Problem: Consider the non–aqueous cell reaction2 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 kJB)        –287.6 kJ                     E)         None of these choices is correct.C)        +143.7 kJ

🤓 Based on our data, we think this question is relevant for Professor Ginger Jr.'s class at UW-SEATTLE.

FREE Expert Solution
FREE Expert Solution

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:

G=-nFE°cell

ΔG° = Gibbs Free Energy, J
n = # of e- transferred
F = Faraday’s constant = 96485 J/(mol e-)
cell = standard cell potential, V


First, let’s determine how many electrons were transferred from the cell reaction:

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Problem Details

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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