# 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

###### FREE Expert Solution
93% (446 ratings)
###### 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:

$\overline{){\mathbf{∆}}{\mathbf{G}}{\mathbf{=}}{\mathbf{-}}{\mathbf{nFE}}{{\mathbf{°}}}_{{\mathbf{cell}}}}$

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:

93% (446 ratings)
###### 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

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Cell Potential concept. If you need more Cell Potential practice, you can also practice Cell Potential practice problems.

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Our tutors rated the difficulty ofConsider the non–aqueous cell reaction2 K(s) + Fe2+ (aq)  → ...as medium difficulty.

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