Derive the rate law for the decomposition of ozone (in terms of k1, k2, and k−1) from the following steps. Ozone, O3, decomposes to molecular oxygen, O2, via the following process: 2O3(g) → 3O2(g) The rate law for the decomposition of ozone to molecular oxygen is rate = k[O3]2/ [O2] The mechanism proposed for this process is O3 = O + O2 (equilibrium k1 is forward and K-1 is reverse) O + O3 = 2O2 (k2) What is the rate law in terms of k1, k2, and k−1?

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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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Derive the rate law for the decomposition of ozone (in terms of k₁, k₂, and k₋₁) from the following steps.

Ozone, O₃, decomposes to molecular oxygen, O₂, via the following process:

2O₃(g) → 3O₂(g)

The rate law for the decomposition of ozone to molecular oxygen is

rate = k[O₃]²/ [O₂]
The mechanism proposed for this process is

O₃ = O + O₂ (equilibrium k1 is forward and K-1 is reverse)

O + O₃ = 2O₂ (k2)

What is the rate law in terms of k₁, k₂, and k₋₁?

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