(a) The second step of this mechanism is rate-determining (slow). What is the rate law for this reaction? Rate = k [NO] [O2] Rate = k [NO]2 [O2] Rate = k [NO] [O2]2 Rate = k [NO]1/2 [
(a) The second step of this mechanism is rate-determining (slow). What is the rate law for this reaction? Rate = k [NO] [O2] Rate = k [NO]2 [O2] Rate = k [NO] [O2]2 Rate = k [NO]1/2 [
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter11: Chemical Kinetics: Rates Of Reactions
Section11.7: Reaction Mechanisms
Problem 11.12E
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Question
The reaction 2 NO(g) + O2(g) --> 2 NO2(g) proceeds through the following mechanism:
2 NO(g) --> N2O2(g)
N2O2(g) + O2(g) --> 2 NO2(g)
N2O2(g) + O2(g) --> 2 NO2(g)
(a) The second step of this mechanism is rate-determining (slow). What is the rate law for this reaction?
Rate = k [NO] [O2]
Rate = k [NO]2 [O2]
Rate = k [NO] [O2]2
Rate = k [NO]1/2 [O2]
Rate = k [NO] [O2]1/2
Rate = k [NO]2
Rate = k [NO]2 [O2]1/2
(b) What would the rate law be if the first step of this mechanism were rate-determining?
Rate = k [NO] [O2]
Rate = k [NO]2 [O2]
Rate = k [NO] [O2]2
Rate = k [NO]1/2 [O2]
Rate = k [NO] [O2]1/2
Rate = k [NO]2
Rate = k [NO]2 [O2]1/2
Rate = k [NO]
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