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Using the given standard electrode potentials, decide whether the reaction Sn2+ (aq) + Br2 (l) -> Sn4+ (aq) + 2Br- (aq) is feasible (spontaneous) under standard conditions. Given: E°(Sn4+/Sn2+) = +0.15 V, E°(Br2/Br-) = +1.06 V.

1. Yes, feasible; E°cell = +0.91 V
2. No, not feasible; E°cell = -0.91 V
3. Yes, feasible; E°cell = +1.21 V
4. No, not feasible; E°cell = -1.21 V

Correct answer: Yes, feasible; E°cell = +0.91 V

Solution

Br2 has the higher reduction potential (+1.06 V) so it is reduced (cathode), while Sn2+ is oxidised to Sn4+ (anode, +0.15 V). E°cell = 1.06 - 0.15 = +0.91 V. Since E°cell is positive, ΔG = -nFE°cell is negative and the reaction proceeds spontaneously under standard conditions.

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