Abstract
The oxidation of l-ascorbic acid has been studied in sulphuric acid solutions at a bright platinum electrode, by employing cyclic voltammetry, controlled-potential electrolysis and potential-step measurements. On the basis of kinetic parameters—Tafel slopes, reaction orders and pH effects—a possible mechanism is proposed for the overall oxidation process. There is evidence of two rapid and thermodynamically reversible charge-transfer steps which are followed by a slow non-activated desorption and rate-determining step. The kinetics are explained with the aid of the Temkin adsorption isotherm.
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