AbstractThe kinetics of the oxidation of iodide by hydrogen peroxide catalyzed by acidic molybdate have been studied by a spectrophotometric stopped‐flow method. The results are interpreted in terms of the mechanismand the implied rate law\documentclass{article}\pagestyle{empty}\begin{document}$$ - d[{\rm H}_{\rm 2} {\rm O}]/dt = \frac{{k_4 k_1 k_2 [{\rm H}_2 {\rm O}_2]^2 [{\rm mol}][{\rm I}^ -]}}{{1 + k_1 [{\rm H}_2 {\rm O}_2] + k_1 k_2 [{\rm H}_2 {\rm O}_2]^2 + {\rm K}_{\rm 3} [{\rm I}^{\rm -}]}}$$\end{document}where [mol] is total analytical concentration of molybdate. The values obtained for the rate and equilibrium constants arek4= (3.3 ± 1) × 1021./mole · s,K1= (1.2 ± 0.6) × 1041./mole,K2= (1.3 ± 0.7) × 1031./mole, andK3= (4 ± 3) × 1021./mol