Suppose the decomposition of nitrogen dioxide proceeds by the following mechanism: step elementary reaction 1 NO₂(9) NO(g) + O(g) k₁ 2 O(g) + NO₂(g) → O₂(g) + NO(g) k₂ Suppose also k₁k₂. 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 i 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 k₂ for the reverse of the two elementary reactions in the mechanism. 0 rate= - 0 k= *0 rate constant 0-0 Do 00 X 5 ?
Suppose the decomposition of nitrogen dioxide proceeds by the following mechanism: step elementary reaction 1 NO₂(9) NO(g) + O(g) k₁ 2 O(g) + NO₂(g) → O₂(g) + NO(g) k₂ Suppose also k₁k₂. 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 i 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 k₂ for the reverse of the two elementary reactions in the mechanism. 0 rate= - 0 k= *0 rate constant 0-0 Do 00 X 5 ?
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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![Suppose the decomposition of nitrogen dioxide proceeds by the following mechanism:
step
elementary reaction
1
NO₂(g) → NO(g) + O(g)
2 O(g) + NO₂(g) → O₂(g) + NO(g)
k₂
Suppose also k₁k₂. 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.
0
rate=0
- 0
rate constant
0-0
100
X n
?](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F07786edc-230e-4384-a5b9-b789b3f6d167%2F859959c3-02e7-4a3e-b555-4318c58c11b5%2Fnmq67im_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Suppose the decomposition of nitrogen dioxide proceeds by the following mechanism:
step
elementary reaction
1
NO₂(g) → NO(g) + O(g)
2 O(g) + NO₂(g) → O₂(g) + NO(g)
k₂
Suppose also k₁k₂. 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.
0
rate=0
- 0
rate constant
0-0
100
X n
?
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