Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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![**Title: Understanding Reaction Rates – A Case Study**
**Overview:**
A chemistry graduate student is studying the rate of the reaction:
\[ \text{H}_2\text{CO}_3 \,(\text{aq}) \rightarrow \text{H}_2\text{O} \,(\text{aq}) + \text{CO}_2 \,(\text{aq}) \]
She fills a reaction vessel with \(\text{H}_2\text{CO}_3\) and measures its concentration as the reaction proceeds.
**Data Table:**
| Time (seconds) | \([\text{H}_2\text{CO}_3]\) |
|----------------|----------------------|
| 0 | 0.800 M |
| 1.0 | 0.144 M |
| 2.0 | 0.0794 M |
| 3.0 | 0.0547 M |
| 4.0 | 0.0418 M |
**Instructions:**
Use this data to answer the following questions.
1. **Write the rate law for this reaction:**
\[
\text{rate} = k [\text{H}_2\text{CO}_3]
\]
2. **Calculate the value of the rate constant \(k\):**
Round your answer to 2 significant digits. Also, ensure your answer has the correct unit symbol.
\[
k = \, [\text{Enter your answer here}]
\]
**Graph Explanation:**
The graph provided illustrates changes in \([\text{H}_2\text{CO}_3]\) over time, with concentration on the y-axis and time on the x-axis. The data points plot the measured concentrations at each time interval. Analysis of these points helps determine the rate of reaction and calculate the rate constant.
**Note:**
Ensure calculations reflect changes in concentration over time to properly derive \(k\).](https://content.bartleby.com/qna-images/question/a60cc6ce-11de-444a-af29-e9eb1b50e640/810a9451-df4a-4d93-a7d6-14f59114d7fa/hyjulsc_processed.png)
Transcribed Image Text:**Title: Understanding Reaction Rates – A Case Study**
**Overview:**
A chemistry graduate student is studying the rate of the reaction:
\[ \text{H}_2\text{CO}_3 \,(\text{aq}) \rightarrow \text{H}_2\text{O} \,(\text{aq}) + \text{CO}_2 \,(\text{aq}) \]
She fills a reaction vessel with \(\text{H}_2\text{CO}_3\) and measures its concentration as the reaction proceeds.
**Data Table:**
| Time (seconds) | \([\text{H}_2\text{CO}_3]\) |
|----------------|----------------------|
| 0 | 0.800 M |
| 1.0 | 0.144 M |
| 2.0 | 0.0794 M |
| 3.0 | 0.0547 M |
| 4.0 | 0.0418 M |
**Instructions:**
Use this data to answer the following questions.
1. **Write the rate law for this reaction:**
\[
\text{rate} = k [\text{H}_2\text{CO}_3]
\]
2. **Calculate the value of the rate constant \(k\):**
Round your answer to 2 significant digits. Also, ensure your answer has the correct unit symbol.
\[
k = \, [\text{Enter your answer here}]
\]
**Graph Explanation:**
The graph provided illustrates changes in \([\text{H}_2\text{CO}_3]\) over time, with concentration on the y-axis and time on the x-axis. The data points plot the measured concentrations at each time interval. Analysis of these points helps determine the rate of reaction and calculate the rate constant.
**Note:**
Ensure calculations reflect changes in concentration over time to properly derive \(k\).
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