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