The kinetics and mechanisms of the oxidation k3[Fe(C2O4)3].3H2O by permanganate ion in acid solution has been studied. The data are consistent with the rate law: d[Fe(C2O4)3-]/dt (a + b [H+])[Fe2(C2O4)3[MnO4] with a = 0.12 s-1 and b = 1.35 dm6 mol2 s-1, at T = 27.0±1.0°C,[H+] = 0.2 mol dm-3, I= 0.2 mol dm-3 (NaCl), and ëmax = 420 nm. There is evidence for the formation of an intermediate complex of significant stability and free radicals are important in the reaction. The reaction is rationalised in terms of an inner-sphere mechanism.
Key words: Kinetics, mechanism, rate constants.
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