The standard free energy of formation of `AgCl(s)` at `25^(@)C` is `-109.7kJ mol^(-1)` and `[H^(o+)+Cl^(c-)](aq)` is `-131.2kJ mol^(-1)`. Find `E^(c-)` of a cell up cells, with standard hydrogen electrode, and `Cl^(c-)|Ag|AgCl(s)`.

Explanation

Anode reaction `:(1)/(2)H_(2)(g)rarr H^(o+)(aq)+e^(-)`
Cathode reaction `:`
`AgCl(s)+e^(-) rarr Ag (s) +Cl^(c-)(aq)`
Cell reaction `:`
`ulbar((1)/(2)H_(2)(g)+AgCl(s)rarr H^(o+)(aq)+Cl^(c-)(aq)+Ag(s))`
`Delta_(r)G^(c-)=SigmaG^(c-)._(P)-SigmaG^(c-)._(R)`
`=DeltaG^(c-)._(P)-DeltaG^(c-)._(R)`
`=DeltaG^(c-)._((H^(o+)+Cl^(c-)))-DeltaG^(c-)._((AgCl))`
`=-131.2-(-109.7)=-21.5kJ mol ^(-1)`
`=-nFE^(c-)._(cell)`
`E^(c-)._(cell)=(-Delta_(r)G^(c-))/(nF)=(-21.5kJ mol^(-1))/(1xx96500C)`
`=0.2228~~0.223V`