6. Consider the decomposition of perbenzoic acid in water: 2 C6H5CO3(aq) → 2 C6H5COOH(aq) + O₂(g). The reaction may proceed according to the following mechanism: C6H5CO3HC6H5CO¾¯ + H* C6H5CO3H + C6H5CO3 O₂ + C6H5CO₂ + С6H5COOH Assuming that the second step is rate-limiting, and the first step in the reaction satisfies the pre-equilibrium condition, determine the rate of formation of O₂. Assume the pH remains constant throughout the reaction. Would the rate of reaction increase or decrease with a more acidic pH?
6. Consider the decomposition of perbenzoic acid in water: 2 C6H5CO3(aq) → 2 C6H5COOH(aq) + O₂(g). The reaction may proceed according to the following mechanism: C6H5CO3HC6H5CO¾¯ + H* C6H5CO3H + C6H5CO3 O₂ + C6H5CO₂ + С6H5COOH Assuming that the second step is rate-limiting, and the first step in the reaction satisfies the pre-equilibrium condition, determine the rate of formation of O₂. Assume the pH remains constant throughout the reaction. Would the rate of reaction increase or decrease with a more acidic pH?
Chapter13: Kinetic Methods
Section: Chapter Questions
Problem 3P
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![6. Consider the decomposition of perbenzoic acid in water: 2 C6H5CO3(aq) → 2 C₂H5COOH(aq) + O₂(g). The
reaction may proceed according to the following mechanism:
C6H5CO3H
k₁
k₁
C6H5CO3 + H*
k₂
C6H5CO3H + C6H5CO3 → O₂ + С6H5CO₂ + C₂H5COOH
Assuming that the second step is rate-limiting, and the first step in the reaction satisfies the pre-equilibrium
condition, determine the rate of formation of O₂. Assume the pH remains constant throughout the reaction.
Would the rate of reaction increase or decrease with a more acidic pH?](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F5cf787c2-6f6a-44c6-a9e4-1d29c994970c%2F9d5fde7b-58aa-43f4-ad36-2f7c735e5306%2F1epa5u_processed.png&w=3840&q=75)
Transcribed Image Text:6. Consider the decomposition of perbenzoic acid in water: 2 C6H5CO3(aq) → 2 C₂H5COOH(aq) + O₂(g). The
reaction may proceed according to the following mechanism:
C6H5CO3H
k₁
k₁
C6H5CO3 + H*
k₂
C6H5CO3H + C6H5CO3 → O₂ + С6H5CO₂ + C₂H5COOH
Assuming that the second step is rate-limiting, and the first step in the reaction satisfies the pre-equilibrium
condition, determine the rate of formation of O₂. Assume the pH remains constant throughout the reaction.
Would the rate of reaction increase or decrease with a more acidic pH?
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