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Consider the mechanism. Step 1: 2A B+C slow Step 2: B +C → E fast Overall: 2 A → E Determine the rate law for the overall reaction, where the overall rate constant is represented as k. rate =

Consider the mechanism. Step 1: 2A B+C slow Step 2: B +C → E fast Overall: 2 A → E Determine the rate law for the overall reaction, where the overall rate constant is represented as k. rate =

Chemistry
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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#6, please give me the correct answer!
**Chemical Reaction Mechanisms and Rate Law Determination** **Consider the mechanism:** \[ \text{Step 1:} \quad 2A \rightarrow B + C \quad \text{(slow)} \] \[ \text{Step 2:} \quad B + C \rightarrow E \quad \text{(fast)} \] \[ \text{Overall:} \quad 2A \rightarrow E \] **Determine the rate law for the overall reaction, where the overall rate constant is represented as \( k \):** \[ \text{rate} = \underline{\hspace{5cm}} \] In this problem, we are given a two-step reaction mechanism. The first step \( (2A \rightarrow B + C) \) is slow, indicating it is the rate-determining step. The second step \( (B + C \rightarrow E) \) is fast. The overall reaction, combining these two steps, is \( 2A \rightarrow E \). To determine the rate law for the overall reaction: - We focus on the slowest step (rate-determining step) because it limits the speed of the overall reaction. - The rate law for the rate-determining step involves the reactants in that step. Given the slow step \( 2A \rightarrow B + C \), the rate law will be of the form: \[ \text{rate} = k [A]^2 \] Here, \( k \) is the rate constant, and \([A]\) is the concentration of reactant A. **Conclusion:** \[ \text{rate} = k [A]^2 \] This equation provides the rate law for the overall reaction based on the given mechanism.
Transcribed Image Text:**Chemical Reaction Mechanisms and Rate Law Determination** **Consider the mechanism:** \[ \text{Step 1:} \quad 2A \rightarrow B + C \quad \text{(slow)} \] \[ \text{Step 2:} \quad B + C \rightarrow E \quad \text{(fast)} \] \[ \text{Overall:} \quad 2A \rightarrow E \] **Determine the rate law for the overall reaction, where the overall rate constant is represented as \( k \):** \[ \text{rate} = \underline{\hspace{5cm}} \] In this problem, we are given a two-step reaction mechanism. The first step \( (2A \rightarrow B + C) \) is slow, indicating it is the rate-determining step. The second step \( (B + C \rightarrow E) \) is fast. The overall reaction, combining these two steps, is \( 2A \rightarrow E \). To determine the rate law for the overall reaction: - We focus on the slowest step (rate-determining step) because it limits the speed of the overall reaction. - The rate law for the rate-determining step involves the reactants in that step. Given the slow step \( 2A \rightarrow B + C \), the rate law will be of the form: \[ \text{rate} = k [A]^2 \] Here, \( k \) is the rate constant, and \([A]\) is the concentration of reactant A. **Conclusion:** \[ \text{rate} = k [A]^2 \] This equation provides the rate law for the overall reaction based on the given mechanism.
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