Abstract
Abstract The oxidation of boronated graphite occurs by two competing reactions in the temperature range 580–780°C, namely, the oxidation of carbon to yield CO2 and the oxidation of B4C to yield B2O3 and CO2. The former reaction is appreciably faster than the latter. The formation of molten B2O3 yields a physical barrier to reactant diffusion and, in the case of grey boronated graphite, leads to a maximum in the rate as a function of time. Because less B2O3 is formed in black boronated graphite, it behaves much like ordinary nuclear graphite. Upon removal of the B2O3 by leaching in boiling water, the oxidation rate is appreciably increased. This is particularly true for the grey boronated graphite, because the amount of B2O3 formed is greater than in black boronated graphite where the B4C is apparently not as accessible to the oxidant.
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