in July 1965. LIST OF CONTENTS

Page 1 . Introduction 1

2. Experimental 1 2. 1 Materials 1 2.2 Irradiation procedure 1

2. 3 Analysis 2

3. • Results and discussion 2

4. Conclusion 4

References 6

Tables 8

Figures 10 ]_. Introduction

The radiolysis of aqueous benzene solutions has been extensi- vely studied [1 -83 and Christensen [83 has recently given a review of the system. In the investigations by Preve and Montarnal [5, 6 3 and by Yumoto et al.[7 3 the effect of the addition of various semicon- ductors in alkaline solution has been studied. In this investigation we have studied the effect of the addition of inorganic oxides on the radiolysis of aqueous alkaline solutions at room temperature. In another investigation [103 results are included on the effect of the addition of oxides to the system under irradiation at higher temperatures.

2_. Experimental

lL'1. Materials

Benzene and were purified as described previously [83« and (Merck), and silica gel (Kebo), copper(ll) oxide (Baker), chromium(lll) oxide (Matheson, Coleman and Bell), and (sample from AB Atomenergi) were used without further pvirification. Chromium(lll) oxide gel was prepared by a method described in the literature [93- The specific surface area of the oxides (see table 1) was determined according to the BET method. Other chemicals were of p. a. quality and were used without further purification.

2,-2 l£

Saturated aqueous solutions of benzene made up by shaking ex<- cess of benzene with water and made 0. 1 N alkaline with hy- droxide were used for the irradiations. 50 ml of the solution and 5 g of the oxide were irradiated in a container. , saturated with benzene vapour, bubbled through the solution and a magnetic stirrer ensured good mixing of the oxide and the solution. The sam- ples were irradiated with Co y~rays in a Gammacell Z20 (Manu- facturer: Atomic Energy of Canada Ltd.). The dose rate in the solu- tion determined with the Fricke dosimeter using a G value of 15.6 was 5 700 rad/min (October 1963). - 2

After irradiation the oxide was removed by centrifugation and filtration. The solution was made with sulphuric acid and analysed for phenol according to the method proposed by Baxendale and Mageejjl], In order to ensure that no phenol disappeared by adsorption on the oxide, we made similar experiments without irradiation on solutions containing and silica gel to which a known quantity of phenol had been added. The analysis showed that no phenol was adsorbed on the solid. We also tried to ascertain whether further phenol was produced by an after-irradiation effect, but found that no phenol was produced after termination of the irradiation.

3L Results and discussion

Fig. 1 shows the yield of phenol in 0. 1 N sodium hydroxide solu- tion as a function of the absorbed dose in the range 0 -200 krad. The G value of phenol, G(Ph), calculated from the curve after a dose of 40 krad is 2. 55. In fig. 2 is shown the effect of the addition of chromium(lll) oxide, which does not increase the yield of phenol, and of chromium(lll) . oxide gel, which slightly increases the yield (table 2). Figs. 3 and 4 show the yield of phenol as a function of the absorbed dose in the pre- sence of various oxides. The G values given in table 2 are calculated as described above, only the dose absorbed in the solution being consid- ered. It is seen that copper(ll) oxide and silica gel do not increase the yield, while zinc oxide and titanium dioxide give a small increase (l 3 per cent) and thorium dioxide and uranium dioxide a greater increase (39 and 31 per cent, respectively) of the phenol yield. Fig. 5 shows the dependence of the yie,ld on the amount of added uranium dioxide. If we approximate the dose absorbed in the solid (D ) as the s dose absorbed in the liquid (Dx) multiplied by the ratio between the of the two materials, D may be calculated. In or- s der to calculate D for the oxides of the heavy metals, the dose con- s tribution from the photoelectric absorption (Dp«) was added to the dose from the Compton effect (D.-™). The contribution from pair production has been disregarded. The energy transferred to the electron by a Compton scatter- ing E«p and the ratio between the cross sections for the photoelectric - 3 -

effect and the Compton effect ?~= have been calculated from data in

the literature [12, 13]. DpE is then calculated as follows:

n n SEE ^ PE ~ CE CTCE Git-

•where f is the fraction of of the oxide belonging to the heavy metal. The increase in the concentration of phenol when an oxide is pre- sent, AC, may then be related to the energy primarily absorbed in the oxide and the G value calculated as follows: ox

r - AC J-n rnolecules per g solution 50 ox" D in 100 eV units 5 s

The results, given in table 3, disagree with the results of Preve and Montarnal [5, 6], who used 200 kev X-rays for the irradiation of 6 g of the oxide in 1 60 ml solution. They found G™ _ = 1 6 and G-, ~ = Z.nU 1 №-)% = 4. 1 , the G values being defined as above. If, however, we compare the G values of phenol calculated in relation to the energy absorbed in the liquid we get a better agreement. Thus Preve and Montarnal found

