= Solution
One mole of CF consumes one mole of electrons, so the equilibrium electrical work gives
$$
\boxed{\Delta_rG^\circ=-FE^\circ
=-(96540)(3.2)\,\mathrm{J\,mol^{-1}}
=-308.9\,\mathrm{kJ\,mol^{-1}}}.
$$
Interpreting the measured OCV as $E^\circ$ assumes an equilibrated cell and the appropriate standard-state activities; pure solid reactants and products make the ideal activity correction simple. A nonequilibrium or composition-dependent OCV would instead determine the corresponding reaction free energy under those conditions.
The temperature coefficient is
$$
\boxed{\left(\frac{\partial E}{\partial T}\right)_p
=\frac{\Delta_rS}{F}}.
$$
The net reaction involves condensed phases and no gas, so one expects a more modest entropy-driven voltage change than for a reaction creating or consuming substantial gas. However, it is not exactly zero, and its magnitude or sign cannot be calculated from the single OCV value without entropy or temperature-dependent data. This should be separated from potentially strong temperature effects on loaded-cell kinetics and resistance.
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