1 ### Reaction Rate LawThe rate of a certain reaction is given by the following rate law:\[\text{rate} = k [N_2]^2 [H_2]^2\]Use this information to answer the questions below.#### Questions:1. **What is the reaction order in \(N_2\)?** - **Answer:**2. **What is the reaction order in \(H_2\)?** - **Answer:**3. **What is the overall reaction order?** - **Answer:**4. **At a certain concentration of \(N_2\) and \(H_2\), the initial rate of reaction is \(7.0 \times 10^5 \, M/s\). What would the initial rate of the reaction be if the concentration of \(N_2\) were halved? Round your answer to 2 significant digits.** \[ \text{Answer:} \quad \boxed{ \, M/s \, } \]5. **The rate of the reaction is measured to be \(41.0 \, M/s\) when \([N_2] = 0.39 \, M\) and \([H_2] = 0.78 \, M\). Calculate the value of the rate constant. Round your answer to 2 significant digits.** \[ k = \boxed{ \, M^{-3} \cdot s^{-1} \, } \]#### Explanation of Graphs or DiagramsThere are no graphs or diagrams in the provided text. This section includes only mathematical representations and questions for students to solve based on given reaction data.

Answered: Image /qna-images/answer/9976df96-ab3c-45af-aec1-d20d2ab4091b.jpg

The rate of a certain reaction is given by the following rate law: rate= = K[N₂] ² [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 7.0 x 105 M/s. What would the initial rate of the reaction be if the concentration of N₂ were halved? Round your answer to 2 significant digits. The rate of the reaction is measured to be 41.0 M/s when [N₂] = 0.39 M and [H₂] = 0.78 M. Calculate the value of the 0 0 0-- -3 S - 1

The rate of a certain reaction is given by the following rate law: rate= = K[N₂] ² [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 7.0 x 105 M/s. What would the initial rate of the reaction be if the concentration of N₂ were halved? Round your answer to 2 significant digits. The rate of the reaction is measured to be 41.0 M/s when [N₂] = 0.39 M and [H₂] = 0.78 M. Calculate the value of the 0 0 0-- -3 S - 1

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter11: Chemical Kinetics

Section: Chapter Questions

Problem 5RQ

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Experimental data are listed here for the reaction A 2 B. (a) Prepare a graph from these data; connect the points with a smooth line; and calculate the rate of change of [B] for each 10-second interval from 0.0 to 40.0 seconds. Does the rate of change decrease from one time interval to the next? Suggest a reason for this result. (b) How is the rate of change of [A] related to the rate of change of [B] in each time interval? Calculate the rate of change of [A] for the time interval from 10.0 to 20.0 seconds.
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Consider the hypothetical reaction A+B+2C2D+3E In a study of this reaction three experiments were run at the same temperature. The rate is defined as [B]/t. Experiment 1: [A]0 = 2.0 M [B]0 = 1.0 103 M [C]0 = 1.0 M [B] (mol/L) Time(s) 2.7 104 1.0 105 1.6 104 2.0 105 1.1 104 3.0 105 8.5 105 4.0 105 6.9 105 5.0 105 5.8 105 6.0 105 Experiment 2: [A]0 = 1.0 102M [B]0 = 3.0 M [C]0 = 1.0 M [A] (mol/L) Time(s) 8.9 103 1.0 7.1 103 3.0 5.5 103 5.0 3.8 103 8.0 2.9 103 10.0 2.0 103 13.0 Experiment 3: [A]0 = 10.0 M [B]0 = 5.0 M [C]0 = 5.0 101M [C] (mol/L) Time(s) 0.43 1.0 102 0.36 2.0 102 0.29 3.0 102 0.22 4.0 102 0.15 5.0 102 0.08 6.0 102 Write the rate law for this reaction, and calculate the value of the rate constant.
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