A galvanic cell operates according to the following balanced equation at \(298\text{ K}\):

\[\text{X(s)} + 2\text{Y}^+\text{(aq)} \rightarrow \text{X}^{2+}\text{(aq)} + 2\text{Y(s)}\]

The standard reduction potentials for the two half-reactions are given in the table below.

Half-reaction	\(E^\circ\text{ (V)}\)
\(\text{Y}^+\text{(aq)} + e^- \rightarrow \text{Y(s)}\)	\(+0.80\)
\(\text{X}^{2+}\text{(aq)} + 2e^- \rightarrow \text{X(s)}\)	\(+0.30\)

Based on the information above and Faraday's constant (\(F = 96{,}500\text{ J}/(\text{V}\cdot\text{mol } e^-)\)), what is the value of the standard Gibbs free energy change, \(\Delta G^\circ\), for the overall cell reaction at \(298\text{ K}\)?