# Problem: A voltaic cell (same as a galvanic cell) is created from an Co/Co2+ half-cell (E°red = -0.28) and an Al/Al3+ half-cell (E°red = -1.66 V). Calculate the value of ∆G° for this cell.a. -800 Jb. -7.99x105 Jc.  +800 Jd. +7.99x105 Je. -2.66x105 J

###### FREE Expert Solution

We’re being asked to calculate for ΔG° for the voltaic cell (same as a galvanic cell) that is created from an Co/Co2+ half-cell (E°red = -0.28) and an Al/Al3+ half-cell (E°red = -1.66 V).

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:

84% (396 ratings) ###### Problem Details

A voltaic cell (same as a galvanic cell) is created from an Co/Co2+ half-cell (E°red = -0.28) and an Al/Al3+ half-cell (E°red = -1.66 V). Calculate the value of ∆G° for this cell.

a. -800 J
b. -7.99x105 J
c.  +800 J
d. +7.99x105 J
e. -2.66x105 J