A student constructs a standard galvanic cell at \(298\text{ K}\) using a silver electrode in a \(1.0\text{ M }\text{AgNO}_3\text{(aq)}\) solution and a nickel electrode in a \(1.0\text{ M }\text{Ni(NO}_3)_2\text{(aq)}\) solution. The two half-cells are connected by a salt bridge and a voltmeter.

Half-reaction	\(E^\circ\text{ (V)}\)
\(\text{Ag}^+\text{(aq)} + \text{e}^- \rightarrow \text{Ag(s)}\)	\(+0.80\)
\(\text{Ni}^{2+}\text{(aq)} + 2\,\text{e}^- \rightarrow \text{Ni(s)}\)	\(-0.25\)

Based on the data in the table, what is the value of the standard cell potential, \(E^\circ_{\text{cell}}\), for the galvanic cell?