We’re being asked to calculate for ΔG° for the voltaic cell (same as a galvanic cell) that is created from an Co/Co^{2+} half-cell (E°_{red} = -0.28) and an Al/Al^{3+} half-cell (E°_{red} = -1.66 V).

**ΔG° can be calculated from the cell potential using the following equation:**

$\overline{){\mathbf{\u2206}}{\mathbf{G}}{\mathbf{=}}{\mathbf{-}}{\mathbf{nFE}}{{\mathbf{\xb0}}}_{{\mathbf{cell}}}}$

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:**

A voltaic cell (same as a galvanic cell) is created from an Co/Co^{2+} half-cell (E°_{red} = -0.28) and an Al/Al^{3+} half-cell (E°_{red} = -1.66 V). Calculate the value of ∆G° for this cell.

a. -800 J

b. -7.99x10^{5} J

c. +800 J

d. +7.99x10^{5} J

e. -2.66x10^{5} J

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