Suppose the formation of nitryl fluoride proceeds by the following mechanism: step elementary reaction 1 NO₂ (g) +F₂ (g) → NO₂F (g) +F (g) k₁ 2 F (g) + NO₂ (g) → NO₂F (g) k₂ 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. rate = k rate constant
Suppose the formation of nitryl fluoride proceeds by the following mechanism: step elementary reaction 1 NO₂ (g) +F₂ (g) → NO₂F (g) +F (g) k₁ 2 F (g) + NO₂ (g) → NO₂F (g) k₂ 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. rate = k rate constant
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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![Writing the rate law implied by a simple mechanism with an initial slow...
Suppose the formation of nitryl fluoride proceeds by the following mechanism:
elementary reaction
step
1 NO₂ (g) +F₂ (g)
2
k₁
k₂
2
F (g) + NO₂(g) → NO₂F (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.
NO₂F (g) +F (g)
Note: your answer should not
contain the concentrations of
any intermediates.
rate constant
rate = k
0+
00
X
Ś](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fd38dc3ae-53e5-4279-afed-9e69fa663b8c%2Ff76fb938-15fa-4d64-890f-e5c0a83383c7%2Fy1v3ibk_processed.png&w=3840&q=75)
Transcribed Image Text:Writing the rate law implied by a simple mechanism with an initial slow...
Suppose the formation of nitryl fluoride proceeds by the following mechanism:
elementary reaction
step
1 NO₂ (g) +F₂ (g)
2
k₁
k₂
2
F (g) + NO₂(g) → NO₂F (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.
NO₂F (g) +F (g)
Note: your answer should not
contain the concentrations of
any intermediates.
rate constant
rate = k
0+
00
X
Ś
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