### Reaction Study Data and AnalysisThe reaction \(2 \text{NO}_2(g) + \text{O}_3(g) \rightarrow \text{N}_2\text{O}_5(g) + \text{O}_2(g)\) was studied at a certain temperature, with the following experimental results:| Experiment | \([\text{NO}_2(g)]\) (M) | \([\text{O}_3(g)]\) (M) | Rate (M/s) ||------------|------------------|-----------------|-------------|| 1 | 0.559 | 0.559 | 22200 || 2 | 0.559 | 1.12 | 44500 || 3 | 1.12 | 0.559 | 44500 || 4 | 1.12 | 1.12 | 89100 |#### Questions and Analysis**(a) What is the rate law for this reaction?**Options:- Rate = \( k [\text{NO}_2(g)] [\text{O}_3(g)] \)- Rate = \( k [\text{NO}_2(g)]^2 [\text{O}_3(g)] \)- Rate = \( k [\text{NO}_2(g)] [\text{O}_3(g)]^2 \)- Rate = \( k [\text{NO}_2(g)]^2 [\text{O}_3(g)]^2 \)- Rate = \( k [\text{NO}_2(g)] [\text{O}_3(g)]^3 \)- Rate = \( k [\text{NO}_2(g)]^4 [\text{O}_3(g)] \)**(b) What is the value of the rate constant?**[________]**(c) What is the reaction rate when the concentration of \(\text{NO}_2(g)\) is 0.912 M and that of \(\text{O}_3(g)\) is 1.36 M if the temperature is the same as that used to obtain the data shown above?**[________] M/s### ExplanationIn this study, the effect of varying concentrations of \(\text{NO}_2(g)\) and \

Answered: Image /qna-images/answer/56aac154-73b7-4bfd-a79d-c1223bfd91f3.jpg

The reaction 2 NO₂(g) + O3(g) → N₂O5(g) + O₂(g) was studied at a certain temperature with the following results: Experiment 1 2 AWN T 3 4 (a) What is the rate law for this reaction? M/S Rate = k [NO₂(g)] [03(9)] O Rate = k [NO₂(g)]² [03(9)] Rate = k [NO₂(g)] [03(g)]² Rate = k [NO₂(g)]² [03(g)]² Rate = k [NO₂(g)] [03(g)]³ Rate = k [NO₂(g)]4 [03(g)] [NO₂(g)] (M) (b) What is the value of the rate constant? 0.559 0.559 1.12 1.12 [03(g)] (M) 0.559 1.12 0.559 1.12 Rate (M/s) 22200 44500 44500 89100 (c) What is the reaction rate when the concentration of NO₂(g) is 0.912 M and that of O3(g) is 1.36 M if the temperature is the same as that used to obtain the data shown above?

The reaction 2 NO₂(g) + O3(g) → N₂O5(g) + O₂(g) was studied at a certain temperature with the following results: Experiment 1 2 AWN T 3 4 (a) What is the rate law for this reaction? M/S Rate = k [NO₂(g)] [03(9)] O Rate = k [NO₂(g)]² [03(9)] Rate = k [NO₂(g)] [03(g)]² Rate = k [NO₂(g)]² [03(g)]² Rate = k [NO₂(g)] [03(g)]³ Rate = k [NO₂(g)]4 [03(g)] [NO₂(g)] (M) (b) What is the value of the rate constant? 0.559 0.559 1.12 1.12 [03(g)] (M) 0.559 1.12 0.559 1.12 Rate (M/s) 22200 44500 44500 89100 (c) What is the reaction rate when the concentration of NO₂(g) is 0.912 M and that of O3(g) is 1.36 M if the temperature is the same as that used to obtain the data shown above?

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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