Suppose the decomposition of ozone proceeds by the following mechanism: step elementary reaction rate constant 1 03(g) → O₂(g) + O(g) k₁ 2 03(g) + O(g) → 20₂(g) k₂ Suppose also k₁<
Suppose the decomposition of ozone proceeds by the following mechanism: step elementary reaction rate constant 1 03(g) → O₂(g) + O(g) k₁ 2 03(g) + O(g) → 20₂(g) k₂ Suppose also k₁<
Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter11: Rate Of Reaction
Section: Chapter Questions
Problem 86QAP
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![Suppose the decomposition of ozone proceeds by the following mechanism:
step elementary reaction rate constant
103(g) 0₂(g) + O(g)
2 O3(g) + O(g) → 20₂(g)
Suppose also k₁<<k₂. That is, the first step is much slower 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.
0
rate = k
k =
k₁
k₂
0
1-0
X
5
?](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F093e7116-3e01-49ad-9157-7a22a5caeb16%2F04165b13-5c15-47b1-80db-08cb2efb68b6%2F9qb0b_processed.png&w=3840&q=75)
Transcribed Image Text:Suppose the decomposition of ozone proceeds by the following mechanism:
step elementary reaction rate constant
103(g) 0₂(g) + O(g)
2 O3(g) + O(g) → 20₂(g)
Suppose also k₁<<k₂. That is, the first step is much slower 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.
0
rate = k
k =
k₁
k₂
0
1-0
X
5
?
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