Suppose the formation of nitryl fluoride proceeds by the following mechanism:stepelementary reaction1 NO₂ (g) +F₂ (g) → NO₂F (g) +F (g)k₁2F (g) + NO₂ (g) → NO₂F (g)k₂Suppose 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.rate = krate constantロ→ロ0|0X

For any reaction: aA+bB→cC The rate law is given by: rate=kAxBy Here x and y are the partial…

Suppose the formation of nitryl fluoride proceeds by the following mechanism: rate constant step 1 elementary reaction NO₂ (g)+F₂ (g) → NO₂F (g) +F (g) - k₁ F (g) + NO₂ (g) → NO₂F (g) k₂ Suppose also k₁ «k₂. That is, the first step is much slower than the second. 2 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 ローロ 00 X

Suppose the formation of nitryl fluoride proceeds by the following mechanism: rate constant step 1 elementary reaction NO₂ (g)+F₂ (g) → NO₂F (g) +F (g) - k₁ F (g) + NO₂ (g) → NO₂F (g) k₂ Suppose also k₁ «k₂. That is, the first step is much slower than the second. 2 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 ローロ 00 X

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter11: Chemical Kinetics

Section: Chapter Questions

Problem 11.104PAE

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