We’re being asked to calculate for ΔG° for the given non-aqueous cell reaction at 298 K.
ΔG° can be calculated from the cell potential using the following equation:
ΔG° = Gibbs Free Energy, J
n = # of e- transferred
F = Faraday’s constant = 96485 J/(mol e-)
E°cell = standard cell potential, V
First, let’s determine how many electrons were transferred from the cell reaction:
Consider the non–aqueous cell reaction
2 K(s) + Fe2+ (aq) → 2 K+ (aq) + Fe(s)
for which E°cell = 1.49 V at 298 K. ΔG° at this temperature is
A) +287.6 kJ D) –143.7 kJ
B) –287.6 kJ E) None of these choices is correct.
C) +143.7 kJ
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