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Suppose the formation of nitryl fluoride proceeds by the following mechanism: step elementary reaction rate constant 1 NO, (g)+F2 (g) NO,F (g) + F (g) k1 2 F (g) + NO, (g) –→ NO,F (g) k2 Suppose also k, « k,. 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. rate = k U

Suppose the formation of nitryl fluoride proceeds by the following mechanism: step elementary reaction rate constant 1 NO, (g)+F2 (g) NO,F (g) + F (g) k1 2 F (g) + NO, (g) –→ NO,F (g) k2 Suppose also k, « k,. 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. rate = k U

Principles of Modern Chemistry
Principles of Modern Chemistry
8th Edition
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Chapter18: Chemical Kinetics
Section: Chapter Questions
Problem 66AP
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Suppose the formation of nitryl fluoride proceeds by the following mechanism: step elementary reaction rate constant 1 NO, g) +F, (g) NO,F (g) +F (g) k1 2 F (g) + NO, (g) → NO,F (g) k2 Suppose also k, « k,. 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. rate = k U Note: your answer should not contain the concentrations of any intermediates.
Transcribed Image Text:Suppose the formation of nitryl fluoride proceeds by the following mechanism: step elementary reaction rate constant 1 NO, g) +F, (g) NO,F (g) +F (g) k1 2 F (g) + NO, (g) → NO,F (g) k2 Suppose also k, « k,. 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. rate = k U Note: your answer should not contain the concentrations of any intermediates.
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