Consider the Following Mechanism for the Oxidation of Bromide Ions

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?

A) Rate = k[H ₂O ₂][H ⁺] ²[Br ⁻]
B) Rate = k[H ₂O ⁺−OH][Br ⁻]
C) Rate = k[H ₂O ₂][H ⁺][Br ⁻]
D) Rate = k[HOBr][H ⁺][Br ⁻][H ₂O ₂]
E) Rate = k[Br ⁻]