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Consider the following mechanism for the oxidation of bromide ions by hydrogen peroxide in aqueous acid solution. Step 1 (rapid equilibrium) H* + H₂O₂ = {H₂O*-OH) Step 2 (H₂O*-OH) + Br¯ → HOBr + H₂O (slowest) Step 3 (fast) HOBr + H* + Br¯ → Br₂ + H₂O What is the rate law supported by this mechanism? A) rate = k[H₂O₂] [H*]²[Br]² B) rate = K[H₂O₂] [H*][Br] C) rate = k[H₂O+-OH] [Br] D) rate = K[H*][H₂O₂]

Consider the following mechanism for the oxidation of bromide ions by hydrogen peroxide in aqueous acid solution. Step 1 (rapid equilibrium) H* + H₂O₂ = {H₂O*-OH) Step 2 (H₂O*-OH) + Br¯ → HOBr + H₂O (slowest) Step 3 (fast) HOBr + H* + Br¯ → Br₂ + H₂O What is the rate law supported by this mechanism? A) rate = k[H₂O₂] [H*]²[Br]² B) rate = K[H₂O₂] [H*][Br] C) rate = k[H₂O+-OH] [Br] D) rate = K[H*][H₂O₂]

Chemistry: An Atoms First Approach
Chemistry: An Atoms First Approach
2nd Edition
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Steven S. Zumdahl, Susan A. Zumdahl
Chapter11: Chemical Kinetics
Section: Chapter Questions
Problem 37E: The decomposition of hydrogen peroxide was studied, and the following data were obtained at a...
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Consider the following mechanism for the oxidation of bromide ions by hydrogen peroxide in aqueous acid solution. Step 1 (rapid equilibrium) Step 2 (H₂O*-OH) + Br¯ → HOBr + H₂O (slowest) Step 3 (fast) H* + H₂O₂ = {H₂O*-OH) HOBr + H* + Br¯ → Br₂ + H₂O What is the rate law supported by this mechanism? A) rate = K[H₂O₂] [H*]²[Br¯]² B) rate = K[H₂O₂] [H*][Br¯] C) rate = k[H₂O*-OH][Br¯] D) rate = K[H*][H₂O₂]
Transcribed Image Text:Consider the following mechanism for the oxidation of bromide ions by hydrogen peroxide in aqueous acid solution. Step 1 (rapid equilibrium) Step 2 (H₂O*-OH) + Br¯ → HOBr + H₂O (slowest) Step 3 (fast) H* + H₂O₂ = {H₂O*-OH) HOBr + H* + Br¯ → Br₂ + H₂O What is the rate law supported by this mechanism? A) rate = K[H₂O₂] [H*]²[Br¯]² B) rate = K[H₂O₂] [H*][Br¯] C) rate = k[H₂O*-OH][Br¯] D) rate = K[H*][H₂O₂]
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