The reaction 2 NO2(g) + O3(g) N2O5(g) + O2(g) was studied at a certain temperature with the following results: Experiment[NO2(g)] (M)[O3(g)] (M)Rate (M/s) 10.7620.7624940020.7621.529850031.520.7629850041.521.521.96e+05(a) 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) What is the value of the rate constant? (c) What is the reaction rate when the concentration of NO2(g) is 1.41 M and that of O3(g) is 1.86 M if the temperature is the same as that used to obtain the data shown above? M/s

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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 75E: One mechanism for the destruction of ozone in the upper atmosphere is a. Which species is a...

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The reaction 2 NO₂(g) + O₃(g) N₂O₅(g) + O₂(g) was studied at a certain temperature with the following results:

Experiment	[NO₂(g)] (M)	[O₃(g)] (M)	Rate (M/s)


1	0.762	0.762	49400
2	0.762	1.52	98500
3	1.52	0.762	98500
4	1.52	1.52	1.96e+05

(a) 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) What is the value of the rate constant?

(c) What is the reaction rate when the concentration of NO₂(g) is 1.41 M and that of O₃(g) is 1.86 M if the temperature is the same as that used to obtain the data shown above?

M/s

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