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For the reaction 2NO + Cl2  2NOCl Match the appropriate rate law to each postulated mechanism. A Rate = k[NO][Cl2] B Rate = k[NO]2 C Rate = k[Cl2] D Rate = k[Cl2]2 E Rate = k[NO]2[Cl2] F Rate = k[NO]2[Cl2]2 G Rate = k[NO] H Rate = k[NO][Cl2]2 I None of the above            NO + Cl2  NOCl + Cl     slow Cl + NO  NOCl     fast            2NO  N2O2     fast equilibrium N2O2 + Cl2  2NOCl     slow            NO + Cl2  NOCl2     fast equilibrium 2NOCl2  NOCl3 + NOCl     slow NOCl3  NOCl + Cl2     fast            2NO  N2O2     slow N2O2 + Cl2  2NOCl     fast

For the reaction 2NO + Cl2  2NOCl Match the appropriate rate law to each postulated mechanism. A Rate = k[NO][Cl2] B Rate = k[NO]2 C Rate = k[Cl2] D Rate = k[Cl2]2 E Rate = k[NO]2[Cl2] F Rate = k[NO]2[Cl2]2 G Rate = k[NO] H Rate = k[NO][Cl2]2 I None of the above            NO + Cl2  NOCl + Cl     slow Cl + NO  NOCl     fast            2NO  N2O2     fast equilibrium N2O2 + Cl2  2NOCl     slow            NO + Cl2  NOCl2     fast equilibrium 2NOCl2  NOCl3 + NOCl     slow NOCl3  NOCl + Cl2     fast            2NO  N2O2     slow N2O2 + Cl2  2NOCl     fast

Chemistry for Engineering Students
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 11.24PAE: Second-order rate constants used in modeling atmospheric chemistry are commonly reported in units of...
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For the reaction

2NO + Cl2  2NOCl


Match the appropriate rate law to each postulated mechanism.

A Rate = k[NO][Cl2]
B Rate = k[NO]2
C Rate = k[Cl2]
D Rate = k[Cl2]2
E Rate = k[NO]2[Cl2]
F Rate = k[NO]2[Cl2]2
G Rate = k[NO]
H Rate = k[NO][Cl2]2
I None of the above


          

NO + Cl2  NOCl + Cl     slow
Cl + NO  NOCl     fast


          

2NO  N2O2     fast equilibrium
N2O2 + Cl2  2NOCl     slow


          

NO + Cl2  NOCl2     fast equilibrium
2NOCl2  NOCl3 + NOCl     slow
NOCl3  NOCl + Cl2     fast


          

2NO  N2O2     slow
N2O2 + Cl2  2NOCl     fast
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