Consider the mechanism. O, + NO, → NO, + O, slow NO, + NO, → N,O5 fast O, + 2 NO, → O, + N,O5 - Identify the rate law for the overall reaction based on the mechanism. O rate = k[O,][NO,] = k[NO,]² O rate = k[O,][NO,J² rate = k[O,] O rate = k[NO, ][NO,]
Consider the mechanism. O, + NO, → NO, + O, slow NO, + NO, → N,O5 fast O, + 2 NO, → O, + N,O5 - Identify the rate law for the overall reaction based on the mechanism. O rate = k[O,][NO,] = k[NO,]² O rate = k[O,][NO,J² rate = k[O,] O rate = k[NO, ][NO,]
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter11: Chemical Kinetics: Rates Of Reactions
Section: Chapter Questions
Problem 115QRT
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![### Understanding the Mechanism
Consider the given mechanism involving two elementary steps:
**Step 1:**
\[ \text{O}_3 + \text{NO}_2 \rightarrow \text{NO}_3 + \text{O}_2 \quad (\text{slow}) \]
**Step 2:**
\[ \text{NO}_2 + \text{NO}_3 \rightarrow \text{N}_2\text{O}_5 \quad (\text{fast}) \]
The overall reaction derived from these steps is:
\[ \text{O}_3 + 2\text{NO}_2 \rightarrow \text{O}_2 + \text{N}_2\text{O}_5 \]
### Determining the Rate Law
The rate law for the overall reaction depends on the slow (rate-determining) step. The rate of the reaction is governed by the reactants in this slow step.
In the given mechanism, the slow (rate-determining) step is:
\[ \text{O}_3 + \text{NO}_2 \rightarrow \text{NO}_3 + \text{O}_2 \]
Therefore, the rate law can be written based on this step:
\[ \text{rate} = k[\text{O}_3][\text{NO}_2] \]
From the given options, the correct rate law is:
- \(\bigcirc\) \(\text{rate} = k[\text{O}_3][\text{NO}_2]\)
### Answer Choices:
- \(\bigcirc\) \(\text{rate} = k[\text{O}_3][\text{NO}_2]\)
- \(\textstyle\bigcirc\) \(\text{rate} = k[\text{NO}_2]^2\)
- \(\text{rate} = k[\text{O}_3][\text{NO}_2]^2\)
- \(\text{rate} = k[\text{O}_3]\)
- \(\text{rate} = k[\text{NO}_2][\text{NO}_3]\)](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F0fb1b0dd-f924-4eb5-b32c-ca16550cc38a%2Ff292560f-9091-4eeb-b6ce-3dffb55bf0df%2Fimuzf8g_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Understanding the Mechanism
Consider the given mechanism involving two elementary steps:
**Step 1:**
\[ \text{O}_3 + \text{NO}_2 \rightarrow \text{NO}_3 + \text{O}_2 \quad (\text{slow}) \]
**Step 2:**
\[ \text{NO}_2 + \text{NO}_3 \rightarrow \text{N}_2\text{O}_5 \quad (\text{fast}) \]
The overall reaction derived from these steps is:
\[ \text{O}_3 + 2\text{NO}_2 \rightarrow \text{O}_2 + \text{N}_2\text{O}_5 \]
### Determining the Rate Law
The rate law for the overall reaction depends on the slow (rate-determining) step. The rate of the reaction is governed by the reactants in this slow step.
In the given mechanism, the slow (rate-determining) step is:
\[ \text{O}_3 + \text{NO}_2 \rightarrow \text{NO}_3 + \text{O}_2 \]
Therefore, the rate law can be written based on this step:
\[ \text{rate} = k[\text{O}_3][\text{NO}_2] \]
From the given options, the correct rate law is:
- \(\bigcirc\) \(\text{rate} = k[\text{O}_3][\text{NO}_2]\)
### Answer Choices:
- \(\bigcirc\) \(\text{rate} = k[\text{O}_3][\text{NO}_2]\)
- \(\textstyle\bigcirc\) \(\text{rate} = k[\text{NO}_2]^2\)
- \(\text{rate} = k[\text{O}_3][\text{NO}_2]^2\)
- \(\text{rate} = k[\text{O}_3]\)
- \(\text{rate} = k[\text{NO}_2][\text{NO}_3]\)
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