Consider the standard electrode potentials:

\[{\text{F}}{{\text{e}}^{{\text{2 + }}}}{\text{(aq)}} + {\text{2}}{{\text{e}}^ - } \rightleftharpoons {\text{Fe(s)     }}  {E^\Theta } =  - {\text{0.45 V}}\]

\[\frac{1}{2}{\text{C}}{{\text{l}}_{\text{2}}}{\text{(g)}} + {{\text{e}}^ - } \rightleftharpoons {\text{C}}{{\text{l}}^ - }{\text{(aq)     }}  {E^\Theta } = {\text{ }} + {\text{1.36 V}}\]

What is the standard cell potential, in V, for the reaction?

\[{\text{C}}{{\text{l}}_{\text{2}}}{\text{(g)}} + {\text{Fe(s)}} \to {\text{2C}}{{\text{l}}^ - }{\text{(aq)}} + {\text{F}}{{\text{e}}^{2 + }}{\text{(aq)}}\]

A.     \( + {\text{0.91}}\)

B.     \( + {\text{1.81}}\)

C.     \( + {\text{2.27}}\)

D.     \( + {\text{3.17}}\)

B