A Kinetic Study of the Oxidation of Lactic Acid by Vanadium (V)

The kinetics of oxidation of lactic acid by quinquevalent vanadium is found to be of first order with respect to both vanadium(v) and lactic acid. The Arrhenius equation is found to be valid for the reaction between 25° and 35°. The values for the energy of activation, entropy of activation, and frequency factor are found to be 164 kcal., -13.70 cal./MA°, and 6.687 X 10⁹ sec^—I respectively. These experimental findings are consistent with the postulate that the rate-determining step in the reaction involves the first order disproportionation of a co-ordination complex between lactic acid and vanadium(v), affording products through free-radical formation.