Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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### Reaction Rate Study: H₃PO₄ Decomposition
A chemistry graduate student is studying the rate of this reaction:
\[ 2 \text{H}_3\text{PO}_4 (aq) \rightarrow \text{P}_2\text{O}_5 (aq) + 3 \text{H}_2\text{O} (aq) \]
The student fills a reaction vessel with \(\text{H}_3\text{PO}_4\) and measures its concentration as the reaction proceeds:
| Time (milliseconds) | \([\text{H}_3\text{PO}_4]\) (M) |
|--------------------|-------------------------|
| 0 | 0.0600 |
| 10 | 0.0320 |
| 20 | 0.0218 |
| 30 | 0.0165 |
| 40 | 0.0133 |
#### Use this data to answer the following questions:
1. **Write the rate law for this reaction.**
\[
\text{rate} = k \left[ \text{H}_3\text{PO}_4 \right]^n
\]
2. **Calculate the value of the rate constant \(k\).**
**Hint:** Round your answer to 2 significant digits. Also be sure your answer has the correct unit symbol.
\[
k = \_\_\_\_
\]
---
#### Diagram Explanation:
There is a graph-like icon and a calculator icon presented on the right side of the page. Below the questions, there is an option to select different graph boxes with points that might represent data plots or visual aids for calculations.
---
Note: The rate law shows the dependence of the reaction rate on the concentration of \(\text{H}_3\text{PO}_4\). \(k\) is the rate constant, and \(n\) is the order of the reaction with respect to \(\text{H}_3\text{PO}_4\). To calculate \(k\), you need to determine the order of the reaction and then apply an appropriate calculation method.](https://content.bartleby.com/qna-images/question/1067c048-27d4-462b-825c-b686bc07047b/ffb52a04-cd85-4fd9-9746-bf40585a25c0/03ri0fj.png)
Transcribed Image Text:---
### Reaction Rate Study: H₃PO₄ Decomposition
A chemistry graduate student is studying the rate of this reaction:
\[ 2 \text{H}_3\text{PO}_4 (aq) \rightarrow \text{P}_2\text{O}_5 (aq) + 3 \text{H}_2\text{O} (aq) \]
The student fills a reaction vessel with \(\text{H}_3\text{PO}_4\) and measures its concentration as the reaction proceeds:
| Time (milliseconds) | \([\text{H}_3\text{PO}_4]\) (M) |
|--------------------|-------------------------|
| 0 | 0.0600 |
| 10 | 0.0320 |
| 20 | 0.0218 |
| 30 | 0.0165 |
| 40 | 0.0133 |
#### Use this data to answer the following questions:
1. **Write the rate law for this reaction.**
\[
\text{rate} = k \left[ \text{H}_3\text{PO}_4 \right]^n
\]
2. **Calculate the value of the rate constant \(k\).**
**Hint:** Round your answer to 2 significant digits. Also be sure your answer has the correct unit symbol.
\[
k = \_\_\_\_
\]
---
#### Diagram Explanation:
There is a graph-like icon and a calculator icon presented on the right side of the page. Below the questions, there is an option to select different graph boxes with points that might represent data plots or visual aids for calculations.
---
Note: The rate law shows the dependence of the reaction rate on the concentration of \(\text{H}_3\text{PO}_4\). \(k\) is the rate constant, and \(n\) is the order of the reaction with respect to \(\text{H}_3\text{PO}_4\). To calculate \(k\), you need to determine the order of the reaction and then apply an appropriate calculation method.
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