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)
What is the overall reaction equation for this process?

Question

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> → HOBr + H<sub>2</sub>O (slow) HOBr + H<sup>+</sup> + Br<sup>-</sup> → 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> → 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> → 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 → 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> → Br<sub>2</sub> + H<sub>2</sub>O E) None of these choices are correct.

H₂O⁺-OH (rapid equilibrium)
H₂O⁺-OH + Br^- → HOBr + H₂O (slow)
HOBr + H⁺ + Br^- → Br₂ + H₂O (fast)
What is the overall reaction equation for this process?

Quizplus · Accepted Answer

The Answer of 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) What is the overall reaction equation for this process?

Consider the Following Mechanism for the Oxidation of Bromide Ions