
%0 Journal Article
%A Smith, RH 
%A Wilson, IR 
%T The mechanism of the oxidation of thiocyanate ion by peroxomonosulphate in aqueous solution. II. Kinetics of the reaction
%J Australian Journal of Chemistry
%D 1966/08/01
%V 19
%N 8
%P 1365-1375
%K 
%R https://doi.org/10.1071/CH9661365
%U https://www.publish.csiro.au/paper/CH9661365 
%X Initial rates of reaction for the above oxidation have been measured by a stopped-flow conductance method. Between pH 2 and 3.6, the initial rate of reaction, R, is given by the expression     R{[HSO5-]+[SCN-]} = {kb+kc[H+]}[HSO5-]0[SCN-]20+ka[H+]-1[HSO5]20[SCN-]0  As pH increases, there is a transition to a pH-independent rate, first order in each thiocyanate and peroxomonosulphate concentrations. 
