Abstract
The kinetics of oxidative dissolution of RuO2·xH2O to RuO4 by CeIV ions are studied. Under conditions of a low [CeIV] : [RuO2·xH2O] ratio (e.g. 0.35 : 1) and a high background concentration of CeIII ions (which impede dissolution) the initial reduction of CeIV ions is due to charging of the RuO2·xH2O microelectrode particles. The initial rate of charging depends directly upon [RuO2·xH2O] and has an activation energy of 25 ± 5 kJ mol–1. Under conditions of a high [CeIV] : [RuO2·xH2O](e.g. 9 : 1) and a low background [CeIII] the reduction of CeIV ions is almost totally associated with the dissolution of RuO2·xH2O to RuO4, i.e. not charging. The kinetics of dissolution obey an electrochemical model in which the reduction of CeIV ions and the oxidation of RuO2·xH2O to RuO4 are assumed to be highly reversible and irreversible processes, respectively, mediated by dissolving the microelectrode particles of RuO2·xH2O. Assuming this electrochemical model, from an analysis of the kinetics of dissolution the activation energy for this process was estimated to be 39 ± 5 kJ mol–1 and the Tafel slope for RuO2·xH2O corrosion was calculated to be 15 mV per decade. The mechanistic implications of these results are discussed.
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