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> → HOBr + H<sub>2</sub>O (slow) HOBr + H<sup>+</sup> + Br<sup>-</sup> → Br<sub>2</sub> + H<sub>2</sub>O (fast) Which of the following rate laws is consistent with the mechanism? A) Rate = k[H<sub>2</sub>O<sub>2</sub>][H<sup>+</sup>]<sup>2</sup>[Br<sup>-</sup>] B) Rate = k[H<sub>2</sub>O+-OH][Br<sup>-</sup>] C) Rate = k[H<sub>2</sub>O<sub>2</sub>][H<sup>+</sup>][Br<sup>-</sup>] D) Rate = k[HOBr][H<sup>+</sup>][Br<sup>-</sup>][H<sub>2</sub>O<sub>2</sub>] E) Rate = k[Br<sup>-</sup>]](https://d2lvgg3v3hfg70.cloudfront.net/TB7800/11eac68a_1c6d_1a1c_a448_d949d67ff975_TB7800_11.jpg)
H2O+-OH (rapid equilibrium)
H2O+-OH + Br- → HOBr + H2O (slow)
HOBr + H+ + Br- → 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-]
Correct Answer:
Verified
Correct Answer:
Verified
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