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(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
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
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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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)




(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]



Expert Solution
Step 1

Slow step is rate determining step .

And any species which formed during reaction but not part of overall reaction is intermediate.

We apply steady state approximation to intermediate and assume that it's concentration remains constant.

 

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