# Problem: The value of E°cell for Cr|Cr 3+||Hg 2 2+|Hg(l) is 1.78 V. Calculate ΔG° for this reaction at 25 . a. -1220 kJb. -1031 kJc. -872 kJd. -851 kJe. -621 kJ

###### FREE Expert Solution

We’re being asked to calculate for ΔG° for the Ecell with the cell notation:

Cr|Cr 3+||Hg 2 2+|Hg(l)

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 the cell potential and the number of electrons transferred from the cell reaction:

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###### Problem Details

The value of E°cell for Cr|Cr 3+||Hg 2 2+|Hg(l) is 1.78 V. Calculate ΔG° for this reaction at 25 .

a. -1220 kJ

b. -1031 kJ

c. -872 kJ

d. -851 kJ

e. -621 kJ

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