The given cell consists of an iron (Fe) electrode and a copper (Cu) electrode. Based on the standard reduction potentials, iron acts as the anode and copper acts as the cathode. Standard reduction potentials: $$ \begin{aligned} E^0_{\text{Fe}^{2+}/\text{Fe}} &= -0.44 \text{ V} \\ E^0_{\text{Cu}^{2+}/\text{Cu}} &= +0.34 \text{ V} \end{aligned} $$ The cell reaction is: $$ \text{Fe(s)} + \text{Cu}^{2+}(\text{aq}) \rightarrow \text{Fe}^{2+}(\text{aq}) + \text{Cu(s)} $$ The standard electromotive force (emf) of the cell, $E^0_{\text{cell}}$, is calculated as: $$ \begin{aligned} E^0_{\text{cell}} &= E^0_{\text{cathode}} - E^0_{\text{anode}} \\ &= E^0_{\text{Cu}^{2+}/\text{Cu}} - E^0_{\text{Fe}^{2+}/\text{Fe}} \\ &= 0.34 \text{ V} - (-0.44 \text{ V}) \\ &= 0.34 \text{ V} + 0.44 \text{ V} \\ &= 0.78 \text{ V} \end{aligned} $$