Im having a lot of trouble with this question:
4. The decomposition of hydrogen peroxide is catalyzed by iodide ion. The
Catalyzed reaction is thought to proceed by a two-step mechanism:
H2O2(aq) + I-(aq) → H2O(l) + IO-(aq) (slow)
IO-(aq) + H2O2(aq) → H2O(l) + O2(g) + I-(aq) (fast)
(a) Write the rate law for each of the elementary reactions of the mechanism.
(b) Write the chemical equation for the overall reaction.
(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.
I know the overall reaction is 2 H2O2 -> 2 H2O + O2 (or at least i think I know) but other than that I don't really know what to do or how to identify and intermediate.
Any help?