In the button cells widely used in watches and other devices,the following reaction takes place:
$Zn_{(s)} + Ag_2O_{(s)} + H_2O_{(l)} \rightarrow Zn^{2+}_{(aq)} + 2Ag_{(s)} + 2OH^{-}_{(aq)}$
Determine $\Delta_r G^\Theta$ and $E^\Theta$ for the reaction.
$Zn_{(s)} + Ag_2O_{(s)} + H_2O_{(l)} \rightarrow Zn^{2+}_{(aq)} + 2Ag_{(s)} + 2OH^{-}_{(aq)}$
Determine $\Delta_r G^\Theta$ and $E^\Theta$ for the reaction.
(N/A) The standard cell potential $E^\Theta$ is given as $1.104 \ V$.
The reaction involves the transfer of $n = 2$ electrons.
Using the formula $\Delta_r G^\Theta = -nFE^\Theta$,where $F = 96487 \ C \ mol^{-1}$:
$\Delta_r G^\Theta = -2 \times 96487 \ C \ mol^{-1} \times 1.104 \ V$
$= -213043.296 \ J \ mol^{-1}$
$= -213.04 \ kJ \ mol^{-1}$
The reaction involves the transfer of $n = 2$ electrons.
Using the formula $\Delta_r G^\Theta = -nFE^\Theta$,where $F = 96487 \ C \ mol^{-1}$:
$\Delta_r G^\Theta = -2 \times 96487 \ C \ mol^{-1} \times 1.104 \ V$
$= -213043.296 \ J \ mol^{-1}$
$= -213.04 \ kJ \ mol^{-1}$
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