An electric cell has the following chemical reaction

\[\mathrm{Zn}(\mathrm{s})+2 \mathrm{AgCl}(\mathrm{s})=\mathrm{ZnCl}_{2}+2 \mathrm{Ag}(\mathrm{s})\]

and produces an emf of \(1.005 \mathrm{~V}\) at \(25^{\circ} \mathrm{C}\) and \(1.015 \mathrm{~V}\) at \(0^{\circ} \mathrm{C}\), at a pressure of \(1 \mathrm{bar}\). Estimate the following parameters at \(25^{\circ} \mathrm{C}\) and \(1 \mathrm{bar}\) :

1. change in enthalpy during the reaction, 2. amount of heat absorbed by the cell, per unit amount of zinc, to maintain the temperature constant during reversible operation.

[-216,937 kJ/kmol Zn; -23,002 kJ/kmol Zn]