Question

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 [Ce⁴⁺]²

Rate = k [Ce⁴⁺] [Tl⁺]

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

Rate = k [Mn³⁺] [Tl⁺]

Rate = k [Ce⁴⁺]² [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⁺Mn³⁺ Ce³⁺Ce⁴⁺

(d) Identify the catalyst in the reaction.

Mn³⁺Ce³⁺ Ce⁴⁺Mn²⁺

(e) Identify a reactant in the reaction.

Mn³⁺Mn²⁺ Ce³⁺Ce⁴⁺

(f) Identify a product in the reaction.

Ce³⁺Ce⁴⁺ Mn³⁺Mn²⁺