H2g) +O2e) 2HCl Time (s) [H2] (M) [C] (M) [HCI) (M) 0.00 0.300 0.400 0.000 2.00 0.200 0.300 0.200 What is the rate of reaction for chlorine for the reaction?
H2g) +O2e) 2HCl Time (s) [H2] (M) [C] (M) [HCI) (M) 0.00 0.300 0.400 0.000 2.00 0.200 0.300 0.200 What is the rate of reaction for chlorine for the reaction?
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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![### Reaction Rate Analysis
The chemical reaction provided is:
\[ \text{H}_2 (g) + \text{O}_2 (g) \rightarrow 2\text{HCl} (g) \]
The table below shows the concentrations of the reactants and products over a period of time:
| Time (s) | \([\text{H}_2]\) (M) | \([\text{Cl}_2]\) (M) | \([\text{HCl}]\) (M) |
|----------|--------------------|---------------------|-------------------|
| 0.00 | 0.300 | 0.400 | 0.000 |
| 2.00 | 0.200 | 0.300 | 0.200 |
### Explanation of the Data
The reaction starts with initial concentrations of hydrogen \((\text{H}_2)\) and chlorine \((\text{Cl}_2)\) and no hydrogen chloride \((\text{HCl})\) is present at time zero. As the reaction progresses to 2 seconds, the concentration of \((\text{H}_2)\) decreases to 0.200 M, \((\text{Cl}_2)\) decreases to 0.300 M, and \((\text{HCl})\) increases to 0.200 M.
### Rate of Reaction for Chlorine
The rate of reaction for chlorine can be calculated using the change in concentration over time:
\[
\text{Rate of } [\text{Cl}_2] = \frac{\text{Change in concentration of } [\text{Cl}_2]}{\text{Change in time}} = \frac{0.300 \, \text{M} - 0.400 \, \text{M}}{2.00 \, \text{s} - 0.00 \, \text{s}} = -0.050 \, \text{M/s}
\]
This indicates the rate at which chlorine is being consumed in the reaction. The negative sign indicates a decrease in concentration.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F6874e1f1-5298-4a44-ae8e-fa9c3662cb0d%2Fdbe2b24c-2226-4acc-b67b-6a384312d0c4%2Fx1tumin_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Reaction Rate Analysis
The chemical reaction provided is:
\[ \text{H}_2 (g) + \text{O}_2 (g) \rightarrow 2\text{HCl} (g) \]
The table below shows the concentrations of the reactants and products over a period of time:
| Time (s) | \([\text{H}_2]\) (M) | \([\text{Cl}_2]\) (M) | \([\text{HCl}]\) (M) |
|----------|--------------------|---------------------|-------------------|
| 0.00 | 0.300 | 0.400 | 0.000 |
| 2.00 | 0.200 | 0.300 | 0.200 |
### Explanation of the Data
The reaction starts with initial concentrations of hydrogen \((\text{H}_2)\) and chlorine \((\text{Cl}_2)\) and no hydrogen chloride \((\text{HCl})\) is present at time zero. As the reaction progresses to 2 seconds, the concentration of \((\text{H}_2)\) decreases to 0.200 M, \((\text{Cl}_2)\) decreases to 0.300 M, and \((\text{HCl})\) increases to 0.200 M.
### Rate of Reaction for Chlorine
The rate of reaction for chlorine can be calculated using the change in concentration over time:
\[
\text{Rate of } [\text{Cl}_2] = \frac{\text{Change in concentration of } [\text{Cl}_2]}{\text{Change in time}} = \frac{0.300 \, \text{M} - 0.400 \, \text{M}}{2.00 \, \text{s} - 0.00 \, \text{s}} = -0.050 \, \text{M/s}
\]
This indicates the rate at which chlorine is being consumed in the reaction. The negative sign indicates a decrease in concentration.
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