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The manganese(II)-catalyzed redox reaction between cerium(IV) and thallium(I) is thought to proceed by a three-step mechanism: Ce4+(aq) + Mn2+(aq) --> Ce3+(aq) + Mn3+(aq) (slow) Ce4+(aq) + Mn3+(aq) --> Ce3+(aq) + Mn4+(aq) Mn4+(aq) + Tl+(aq) --> Mn2+(aq) + Tl3+(aq) (a) If the first step of this mechanism is rate-determining (slow), choose the correct rate law for the overall process. Rate = k [Mn2+] [Mn3+] Rate = k [Ce4+]2 Rate = k [Ce4+] [Tl+] Rate = k [Mn2+] [Ce4+] Rate = k [Ce4+]2 [Tl+] Rate = k [Mn3+] [Tl+] (b) Choose the correct chemical equation for the overall process. Ce4+(aq) + Mn2+(aq) --> Ce3+(aq) + Mn3+(aq) Ce4+(aq) + Mn3+(aq) --> Ce3+(aq) + Mn4+(aq) 2 Ce4+(aq) + Tl+(aq) --> 2 Ce3+(aq) + Tl3+(aq) (c) Identify an intermediate in the reaction. Mn2+ Ce3+ Mn3+ Ce4+ (d) Identify the catalyst in the reaction. Mn2+ Mn3+ Ce3+ Ce4+ (e) Identify a reactant in the reaction. Ce3+ Ce4+ Mn2+ Mn3+ (f) Identify a product in the reaction. Mn3+ Mn2+ Ce4+ Ce3+

The manganese(II)-catalyzed redox reaction between cerium(IV) and thallium(I) is thought to proceed by a three-step mechanism: Ce4+(aq) + Mn2+(aq) --> Ce3+(aq) + Mn3+(aq) (slow) Ce4+(aq) + Mn3+(aq) --> Ce3+(aq) + Mn4+(aq) Mn4+(aq) + Tl+(aq) --> Mn2+(aq) + Tl3+(aq) (a) If the first step of this mechanism is rate-determining (slow), choose the correct rate law for the overall process. Rate = k [Mn2+] [Mn3+] Rate = k [Ce4+]2 Rate = k [Ce4+] [Tl+] Rate = k [Mn2+] [Ce4+] Rate = k [Ce4+]2 [Tl+] Rate = k [Mn3+] [Tl+] (b) Choose the correct chemical equation for the overall process. Ce4+(aq) + Mn2+(aq) --> Ce3+(aq) + Mn3+(aq) Ce4+(aq) + Mn3+(aq) --> Ce3+(aq) + Mn4+(aq) 2 Ce4+(aq) + Tl+(aq) --> 2 Ce3+(aq) + Tl3+(aq) (c) Identify an intermediate in the reaction. Mn2+ Ce3+ Mn3+ Ce4+ (d) Identify the catalyst in the reaction. Mn2+ Mn3+ Ce3+ Ce4+ (e) Identify a reactant in the reaction. Ce3+ Ce4+ Mn2+ Mn3+ (f) Identify a product in the reaction. Mn3+ Mn2+ Ce4+ Ce3+

Chemistry for Engineering Students
Chemistry for Engineering Students
4th Edition
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter13: Electrochemistry
Section: Chapter Questions
Problem 13.90PAE: A chemical engineering student is studying the effect of pH on the corrosion of iron. Ellie...
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The manganese(II)-catalyzed redox reaction between cerium(IV) and thallium(I) is thought to proceed by a three-step mechanism:

Ce4+(aq) + Mn2+(aq) --> Ce3+(aq) + Mn3+(aq) (slow)
Ce4+(aq) + Mn3+(aq) --> Ce3+(aq) + Mn4+(aq)
Mn4+(aq) + Tl+(aq) --> Mn2+(aq) + Tl3+(aq)



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


Rate = k [Mn2+] [Mn3+]
Rate = k [Ce4+]2    
Rate = k [Ce4+] [Tl+]
Rate = k [Mn2+] [Ce4+]
Rate = k [Ce4+]2 [Tl+]
Rate = k [Mn3+] [Tl+]





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


Ce4+(aq) + Mn2+(aq) --> Ce3+(aq) + Mn3+(aq)
Ce4+(aq) + Mn3+(aq) --> Ce3+(aq) + Mn4+(aq)    
2 Ce4+(aq) + Tl+(aq) --> 2 Ce3+(aq) + Tl3+(aq)





(c) Identify an intermediate in the reaction.


Mn2+
Ce3+   
 Mn3+
Ce4+





(d) Identify the catalyst in the reaction.


Mn2+
Mn3+    
Ce3+
Ce4+





(e) Identify a reactant in the reaction.


Ce3+
Ce4+ 
  Mn2+
Mn3+





(f) Identify a product in the reaction.


Mn3+
Mn2+    
Ce4+
Ce3+
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