## Gas Phase Decomposition of Sulfuryl Chloride The following data are for the gas phase decomposition of sulfuryl chloride at 600 K. Reaction equation: $$\text{SO}_2\text{Cl}_2 (\text{g}) \rightarrow \text{SO}_2 (\text{g}) + \text{Cl}_2 (\text{g})$$ ### Data Table | [SO₂Cl₂], M | 1.75×10⁻³ | 8.75×10⁻⁴ | 4.38×10⁻⁴ | 2.19×10⁻⁴ | |----------------|----------|-----------|-----------|-----------| | time, min | 0 | 182 | 364 | 546 | ### Analysis **Hint:** It is not necessary to graph these data. 1. The half-life observed for this reaction is _______ min. 2. Based on these data, the rate constant for this ____ order reaction is _______ min⁻¹. ### Additional Instructions To complete the analysis, fill in the following: 1. Calculate the half-life of the reaction by examining the time it takes for the concentration of SO₂Cl₂ to decrease by half. 2. Determine the order of the reaction (zero, first, or second) and calculate the rate constant, \( k \). Select the appropriate order from the dropdown and calculate the rate constant based on your selected order. #### Submission Use the form below to submit your answers. - **Submit Answer** - **Try Another Version** - 10 item attempts remaining --- This information and data analysis is crucial for understanding the kinetics of the reaction under study. Make sure to perform the calculations carefully, paying close attention to the units and the consistency of the data.
## Gas Phase Decomposition of Sulfuryl Chloride The following data are for the gas phase decomposition of sulfuryl chloride at 600 K. Reaction equation: $$\text{SO}_2\text{Cl}_2 (\text{g}) \rightarrow \text{SO}_2 (\text{g}) + \text{Cl}_2 (\text{g})$$ ### Data Table | [SO₂Cl₂], M | 1.75×10⁻³ | 8.75×10⁻⁴ | 4.38×10⁻⁴ | 2.19×10⁻⁴ | |----------------|----------|-----------|-----------|-----------| | time, min | 0 | 182 | 364 | 546 | ### Analysis **Hint:** It is not necessary to graph these data. 1. The half-life observed for this reaction is _______ min. 2. Based on these data, the rate constant for this ____ order reaction is _______ min⁻¹. ### Additional Instructions To complete the analysis, fill in the following: 1. Calculate the half-life of the reaction by examining the time it takes for the concentration of SO₂Cl₂ to decrease by half. 2. Determine the order of the reaction (zero, first, or second) and calculate the rate constant, \( k \). Select the appropriate order from the dropdown and calculate the rate constant based on your selected order. #### Submission Use the form below to submit your answers. - **Submit Answer** - **Try Another Version** - 10 item attempts remaining --- This information and data analysis is crucial for understanding the kinetics of the reaction under study. Make sure to perform the calculations carefully, paying close attention to the units and the consistency of the data.
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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For the drop down menu on number 2, the options are zero, first, and second.
![## Gas Phase Decomposition of Sulfuryl Chloride
The following data are for the gas phase decomposition of sulfuryl chloride at 600 K.
Reaction equation:
$$\text{SO}_2\text{Cl}_2 (\text{g}) \rightarrow \text{SO}_2 (\text{g}) + \text{Cl}_2 (\text{g})$$
### Data Table
| [SO₂Cl₂], M | 1.75×10⁻³ | 8.75×10⁻⁴ | 4.38×10⁻⁴ | 2.19×10⁻⁴ |
|----------------|----------|-----------|-----------|-----------|
| time, min | 0 | 182 | 364 | 546 |
### Analysis
**Hint:** It is not necessary to graph these data.
1. The half-life observed for this reaction is _______ min.
2. Based on these data, the rate constant for this ____ order reaction is _______ min⁻¹.
### Additional Instructions
To complete the analysis, fill in the following:
1. Calculate the half-life of the reaction by examining the time it takes for the concentration of SO₂Cl₂ to decrease by half.
2. Determine the order of the reaction (zero, first, or second) and calculate the rate constant, \( k \).
Select the appropriate order from the dropdown and calculate the rate constant based on your selected order.
#### Submission
Use the form below to submit your answers.
- **Submit Answer**
- **Try Another Version**
- 10 item attempts remaining
---
This information and data analysis is crucial for understanding the kinetics of the reaction under study. Make sure to perform the calculations carefully, paying close attention to the units and the consistency of the data.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F848b3b37-0e47-4626-8c62-5eaa520ec29b%2Fd8065dee-d968-43de-9dfd-1c521cb315ba%2Fc49l038.jpeg&w=3840&q=75)
Transcribed Image Text:## Gas Phase Decomposition of Sulfuryl Chloride
The following data are for the gas phase decomposition of sulfuryl chloride at 600 K.
Reaction equation:
$$\text{SO}_2\text{Cl}_2 (\text{g}) \rightarrow \text{SO}_2 (\text{g}) + \text{Cl}_2 (\text{g})$$
### Data Table
| [SO₂Cl₂], M | 1.75×10⁻³ | 8.75×10⁻⁴ | 4.38×10⁻⁴ | 2.19×10⁻⁴ |
|----------------|----------|-----------|-----------|-----------|
| time, min | 0 | 182 | 364 | 546 |
### Analysis
**Hint:** It is not necessary to graph these data.
1. The half-life observed for this reaction is _______ min.
2. Based on these data, the rate constant for this ____ order reaction is _______ min⁻¹.
### Additional Instructions
To complete the analysis, fill in the following:
1. Calculate the half-life of the reaction by examining the time it takes for the concentration of SO₂Cl₂ to decrease by half.
2. Determine the order of the reaction (zero, first, or second) and calculate the rate constant, \( k \).
Select the appropriate order from the dropdown and calculate the rate constant based on your selected order.
#### Submission
Use the form below to submit your answers.
- **Submit Answer**
- **Try Another Version**
- 10 item attempts remaining
---
This information and data analysis is crucial for understanding the kinetics of the reaction under study. Make sure to perform the calculations carefully, paying close attention to the units and the consistency of the data.
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