For the cell (at 298 K ) `Ag_((g)) // AgCl_((s)) // Cl_((aq))^(-) ||AgNO_(3(aq)) // Ag_((s))`
Which of the following is correct ?

Options

A. The EMF of the cell is zero when `[Ag^(+)]_("anodic " ) = (Ag^(+) )_("cathodic")`
B. The amount of `AgCl_((s))` precipitate in anodic compartment will decrease with the working of the cell
C. The concentration of `[Ag^(+)]` is constant in anodic compartment with the working of cell
D. `E_("cell") = E_(Ag^(+)//Ag)^(0)-E_(Cr^(-)//AgCl//Ag^(-))^(0) (0.059)/(1) log""(1)/([Cl^(-1)]) ` anodic

Answer

B, C, D

Explanation

`underset("anode")(Ag//AgCl)//KCl_((aq)) // //AgnO_(3(aq)) //underset("cathode")(Ag_((s)) ) , E_("cell") = E_("cathode")^(0) -E_("anodic")^(0)`
`E_("cathode")^(0) = E_(Ag^(+)//Ag)^(0) + (0.059)/(1) log [Ag^(+)] , E_("cell") =E_(O.P)^(0)-(0.059)/(1) log[Ag^(+)] + E_(R.P)^(0) + (0.059)/(1) log""(1)/([Cl^(-)])`
E.M.F of cell is zero when `[Ag^(+)]_("cathode") = [Ag^(+)]_("anode")`