Some measurements of the initial rate of a certain reaction are given in the table below. [₂] [H₂] initial rate of reaction 0.785 M 0.273 M 0.859 M/s 2.30M 0.273 M 2.52 M/s 0.785 M 0.347 M 1.39 M/s Use this information to write a rate law for this reaction, and calculate the value of the rate constant k. Round your value for the rate constant to 2 significant digits. Also be sure your answer has the correct unit symbol. rate = & k = x10 X 00 5
Some measurements of the initial rate of a certain reaction are given in the table below. [₂] [H₂] initial rate of reaction 0.785 M 0.273 M 0.859 M/s 2.30M 0.273 M 2.52 M/s 0.785 M 0.347 M 1.39 M/s Use this information to write a rate law for this reaction, and calculate the value of the rate constant k. Round your value for the rate constant to 2 significant digits. Also be sure your answer has the correct unit symbol. rate = & k = x10 X 00 5
Chemistry
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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
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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![### Initial Rate of Reaction Data Analysis
Some measurements of the initial rate of a certain reaction are given in the table below.
| [N\(_2\)] | [H\(_2\)] | Initial Rate of Reaction |
|:---------:|:---------:|:------------------------:|
| 0.785 M | 0.273 M | 0.859 M/s |
| 2.30 M | 0.273 M | 2.52 M/s |
| 0.785 M | 0.347 M | 1.39 M/s |
Use this information to write a rate law for this reaction and calculate the value of the rate constant \( k \).
1. **Rate Law Expression**:
The rate law for a reaction can be expressed in the form:
\[
\text{rate} = k [N_2]^x [H_2]^y
\]
2. **Experimental Data Analysis**:
By comparing the initial rates when one concentration is changed while the other is kept constant, you can determine the order of the reaction with respect to each reactant.
3. **Calculate the Rate Constant \( k \)**:
Rearrange the formula to solve for \( k \):
\[
k = \frac{\text{rate}}{[N_2]^x [H_2]^y}
\]
4. **Significant Figures and Units**:
Ensure the calculated value for the rate constant is rounded to 2 significant digits and includes the proper unit.
5. **Example Calculation**:
Suppose analysis yields the reaction orders \( x \) and \( y \). Substituting the values allows computation of \( k \), which will have the unit \(\text{M}^{-1}\text{s}^{-1}\) or similar, depending on the reaction orders.
### Editable Areas:
- **Rate Law Expression**:
\[
\text{rate} = k [N_2]^x [H_2]^y
\]
Fill in the determined exponents \( x \) and \( y \).
- **Rate Constant \( k \)**:
\[
k = \text{value with correct units}
\]
6. **Graphical/Diagram Descriptions**:
The provided image includes an interactive space for calculating and entering](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F12c0a0e9-4d98-45bb-8c42-bb6fd08d9097%2F0b33baee-dec8-450d-a7a3-fe0947885869%2F0167rds_processed.png&w=3840&q=75)
Transcribed Image Text:### Initial Rate of Reaction Data Analysis
Some measurements of the initial rate of a certain reaction are given in the table below.
| [N\(_2\)] | [H\(_2\)] | Initial Rate of Reaction |
|:---------:|:---------:|:------------------------:|
| 0.785 M | 0.273 M | 0.859 M/s |
| 2.30 M | 0.273 M | 2.52 M/s |
| 0.785 M | 0.347 M | 1.39 M/s |
Use this information to write a rate law for this reaction and calculate the value of the rate constant \( k \).
1. **Rate Law Expression**:
The rate law for a reaction can be expressed in the form:
\[
\text{rate} = k [N_2]^x [H_2]^y
\]
2. **Experimental Data Analysis**:
By comparing the initial rates when one concentration is changed while the other is kept constant, you can determine the order of the reaction with respect to each reactant.
3. **Calculate the Rate Constant \( k \)**:
Rearrange the formula to solve for \( k \):
\[
k = \frac{\text{rate}}{[N_2]^x [H_2]^y}
\]
4. **Significant Figures and Units**:
Ensure the calculated value for the rate constant is rounded to 2 significant digits and includes the proper unit.
5. **Example Calculation**:
Suppose analysis yields the reaction orders \( x \) and \( y \). Substituting the values allows computation of \( k \), which will have the unit \(\text{M}^{-1}\text{s}^{-1}\) or similar, depending on the reaction orders.
### Editable Areas:
- **Rate Law Expression**:
\[
\text{rate} = k [N_2]^x [H_2]^y
\]
Fill in the determined exponents \( x \) and \( y \).
- **Rate Constant \( k \)**:
\[
k = \text{value with correct units}
\]
6. **Graphical/Diagram Descriptions**:
The provided image includes an interactive space for calculating and entering
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