Chemistry - Electrochemistry Question with Solution | TestHub

The cell reaction for the given cell is:

${\mathrm{Zn}}_{(\mathrm{s})}+2{\mathrm{Ag}}_{(\mathrm{aq})}^{+}\to {\mathrm{Zn}}_{(\mathrm{aq})}^{2+}+2{\mathrm{Ag}}_{(\mathrm{s})}$

The number of moles of electrons transferred in the balanced cell reaction is $n=2$.

Standard emf of the cell, $E^{\circ }=1.55\text{ V}$.

Faraday's constant, $F=96500{\text{ C mol}}^{-1}$.

The electrical work done under standard conditions is given by the standard Gibbs free energy change ($\Delta G^{\circ }$):

$\Delta G^{\circ }=-nF{E}^{\circ }$

$\Delta G^{\circ }=-2\times 96500\times 1.55$

$\Delta G^{\circ }=-299150\text{ J}$

$\Delta G^{\circ }=-299.150\text{ kJ}$

Answer: $-299.150\mathrm{kJ}$