To determine the correct cell potential ($E^{\circ}_{cell}$), we identify the cathode and the anode based on their standard reduction potentials ($E^{\circ}$). The half-cell with the higher standard reduction potential will undergo reduction and act as the cathode. The half-cell with the lower standard reduction potential will undergo oxidation and act as the anode. Given: $E^{\circ}_{Cr_2O_7^{2-}/Cr^{3+}} = +1.33\text{ V}$ (Cathode) $E^{\circ}_{Fe^{2+}/Fe} = -0.44\text{ V}$ (Anode)

The standard cell potential is calculated as: $E^{\circ}_{cell} = E^{\circ}_{cathode} - E^{\circ}_{anode}$ $E^{\circ}_{cell} = 1.33\text{ V} - (-0.44\text{ V})$ $E^{\circ}_{cell} = 1.33 + 0.44 = +1.77\text{ V}$