Answered: Suppose the decomposition of ozone…

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter18: Chemical Kinetics

Section: Chapter Questions

Problem 66AP

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Question

Suppose the decomposition of ozone proceeds by the following mechanism: step elementary reaction rate constant (g) (g) (g) (g) (g) (g) Suppose also ≫. That is, the first step is much faster than the second. Write the balanced chemical equation for the overall chemical reaction: Write the experimentally-observable rate law for the overall chemical reaction. Note: your answer should not contain the concentrations of any intermediates. Express the rate constant k for the overall chemical reaction in terms of k1, k2, and (if necessary) the rate constants k-1 and k-2 for the reverse of the two elementary reactions in the mechanism.

Suppose the decomposition of ozone proceeds by the following mechanism:
step elementary reaction
rate constant
1
03(g) → O₂(g) + O(g)
k₁
2 O3(g) + O(g) → 20₂(g)
k₂
Suppose also k₁>>k₂. That is, the first step is much faster than the second.
Write the balanced
chemical equation for the
overall chemical reaction:
Write the experimentally-
observable rate law for the
overall chemical reaction.
rate = k
Note: your answer should
not contain the
concentrations of any
intermediates.
Express the rate constant
k for the overall chemical
reaction in terms of K₁, K2,
and (if necessary) the rate
for
constante //
k =
U
>

O(g) →
k₂
Suppose also k₁»k₂. That is, the first step is much faster than the second.
Write the balanced
chemical equation for the
overall chemical reaction:
0
Write the experimentally-
observable rate law for the
overall chemical reaction.
Note:
answer should
not contain the
concentrations of any
intermediates.
Express the rate constant
k for the overall chemical
reaction in terms of K₁, K₂,
and (if necessary) the rate
constants k-1 and k-2 for
the reverse of the two
elementary reactions in
the mechanism.
rate = k
k = 0

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