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

question 27

Multiple Choice

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^-]

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