Calculate `Delta G^@` for the following reaction.
`Ag^(+) (aq) + Cl^(-) (aq) to AgCl(s)`
Given `Delta G_f^@ (AgCl) = - 109kJ //"mol" `
`Delta G_f^@ (Cl^-) = -129 `kJ/mol
`Delta G_f^@ (Ag^+) = 77` kJ/mol
Represent the above reaction in the form of a cell. Also calculate `E^@` of the cell and find log `K_(sp)` of AgCl.

Explanation

`(Ag|AgCl, Cl^(-) Ag^(+) | Ag) 0.59V, -10`