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)
What is the overall reaction equation for this process?

A) 2H₂O⁺-OH + 2Br^- $\to$ H₂O₂ + Br₂ + 2H₂O
B) 2H⁺ + 2Br^- + H₂O₂ $\to$ Br₂ + 2H₂O
C) 2H⁺ + H₂O₂ + Br^- + HOBr $\to$ H₂O⁺-OH + Br₂ + H₂O
D) H₂O⁺-OH + Br^- + H⁺ $\to$ Br₂ + H₂O
E) None of these choices is correct.