6.5 for ThOa, 4.6 for ZnO, 5.5 for TiO2, and 5.9 for CuO, while silica gel did not increase the yield over the value in the absence of oxide (3. l). Except for the yield in the presence of copper(ll) oxide our results are in qualitative agreement with these values (see table 2), as well as with the results of Yumoto et al. [7], who report an in- crease of G(Ph) from 1 . 57 to 1 . 84 in the presence of zinc oxide for the irradiation with Co y-rays. Our results in the presence of chromiurn(lll} oxide and chromi- um(lll) oxide gel indicate that the size of the surface area may be of some importance. We calculated the fraction of the oxide in a mono- molecular surface layer as shown in table 1 , and we see that for tho- rium dioxide, which gives the highest G value, this fraction is an order of magnitude higher than for the other oxides. Preve and Montarnal did not give the specific surface of their oxides. Our re- sults are thus compatible with the assumption that the specific sur- face area is important for the transfer of energy to the liquid. The _ 4 -

mechanism of the transfer of energy from a semiconductor to the liq- uid may be that proposed by Veselovsky [14]. As a result of the ab- sorption of radiation in the solid, electrons are raised into the conduc- tion band. The electrons which escape trapping may migrate to the sur- face and react with the adsorbed oxygen. OH are then discharged on the oxide which is positively charged due to the loss of electrons and as a result OH radicals are produceds which increase the phenol yield. The increase of the yield is then dependent on the number of electrons which have migrated to the surface and on the amount of oxygen adsorbed on the surface, and this amount depends on the sur- face area. If only the energy transfer as explained above is considered, the increase of the phenol yield for thorium dioxide and uranium dioxide is higher than the G values given in table 3 because most (> 75 per cent) of the energy of the photoelectrons is absorbed outside the oxide particle. However, the photoelectron originated in the oxide is totally absorbed in the oxide and the liquid, so the G values express the in- crease of the phenol yield due to the presence of the oxide. From fig. 5 it is seen that the increase of the phenol concentra- tion per g of added uranium dioxide is greatest in connection with small amounts of oxide. A calculation of the G value from the lin- ox ear part of the curve gave a value 3 times smaller and a calculation made after the addition of 1 g of oxide gave a value 3 times higher than the value given in table 2. The explanation for this may be as follows. A monomolecular layer of the oxygen molecules dissolved in 50 ml of a saturated oxygen solution would cover about 3 ms (~ 1 g) of the uranium dioxide if it is assumed that the and the oxygen surface area are about equal. Even if oxygen is continuously bubbled through the solution a monomolecular layer of oxygen would not be ex- pected in an aqueous solution, but the difference between the equilib- rium concentration and the actual concentration of oxygen on the sur- face may be larger for the larger amounts of oxide in the solution. 4. Conclusion

The addition of inorganic oxides to aqueous 0. 1 N alkaline solu- tions of benzene has resulted in an increase of the phenol yield for some of the oxides. Our results indicate that the size of the specific - 5 -

surface area may have an influence on the increase of the yield. The explanation for this may be that the oxygen adsorbed on the oxide plays an important role in the energy transfer from solid to liquid by trapping electrons which are produced by radiation in the solid and transferred to the surface. The disagreement with some of Preve and Montarnal's results may be explained by a possible difference between the specific surface areas of the oxides. The increase of the phenol yield may thus be a function of the number of the electrons transferred to the surface of the solid and of the amount of oxygen adsorbed on this surface. - 6 -

References 1. STEIN, G and WEISS, J, Chemical actions of ionizing on aqueous solutions. Part II. The formation of free radicals. The action of X-rays on benzene and benzoic acid. Part III. The action of neutrons and of a-particles on benzene. J. Chem. Soc. (1949) 3241 - 56.

2. PHUNG, P V and BURTON, M, Radiolysis of aqueous solutions of hydrocarbons. Benzene, benzene-d6} eye lohexane. Radiation Research 7_ (i 957} 1 99 - 216.

3. DORFMAN, L M, TAUB, I A and BUHLER, R E, Pulse radiolysis studies. I. Transient spectra and reaction-rate constants in irradiated aqueous solutions of benzene. " J. Chem. Phys. 36 (l 962) 3051 - 61 .

4. BARELKO, E V et al. , Radioinitiation of chain branched reactions and its sensitiza- tion. Conf. Application of Large Radiation Sources in Industry and Especially to Chemical Processes. Warsaw 1959, Proceedings J_(196O) 407 - 21, (in Russian). (French transl. CEA-tr-R 1093. English transl. NP-tr~695.)

5. PREVE, J and MONTARNAL, R, Formation radiochimique de phenol sensibilisee par les semi- conducteurs. Comp. rend. 249 (1959) 1667 - 69.

