For a Ag-Zn button cell,the net reaction is Z | vedclass

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(C) The net cell reaction is $Zn_{(s)} + Ag_{2}O_{(s)} \rightarrow ZnO_{(s)} + 2Ag_{(s)}$.The standard Gibbs free energy change for the reaction is gi

Vedclass · Accepted Answer

$1.591$

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(C) The net cell reaction is $Zn_{(s)} + Ag_{2}O_{(s)} ightarrow ZnO_{(s)} + 2Ag_{(s)}$.The standard Gibbs free energy change for the reaction is given by $\Delta G^{o} = \Delta G_{f}^{o}(ZnO) - \Delta G_{f}^{o}(Ag_{2}O)$.Substituting the values: $\Delta G^{o} = -318.3 - (-11.21) = -307.09 \ kJ \ mol^{-1} = -307.09 	imes 10^{3} \ J \ mol^{-1}$.Using the relation $\Delta G^{o} = -n F E^{o}_{cell}$,where $n = 2$ (number of electrons transferred) and $F = 96500 \ C \ mol^{-1}$.$-307.09 	imes 10^{3} = -2 	imes 96500 	imes E^{o}_{cell}$.$E^{o}_{cell} = \frac{307.09 	imes 10^{3}}{2 	imes 96500} = 1.591 \ V$.

For a $Ag-Zn$ button cell,the net reaction is $Zn_{(s)} + Ag_{2}O_{(s)} \rightarrow ZnO_{(s)} + 2Ag_{(s)}$. Given $\Delta G_{f}^{o}(Ag_{2}O) = -11.21 \ kJ \ mol^{-1}$ and $\Delta G_{f}^{o}(ZnO) = -318.3 \ kJ \ mol^{-1}$,the $E^{o}_{cell}$ of the button cell is ......... $V$.

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