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Reaction Mechanism and Rate Law For the reaction 2NO + Cl2 2NOCI Match the appropriate rate law to each postulated mechanism. A Rate = K[NO] B Rate = K[NO][Cl₂] C Rate = k[Cl₂] D Rate = K[NO]²[Cl₂]² E Rate = k[Cl₂]² F Rate = K[NO]²[Cl₂] G Rate = H Rate = K[NO]² = k[NO][Cl₂]² I None of the above NO + Cl2 NOCI2 fast equilibrium slow fast 2NOCI 2 → NOCI 3 + NOCI NOCI 3 NOCI + Cl2 NO + Cl2 NOCI 2 fast equilibrium NOCI 2 + NO >2NOCI slow 2NON₂O2 fast equilibrium N2O2 + Cl2 > 2NOCI slow NO + Cl2 NOCI + CI slow CI + NO NOCI fast

Reaction Mechanism and Rate Law For the reaction 2NO + Cl2 2NOCI Match the appropriate rate law to each postulated mechanism. A Rate = K[NO] B Rate = K[NO][Cl₂] C Rate = k[Cl₂] D Rate = K[NO]²[Cl₂]² E Rate = k[Cl₂]² F Rate = K[NO]²[Cl₂] G Rate = H Rate = K[NO]² = k[NO][Cl₂]² I None of the above NO + Cl2 NOCI2 fast equilibrium slow fast 2NOCI 2 → NOCI 3 + NOCI NOCI 3 NOCI + Cl2 NO + Cl2 NOCI 2 fast equilibrium NOCI 2 + NO >2NOCI slow 2NON₂O2 fast equilibrium N2O2 + Cl2 > 2NOCI slow NO + Cl2 NOCI + CI slow CI + NO NOCI fast

Chemistry
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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Reaction Mechanism and Rate Law For the reaction 2NO + Cl2 2NOCI Match the appropriate rate law to each postulated mechanism. A Rate = K[NO] B Rate = K[NO][Cl₂] C Rate = k[Cl₂] D Rate = K[NO]²[Cl₂]² E Rate = k[Cl₂]² F Rate = K[NO]²[Cl₂] G Rate = H Rate = K[NO]² = k[NO][Cl₂]² I None of the above NO + Cl2 NOCI2 fast equilibrium slow fast 2NOCI 2 → NOCI 3 + NOCI NOCI 3 NOCI + Cl2 NO + Cl2 NOCI 2 fast equilibrium NOCI 2 + NO >2NOCI slow 2NON₂O2 fast equilibrium N2O2 + Cl2 > 2NOCI slow NO + Cl2 NOCI + CI slow CI + NO NOCI fast
Transcribed Image Text:Reaction Mechanism and Rate Law For the reaction 2NO + Cl2 2NOCI Match the appropriate rate law to each postulated mechanism. A Rate = K[NO] B Rate = K[NO][Cl₂] C Rate = k[Cl₂] D Rate = K[NO]²[Cl₂]² E Rate = k[Cl₂]² F Rate = K[NO]²[Cl₂] G Rate = H Rate = K[NO]² = k[NO][Cl₂]² I None of the above NO + Cl2 NOCI2 fast equilibrium slow fast 2NOCI 2 → NOCI 3 + NOCI NOCI 3 NOCI + Cl2 NO + Cl2 NOCI 2 fast equilibrium NOCI 2 + NO >2NOCI slow 2NON₂O2 fast equilibrium N2O2 + Cl2 > 2NOCI slow NO + Cl2 NOCI + CI slow CI + NO NOCI fast
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