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?
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?
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter11: Chemical Kinetics: Rates Of Reactions
Section: Chapter Questions
Problem 98QRT: For a reaction involving the decomposition of a hypothetical substance Y, these data are...
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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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