10. Determine the direction in which the spontaneous reaction occurs from the following standard reduction potentials....

10. Determine the direction in which the spontaneous reaction occurs from the following standard reduction potentials. Indicate the reaction that is occurring at the anode, the cathode, the cell potential and the net ionic reaction.
Sn^4+ (ac) + 2e ----> Sn^2+ (ac) E = 0.15V
Fe^3+ (ac) + 1e ----> Fe^2+ (ac) E = 0.77V

Expert Solution

Solution:- The oxidation and reduction half cell reactions are given as :-

Sn²⁺ (aq) Sn⁺⁴ (aq) + 2e^-( Oxidation at anode)

[ Fe⁺³ (aq) + e^- Fe⁺² (aq) ] × 2 (Reduction at cathode)

Net ionic reaction :- Sn²⁺ (aq) + 2 Fe⁺³ (aq) Sn⁺⁴ (aq) + 2 Fe⁺² (aq)

E° cell (standard cell potential) = E°_R - E°_L = E°_{Fe⁺³/Fe⁺²} - E°_{Sn⁺⁴/Sn⁺²} = 0.77 - 0.15 = +0.62 V

Since, the cell potential E°cell is positive , reaction is spontaneous.

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queen_honey_blossom answered 2 years ago

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