Determine the average rate of change of B from t = 0 s to Time (s) Concentration of A (M) t = 352 s. 0.760 176 0.450 A → 2 B 352 0.140 rateg = M/s TOOLS x10
Determine the average rate of change of B from t = 0 s to Time (s) Concentration of A (M) t = 352 s. 0.760 176 0.450 A → 2 B 352 0.140 rateg = M/s TOOLS x10
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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![**Title: Calculating the Average Rate of Reaction**
**Objective:**
Determine the average rate of change of B from \( t = 0 \, \text{s} \) to \( t = 352 \, \text{s} \).
**Reaction:**
\[ \text{A} \rightarrow 2\text{B} \]
**Data Table:**
| Time (s) | Concentration of A (M) |
|----------|-------------------------|
| 0 | 0.760 |
| 176 | 0.450 |
| 352 | 0.140 |
**Formula:**
To calculate the average rate of reaction for B:
\[ \text{rate}_B = \]
**Tools:**
- Calculation tools (e.g., scientific calculator)
- Option for multiplying by \( \times 10^n \)
**Instruction for Calculation:**
1. Identify the change in concentration of A over the given time period.
2. Use stoichiometry to determine the change in concentration of B.
3. Calculate the rate using the formula:
\[
\text{rate}_B = \frac{\Delta [B]}{\Delta t}
\]
where \(\Delta [B] = 2 \times (\text{initial } [A] - \text{final } [A])\).
**Note:**
The diagram or equation space provided allows integration of tools for precise calculation, ensuring accuracy in determining the reaction rate.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ffe9fe32c-b492-41de-b627-5e5dec5bc081%2Fd16a51ac-bdce-43e8-b9f2-bd28b54bdd80%2Fae7iyim_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Title: Calculating the Average Rate of Reaction**
**Objective:**
Determine the average rate of change of B from \( t = 0 \, \text{s} \) to \( t = 352 \, \text{s} \).
**Reaction:**
\[ \text{A} \rightarrow 2\text{B} \]
**Data Table:**
| Time (s) | Concentration of A (M) |
|----------|-------------------------|
| 0 | 0.760 |
| 176 | 0.450 |
| 352 | 0.140 |
**Formula:**
To calculate the average rate of reaction for B:
\[ \text{rate}_B = \]
**Tools:**
- Calculation tools (e.g., scientific calculator)
- Option for multiplying by \( \times 10^n \)
**Instruction for Calculation:**
1. Identify the change in concentration of A over the given time period.
2. Use stoichiometry to determine the change in concentration of B.
3. Calculate the rate using the formula:
\[
\text{rate}_B = \frac{\Delta [B]}{\Delta t}
\]
where \(\Delta [B] = 2 \times (\text{initial } [A] - \text{final } [A])\).
**Note:**
The diagram or equation space provided allows integration of tools for precise calculation, ensuring accuracy in determining the reaction rate.
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