# Problem: Calculate the standard free-energy change for the following reaction at 25 °C. 2 Au3+(aq) + 3 Cr(s) ↔ 2 Au(s) + 3Cr2+(aq)

###### FREE Expert Solution

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:

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

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:

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###### Problem Details

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

2 Au3+(aq) + 3 Cr(s) ↔ 2 Au(s) + 3Cr2+(aq)