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Nitric oxide (NO) reacts with H2 to form N2O and H2O. It is known that there are two elementarysteps to this reaction:Step I: NO(g) + NO(g) ---> N2O2(g)Step II: N2O2(g) + H2(g) ---> N2O(g) + H2O(g)The measured rate law for this overall reaction is:Rate = k[NO]2 [H2]What can we conclude about the above elementary reaction steps based on this rate law?(A) Steps I & II are about the same rate.(B) Step I is much faster than step II.(C) Step II is much faster than step I.(D) Not enough information to tell.

Nitric oxide (NO) reacts with H2 to form N2O and H2O. It is known that there are two elementarysteps to this reaction:Step I: NO(g) + NO(g) ---> N2O2(g)Step II: N2O2(g) + H2(g) ---> N2O(g) + H2O(g)The measured rate law for this overall reaction is:Rate = k[NO]2 [H2]What can we conclude about the above elementary reaction steps based on this rate law?(A) Steps I & II are about the same rate.(B) Step I is much faster than step II.(C) Step II is much faster than step I.(D) Not enough information to tell.

Chemistry: An Atoms First Approach
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 7ALQ
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Nitric oxide (NO) reacts with H2 to form N2O and H2O. It is known that there are two elementary
steps to this reaction:
Step I: NO(g) + NO(g) ---> N2O2(g)
Step II: N2O2(g) + H2(g) ---> N2O(g) + H2O(g)
The measured rate law for this overall reaction is:
Rate = k[NO]2 [H2]
What can we conclude about the above elementary reaction steps based on this rate law?
(A) Steps I & II are about the same rate.
(B) Step I is much faster than step II.
(C) Step II is much faster than step I.
(D) Not enough information to tell.

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