(i) Electrons move from Zn to Ag as `E^(@)` is more negative for Zn so Zn undergoes oxidation and ` Ag^(+)` undergoes reduction.
(ii) Ag is the cathode as it is the site of reduction where `Ag^(+)` takes electrons from medium and deposit at cathode.
(iii) Cell will stop functioning because cell potential drops to zero. AT E=0 reaction reaches equilibrium.
(iv) When `E_("cell")`=0 because at this condition reaction reaches to equilibrium.
(v) concentration of `Zn^(2+)` ions will increase and concentartion of `Ag^(+)` ions will decreases because Zn is converted into `Zn^(2+)` and `Ag^(+)` is converted into Ag.
(vi) when `E_("cell")=0` equilibrium is reached and concentration of `Zn^(2+)` ions and `Ag^(+)` will not change.