Consider the Following Mechanism for the Oxidation of Bromide Ions $\to$

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^- $\to$ HOBr + H₂O (slow)
HOBr + H⁺ + Br^- $\to$ Br₂ + H₂O (fast)
Which of the following rate laws is consistent with the mechanism?

A) Rate = k[H₂O₂][H⁺]²[Br^-]
B) Rate = k [H₂O⁺-OH][Br^-]
C) Rate = k[H₂O₂][H⁺][Br^-]
D) Rate = k[HOBr][H⁺][Br^-][H₂O₂]
E) Rate = k[Br^-]