Textbook Problem

Consider the following galvanic cell at 25°C:

$\text{Pt}\left|{\text{Cr}}^{\text{2+}}\text{(0}\text{.30}M{\text{),Cr}}^{\text{3+}}\text{(2}\text{.0}M\text{)}\right|\left|{\text{Co}}^{\text{2+}}\text{(0}\text{.20}M\text{)}\right|\text{Co}$

The overall reaction and equilibrium constant value are

$2{\text{Cr}}^{2+}(aq)+{\text{Co}}^{2+}(aq)\to 2{\text{Cr}}^{3+}(aq)+\text{Co}(s) K=2.79\times {10}^7$

Calculate the cell potential, for this galvanic cell and ΔG for the cell reaction at these conditions.