The rate of a certain reaction is given by the following rate law: -K[N=][H] rate=k Use this information to answer the questions below. What is the reaction order in N,? 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 0.930 M / s. What would the initial rate of the reaction be if the concentration of N, were doubled? Round M your answer to 3 significant digits. The rate of the reaction is measured to be 34.0 M / s when [N2] = 1.8 M and [H2] = 1.3 M. Calculate the value of the rate k = constant. Round your answer to 2 significant digits.
The rate of a certain reaction is given by the following rate law: -K[N=][H] rate=k Use this information to answer the questions below. What is the reaction order in N,? 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 0.930 M / s. What would the initial rate of the reaction be if the concentration of N, were doubled? Round M your answer to 3 significant digits. The rate of the reaction is measured to be 34.0 M / s when [N2] = 1.8 M and [H2] = 1.3 M. Calculate the value of the rate k = 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 Problem Set
The rate of a certain reaction is given by the following rate law:
\[ \text{rate} = k[\text{N}_2][\text{H}_2]^2 \]
Use this information to answer the questions below.
| Question | Answer |
|----------|--------|
| **What is the reaction order in \( \text{N}_2 \)?** | |
| **What is the reaction order in \( \text{H}_2 \)?** | |
| **What is overall reaction order?** | |
**Question:**
At a certain concentration of \( \text{N}_2 \) and \( \text{H}_2 \), the initial rate of reaction is 0.930 \( \frac{M}{s} \). What would the initial rate of the reaction be if the concentration of \( \text{N}_2 \) were doubled? Round your answer to 3 significant digits.
| Rate | \( \frac{M}{s} \) |
**Question:**
The rate of the reaction is measured to be 34.0 \( \frac{M}{s} \) when \([\text{N}_2] = 1.8\ M\) and \([\text{H}_2] = 1.3\ M\). Calculate the value of the rate constant. Round your answer to 2 significant digits.
\[ k = \, M^{-2} \cdot s^{-1} \]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Faf1fd5ea-80f6-47fe-ac10-02a0625e13d5%2F15e30795-420a-4c3b-825b-c5a1390ff399%2F0s109iw_processed.png&w=3840&q=75)
Transcribed Image Text:### Reaction Rate Law Problem Set
The rate of a certain reaction is given by the following rate law:
\[ \text{rate} = k[\text{N}_2][\text{H}_2]^2 \]
Use this information to answer the questions below.
| Question | Answer |
|----------|--------|
| **What is the reaction order in \( \text{N}_2 \)?** | |
| **What is the reaction order in \( \text{H}_2 \)?** | |
| **What is overall reaction order?** | |
**Question:**
At a certain concentration of \( \text{N}_2 \) and \( \text{H}_2 \), the initial rate of reaction is 0.930 \( \frac{M}{s} \). What would the initial rate of the reaction be if the concentration of \( \text{N}_2 \) were doubled? Round your answer to 3 significant digits.
| Rate | \( \frac{M}{s} \) |
**Question:**
The rate of the reaction is measured to be 34.0 \( \frac{M}{s} \) when \([\text{N}_2] = 1.8\ M\) and \([\text{H}_2] = 1.3\ M\). Calculate the value of the rate constant. Round your answer to 2 significant digits.
\[ k = \, M^{-2} \cdot s^{-1} \]
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