The zinc/silver oxide cell is used in electric watches. The reaction is as following,
$$Zn^{2+} + 2e^- \rightarrow Zn; E^0 = - 0.760 V$$
$$Ag_2O + H_2 O + 2e^- \rightarrow 2Ag + 2OH^- ; E^0 = 0.344 V$$
If F is $$96,500 C mol^{-1}, \triangle G^0$$ of the cell will be

A

413.021 kJ $$mol^{-1}$$

B

113.072 kJ $$mol^{-1}$$

C

213.072 kJ $$mol^{-1}$$

D

313.082 kJ $$mol^{-1}$$