The kinetics and mechanism of oxidation of silver (I) by permanganate ion in aqueous perchlorate solutions at a constant ionic strength of 1.0 mol dm-3 have been studied spectrophotometrically. The reaction time curves of the pseudo first-order plots were found to be of sigmoidal shape throughout the entire course of reaction. The initial rates were found to be relatively fast in the early stages, followed by a more slow reaction over longer time periods. The experimental results indicated a first-order dependence in [MnO4 - ] and fractional first-order kinetics with respect to [Ag+ ] for both stages. The results showed that the oxidation reaction was acid-catalyzed in which the reaction rates were increased with increasing the [H+ ]. Kinetic and spectrophotometric evidences for formation of 1:1 binuclear intermediate complex have been revealed in both two -stages. The activation parameters have been evaluated and a tentative reaction mechanism consistent with the kinetic results was discussed.