Consider the following mechanism for the oxidation of bromide ions by hydrogen peroxide in aqueous acid solution. H+ + H2O2 ? H3O2+ (rapid equilibrium) H3O2+ + Br- ? HOBr + H2O (slow) HOBr+H+ +Br- ?Br2 +H2O(fast) Which rate law is consistent with this mechanism?

a. k[Br-][H+]-1[H2O2]-1
b. k[H+][H2O2][Br-]
c. k[H+][H2O2]
d. k[HOBr][H+][Br-]

The rate law for the reaction is

Explanation:

Rate law is the expression which is used to express the rate of the reaction in terms of the molar concentration of reactants where each term is raised to the power their stoichiometric coefficient respectively from a balanced chemical equation.

In a mechanism of the reaction, the slow step in the mechanism determines the rate of the reaction.

The chemical equation for the oxidation of bromide ions by hydrogen peroxide in aqueous acid solution follows:

The intermediate reaction of the mechanism follows:

Step 1:  

Step 2:  

Step 3:  

As, step 2 is the slow step. It is the rate determining step

Rate law for the reaction follows:

         ......(1)

As, is not appearing as a reactant in the overall reaction. So, we apply steady state approximation in it.

Applying steady state approximation for from step 1, we get:

Putting the value of in equation 1, we get:

Hence, the rate law for the reaction is