Given the standard reduction potentials \((E^\Theta)\) for the half-cell reactions below, the standard Gibbs free energy of the dissolution of silver chloride in water, at 298 K, is ---- J mol\(^{-1}\) (rounded off to the nearest integer).
\[
\text{(Given: Faraday constant, } F = 96500 \text{ C mol}^{-1}; \quad J = C \times V)
\]
The standard reduction half-cell reactions are:
\[
\text{AgCl(s) + e}^- \rightarrow \text{Ag(s) + Cl}^-(\text{aq}); \quad E^\Theta = 0.22 \text{ V at 298 K}
\]
\[
\text{Ag}^+(\text{aq}) + e^- \rightarrow \text{Ag(s)}; \quad E^\Theta = 0.80 \text{ V at 298 K}
\]