3. The decomposition of N₂O5 in the gas phase was studied at constant temperature, 2N2O5 (g) → 4NO₂ (g) + O₂(g) The following results were collected: [N₂O5] Ln[N₂O5] Time (s) 0.1000 0 0.0707 50 0.0500 100 0.0250 200 0.0125 300 0.00625 400 a. Complete the table. Using the data and graph paper, plot the [N₂O5] versus time and Ln[N₂O5] versus time. Determine the value of k. Which graph did y you use?
3. The decomposition of N₂O5 in the gas phase was studied at constant temperature, 2N2O5 (g) → 4NO₂ (g) + O₂(g) The following results were collected: [N₂O5] Ln[N₂O5] Time (s) 0.1000 0 0.0707 50 0.0500 100 0.0250 200 0.0125 300 0.00625 400 a. Complete the table. Using the data and graph paper, plot the [N₂O5] versus time and Ln[N₂O5] versus time. Determine the value of k. Which graph did y you use?
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
Section: Chapter Questions
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![### Study of N₂O₅ Decomposition in the Gas Phase
#### Chemical Reaction
The decomposition of \( \text{N}_2\text{O}_5 \) in the gas phase was studied at a constant temperature. The reaction is represented by the following chemical equation:
\[ 2\text{N}_2\text{O}_5 (\text{g}) \rightarrow 4\text{NO}_2 (\text{g}) + \text{O}_2 (\text{g}) \]
#### Experimental Data
The following results were collected during the experiment:
| [N₂O₅] (M) | Ln[N₂O₅] | Time (s) |
|------------|----------|----------|
| 0.1000 | | 0 |
| 0.0707 | | 50 |
| 0.0500 | | 100 |
| 0.0250 | | 200 |
| 0.0125 | | 300 |
| 0.00625 | | 400 |
#### Instructions for Analysis
1. **Complete the Table:**
- Calculate Ln[N₂O₅] for each concentration.
- Fill in the corresponding Ln[N₂O₅] values in the table above.
2. **Graphing:**
- Using the data and graph paper, plot the concentration of \( \text{N}_2\text{O}_5 \) ([N₂O₅]) versus time.
- Also, plot the natural logarithm of the concentration of \( \text{N}_2\text{O}_5 \) (Ln[N₂O₅]) versus time.
- Determine the rate constant \( k \).
- Identify which graph (linear plot) you used for this calculation.
3. **Half-Life Calculations:**
- On your graph of [N₂O₅] versus time, highlight the times it takes for each halving of the reactant concentration.
- Calculate the half-life using this information.
- Using the half-life, calculate the rate constant \( k \).](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F06775211-663a-4915-8f33-409e31fb1882%2Fedefecde-f856-46d1-b81c-c2fd232f6871%2F58dbds5_processed.png&w=3840&q=75)
Transcribed Image Text:### Study of N₂O₅ Decomposition in the Gas Phase
#### Chemical Reaction
The decomposition of \( \text{N}_2\text{O}_5 \) in the gas phase was studied at a constant temperature. The reaction is represented by the following chemical equation:
\[ 2\text{N}_2\text{O}_5 (\text{g}) \rightarrow 4\text{NO}_2 (\text{g}) + \text{O}_2 (\text{g}) \]
#### Experimental Data
The following results were collected during the experiment:
| [N₂O₅] (M) | Ln[N₂O₅] | Time (s) |
|------------|----------|----------|
| 0.1000 | | 0 |
| 0.0707 | | 50 |
| 0.0500 | | 100 |
| 0.0250 | | 200 |
| 0.0125 | | 300 |
| 0.00625 | | 400 |
#### Instructions for Analysis
1. **Complete the Table:**
- Calculate Ln[N₂O₅] for each concentration.
- Fill in the corresponding Ln[N₂O₅] values in the table above.
2. **Graphing:**
- Using the data and graph paper, plot the concentration of \( \text{N}_2\text{O}_5 \) ([N₂O₅]) versus time.
- Also, plot the natural logarithm of the concentration of \( \text{N}_2\text{O}_5 \) (Ln[N₂O₅]) versus time.
- Determine the rate constant \( k \).
- Identify which graph (linear plot) you used for this calculation.
3. **Half-Life Calculations:**
- On your graph of [N₂O₅] versus time, highlight the times it takes for each halving of the reactant concentration.
- Calculate the half-life using this information.
- Using the half-life, calculate the rate constant \( k \).
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