Question

1. A proposed mechanism for the oxidation of thallium(I) by the cerium(IV) ion is:

Ce⁺⁴(aq) + Mn⁺²(aq) $=$ Ce⁺³(aq) + Mn⁺³(aq)

Ce⁺⁴(aq) + Mn⁺³ (aq)   → Ce⁺³(aq) + Mn⁺⁴(aq)

Mn⁴⁺(aq) + Tl⁺(aq)       →     Mn⁺²(aq) + Tl⁺³(aq)

(a) Write the balanced chemical equation for the overall reaction described by this mechanism.

(b) Write the chemical formula(s) for all intermediates involved in this mechanism.

(c) Write the chemical formula(s) for all catalyst(s) involved in this mechanism

(d) Write the overall rate law predicted by this mechanism if the first step is the slowest step.

Answer 1

Answers. (a). overall balanced eqreation is - ce 4+(99.) + M712+(99.) —Ce3+(99.) + Mn3+ (aq). Ce47(aq) + Mast (aq) + Ce 3+ (aq) + Mn4+(99-). Mot4(aq.) + Tlti (a9.) → Mona+(a9.) + TC 3+ (aq) 26e4+ + Mah 2+ +mha+ + 6444 Tiet → 20e3++ pm 27 mm 34 mon +4 Te 3+ overall balanced equation is - 2ce4+ + T4+1 26€3++ Tet3 (6) Intermediates are those which produced in one step are consumed in other step. In this reaction, Intermediates are M793t and Mo 4+ Mn3+ produced in first step, consumed in second step. Mn4+ produced in to second step, consumed in third step. (C) Catalyst Poinvolved is Mn2+ catalyst are those which take part in reaction and remain i unchanged. (d) The slowest step is. Ce4+ (aq) + M72+ (09.)76377 Most slowest step is the Rate determining step- Pirate = k [ce4+][ Mn 2+1 |