23. Consider the following reaction:2 NO2(g) + O3(g) N2O5(g) + O2(g)(a) The rate law for this reaction is first order in NO2(g) and first order in O3(g). What is the rate law for this reaction?Rate = k [NO2(g)] [O3(g)]Rate = k [NO2(g)]2 [O3(g)] Rate = k [NO2(g)] [O3(g)]2Rate = k [NO2(g)]2 [O3(g)]2Rate = k [NO2(g)] [O3(g)]3Rate = k [NO2(g)]4 [O3(g)](b) If the rate constant for this reaction at a certain temperature is 62500, what is the reaction rate when [NO2(g)] = 0.530 M and [O3(g)] = 1.08 M?Rate =_____ M/s.(c) What is the reaction rate when the concentration of NO2(g) is doubled, to 1.06 M while the concentration of O3(g) is 1.08 M?Rate =____ M/s

The question is based on the concept of chemical kinetics. We have to calculate rate of the reaction…

Answered: 23. Consider the following reaction:…

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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Question

23. Consider the following reaction:

2 NO₂(g) + O₃(g) N₂O₅(g) + O₂(g)

(a) The rate law for this reaction is first order in NO₂(g) and first order in O₃(g). What is the rate law for this reaction?

Rate = k [NO₂(g)] [O₃(g)]

Rate = k [NO₂(g)]² [O₃(g)]

Rate = k [NO₂(g)] [O₃(g)]²

Rate = k [NO₂(g)]² [O₃(g)]²

Rate = k [NO₂(g)] [O₃(g)]³

Rate = k [NO₂(g)]⁴ [O₃(g)]

(b) If the rate constant for this reaction at a certain temperature is 62500, what is the reaction rate when [NO₂(g)] = 0.530 M and [O₃(g)] = 1.08 M?

Rate =_____ M/s.

(c) What is the reaction rate when the concentration of NO₂(g) is doubled, to 1.06 M while the concentration of O₃(g) is 1.08 M?

Rate =____ M/s