The rate of a certain reaction is given by the following rate law: rate=k[N₂] [H₂]² Use this information to answer the questions below. What is the reaction order in N₂? What is the reaction order in H₂? What is overall reaction order? At a certain concentration of N₂ and H₂, the initial rate of reaction is 0.750 M/s. What would the initial rate of the reaction be if the concentration of N₂ were doubled? Round your answer to 3 significant digits. The rate of the reaction is measured to be 18.0 M/s when [N₂] =.0.52 M and [H₂] = 1.0 M. Calculate the value of the rate constant. Round your answer to 2 significant digits. Explanation 18,177 Check OCT 13 k= tv 0 0 0 04/1 -1 'S MacBook Pro x10 X Ⓒ2022 Mc 7A
The rate of a certain reaction is given by the following rate law: rate=k[N₂] [H₂]² Use this information to answer the questions below. What is the reaction order in N₂? What is the reaction order in H₂? What is overall reaction order? At a certain concentration of N₂ and H₂, the initial rate of reaction is 0.750 M/s. What would the initial rate of the reaction be if the concentration of N₂ were doubled? Round your answer to 3 significant digits. The rate of the reaction is measured to be 18.0 M/s when [N₂] =.0.52 M and [H₂] = 1.0 M. Calculate the value of the rate constant. Round your answer to 2 significant digits. Explanation 18,177 Check OCT 13 k= tv 0 0 0 04/1 -1 'S MacBook Pro x10 X Ⓒ2022 Mc 7A
Chemistry
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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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![## Using a Rate Law
The rate of a certain reaction is given by the following rate law:
\[ \text{rate} = k[N_2][H_2]^2 \]
Use this information to answer the questions below:
1. **What is the reaction order in \(N_2\)?**
[Input Box]
2. **What is the reaction order in \(H_2\)?**
[Input Box]
3. **What is overall reaction order?**
[Input Box]
4. **At a certain concentration of \(N_2\) and \(H_2\), the initial rate of reaction is 0.750 M/s. What would the initial rate of the reaction be if the concentration of \(N_2\) were doubled? Round your answer to 3 significant digits.**
\[ \text{Rate} \quad \left(\frac{\text{M}}{\text{s}}\right) \]
[Input Box]
5. **The rate of the reaction is measured to be 18.0 M/s when \([N_2] = 0.52 \, \text{M}\) and \([H_2] = 1.0 \, \text{M}\). Calculate the value of the rate constant. Round your answer to 2 significant digits.**
\[ k = \text{M}^{-2} \, \text{s}^{-1} \]
[Input Box]
### Buttons:
- **Explanation**
- **Check**](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F1ac9d9fd-0ce6-4ad9-ac74-440cab402247%2F88c73ef7-1b26-418b-855c-31aef647a560%2Fn3o1i6j_processed.jpeg&w=3840&q=75)
Transcribed Image Text:## Using a Rate Law
The rate of a certain reaction is given by the following rate law:
\[ \text{rate} = k[N_2][H_2]^2 \]
Use this information to answer the questions below:
1. **What is the reaction order in \(N_2\)?**
[Input Box]
2. **What is the reaction order in \(H_2\)?**
[Input Box]
3. **What is overall reaction order?**
[Input Box]
4. **At a certain concentration of \(N_2\) and \(H_2\), the initial rate of reaction is 0.750 M/s. What would the initial rate of the reaction be if the concentration of \(N_2\) were doubled? Round your answer to 3 significant digits.**
\[ \text{Rate} \quad \left(\frac{\text{M}}{\text{s}}\right) \]
[Input Box]
5. **The rate of the reaction is measured to be 18.0 M/s when \([N_2] = 0.52 \, \text{M}\) and \([H_2] = 1.0 \, \text{M}\). Calculate the value of the rate constant. Round your answer to 2 significant digits.**
\[ k = \text{M}^{-2} \, \text{s}^{-1} \]
[Input Box]
### Buttons:
- **Explanation**
- **Check**
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