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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
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
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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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 ?
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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