Suppose the formation of nitryl fluoride proceeds by the following mechanism: step elementary reaction rate constant 1 NO2(9) + F2(9) NO,F(9) + F(g) → 2 F(g) + NO,(9) → NO,F(g) k2 Suppose also k,»k,. 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. rate = k U 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 k = elementary reactions in the mechanism.

Suppose the formation of nitryl fluoride proceeds by the following mechanism: step elementary reaction rate constant 1 NO2(9) + F2(9) NO,F(9) + F(g) → 2 F(g) + NO,(9) → NO,F(g) k2 Suppose also k,»k,. 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. rate = k U 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 k = elementary reactions in the mechanism.

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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