### Gas Phase Decomposition of Sulfuryl Chloride **Decomposition Reaction:** \[ \text{SO}_2\text{Cl}_2 \rightarrow \text{SO}_2 + \text{Cl}_2 \] **Conditions:** - Temperature: 600 K **Experimental Data:** The following table represents the concentration of sulfuryl chloride \((\text{SO}_2\text{Cl}_2)\) over different time intervals: | \([\text{SO}_2\text{Cl}_2]\), M | 3.55 × 10\(^-3\) | 2.35 × 10\(^-3\) | 1.55 × 10\(^-3\) | 1.02 × 10\(^-3\) | |--------------------------------|------------------|------------------|------------------|------------------| | **Time, min** | 0 | 148 | 296 | 444 | **Calculation Task:** Determine the average rate of disappearance of \(\text{SO}_2\text{Cl}_2\) using the concentration data from \( t = 0 \, \text{min} \) to \( t = 148 \, \text{min} \). **Required Answer:** The average rate of disappearance of \(\text{SO}_2\text{Cl}_2\) over the given time period is as follows: \[ \text{Rate} = \frac{\Delta [\text{SO}_2\text{Cl}_2]}{\Delta t} \] Where: - \(\Delta [\text{SO}_2\text{Cl}_2] = (\text{Final concentration} - \text{Initial concentration})\) - \(\Delta t = (\text{Final time} - \text{Initial time})\) Substitute the values: \[ \Delta [\text{SO}_2\text{Cl}_2] = 2.35 \times 10^{-3} \, \text{M} - 3.55 \times 10^{-3} \, \text{M} = -1.20 \times 10^{-3} \, \text{M} \] \[ \Delta t = 148 \, \text{min} - 0 \, \text{min} = 148
### Gas Phase Decomposition of Sulfuryl Chloride **Decomposition Reaction:** \[ \text{SO}_2\text{Cl}_2 \rightarrow \text{SO}_2 + \text{Cl}_2 \] **Conditions:** - Temperature: 600 K **Experimental Data:** The following table represents the concentration of sulfuryl chloride \((\text{SO}_2\text{Cl}_2)\) over different time intervals: | \([\text{SO}_2\text{Cl}_2]\), M | 3.55 × 10\(^-3\) | 2.35 × 10\(^-3\) | 1.55 × 10\(^-3\) | 1.02 × 10\(^-3\) | |--------------------------------|------------------|------------------|------------------|------------------| | **Time, min** | 0 | 148 | 296 | 444 | **Calculation Task:** Determine the average rate of disappearance of \(\text{SO}_2\text{Cl}_2\) using the concentration data from \( t = 0 \, \text{min} \) to \( t = 148 \, \text{min} \). **Required Answer:** The average rate of disappearance of \(\text{SO}_2\text{Cl}_2\) over the given time period is as follows: \[ \text{Rate} = \frac{\Delta [\text{SO}_2\text{Cl}_2]}{\Delta t} \] Where: - \(\Delta [\text{SO}_2\text{Cl}_2] = (\text{Final concentration} - \text{Initial concentration})\) - \(\Delta t = (\text{Final time} - \text{Initial time})\) Substitute the values: \[ \Delta [\text{SO}_2\text{Cl}_2] = 2.35 \times 10^{-3} \, \text{M} - 3.55 \times 10^{-3} \, \text{M} = -1.20 \times 10^{-3} \, \text{M} \] \[ \Delta t = 148 \, \text{min} - 0 \, \text{min} = 148
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...
Related questions
Question
![### Gas Phase Decomposition of Sulfuryl Chloride
**Decomposition Reaction:**
\[ \text{SO}_2\text{Cl}_2 \rightarrow \text{SO}_2 + \text{Cl}_2 \]
**Conditions:**
- Temperature: 600 K
**Experimental Data:**
The following table represents the concentration of sulfuryl chloride \((\text{SO}_2\text{Cl}_2)\) over different time intervals:
| \([\text{SO}_2\text{Cl}_2]\), M | 3.55 × 10\(^-3\) | 2.35 × 10\(^-3\) | 1.55 × 10\(^-3\) | 1.02 × 10\(^-3\) |
|--------------------------------|------------------|------------------|------------------|------------------|
| **Time, min** | 0 | 148 | 296 | 444 |
**Calculation Task:**
Determine the average rate of disappearance of \(\text{SO}_2\text{Cl}_2\) using the concentration data from \( t = 0 \, \text{min} \) to \( t = 148 \, \text{min} \).
**Required Answer:**
The average rate of disappearance of \(\text{SO}_2\text{Cl}_2\) over the given time period is as follows:
\[ \text{Rate} = \frac{\Delta [\text{SO}_2\text{Cl}_2]}{\Delta t} \]
Where:
- \(\Delta [\text{SO}_2\text{Cl}_2] = (\text{Final concentration} - \text{Initial concentration})\)
- \(\Delta t = (\text{Final time} - \text{Initial time})\)
Substitute the values:
\[ \Delta [\text{SO}_2\text{Cl}_2] = 2.35 \times 10^{-3} \, \text{M} - 3.55 \times 10^{-3} \, \text{M} = -1.20 \times 10^{-3} \, \text{M} \]
\[ \Delta t = 148 \, \text{min} - 0 \, \text{min} = 148](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F77bfbc94-404c-40d5-8c71-b661b10ff379%2Fc369a52e-b7e4-4730-8c40-e30b4a0c6e6c%2F0mftqc5_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Gas Phase Decomposition of Sulfuryl Chloride
**Decomposition Reaction:**
\[ \text{SO}_2\text{Cl}_2 \rightarrow \text{SO}_2 + \text{Cl}_2 \]
**Conditions:**
- Temperature: 600 K
**Experimental Data:**
The following table represents the concentration of sulfuryl chloride \((\text{SO}_2\text{Cl}_2)\) over different time intervals:
| \([\text{SO}_2\text{Cl}_2]\), M | 3.55 × 10\(^-3\) | 2.35 × 10\(^-3\) | 1.55 × 10\(^-3\) | 1.02 × 10\(^-3\) |
|--------------------------------|------------------|------------------|------------------|------------------|
| **Time, min** | 0 | 148 | 296 | 444 |
**Calculation Task:**
Determine the average rate of disappearance of \(\text{SO}_2\text{Cl}_2\) using the concentration data from \( t = 0 \, \text{min} \) to \( t = 148 \, \text{min} \).
**Required Answer:**
The average rate of disappearance of \(\text{SO}_2\text{Cl}_2\) over the given time period is as follows:
\[ \text{Rate} = \frac{\Delta [\text{SO}_2\text{Cl}_2]}{\Delta t} \]
Where:
- \(\Delta [\text{SO}_2\text{Cl}_2] = (\text{Final concentration} - \text{Initial concentration})\)
- \(\Delta t = (\text{Final time} - \text{Initial time})\)
Substitute the values:
\[ \Delta [\text{SO}_2\text{Cl}_2] = 2.35 \times 10^{-3} \, \text{M} - 3.55 \times 10^{-3} \, \text{M} = -1.20 \times 10^{-3} \, \text{M} \]
\[ \Delta t = 148 \, \text{min} - 0 \, \text{min} = 148
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
Step by step
Solved in 2 steps
Recommended textbooks for you
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY