For the cell (at 298K)
`Ag(s) | AgCl(s) | Cl^(-)(aq)|| AgNO_(3)(aq) | Ag(s)`
Which of the following is correct?

Options

A. The cell emf will be zero when `[Ag^(+)]_(a)=[Ag^(+)]_(c)([Ag^(+)]` in anodic compartment`=[Ag^(+)]` in cathode compartment)
B. The amount of `AgCl(s)` precipitate in anodic compartment will decrease with the working of the cell.
C. The concentration of `[Ag^(+)]=` constant, in anodic compartment during work of cell.
D. `E_(cell)=E_(Ag^(+)|Ag)^(0)-E_(Cl^(-)|AgCl|Ag)^(0)-(0.059)/(1)log((1)/(|Cl^(-)|_(a)))`

Answer

A

Explanation

`E_(cell)=E_(cell)^(@)-(0.059)/(1)log((1)/([Cl^(-)]_(a)[Ag^(+)]_(c)))`, at `[Ag^(+)]_(c)=[Ag^(+)]_(a)` equilibrium will achieve and `K=K_(sp)=[Ag^(+)]_(a)[Cl^(-)]_(a)`