The decomposition of hydrogen peroxide is catalyzed by iodide ion. The catalyzed reaction is thought to proceed by a two-step mechanism:$\begin{array}{rlr}{\mathrm{H}}_2{\mathrm{O}}_2(aq)+{\mathrm{I}}^{-}(aq)& ⟶{\mathrm{H}}_2\mathrm{O}(l)+{\mathrm{IO}}^{-}(aq)& \text{ (slow) }\\ {\mathrm{IO}}^{-}(aq)+{\mathrm{H}}_2{\mathrm{O}}_2(aq)& ⟶{\mathrm{H}}_2\mathrm{O}(l)+{\mathrm{O}}_2(g)+{\mathrm{I}}^{-}(aq)& \text{ (fast) }\end{array}$(a) Write the rate law for each of the elementary reactions of the mechanism. (b) Write the chemical equation for the overall process. (c) Identify the intermediate, if any, in the mechanism. (d) Assuming that the first step of the mechanism is rate determining, predict the rate law for the overall process.

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