For the reaction 2NO + Cl2 ---> 2NOCl Match the appropriate rate law to each postulated mechanism. A Rate = k[NO]2[Cl2] B Rate = k[Cl2] C Rate = k[NO]2[Cl2]2 D Rate = k[Cl2]2 E Rate = k[NO] F Rate = k[NO][Cl2]2 G Rate = k[NO]2 H Rate = k[NO][Cl2] I None of the above NO + Cl2 NOCl2 fast equilibrium NOCl2 + NO 2NOCl slow 2NO N2O2 fast equilibrium N2O2 + Cl2 2NOCl slow Cl2 2Cl slow Cl + NO NOCl fast NO + Cl2 NOCl + Cl slow Cl + NO NOCl fast
For the reaction 2NO + Cl2 ---> 2NOCl Match the appropriate rate law to each postulated mechanism. A Rate = k[NO]2[Cl2] B Rate = k[Cl2] C Rate = k[NO]2[Cl2]2 D Rate = k[Cl2]2 E Rate = k[NO] F Rate = k[NO][Cl2]2 G Rate = k[NO]2 H Rate = k[NO][Cl2] I None of the above NO + Cl2 NOCl2 fast equilibrium NOCl2 + NO 2NOCl slow 2NO N2O2 fast equilibrium N2O2 + Cl2 2NOCl slow Cl2 2Cl slow Cl + NO NOCl fast NO + Cl2 NOCl + Cl slow Cl + NO NOCl fast
Chemistry: An Atoms First Approach
2nd Edition
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Steven S. Zumdahl, Susan A. Zumdahl
Chapter11: Chemical Kinetics
Section: Chapter Questions
Problem 6ALQ: For the reaction A + B C, explain at least two ways in which the rate law could be zero order in...
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Question
For the reaction
2NO + Cl2 ---> 2NOCl |
Match the appropriate rate law to each postulated mechanism.
A | Rate = k[NO]2[Cl2] |
B | Rate = k[Cl2] |
C | Rate = k[NO]2[Cl2]2 |
D | Rate = k[Cl2]2 |
E | Rate = k[NO] |
F | Rate = k[NO][Cl2]2 |
G | Rate = k[NO]2 |
H | Rate = k[NO][Cl2] |
I | None of the above |
NO + Cl2 NOCl2 fast equilibrium NOCl2 + NO 2NOCl slow |
2NO N2O2 fast equilibrium N2O2 + Cl2 2NOCl slow |
Cl2 2Cl slow Cl + NO NOCl fast |
NO + Cl2 NOCl + Cl slow Cl + NO NOCl fast |
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