Consider the following mechanism for the oxidation of bromide ions by hydrogen peroxide in aqueous acid solution. H+ + H2O2 ↔ H2O+-OH (rapid equilibrium)

H2O+-OH + Br-→ HOBr + H2O (slow)

HOBr + H+ + Br- → Br2 + H2O (fast)

Which of the following rate laws is consistent with the mechanism?

Select one:
a. Rate = k [H2O+-OH][Br-]
b. Rate = k[Br-]
c. Rate = k[HOBr][H+][Br-][H2O2]
d. Rate = k[H2O2][H+][Br-]
e. Rate = k[H2O2][H+]2[Br-]