The rate constant was determined at four temperatures for the following reaction: 2 CIO (g) →Cl2 (g) + O2 (g) The data were then plotted in the form In k versus 1/T in the plot on the right, which was found to have a best-fit line: y=-1590 x + 28.0 In k 22 21 0.0032 0.0036 0.0040 0.0044 1/T (K-¹) 23. Using the information provided, determine the activation energy for the reaction.
The rate constant was determined at four temperatures for the following reaction: 2 CIO (g) →Cl2 (g) + O2 (g) The data were then plotted in the form In k versus 1/T in the plot on the right, which was found to have a best-fit line: y=-1590 x + 28.0 In k 22 21 0.0032 0.0036 0.0040 0.0044 1/T (K-¹) 23. Using the information provided, determine the activation energy for the reaction.
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Chapter1: Chemical Foundations
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Using the information provided, determine the activation energy for the reaction. Please explain why the hilighted answer is correct.. thank you!
![The rate constant was determined at four temperatures for the following reaction:
\[2 \text{ClO} (g) \rightarrow \text{Cl}_2 (g) + \text{O}_2 (g)\]
The data were then plotted in the form \(\ln k\) versus \(1/T\) in the plot on the right, which was found to have a best-fit line:
\[y = -1590x + 28.0\]
**Graph Explanation:**
- The graph plots \(\ln k\) on the y-axis against \(1/T\) (in K\(^{-1}\)) on the x-axis.
- The graph is a straight line with a negative slope, indicating an exponential decrease in the reaction rate constant with increasing inverse temperature.
- The slope of the line \(-1590\) is related to the activation energy of the reaction.
**Question 23:**
Using the information provided, determine the activation energy for the reaction.
Options:
- A. 28.0 J/mol
- B. 1590 J/mol
- C. 1.32 × 10\(^4\) J/mol
- *D. 191 J/mol*
- E. 1.32 × 10\(^{-3}\) J/mol
The correct answer is highlighted: **C. 1.32 × 10\(^4\) J/mol**.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F87896b23-33e0-4e58-a967-e6f5a2b8fe91%2F89538cda-014a-47e6-a29a-34e04f09547f%2F6qvg7ha_processed.png&w=3840&q=75)
Transcribed Image Text:The rate constant was determined at four temperatures for the following reaction:
\[2 \text{ClO} (g) \rightarrow \text{Cl}_2 (g) + \text{O}_2 (g)\]
The data were then plotted in the form \(\ln k\) versus \(1/T\) in the plot on the right, which was found to have a best-fit line:
\[y = -1590x + 28.0\]
**Graph Explanation:**
- The graph plots \(\ln k\) on the y-axis against \(1/T\) (in K\(^{-1}\)) on the x-axis.
- The graph is a straight line with a negative slope, indicating an exponential decrease in the reaction rate constant with increasing inverse temperature.
- The slope of the line \(-1590\) is related to the activation energy of the reaction.
**Question 23:**
Using the information provided, determine the activation energy for the reaction.
Options:
- A. 28.0 J/mol
- B. 1590 J/mol
- C. 1.32 × 10\(^4\) J/mol
- *D. 191 J/mol*
- E. 1.32 × 10\(^{-3}\) J/mol
The correct answer is highlighted: **C. 1.32 × 10\(^4\) J/mol**.
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