Consider this reaction: CICH₂CH₂C1 (g) → CH₂CHC1 (g) + HC1 (g) At a certain temperature it obeys this rate law. rate = = (0.00818 M S ¹) [CICH₂CH₂CI]² Suppose a vessel contains CICH₂CH₂Cl at a concentration of 1.16 M. Calculate how long it takes for the concentration of CICH₂CH₂Cl to decrease to 11.0% of its initial value. You may assume no other reaction is important. Round your answer to 2 significant digits. s □
Consider this reaction: CICH₂CH₂C1 (g) → CH₂CHC1 (g) + HC1 (g) At a certain temperature it obeys this rate law. rate = = (0.00818 M S ¹) [CICH₂CH₂CI]² Suppose a vessel contains CICH₂CH₂Cl at a concentration of 1.16 M. Calculate how long it takes for the concentration of CICH₂CH₂Cl to decrease to 11.0% of its initial value. You may assume no other reaction is important. Round your answer to 2 significant digits. s □
Chemistry
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Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
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![### Chemical Reaction and Rate Law
**Consider the following reaction:**
\[ \text{CICH}_2\text{CH}_2\text{Cl} \, (g) \rightarrow \text{CH}_2\text{CCl} \, (g) + \text{HCl} \, (g) \]
**At a given temperature, the reaction obeys the following rate law:**
\[ \text{rate} = (0.00818 \, \text{M}^{-1} \text{s}^{-1}) [\text{CICH}_2\text{CH}_2\text{Cl}]^2 \]
**Problem Statement:**
Suppose a vessel contains CICH₂CH₂Cl at a concentration of 1.16 M. Calculate how long it takes for the concentration of CICH₂CH₂Cl to decrease to 11.0% of its initial value. Assume that no other reaction is significant.
**Instructions:**
- Round your answer to 2 significant digits.
**Calculation:**
The detailed steps to solve this calculation will include:
1. Determining the final concentration of CICH₂CH₂Cl, which is 11.0% of 1.16 M.
2. Using the integrated rate law for a second-order reaction to find the time required for the concentration to decrease to this value.
**Final Answer Box:**
\[ \boxed{\phantom{0}} \, \text{s} \]
**Interactive Options:**
- There are interactive controls below the calculation box allowing users to input their answers, clear ("\[\mathsf { \times }\]") their work, and find help or hints ("?").](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F20b515c9-5e3a-448e-90a2-ac3b562e1523%2Fc94f99fd-66b5-4e29-a845-17a3f518f407%2Fytgf4b_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Chemical Reaction and Rate Law
**Consider the following reaction:**
\[ \text{CICH}_2\text{CH}_2\text{Cl} \, (g) \rightarrow \text{CH}_2\text{CCl} \, (g) + \text{HCl} \, (g) \]
**At a given temperature, the reaction obeys the following rate law:**
\[ \text{rate} = (0.00818 \, \text{M}^{-1} \text{s}^{-1}) [\text{CICH}_2\text{CH}_2\text{Cl}]^2 \]
**Problem Statement:**
Suppose a vessel contains CICH₂CH₂Cl at a concentration of 1.16 M. Calculate how long it takes for the concentration of CICH₂CH₂Cl to decrease to 11.0% of its initial value. Assume that no other reaction is significant.
**Instructions:**
- Round your answer to 2 significant digits.
**Calculation:**
The detailed steps to solve this calculation will include:
1. Determining the final concentration of CICH₂CH₂Cl, which is 11.0% of 1.16 M.
2. Using the integrated rate law for a second-order reaction to find the time required for the concentration to decrease to this value.
**Final Answer Box:**
\[ \boxed{\phantom{0}} \, \text{s} \]
**Interactive Options:**
- There are interactive controls below the calculation box allowing users to input their answers, clear ("\[\mathsf { \times }\]") their work, and find help or hints ("?").
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