Calculate the useful work done during the reaction in kJ/mol.
Ag(S)+12 Cl2(g)→AgCl(s)
Given that E0Cl2/Cl−=+1.36V
and E0Ag+|AgCl|Cl−=+0.220V
PCl2=1 atm and T = 298 K
For the cell reaction:
Ag(s)+12 Cl2(g)→AgCl(s)E0=1.36−0.22=1.14 V
or, E=E0−0.0591log 1[Cl2]12
In standard conditions, PCl2=1 atm
∴ log [Cl2]12=0
Useful work=−Wmax=△G=−nEF=(1)×(1.14)×96500×10−3=110 kJ/mol