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
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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![### Chemical Reaction Mechanism and Rate Law Analysis
#### c. Analysis of a Proposed Mechanism
A possible mechanism for the given reaction consists of two steps:
\[ \text{NO}_2(\text{g}) + \text{NO}_2(\text{g}) \rightarrow \text{NO}_3(\text{g}) + \text{NO}(\text{g}) \quad \text{[slow]} \]
\[ \text{NO}_3(\text{g}) + \text{CO}(\text{g}) \rightarrow \text{NO}_2(\text{g}) + \text{CO}_2(\text{g}) \quad \text{[fast]} \]
**Question:** Is this proposed mechanism consistent with the experimentally determined rate law? Explain.
#### d. Identifying the Reaction Intermediate
**Question:** What is the reaction intermediate in the proposed mechanism?
---
### Explanation
**Section c:** The proposed mechanism comprises two steps: the first step is slow, involving the reaction of two nitrogen dioxide \((\text{NO}_2)\) molecules to form nitrogen trioxide \((\text{NO}_3})\) and nitrogen monoxide \((\text{NO})\). The second, faster step involves the reaction of \(\text{NO}_3\) with carbon monoxide \((\text{CO})\) to produce \(\text{NO}_2}\) and carbon dioxide \((\text{CO}_2})\).
To determine consistency with the experimentally determined rate law, one needs to:
- Derive the rate law from the slow step (since it is the rate-determining step).
- Compare this derived rate law with the experimentally determined rate law to check for consistency.
**Section d:** The reaction intermediate is a molecule that is produced in one step of the reaction mechanism and consumed in a subsequent step. In this proposed mechanism, \(\text{NO}_3}\) is produced in the first step and consumed in the second step, thus it is the reaction intermediate.
---
Understanding and analyzing the proposed mechanism helps in verifying its consistency with the experimental observations and further elucidates the steps involved in the chemical reaction.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F93268262-58e0-42e0-b5aa-ce0732a52664%2F4741230d-7b8e-47fe-b955-f7ce6a15f5e3%2F11hwqn_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Chemical Reaction Mechanism and Rate Law Analysis
#### c. Analysis of a Proposed Mechanism
A possible mechanism for the given reaction consists of two steps:
\[ \text{NO}_2(\text{g}) + \text{NO}_2(\text{g}) \rightarrow \text{NO}_3(\text{g}) + \text{NO}(\text{g}) \quad \text{[slow]} \]
\[ \text{NO}_3(\text{g}) + \text{CO}(\text{g}) \rightarrow \text{NO}_2(\text{g}) + \text{CO}_2(\text{g}) \quad \text{[fast]} \]
**Question:** Is this proposed mechanism consistent with the experimentally determined rate law? Explain.
#### d. Identifying the Reaction Intermediate
**Question:** What is the reaction intermediate in the proposed mechanism?
---
### Explanation
**Section c:** The proposed mechanism comprises two steps: the first step is slow, involving the reaction of two nitrogen dioxide \((\text{NO}_2)\) molecules to form nitrogen trioxide \((\text{NO}_3})\) and nitrogen monoxide \((\text{NO})\). The second, faster step involves the reaction of \(\text{NO}_3\) with carbon monoxide \((\text{CO})\) to produce \(\text{NO}_2}\) and carbon dioxide \((\text{CO}_2})\).
To determine consistency with the experimentally determined rate law, one needs to:
- Derive the rate law from the slow step (since it is the rate-determining step).
- Compare this derived rate law with the experimentally determined rate law to check for consistency.
**Section d:** The reaction intermediate is a molecule that is produced in one step of the reaction mechanism and consumed in a subsequent step. In this proposed mechanism, \(\text{NO}_3}\) is produced in the first step and consumed in the second step, thus it is the reaction intermediate.
---
Understanding and analyzing the proposed mechanism helps in verifying its consistency with the experimental observations and further elucidates the steps involved in the chemical reaction.
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