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

question 21

Multiple Choice

Consider the following mechanism for the oxidation of bromide ions by hydrogen peroxide in aqueous acid solution.
H+ + H2O2 Consider the following mechanism for the oxidation of bromide ions by hydrogen peroxide in aqueous acid solution. H<sup>+</sup> + H<sub>2</sub>O<sub>2</sub> H<sub>2</sub>O<sup>+</sup>-OH (rapid equilibrium) H<sub>2</sub>O<sup>+</sup>-OH + Br<sup>-</sup> \to HOBr + H<sub>2</sub>O (slow) HOBr + H<sup>+</sup> + Br<sup>-</sup> \to Br<sub>2</sub> + H<sub>2</sub>O (fast) What is the overall reaction equation for this process? A) 2H<sub>2</sub>O<sup>+</sup>-OH + 2Br<sup>-</sup> \to H<sub>2</sub>O<sub>2</sub> + Br<sub>2</sub> + 2H<sub>2</sub>O B) 2H<sup>+</sup> + 2Br<sup>-</sup> + H<sub>2</sub>O<sub>2</sub> \to Br<sub>2</sub> + 2H<sub>2</sub>O C) 2H<sup>+</sup> + H<sub>2</sub>O<sub>2</sub> + Br<sup>-</sup> + HOBr \to H<sub>2</sub>O<sup>+</sup>-OH + Br<sub>2</sub> + H<sub>2</sub>O D) H<sub>2</sub>O<sup>+</sup>-OH + Br<sup>-</sup> + H<sup>+</sup> \to Br<sub>2</sub> + H<sub>2</sub>O E) None of these choices is correct.
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?

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