Suppose the formation of nitryl fluoride proceeds by the following mechanism:stepelementary reaction1 NO₂ (g) +F₂ (g) → NO₂F (g)+F (g)2F (g) + NO₂ (g) → NO₂F (g)Suppose also k₁ << k₂. That is, the first step is much slower than the second.Write the balanced chemicalequation for the overallchemical reaction.Write the experimentally-observable rate law for theoverall chemical reaction.Note: your answer should notcontain the concentrations ofany intermediates.0rate = &rate constantk₁k₂

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Suppose the formation of nitryl fluoride proceeds by the following mechanism: elementary reaction rate constant NO₂ (g)+F₂ (g) → NO₂F (g) +F (g) 1 k₁ F (g) +NO₂ (g) NO₂F (g) k₂ Suppose also k₁ <

Suppose the formation of nitryl fluoride proceeds by the following mechanism: elementary reaction rate constant NO₂ (g)+F₂ (g) → NO₂F (g) +F (g) 1 k₁ F (g) +NO₂ (g) NO₂F (g) k₂ Suppose also k₁ <

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

Suppose the formation of nitryl fluoride proceeds by the following mechanism:
step
elementary reaction
1 NO₂ (g) +F₂ (g) → NO₂F (g)+F (g)
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.
Note: your answer should not
contain the concentrations of
any intermediates.
0
rate = &
rate constant
k₁
k₂

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