6. PREVE, J and MONTARNAL, R, Sensibilisation radiochimique par les semi-conducteurs. J. Chim, Phys. 58_(l96l) 402 - 08.

7. YUMOTO, T, LIN, H-C and MATSUDA, T, Radiolysis of aqueous solutions of benzene in the presence of anions, metals or metallic oxides. Nagoya Kogyo Gijutsu Shikensho Hokoku \± (l 962) 114 - 18.

8. CHRISTENSEN, HC5 Radiolysis of aqueous benzene solutions. NukleonikX (1965) 1-8.

9. Inorganic syntheses. Ed. : W C Fernelius. Vol. II. New York, Me Graw-Hill, 1946, p. 1 90 - 93.

10. CHRISTENSEN, HC, Radiolysis of aqueous benzene solutions at higher temperatures. To be published.

1 1 . BAXENDALE, J H and MAGEE, " J, The oxidation of benzene by and salts. Disc Faraday. Soc, J_4 (1 953) 160 - 69. - 7 -

12. American Institute of Physics Handbook. 2 ed. New York, Me Gr aw-Hill, 1963, p. 8 - 89.

13. WAPSTRA, AH, NIJGH, G J and LIESHOUT, R van, Nuclear Spectroscopy Tables. Amsterdam, North-Holland Publ. Co, 1959, p. 69.

14. VESELOVSKY, VI, Radiation-chemical processes in inorganic systems. (Electrochemical action of radiations. Sensitization of radia- tion-chemical reactions.) 1 st UN Intern. Conf. on the Peaceful Uses of Atomic Energy. Geneva 1955, Vol. 7, p. 599 - 609. (P/682) TABLE I •

Specific surface area of the oxides, determined by the BET method.

Oxide Specific % of oxide in surface a monomolecu- ms/g lar layer

Cr3O3 3.7

Cr8O3 gel 34 Silica gel 1 100 CuO 0.21 ZnO 4.0 0.6

TiOs 8.6 1.1

UO3 3.1 1 .2

ThO3 38 13

TABLE 2

G values of phenol in 0. 1 N alkaline solution.

Oxide Cr2O3 C^gOg gel SiO3 CuO ZnO TiO3

G value 2.55 2.35 2.77 2.55 2.41 2.88 2.86

Oxide UO ThO3

G value 3. 34 "3.54 TABLE 3

G values — ox

D Dose, , , Mw Electrons Electron CE D total Cone, of phenol AC G PE ox moles/g Dose in water Dose in water at 40 krad = C \i, tnoles/l

ZnO 81 .4 38 0.467 0.842 0.842 120 14 4.0

TiOs 79.9 38 0.475 0.856 0.856 U9 13 3.7 uos 270.0 108 0.400 0.721 0.522 1 .24 139 33 6.4 ThOg 264.0 106 0.402 0.724 0.510 1 .23 147 41 8.0 500 -

100 Dose (krad)

Fig. 1 Yields of phenol in alkaline solution in the absence of oxides.

500 -

100 200 Dose (krad)

Fig. 2 Yields of phenol in alkaline solution in the presence of oxides. +: Cr-O-, 0: chromium (III) oxide gel, - -; the curve from Fig. 1. 500 -

100 200 Dose (krad)

Fig. 3 Yields of phenol in alkaline solution in the presence of oxides. +; Silica gel (No curve is drawn), 0:CuO,

^7 : ZnO, EJ: ThO2, - -j the curve from Fig, 1.

500 -

so 100 200 Dose {krad)

Fig. 4 Yields of phenol in alkaline solution in the presence of

oxides. +: TiO.-,, 0:UO?J - -j the curve from Fig. 1. 500 -

„ 400 -

300 p

200

100

10 15 Weight of oxide (g)

Fig. 5 Yields of phenol in alkaline solution in dependence on the amount of UO_. Dose 120 krad.

LIST OF PUBLISHED AE-REPORTS 160. Measurements of the FeH (n, p) Mn5< reaction cross section in the neutron energy range 2.3—3.8 MeV. By A. Lauber and S. Malmskog. 1964. 13 p. 1—120. (See the back cover earlier reports.) Sw. cr. 8:—. 121. The transistor as low level switch. By A. Lyden. 1963. 47 p. Sw. cr. 8:—. 161. Comparisons of measured and calculated neutron fluxes in laminated 122. The planning of a small pilot plant for development work on aqueous iron and heavy water. By. E. Aalto. 1964. 15. p. Sw. cr. 8:—. reprocessing of nuclear fuels. By T. U. Sjoborg, E. Haeffner and Hult- 162. A needle-type p-i-n [unction semiconductor detector for in-vivo measure- gren. 1963. 20 p. Sw. cr. 8:—. ment of beta tracer activity. By A. Lauber and B. Rosencrantz. 1964. 12 p. 123. The neutron spectrum in a uranium tube. By E. Johansson, E. Jonsson, Sw. cr. 8:—. M. Lindberg and J. Mednis. 1963. 36 p. Sw. cr. 8:—. 163. Flame spectro photometric determination of in water and 124. 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