Suppose the decomposition of nitrogen dioxide proceeds by the following mechanism: step elementary reaction rate constant 1 NO₂ (g) NO(g) +0(g) k₁ 2 O(g) +NO₂(g) → O₂(g) + NO(g) k₂ Suppose also k₂ « 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. e rate = k 2

Suppose the decomposition of nitrogen dioxide proceeds by the following mechanism: step elementary reaction rate constant 1 NO₂ (g) NO(g) +0(g) k₁ 2 O(g) +NO₂(g) → O₂(g) + NO(g) k₂ Suppose also k₂ « 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. e rate = k 2

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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Question

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Suppose the decomposition of nitrogen dioxide proceeds by the following mechanism:
step
elementary reaction
rate constant
1
NO₂ (g) → NO (g) +0 (g)
1
k₁
2 O(g) + NO₂(g) →O₂ (g) + NO (g)
k₂
Suppose also k, << 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.
0
rate = k
4

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