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
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.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F0fb1b0dd-f924-4eb5-b32c-ca16550cc38a%2F067e8221-7c53-4903-9284-255a9f5caf3f%2Fyy7sawj_processed.jpeg&w=3840&q=75)
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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