A student investigates the standard cell potential of an electrochemical cell involving iron and silver species. The standard reduction potentials for the relevant half-reactions at \(298\text{ K}\) are shown in the table below.

Half-reaction	\(E^\circ\text{ (V)}\)
\(\text{Fe}^{3+}\text{(aq)} + \text{e}^- \rightarrow \text{Fe}^{2+}\text{(aq)}\)	\(+0.77\)
\(\text{Ag}^+\text{(aq)} + \text{e}^- \rightarrow \text{Ag(s)}\)	\(+0.80\)

Based on the data, what is the value of \(E^\circ_{\text{cell}}\) for the thermodynamically favored reaction between \(\text{Fe}^{2+}\text{(aq)}\) and \(\text{Ag}^+\text{(aq)}\) under standard conditions at \(298\text{ K}\)?