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The chlorine-catalyzed destruction of ozone in the upper atmosphere is thought to proceed by a two-step mechanism: Cl(g) + O3(g) --> ClO(g) + O2(g) (slow) ClO(g) + O(g) --> Cl(g) + O2(g) (a) If the first step of this mechanism is rate-determining (slow), choose the correct rate law for the overall process. Rate = k [Cl] [O3] Rate = k [Cl] [ClO]     Rate = k [O3] [O] Rate = k [ClO] [O] Rate = k [O3]2 Rate = k [O3]2 [O] (b) Choose the correct chemical equation for the overall process. O(g) + O3(g) --> 2 O2(g) Cl(g) + O3(g) --> ClO(g) + O2(g)     ClO(g) + O(g) --> Cl(g) + O2(g) (c) Identify an intermediate in the reaction. O2 Cl     ClO O3 (d) Identify the catalyst in the reaction. Cl O2     ClO O3 (e) Identify a reactant in the reaction. O2 ClO     Cl O3 (f) Identify a product in the reaction. O2 Cl     ClO O3

The chlorine-catalyzed destruction of ozone in the upper atmosphere is thought to proceed by a two-step mechanism: Cl(g) + O3(g) --> ClO(g) + O2(g) (slow) ClO(g) + O(g) --> Cl(g) + O2(g) (a) If the first step of this mechanism is rate-determining (slow), choose the correct rate law for the overall process. Rate = k [Cl] [O3] Rate = k [Cl] [ClO]     Rate = k [O3] [O] Rate = k [ClO] [O] Rate = k [O3]2 Rate = k [O3]2 [O] (b) Choose the correct chemical equation for the overall process. O(g) + O3(g) --> 2 O2(g) Cl(g) + O3(g) --> ClO(g) + O2(g)     ClO(g) + O(g) --> Cl(g) + O2(g) (c) Identify an intermediate in the reaction. O2 Cl     ClO O3 (d) Identify the catalyst in the reaction. Cl O2     ClO O3 (e) Identify a reactant in the reaction. O2 ClO     Cl O3 (f) Identify a product in the reaction. O2 Cl     ClO O3

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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29. The chlorine-catalyzed destruction of ozone in the upper atmosphere is thought to proceed by a two-step mechanism:

Cl(g) + O3(g) --> ClO(g) + O2(g) (slow)
ClO(g) + O(g) --> Cl(g) + O2(g)




(a) If the first step of this mechanism is rate-determining (slow), choose the correct rate law for the overall process.


Rate = k [Cl] [O3]
Rate = k [Cl] [ClO]    
Rate = k [O3] [O]
Rate = k [ClO] [O]
Rate = k [O3]2
Rate = k [O3]2 [O]





(b) Choose the correct chemical equation for the overall process.


O(g) + O3(g) --> 2 O2(g)
Cl(g) + O3(g) --> ClO(g) + O2(g)    
ClO(g) + O(g) --> Cl(g) + O2(g)





(c) Identify an intermediate in the reaction.


O2
Cl   
 ClO
O3





(d) Identify the catalyst in the reaction.


Cl
O2    
ClO
O3





(e) Identify a reactant in the reaction.


O2
ClO   
 Cl
O3





(f) Identify a product in the reaction.


O2
Cl    
ClO
O3
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