The rate of a certain reaction is given by the following rate law: rate wk[N.J[0,] Use this information to answer the questions below. What is the reaction order in N2? What is the reaction order in 03? What is overall reaction order? At a certain concentration of N2 and 03, the initial rate of reaction is 0.970M/ s. What would the initial rate of the reaction be if the concentration of N2 were halved? Round your answer to 3 significant digits. The rate of the reaction is measured to be 3.0 x 103 M / s when [N2] = 1.7 M and [03] = 1.0 M. Calculate the value of the rate constant. Round your answer to 2 significant digits.
The rate of a certain reaction is given by the following rate law: rate wk[N.J[0,] Use this information to answer the questions below. What is the reaction order in N2? What is the reaction order in 03? What is overall reaction order? At a certain concentration of N2 and 03, the initial rate of reaction is 0.970M/ s. What would the initial rate of the reaction be if the concentration of N2 were halved? Round your answer to 3 significant digits. The rate of the reaction is measured to be 3.0 x 103 M / s when [N2] = 1.7 M and [03] = 1.0 M. Calculate the value of the rate constant. Round your answer to 2 significant digits.
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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![### Reaction Rate Law and Orders
The rate of a certain reaction is given by the following rate law:
\[ \text{rate} = k \left[ \text{N}_2 \right]^3 \left[ \text{O}_3 \right] \]
Use this information to answer the questions below:
| **Question** | **Answer** |
|------------------------------------------------------------------------------------------------------------------------------------------------------------------|--------------------|
| What is the reaction order in \( \text{N}_2 \)? | \(\boxed{3}\) |
| What is the reaction order in \( \text{O}_3 \)? | \(\boxed{1}\) |
| What is overall reaction order? | \(\boxed{4}\) |
| At a certain concentration of \( \text{N}_2 \) and \( \text{O}_3 \), the initial rate of reaction is \( 0.970 \, \text{M/s} \). What would the initial rate of the reaction be if the concentration of \( \text{N}_2 \) were halved? Round your answer to 3 significant digits. | \(\boxed{0.121} \, \text{M/s} \) |
| The rate of the reaction is measured to be \( 3.0 \times 10^3 \, \text{M/s} \) when \([ \text{N}_2 ] = 1.7 \, \text{M} \) and \([ \text{O}_3 ] = 1.0 \, \text{M} \). Calculate the value of the rate constant. Round your answer to 2 significant digits. | \(\boxed{6.1} \, \text{M}^{-3} \cdot \text{s}^{-1} \) |
### Explanation of Diagrams (If Any)
There are no graphs or diagrams in the image.
### Detailed Explanation:
1. **Reaction Order in \( \text{N}_2 \)**:
The exponent of \( [ \text{N}_2 ] \) in the rate law equation is 3.
Therefore, the reaction order with respect to \( \text{N}_2 \) is 3.
2. **Reaction Order in \( \text{O}_3 \)**:
The exponent of \( [ \text{](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F10caddcf-72cd-48c5-b185-0b83dd19834e%2F2bdc01d7-fd27-4345-a31d-831e6b34c9a9%2F4p7et_processed.png&w=3840&q=75)
Transcribed Image Text:### Reaction Rate Law and Orders
The rate of a certain reaction is given by the following rate law:
\[ \text{rate} = k \left[ \text{N}_2 \right]^3 \left[ \text{O}_3 \right] \]
Use this information to answer the questions below:
| **Question** | **Answer** |
|------------------------------------------------------------------------------------------------------------------------------------------------------------------|--------------------|
| What is the reaction order in \( \text{N}_2 \)? | \(\boxed{3}\) |
| What is the reaction order in \( \text{O}_3 \)? | \(\boxed{1}\) |
| What is overall reaction order? | \(\boxed{4}\) |
| At a certain concentration of \( \text{N}_2 \) and \( \text{O}_3 \), the initial rate of reaction is \( 0.970 \, \text{M/s} \). What would the initial rate of the reaction be if the concentration of \( \text{N}_2 \) were halved? Round your answer to 3 significant digits. | \(\boxed{0.121} \, \text{M/s} \) |
| The rate of the reaction is measured to be \( 3.0 \times 10^3 \, \text{M/s} \) when \([ \text{N}_2 ] = 1.7 \, \text{M} \) and \([ \text{O}_3 ] = 1.0 \, \text{M} \). Calculate the value of the rate constant. Round your answer to 2 significant digits. | \(\boxed{6.1} \, \text{M}^{-3} \cdot \text{s}^{-1} \) |
### Explanation of Diagrams (If Any)
There are no graphs or diagrams in the image.
### Detailed Explanation:
1. **Reaction Order in \( \text{N}_2 \)**:
The exponent of \( [ \text{N}_2 ] \) in the rate law equation is 3.
Therefore, the reaction order with respect to \( \text{N}_2 \) is 3.
2. **Reaction Order in \( \text{O}_3 \)**:
The exponent of \( [ \text{
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