The following reaction is studied in room temperature.Cl2(g) H2O(g) ? HCl(g) HClO(g)The first step is promoted by light. The following proposed mechanism using three elementary steps gives the same rate law expression determined by experiments.Step 1: Cl2 ? <---> 2Cl (fast equilibrium)Step 2: Cl H2O —->? HCl OH (slow)Step 3. Cl OH ?—-> HClO (fast)Which of the following rate laws is correct?A. rate = k[Cl][H2O] B rate = k[Cl]?[H2O]C. rate = k[Cl]2[H2O] D. rate = k[Cl2]½[H2O]Provide work and explain why.
