### Calculating the Rate Constant of a ReactionUsing the data in the table below, calculate the rate constant \( k \) of the following reaction:\[ A + B \rightarrow C + D \]#### Data Table| Trial | [A] (M) | [B] (M) | Rate (M/s) ||-------|---------|---------|------------|| 1 | 0.290 | 0.390 | 0.0101 || 2 | 0.290 | 0.858 | 0.0489 || 3 | 0.493 | 0.390 | 0.0172 |#### Calculation\[ k = \]#### Units#### Explanation of Calculation Method:1. **Rate Law Expression**: The rate law for this reaction can be generally expressed as: \[ \text{Rate} = k [A]^m [B]^n \] 2. **Determine Reaction Orders**: By comparing the rates from different trials, determine the reaction orders \( m \) and \( n \) with respect to \( A \) and \( B \).3. **Calculate \( k \)**: Once the reaction orders are known, substitute the concentrations and rates into the rate law expression and solve for \( k \).4. **Units for \( k \)**: Depending on the reaction orders, the units for \( k \) will vary and can be determined from the rearranged rate law expression.Fill in the calculated value for \( k \) and its units in the provided spaces.

The rate constant is defined as the proportionality constant which explains the relationship between…

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Using the data in the table, calculate the rate constant of chis reaction. [A] (M) [B] (М) Trial Rate (M/s) 1 0.290 0.390 0.0101 А +В — С +D 2 0.290 0.858 0.0489 3 0.493 0.390 0.0172 k = Units

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

### Calculating the Rate Constant of a Reaction

Using the data in the table below, calculate the rate constant \( k \) of the following reaction:

\[ A + B \rightarrow C + D \]

#### Data Table

| Trial | [A] (M) | [B] (M) | Rate (M/s) |
|-------|---------|---------|------------|
| 1 | 0.290 | 0.390 | 0.0101 |
| 2 | 0.290 | 0.858 | 0.0489 |
| 3 | 0.493 | 0.390 | 0.0172 |

#### Calculation

\[ k = \]

#### Units

#### Explanation of Calculation Method:

1. **Rate Law Expression**: The rate law for this reaction can be generally expressed as:
\[ \text{Rate} = k [A]^m [B]^n \]

2. **Determine Reaction Orders**: By comparing the rates from different trials, determine the reaction orders \( m \) and \( n \) with respect to \( A \) and \( B \).

3. **Calculate \( k \)**: Once the reaction orders are known, substitute the concentrations and rates into the rate law expression and solve for \( k \).

4. **Units for \( k \)**: Depending on the reaction orders, the units for \( k \) will vary and can be determined from the rearranged rate law expression.

Fill in the calculated value for \( k \) and its units in the provided spaces.

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