**Chemical Reaction and Kinetics**The activation energy for the gas phase isomerization of methyl cis-cinnamate is 174 kJ.**Chemical Equation:**\[ \text{cis-C}_6\text{H}_5 \text{CH} = \text{CHCOOCH}_3 \rightarrow \text{trans-C}_6\text{H}_5 \text{CH} = \text{CHCOOCH}_3 \]**Rate Constants:**- The rate constant at 652 K is $ 4.09 \times 10^{-4} \, \text{s}^{-1} $.- The rate constant will be $ 0.00285 \, \text{s}^{-1} $ at [blank] K.**Interactive Options:**- **Submit Answer**: Click to submit your solution.- **Retry Entire Group**: Option to retry the problem set.- **Attempts Indicator**: Indicates 9 more group attempts remaining. The gas phase decomposition of nitrogen dioxide at 383 °C\[ \text{NO}_2 (g) \rightarrow \text{NO}(g) + \frac{1}{2} \text{O}_2 (g) \]is second order in $\text{NO}_2$.In one experiment, when the initial concentration of $\text{NO}_2$ was 0.136 M, the concentration of $\text{NO}_2$ dropped to $3.62 \times 10^{-2}$ M after 28.7 seconds had passed.Based on these data, the rate constant for the reaction is $\boxed{\,}$ M$^{-1}$ s$^{-1}$.

Answered: The activation energy for the gas phase…

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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**Chemical Reaction and Kinetics**

The activation energy for the gas phase isomerization of methyl cis-cinnamate is 174 kJ.

**Chemical Equation:**
\[ \text{cis-C}_6\text{H}_5 \text{CH} = \text{CHCOOCH}_3 \rightarrow \text{trans-C}_6\text{H}_5 \text{CH} = \text{CHCOOCH}_3 \]

**Rate Constants:**
- The rate constant at 652 K is $ 4.09 \times 10^{-4} \, \text{s}^{-1} $.
- The rate constant will be $ 0.00285 \, \text{s}^{-1} $ at [blank] K.

**Interactive Options:**
- **Submit Answer**: Click to submit your solution.
- **Retry Entire Group**: Option to retry the problem set.
- **Attempts Indicator**: Indicates 9 more group attempts remaining.

The gas phase decomposition of nitrogen dioxide at 383 °C

\[ \text{NO}_2 (g) \rightarrow \text{NO}(g) + \frac{1}{2} \text{O}_2 (g) \]

is second order in $\text{NO}_2$.

In one experiment, when the initial concentration of $\text{NO}_2$ was 0.136 M, the concentration of $\text{NO}_2$ dropped to $3.62 \times 10^{-2}$ M after 28.7 seconds had passed.

Based on these data, the rate constant for the reaction is $\boxed{\,}$ M$^{-1}$ s$^{-1}$.

Expert Solution

Step 1: Arrhenius equation

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Answer-1

$ln straight k subscript 2 over straight k subscript 1 equals straight E subscript straight a over straight R open parentheses 1 over straight T subscript 1 minus 1 over straight T subscript 2 close parentheses$

Here:

$straight E subscript straight a equals Activation space energy straight R equals Universal space gas space constant$

k₁ and k₂ are rate constants at temperatures T₁ and T₂ respectively

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