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