Abstract
The electrochemical reduction of hydrogen peroxide has been studied on uranium dioxide electrodes. The reduction kinetics are found to be influenced by dissolved carbonate/bicarbonate ions. The formation of hydrated U VI species on the electrode surface is avoided in carbonate solutions, allowing H 2O 2 reduction to proceed at less cathodic potentials than in carbonate-free solutions. At more cathodic potentials, the adsorption of carbonate ions on the active reduction sites inhibits the H 2O 2 reduction reaction. Over a narrow potential region, the reduction of peroxide is catalyzed by coadsoption of H 2O 2 and HCO 3 −/CO 3 2−. The pH dependence of the H 2O 2 reduction reaction appears to be stronger in carbonate solutions than in solutions that do not contain carbonate. This can be attributed to the displacement of inhibiting CO 3 2−/HCO 3 − adsorbed ions by OH −.
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