Write a balanced reaction for which the following rate relationships are true. 1 AIN2]A[02] 1 AN20] 2. Rate %3D %3D 2 At At At O 2 N2 + O2→ 2 N20 ㅇ을 시2+02→ N20 O N20 N2 + 2 02 O 2 N20 → 2 N2 + O2 ㅇ글 N20→를 N2+ 02
Write a balanced reaction for which the following rate relationships are true. 1 AIN2]A[02] 1 AN20] 2. Rate %3D %3D 2 At At At O 2 N2 + O2→ 2 N20 ㅇ을 시2+02→ N20 O N20 N2 + 2 02 O 2 N20 → 2 N2 + O2 ㅇ글 N20→를 N2+ 02
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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![### Determining Balanced Reactions Based on Rate Relationships
In this exercise, you are given a set of rate equations and asked to identify which balanced chemical reaction corresponds to these rates. The provided rate equations are:
\[
\text{Rate} = \frac{1}{2} \frac{\Delta[\text{N}_2]}{\Delta t} = \frac{\Delta[\text{O}_2]}{\Delta t} = -\frac{1}{2} \frac{\Delta[\text{N}_2\text{O}]}{\Delta t}
\]
This indicates the relationships between the rates of change of the concentrations of nitrogen (\(\text{N}_2\)), oxygen (\(\text{O}_2\)), and nitrous oxide (\(\text{N}_2\text{O}\)).
Now, you need to identify the balanced reaction among the following options:
1. \(2 \text{N}_2 + \text{O}_2 \rightarrow 2 \text{N}_2\text{O}\)
2. \(\frac{1}{2} \text{N}_2 + \text{O}_2 \rightarrow \frac{1}{2} \text{N}_2\text{O}\)
3. \(\text{N}_2\text{O} \rightarrow \text{N}_2 + \frac{1}{2} \text{O}_2\)
4. \(2 \text{N}_2\text{O} \rightarrow 2 \text{N}_2 + \text{O}_2\)
5. \(\frac{1}{2} \text{N}_2\text{O} \rightarrow \frac{1}{2} \text{N}_2 + \text{O}_2\)
Each option represents a different chemical reaction. The correct reaction should satisfy the given rate relationships, meaning the stoichiometric coefficients in the reaction must align with the coefficients in the rate equations.
Based on the rate equations:
- The rate of change of \(\text{N}_2\) is half that of \(\text{N}_2\text{O}\), implying for every 1 molecule of \(\text{N}_2\text{O}\) reacted, 2 molecules of \(\text{N}_2\) are produced.
- The rate of change of \(\text](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F560885b1-95a6-46a1-8479-9132da42c8bd%2F42336158-cadf-4c39-96ae-370bb6fd86da%2F3wvaob_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Determining Balanced Reactions Based on Rate Relationships
In this exercise, you are given a set of rate equations and asked to identify which balanced chemical reaction corresponds to these rates. The provided rate equations are:
\[
\text{Rate} = \frac{1}{2} \frac{\Delta[\text{N}_2]}{\Delta t} = \frac{\Delta[\text{O}_2]}{\Delta t} = -\frac{1}{2} \frac{\Delta[\text{N}_2\text{O}]}{\Delta t}
\]
This indicates the relationships between the rates of change of the concentrations of nitrogen (\(\text{N}_2\)), oxygen (\(\text{O}_2\)), and nitrous oxide (\(\text{N}_2\text{O}\)).
Now, you need to identify the balanced reaction among the following options:
1. \(2 \text{N}_2 + \text{O}_2 \rightarrow 2 \text{N}_2\text{O}\)
2. \(\frac{1}{2} \text{N}_2 + \text{O}_2 \rightarrow \frac{1}{2} \text{N}_2\text{O}\)
3. \(\text{N}_2\text{O} \rightarrow \text{N}_2 + \frac{1}{2} \text{O}_2\)
4. \(2 \text{N}_2\text{O} \rightarrow 2 \text{N}_2 + \text{O}_2\)
5. \(\frac{1}{2} \text{N}_2\text{O} \rightarrow \frac{1}{2} \text{N}_2 + \text{O}_2\)
Each option represents a different chemical reaction. The correct reaction should satisfy the given rate relationships, meaning the stoichiometric coefficients in the reaction must align with the coefficients in the rate equations.
Based on the rate equations:
- The rate of change of \(\text{N}_2\) is half that of \(\text{N}_2\text{O}\), implying for every 1 molecule of \(\text{N}_2\text{O}\) reacted, 2 molecules of \(\text{N}_2\) are produced.
- The rate of change of \(\text
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