Calculate E° for the Electrochemical Cell Below, Pb |PbCl₂ |

Calculate E° for the electrochemical cell below, Pb |PbCl₂ | Cl^- || Fe³⁺,Fe²⁺ | Pt Given the following reduction half-reactions.
$\begin{array}{ll}\mathrm{Pb}^{2+}(a q) +2 e^{-} \rightarrow \mathrm{Pb}(s) & E^{\circ}=-0.126 \mathrm{~V} \\\mathrm{PbCl}_{2}(s) +2 e^{-} \rightarrow \mathrm{Pb}(s) +2 \mathrm{Cl}^{-}(a q) & E^{\circ}=-0.267 \mathrm{~V} \\\mathrm{Fe}^{3+}(a q) +e^{-} \rightarrow \mathrm{Fe}^{2+}(a q) & E^{\circ}=+0.771 \mathrm{~V} \\\mathrm{Fe}^{2+}(a q) +e^{-} \rightarrow \mathrm{Fe}(s) & E^{\circ}=-0.44 \mathrm{~V}\end{array}$

A) -0.504 V
B) -0.062 V
C) +0.504 V
D) +1.038 V
E) +1.604 V