The following reaction occurs in a button cell:
$(i)$ $Ag_{2}O + H_{2}O + 2e^{-} \rightarrow 2Ag + 2OH^{-}$
$(ii)$ $Zn \rightarrow Zn^{2+} + 2e^{-}$
Calculate the standard Gibbs free energy change $\Delta G^{o}$ for the overall cell reaction.
$[E^{o}_{Zn^{2+}\mid Zn} = -0.76 \ V, E^{o}_{Ag_{2}O\mid Ag} = 0.34 \ V]$

• A
  $-2.12 \times 10^{5} \ J$
• B
  $-1.06 \times 10^{5} \ J$
• C
  $2.12 \times 10^{5} \ J$
• D
  $-4.24 \times 10^{5} \ J$