21. Which is true for the decomposition reaction of hydrogen peroxide if the proposed mechanism below is true? Overall Balanced Reaction: 2H2O2(aq) → 2H2O(I) + O2(g) Step 1: H,0, (aq) + Br (aq) → H,0)+ OBr (g) Step 2: H,O,(aq) + OBr (aq) → H,0() + Br (ag) + O2(g) (fast) (slow, rds) Br is a catalyst and the rate law is Rate = k[H2O2]. - OBr is an intermediate and the rate law is Rate = a. b. k[H2O2][OBr ]. OBr is an intermediate and the rate law is Rate = k[H2O2]°[Br][OB1¯]. d. Pseudo-first order reaction in hydrogen peroxide and the rate law is Rate = i Br is a catalyst and the rate law is Rate = k[HLO2][Br¯]. c. k[H2O2]. e.
21. Which is true for the decomposition reaction of hydrogen peroxide if the proposed mechanism below is true? Overall Balanced Reaction: 2H2O2(aq) → 2H2O(I) + O2(g) Step 1: H,0, (aq) + Br (aq) → H,0)+ OBr (g) Step 2: H,O,(aq) + OBr (aq) → H,0() + Br (ag) + O2(g) (fast) (slow, rds) Br is a catalyst and the rate law is Rate = k[H2O2]. - OBr is an intermediate and the rate law is Rate = a. b. k[H2O2][OBr ]. OBr is an intermediate and the rate law is Rate = k[H2O2]°[Br][OB1¯]. d. Pseudo-first order reaction in hydrogen peroxide and the rate law is Rate = i Br is a catalyst and the rate law is Rate = k[HLO2][Br¯]. c. k[H2O2]. e.
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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![**Decomposition Reaction of Hydrogen Peroxide**
**Question 21:**
Which is true for the decomposition reaction of hydrogen peroxide if the proposed mechanism below is true?
**Overall Balanced Reaction:**
\(2H_2O_2(aq) \rightarrow 2H_2O(l) + O_2(g)\)
**Step 1:**
\(H_2O_2(aq) + Br^-(aq) \rightarrow H_2O(l) + OBr^-(g)\) (slow, rds)
**Step 2:**
\(H_2O_2(aq) + OBr^-(aq) \rightarrow H_2O(l) + Br^-(aq) + O_2(g)\) (fast)
**Options:**
a. \( Br^- \) is a catalyst and the rate law is \( \text{Rate} = k[H_2O_2]^2 \).
b. \( OBr^- \) is an intermediate and the rate law is \( \text{Rate} = k[H_2O_2][OBr^-] \).
c. \( OBr^- \) is an intermediate and the rate law is \( \text{Rate} = k[H_2O_2]^2[Br^-][OBr^-] \).
d. Pseudo-first order reaction in hydrogen peroxide and the rate law is \( \text{Rate} = k[H_2O_2] \).
e. \( Br^- \) is a catalyst and the rate law is \( \text{Rate} = k[H_2O_2][Br^-] \).
**Explanation:**
This problem explores the kinetics of the decomposition reaction of hydrogen peroxide. The overall reaction is the breakdown of hydrogen peroxide into water and oxygen gas. The reaction proceeds through a two-step mechanism, where \( Br^- \) acts as a catalyst and \( OBr^- \) serves as an intermediate. The first step is the rate-determining step (rds).
For an accurate understanding, it's essential to identify the catalysts, intermediates, and the rate law for the reaction.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fc31825ca-e532-4346-8c67-c6f0bc8ad95c%2F1b840cd4-c605-47ff-b620-b50bcba0bb03%2F47lzbqs_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Decomposition Reaction of Hydrogen Peroxide**
**Question 21:**
Which is true for the decomposition reaction of hydrogen peroxide if the proposed mechanism below is true?
**Overall Balanced Reaction:**
\(2H_2O_2(aq) \rightarrow 2H_2O(l) + O_2(g)\)
**Step 1:**
\(H_2O_2(aq) + Br^-(aq) \rightarrow H_2O(l) + OBr^-(g)\) (slow, rds)
**Step 2:**
\(H_2O_2(aq) + OBr^-(aq) \rightarrow H_2O(l) + Br^-(aq) + O_2(g)\) (fast)
**Options:**
a. \( Br^- \) is a catalyst and the rate law is \( \text{Rate} = k[H_2O_2]^2 \).
b. \( OBr^- \) is an intermediate and the rate law is \( \text{Rate} = k[H_2O_2][OBr^-] \).
c. \( OBr^- \) is an intermediate and the rate law is \( \text{Rate} = k[H_2O_2]^2[Br^-][OBr^-] \).
d. Pseudo-first order reaction in hydrogen peroxide and the rate law is \( \text{Rate} = k[H_2O_2] \).
e. \( Br^- \) is a catalyst and the rate law is \( \text{Rate} = k[H_2O_2][Br^-] \).
**Explanation:**
This problem explores the kinetics of the decomposition reaction of hydrogen peroxide. The overall reaction is the breakdown of hydrogen peroxide into water and oxygen gas. The reaction proceeds through a two-step mechanism, where \( Br^- \) acts as a catalyst and \( OBr^- \) serves as an intermediate. The first step is the rate-determining step (rds).
For an accurate understanding, it's essential to identify the catalysts, intermediates, and the rate law for the reaction.
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