### Determining the Rate of Disappearance of \( \text{N}_2\text{O}_5 \)The balanced chemical equation provided is:\[ 2\text{N}_2\text{O}_5(\text{aq}) \rightarrow 4\text{NO}_2(\text{aq}) + \text{O}_2(\text{g}) \]### TaskCalculate the rate of disappearance of \( \text{N}_2\text{O}_5 \) from 0 to 200 seconds.### Data TableThe following table presents the concentration of \( \text{N}_2\text{O}_5 \), \( \text{NO}_2 \), and \( \text{O}_2 \) over a period of time:| **Time (s)** | **[N\(_2\)O\(_5\)] (M)** | **[NO\(_2\)] (M)** | **[O\(_2\)] (M)** ||--------------|----------------------|-----------------|----------------|| 0 | 1.00 | 0 | 0 || 200 | 0.88 | ? | ? || 400 | 0.78 | 0.44 | 0.11 || 600 | 0.69 | 0.62 | 0.16 || 800 | 0.61 | 0.78 | 0.20 |### Calculation of RateThe rate of disappearance of \( \text{N}_2\text{O}_5 \) can be determined using the change in concentration over the change in time. Specifically, from time 0 to 200 seconds:\[ \text{Rate}_{\text{N}_2\text{O}_5} = - \frac{\Delta [\text{N}_2\text{O}_5]}{\Delta t} = - \frac{[N_2O_5]_{200s} - [N_2O_5]_{0s}}{200s - 0s} \]Substitute the values from the table:\[ \text{Rate}_{\text{N}_2\text{O}_5} = - \frac{0.88 - 1.00

Given: 2 N2O5(aq)→4NO2(aq)+O2( g) To find: rate of disappearance of N2O5 from 0 to 200 seconds.

2N₂O5 (aq) → 4NO₂ (aq) + O₂(g) What is the rate of disappearance of N2O5 from 0 to 200 seconds? Time [N₂O5] [NO₂] [0₂] 0 1.00 0 0 200 0.88 ? ? 400 0.78 0.44 0.11 600 0.69 0.62 0.16 800 0.61 0.78 0.20 RateN₂O5 = [?] x 10¹² M/s Coefficient (green) Exponent (yellow) Enter

2N₂O5 (aq) → 4NO₂ (aq) + O₂(g) What is the rate of disappearance of N2O5 from 0 to 200 seconds? Time [N₂O5] [NO₂] [0₂] 0 1.00 0 0 200 0.88 ? ? 400 0.78 0.44 0.11 600 0.69 0.62 0.16 800 0.61 0.78 0.20 RateN₂O5 = [?] x 10¹² M/s Coefficient (green) Exponent (yellow) Enter

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

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Question

### Determining the Rate of Disappearance of \( \text{N}_2\text{O}_5 \)

The balanced chemical equation provided is:
\[ 2\text{N}_2\text{O}_5(\text{aq}) \rightarrow 4\text{NO}_2(\text{aq}) + \text{O}_2(\text{g}) \]

### Task

Calculate the rate of disappearance of \( \text{N}_2\text{O}_5 \) from 0 to 200 seconds.

### Data Table

The following table presents the concentration of \( \text{N}_2\text{O}_5 \), \( \text{NO}_2 \), and \( \text{O}_2 \) over a period of time:

| **Time (s)** | **[N\(_2\)O\(_5\)] (M)** | **[NO\(_2\)] (M)** | **[O\(_2\)] (M)** |
|--------------|----------------------|-----------------|----------------|
| 0 | 1.00 | 0 | 0 |
| 200 | 0.88 | ? | ? |
| 400 | 0.78 | 0.44 | 0.11 |
| 600 | 0.69 | 0.62 | 0.16 |
| 800 | 0.61 | 0.78 | 0.20 |

### Calculation of Rate

The rate of disappearance of \( \text{N}_2\text{O}_5 \) can be determined using the change in concentration over the change in time. Specifically, from time 0 to 200 seconds:

\[ \text{Rate}_{\text{N}_2\text{O}_5} = - \frac{\Delta [\text{N}_2\text{O}_5]}{\Delta t} = - \frac{[N_2O_5]_{200s} - [N_2O_5]_{0s}}{200s - 0s} \]

Substitute the values from the table:

\[ \text{Rate}_{\text{N}_2\text{O}_5} = - \frac{0.88 - 1.00

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