We’re being asked to calculate for ΔG° for the given non-aqueous cell reaction .

**ΔG° can be calculated from the cell potential using the following equation:**

$\overline{){\mathbf{\u2206}}{\mathbf{G}}{\mathbf{=}}{\mathbf{-}}{\mathbf{nFE}}{{\mathbf{\xb0}}}_{{\mathbf{cell}}}}$

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:**

Calculate the standard free-energy change for the following reaction at 25 °C.

2 Au^{3+}(aq) + 3 Cr(s) ↔ 2 Au(s) + 3Cr^{2+}(aq)

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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.