The rate law for 2 NO(g) + O2(g) → 2 NO,(g) is rate = k[NO]?[0,]. The following mechanisms have been proposed: I. 2 NO(g) + O2(g)→ 2 NO2(g) П. 2 NO(g) = N,02(g) [fast] N,O2(g) + O2(g) → 2 NO2(g) [slow] 2 NO(g) = N2(g)+ O2(g) N2(g) + 2 O2(g) –→ 2 NO2(g) III. [fast] [slow] (a) Which of these mechanisms is consistent with the rate law? Check all that apply II. III. None of the above
The rate law for 2 NO(g) + O2(g) → 2 NO,(g) is rate = k[NO]?[0,]. The following mechanisms have been proposed: I. 2 NO(g) + O2(g)→ 2 NO2(g) П. 2 NO(g) = N,02(g) [fast] N,O2(g) + O2(g) → 2 NO2(g) [slow] 2 NO(g) = N2(g)+ O2(g) N2(g) + 2 O2(g) –→ 2 NO2(g) III. [fast] [slow] (a) Which of these mechanisms is consistent with the rate law? Check all that apply II. III. None of the above
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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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![### Reaction Rate Law Analysis
#### Provided Reaction and Rate Law
Be sure to answer all parts.
The rate law for the reaction:
\[ 2 \text{NO}(g) + \text{O}_2(g) \rightarrow 2 \text{NO}_2(g) \]
is given by:
\[ \text{rate} = k[\text{NO}]^2[\text{O}_2] \]
#### Proposed Mechanisms
The following mechanisms have been proposed to explain this rate law:
**Mechanism I:**
\[ 2 \text{NO}(g) + \text{O}_2(g) \rightarrow 2 \text{NO}_2(g) \]
**Mechanism II:**
1. \[ 2 \text{NO}(g) \rightleftharpoons \text{N}_2\text{O}_2(g) \] \[ \text{[fast]} \]
2. \[ \text{N}_2\text{O}_2(g) + \text{O}_2(g) \rightarrow 2 \text{NO}_2(g) \] \[ \text{[slow]} \]
**Mechanism III:**
1. \[ 2 \text{NO}(g) \rightleftharpoons \text{N}_2(g) + \text{O}_2(g) \] \[ \text{[fast]} \]
2. \[ \text{N}_2(g) + 2 \text{O}_2(g) \rightarrow 2 \text{NO}_2(g) \] \[ \text{[slow]} \]
#### Question
(a) Which of these mechanisms is consistent with the rate law? Check all that apply.
- [x] I.
- [x] II.
- [ ] III.
- [ ] None of the above
---
**Explanation:**
1. **Mechanism I** directly converts \( \text{NO} \) and \( \text{O}_2 \) into \( \text{NO}_2 \), consistent with the rate law \( \text{rate} = k[\text{NO}]^2[\text{O}_2] \).
2. **Mechanism II** consists of a fast pre-equilibrium step forming \( \text{N}_2\text{O}_2 \) followed by a slow step](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fe0ae19d5-3750-41df-884f-8ca3aa31e002%2Fa55ec8f7-5db5-47c4-8629-d5b460844848%2Fk0xglki_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Reaction Rate Law Analysis
#### Provided Reaction and Rate Law
Be sure to answer all parts.
The rate law for the reaction:
\[ 2 \text{NO}(g) + \text{O}_2(g) \rightarrow 2 \text{NO}_2(g) \]
is given by:
\[ \text{rate} = k[\text{NO}]^2[\text{O}_2] \]
#### Proposed Mechanisms
The following mechanisms have been proposed to explain this rate law:
**Mechanism I:**
\[ 2 \text{NO}(g) + \text{O}_2(g) \rightarrow 2 \text{NO}_2(g) \]
**Mechanism II:**
1. \[ 2 \text{NO}(g) \rightleftharpoons \text{N}_2\text{O}_2(g) \] \[ \text{[fast]} \]
2. \[ \text{N}_2\text{O}_2(g) + \text{O}_2(g) \rightarrow 2 \text{NO}_2(g) \] \[ \text{[slow]} \]
**Mechanism III:**
1. \[ 2 \text{NO}(g) \rightleftharpoons \text{N}_2(g) + \text{O}_2(g) \] \[ \text{[fast]} \]
2. \[ \text{N}_2(g) + 2 \text{O}_2(g) \rightarrow 2 \text{NO}_2(g) \] \[ \text{[slow]} \]
#### Question
(a) Which of these mechanisms is consistent with the rate law? Check all that apply.
- [x] I.
- [x] II.
- [ ] III.
- [ ] None of the above
---
**Explanation:**
1. **Mechanism I** directly converts \( \text{NO} \) and \( \text{O}_2 \) into \( \text{NO}_2 \), consistent with the rate law \( \text{rate} = k[\text{NO}]^2[\text{O}_2] \).
2. **Mechanism II** consists of a fast pre-equilibrium step forming \( \text{N}_2\text{O}_2 \) followed by a slow step
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