The emf of the cell reaction is 1.1 V. Calcu | vedclass

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(D) The standard free energy change is given by the formula: $\Delta G^o = -nFE^o$ Here,$n = 2$ (number of electrons transferred in the reaction). $F

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$-212.3$

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(D) The standard free energy change is given by the formula: $\Delta G^o = -nFE^o$ Here,$n = 2$ (number of electrons transferred in the reaction). $F = 96500 \ C \ mol^{-1}$ (Faraday's constant). $E^o = 1.1 \ V$. Substituting the values: $\Delta G^o = -2 	imes 96500 	imes 1.1 \ J \ mol^{-1}$ $\Delta G^o = -212300 \ J \ mol^{-1}$ Converting to $kJ \ mol^{-1}$: $\Delta G^o = -212.3 \ kJ \ mol^{-1}$

The $emf$ of the cell reaction is $1.1 \ V$. Calculate the free energy change for the reaction in $kJ$:
$Zn_{(s)} + Cu^{+2}_{(aq)} \longrightarrow Zn^{+2}_{(aq)} + Cu_{(s)}$

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The $emf$ of the cell reaction is $1.1 \ V$. Calculate the free energy change for the reaction in $kJ$: $Zn_{(s)} + Cu^{+2}_{(aq)} \longrightarrow Zn^{+2}_{(aq)} + Cu_{(s)}$