C. A possible mechanism for this reaction involves two steps: NO₂(g) + NO2(g) -> NO3(g) + NO(g) slow NO3(g) + CO(g) → NO2(g) + CO₂(g) fast Is this proposed mechanism consistent with the experimentally determined rate law? Explain. d. What is the reaction intermediate in the proposed mechanism?
C. A possible mechanism for this reaction involves two steps: NO₂(g) + NO2(g) -> NO3(g) + NO(g) slow NO3(g) + CO(g) → NO2(g) + CO₂(g) fast Is this proposed mechanism consistent with the experimentally determined rate law? Explain. d. What is the reaction intermediate in the proposed mechanism?
Chemistry
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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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![### Chemical Reaction Mechanisms and Rate Laws
#### c. Analysis of a Proposed Mechanism
A possible mechanism for the given reaction involves two steps:
1. \( \text{NO}_2(g) + \text{NO}_2(g) \rightarrow \text{NO}_3(g) + \text{NO}(g) \) (slow)
2. \( \text{NO}_3(g) + \text{CO}(g) \rightarrow \text{NO}_2(g) + \text{CO}_2(g) \) (fast)
**Question:**
Is this proposed mechanism consistent with the experimentally determined rate law? Explain.
**Answer:**
To determine if the mechanism is consistent with the experimentally determined rate law, we need to derive the rate law from the proposed mechanism and compare it with the experimental data.
1. The slow step is the rate-determining step (RDS). The rate law for this step is:
\[
\text{Rate} = k[\text{NO}_2]^2
\]
where \( k \) is the rate constant and \( [\text{NO}_2] \) is the concentration of \(\text{NO}_2\).
2. The fast step quickly reaches equilibrium, producing \(\text{NO}_3\), which is consumed immediately as it forms. Therefore, it does not accumulate in the reaction mixture.
Since the rate law derived from the slow step matches the experimental rate law, the proposed mechanism is consistent with the experimentally determined rate law.
#### d. Identifying the Reaction Intermediate
**Question:**
What is the reaction intermediate in the proposed mechanism?
**Answer:**
In the given mechanism, the reaction intermediate is \(\text{NO}_3(g)\). This species is produced in the first step and consumed in the second step without appearing in the overall reaction equation:
\[
\text{NO}_2(g) + \text{NO}_2(g) \rightarrow \text{NO}_3(g) + \text{NO}(g) \quad (slow)
\]
\[
\text{NO}_3(g) + \text{CO}(g) \rightarrow \text{NO}_2(g) + \text{CO}_2(g) \quad (fast)
\]
In summary, the intermediate \(\text{NO}_3(g)\) is essential for the reaction mechanism but is not observed as](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F93268262-58e0-42e0-b5aa-ce0732a52664%2Fa071c518-b649-4acf-8ead-fdc996129c49%2Fpj5lnrk_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Chemical Reaction Mechanisms and Rate Laws
#### c. Analysis of a Proposed Mechanism
A possible mechanism for the given reaction involves two steps:
1. \( \text{NO}_2(g) + \text{NO}_2(g) \rightarrow \text{NO}_3(g) + \text{NO}(g) \) (slow)
2. \( \text{NO}_3(g) + \text{CO}(g) \rightarrow \text{NO}_2(g) + \text{CO}_2(g) \) (fast)
**Question:**
Is this proposed mechanism consistent with the experimentally determined rate law? Explain.
**Answer:**
To determine if the mechanism is consistent with the experimentally determined rate law, we need to derive the rate law from the proposed mechanism and compare it with the experimental data.
1. The slow step is the rate-determining step (RDS). The rate law for this step is:
\[
\text{Rate} = k[\text{NO}_2]^2
\]
where \( k \) is the rate constant and \( [\text{NO}_2] \) is the concentration of \(\text{NO}_2\).
2. The fast step quickly reaches equilibrium, producing \(\text{NO}_3\), which is consumed immediately as it forms. Therefore, it does not accumulate in the reaction mixture.
Since the rate law derived from the slow step matches the experimental rate law, the proposed mechanism is consistent with the experimentally determined rate law.
#### d. Identifying the Reaction Intermediate
**Question:**
What is the reaction intermediate in the proposed mechanism?
**Answer:**
In the given mechanism, the reaction intermediate is \(\text{NO}_3(g)\). This species is produced in the first step and consumed in the second step without appearing in the overall reaction equation:
\[
\text{NO}_2(g) + \text{NO}_2(g) \rightarrow \text{NO}_3(g) + \text{NO}(g) \quad (slow)
\]
\[
\text{NO}_3(g) + \text{CO}(g) \rightarrow \text{NO}_2(g) + \text{CO}_2(g) \quad (fast)
\]
In summary, the intermediate \(\text{NO}_3(g)\) is essential for the reaction mechanism but is not observed as
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