The kinetics of decomposition of N 20 5 was studied by measuring the concentration of N 20 5 as a function of time. The plot of concentration versus time is not linear, but the plot of the natural log of the concentration versus time is linear with a slope of -0.0358. What is the rate law for the decomposition?
The kinetics of decomposition of N 20 5 was studied by measuring the concentration of N 20 5 as a function of time. The plot of concentration versus time is not linear, but the plot of the natural log of the concentration versus time is linear with a slope of -0.0358. What is the rate law for the decomposition?
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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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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![**Question 8**
The kinetics of decomposition of \( \text{N}_2\text{O}_5 \) was studied by measuring the concentration of \( \text{N}_2\text{O}_5 \) as a function of time. The plot of concentration versus time is not linear, but the plot of the natural log of the concentration versus time is linear with a slope of -0.0358. What is the rate law for the decomposition?
- ( ) rate = -0.0358(sec\(^{-1}\))[N\(_2\)O\(_5\)]
- ( ) rate = 0.0358(sec\(^{-1}\))[N\(_2\)O\(_5\)]
- ( ) rate = 0.0358(M\(^{-1}\)s\(^{-1}\))[N\(_2\)O\(_5\)]\(^2\)
- ( ) rate = 0.0358 M/s](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F824fa1c6-40a3-49c1-bdd2-6faa45715099%2F77323d56-2ff1-4979-a287-5d1cdbb1da28%2Fqew2tuh_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Question 8**
The kinetics of decomposition of \( \text{N}_2\text{O}_5 \) was studied by measuring the concentration of \( \text{N}_2\text{O}_5 \) as a function of time. The plot of concentration versus time is not linear, but the plot of the natural log of the concentration versus time is linear with a slope of -0.0358. What is the rate law for the decomposition?
- ( ) rate = -0.0358(sec\(^{-1}\))[N\(_2\)O\(_5\)]
- ( ) rate = 0.0358(sec\(^{-1}\))[N\(_2\)O\(_5\)]
- ( ) rate = 0.0358(M\(^{-1}\)s\(^{-1}\))[N\(_2\)O\(_5\)]\(^2\)
- ( ) rate = 0.0358 M/s
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Plot of log of concentration vs time is linear. This suggests that reaction follows first order kinetics.
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