Consider the following two standard electrode potentials at 298 K.

     ${\text{S}}{{\text{n}}^{2 + }}{\text{(aq)}} + {\text{2}}{{\text{e}}^ - } \rightleftharpoons {\text{Sn(s)}}$     ${E^\Theta } =  - 0.14{\text{ V}}$

     ${\text{F}}{{\text{e}}^{3 + }}{\text{(aq)}} + {{\text{e}}^ - } \rightleftharpoons {\text{F}}{{\text{e}}^{2 + }}{\text{(aq)}}$     ${E^\Theta } =  + 0.77{\text{ V}}$

What is the equation and cell potential for the spontaneous reaction that occurs?

A.     ${\text{2F}}{{\text{e}}^{2 + }}{\text{(aq)}} + {\text{S}}{{\text{n}}^{2 + }}{\text{(aq)}} \to {\text{2F}}{{\text{e}}^{3 + }}{\text{(aq)}} + {\text{Sn(s)}}$     ${E^\Theta } =  - 0.91{\text{ V}}$

B.     ${\text{2F}}{{\text{e}}^{3 + }}{\text{(aq)}} + {\text{Sn(s)}} \to {\text{2F}}{{\text{e}}^{2 + }}{\text{(aq)}} + {\text{S}}{{\text{n}}^{2 + }}{\text{(aq)}}$     ${E^\Theta } =  + 0.91{\text{ V}}$

C.     ${\text{2F}}{{\text{e}}^{2 + }}{\text{(aq)}} + {\text{S}}{{\text{n}}^{2 + }}{\text{(aq)}} \to {\text{2F}}{{\text{e}}^{3 + }}{\text{(aq)}} + {\text{Sn(s)}}$     ${E^\Theta } =  + 0.91{\text{ V}}$

D.     ${\text{2F}}{{\text{e}}^{3 + }}{\text{(aq)}} + {\text{Sn(s)}} \to {\text{2F}}{{\text{e}}^{2 + }}{\text{(aq)}} + {\text{S}}{{\text{n}}^{2 + }}{\text{(aq)}}$     ${E^\Theta } =  + 1.68{\text{ V}}$

B