Consider the decomposition of hydrogen peroxide ($ ext{H}_2 ext{O}_2$) as per the equation given below : $2 ext{H}_2 ext{O}_2 \xrightarrow[ ext{Alkaline medium}]{ ext{I}^-} 2 ext{H}_2 ext{O} + ext{O}_2$ The mechanism for this reaction was found to be : Step I : $ ext{H}_2 ext{O}_2 + ext{I}^- \longrightarrow ext{H}_2 ext{O} + ext{IO}^-$ (slow) Step II : $ ext{H}_2 ext{O}_2 + ext{IO}^- \longrightarrow ext{H}_2 ext{O} + ext{I}^- + ext{O}_2$ (fast) (a) Write the rate law expression. (b) Determine the order of reaction with respect to $ ext{H}_2 ext{O}_2$, $ ext{I}^-$ and overall order of reaction. (c) What is the molecularity of the reaction in Step II ?