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

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:

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

ΔG° = Gibbs Free Energy, J
n = # of e^- transferred
F = Faraday’s constant = 96485 J/(mol e^-)
E°_cell = standard cell potential, V

First, let’s determine the cell potential and the number of electrons transferred from the cell reaction: