Abstract
The hydrogen-oxygen reaction has been studied over three dysprosium oxide catalysts at hydrogen: oxygen ratios from 0.2 to 10, at pressures of hydrogen up to approximately 600 N m −2, and at temperatures in the range 368 to 553 K. The kinetic results can best be explained in terms of an equation of the form: −dP T dt = (kb H 2 2P H 2 2b o 2 P o 2 ) (1 + b H 2 P H 2 + b o 2 P o 2 ) 3 , where k is a proportionality constant, b H 2 and b o 2 are the adsorption coefficients for hydrogen and oxygen, respectively, P T is the total pressure of hydrogen plus oxygen, and P H 2 and P o 2 are the partial pressures for hydrogen and oxygen, respectively. The most likely mechanism is one involving the competitive adsorption of molecular hydrogen and oxygen, with the rate-determining step involving the interaction between H 2O 2(ads) and H 2(ads). There is a change in the availability of sites at approximately 430 K, with the effects of excess gas and the activation energy changing at this temperature.
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