G. A. Hiremath, P. L. Timmanagoudar, S. Nandibewoor
Dec 1, 1996
Citations
0
Influential Citations
9
Citations
Journal
Transition Metal Chemistry
Abstract
SummaryThe permanganate-TlI reaction in aqueous HCl was studied using the stopped-flow technique. The reaction rate increases as both [H+] and [Cl-] increase. It exhibits second-order kinetics and the rate law is given by Equation 1: $$rate = k\left[ {Mn^{III} } \right]^x \left[ {AA} \right]_0 \left[ {OAc^ - } \right]^x \left[ {H^ + } \right]^{ - x} $$ (1) where k is the rate constant of the slow step, and K1 and K4 are the respective formation constants of the active form of the reductant, TlCl, and the protonated species of the oxidant, HMnO4. A composite mechanism and rate law are proposed.