Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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![### Reaction Rate Data Analysis
**Objective:**
Determine the rate constant of the reaction:
\[ 2\text{NO}(g) + \text{Cl}_2(g) \rightarrow 2\text{NOCl}(g) \]
**Data Provided:**
| Experiment | [NO] (M) | [Cl\(_2\)] (M) | Rate (M/s) |
|------------|----------|----------------|------------|
| 1 | 0.0300 | 0.0100 | 3.4 × 10\(^{-4}\) |
| 2 | 0.0150 | 0.0100 | 8.5 × 10\(^{-5}\) |
| 3 | 0.0150 | 0.0400 | 3.4 × 10\(^{-4}\) |
**Explanation of the Data Table:**
- **Experiment:** Denotes the trial number conducted for measuring the reaction rate under different reactant concentrations.
- **[NO] (M):** The molarity of nitrogen monoxide present in each experiment.
- **[Cl\(_2\)] (M):** The molarity of chlorine present during each experiment.
- **Rate (M/s):** The calculated rate of reaction in moles per liter per second for each set of conditions.
**Analysis Guide:**
1. Analyze how changing the concentration of each reactant affects the rate of reaction to determine the reaction order for each reactant.
2. Use the method of initial rates to determine the relationship between reactant concentration and reaction rate.
3. Calculate the rate constant (\( k \)) for the reaction using the rate law derived from the data.
This experiment provides essential data to understand the kinetics of the reaction, primarily focusing on calculating the rate constant and understanding the influence of reactant concentration on reaction rates.](https://content.bartleby.com/qna-images/question/437a6243-7f54-47cd-8dab-1c18de80702c/358b74ab-4f59-42dc-a162-40bdb97890c2/d3zhite_processed.png)
Transcribed Image Text:### Reaction Rate Data Analysis
**Objective:**
Determine the rate constant of the reaction:
\[ 2\text{NO}(g) + \text{Cl}_2(g) \rightarrow 2\text{NOCl}(g) \]
**Data Provided:**
| Experiment | [NO] (M) | [Cl\(_2\)] (M) | Rate (M/s) |
|------------|----------|----------------|------------|
| 1 | 0.0300 | 0.0100 | 3.4 × 10\(^{-4}\) |
| 2 | 0.0150 | 0.0100 | 8.5 × 10\(^{-5}\) |
| 3 | 0.0150 | 0.0400 | 3.4 × 10\(^{-4}\) |
**Explanation of the Data Table:**
- **Experiment:** Denotes the trial number conducted for measuring the reaction rate under different reactant concentrations.
- **[NO] (M):** The molarity of nitrogen monoxide present in each experiment.
- **[Cl\(_2\)] (M):** The molarity of chlorine present during each experiment.
- **Rate (M/s):** The calculated rate of reaction in moles per liter per second for each set of conditions.
**Analysis Guide:**
1. Analyze how changing the concentration of each reactant affects the rate of reaction to determine the reaction order for each reactant.
2. Use the method of initial rates to determine the relationship between reactant concentration and reaction rate.
3. Calculate the rate constant (\( k \)) for the reaction using the rate law derived from the data.
This experiment provides essential data to understand the kinetics of the reaction, primarily focusing on calculating the rate constant and understanding the influence of reactant concentration on reaction rates.
Expert Solution
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Step 1
Rate constant can be find by finding order of equation. Then Putting any experimental values give rate constant.
The procedures for finding rate constant is given below-
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