The following reaction occurs in a button cel | vedclass

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(A) The overall cell reaction is the sum of the two half-reactions:$Zn + Ag_{2}O + H_{2}O \rightarrow Zn^{2+} + 2Ag + 2OH^{-}$The standard cell potent

Vedclass · Accepted Answer

$-2.12 	imes 10^{5} \ J$

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(A) The overall cell reaction is the sum of the two half-reactions:$Zn + Ag_{2}O + H_{2}O ightarrow Zn^{2+} + 2Ag + 2OH^{-}$The standard cell potential $E^{o}_{cell}$ is given by:$E^{o}_{cell} = E^{o}_{cathode} - E^{o}_{anode}$$E^{o}_{cell} = 0.34 \ V - (-0.76 \ V) = 1.10 \ V$The number of electrons transferred in the balanced equation is $n = 2$.The standard Gibbs free energy change is calculated using the formula:$\Delta G^{o} = -nFE^{o}_{cell}$where $F \approx 96500 \ C \ mol^{-1}$.$\Delta G^{o} = -2 	imes 96500 \ C \ mol^{-1} 	imes 1.10 \ V$$\Delta G^{o} = -212300 \ J \ mol^{-1} = -2.123 	imes 10^{5} \ J \ mol^{-1}$.

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