For a cell reaction with standard cell potential $E^\circ_\text{cell} = +1.10\,\text{V}$ and $n = 2$ electrons transferred, the standard Gibbs free energy change $\Delta G^\circ$ is approximately:

$\Delta G^\circ = -nFE^\circ = -(2)(96500)(1.10) = -212{,}300\,\text{J} = -212.3\,\text{kJ}$. The negative sign reflects a spontaneous forward reaction, consistent with $E^\circ_\text{cell}$ being positive.