Consider the galvanic cell reaction,

$\mathrm{Zn}\left(\mathrm{s}\right)+2{\mathrm{Ag}}^{+}\left(\mathrm{aq}\right)⟶{\mathrm{Zn}}^{2+}\left(\mathrm{aq}\right)+2\mathrm{Ag}\left(\mathrm{s}\right)$

Which of the following statements are correct?

The given redox reaction for the galvanic cell is

$\mathrm{Zn}\left(\mathrm{s}\right)+2{\mathrm{Ag}}^{+}\left(\mathrm{aq}\right)⟶{\mathrm{Zn}}^{2+}\left(\mathrm{aq}\right)+2\mathrm{Ag}\left(\mathrm{s}\right)$

At anode Zn is oxidised to ${\mathrm{Zn}}^{2+}$ions and at cathode

${\mathrm{Ag}}^{+}$ ions are reduced to Ag metal. Thus, galvanic cell for the above redox reaction may be depicted as 

$\mathrm{Zn}\left|{\mathrm{Zn}}^{2+}\left(\mathrm{aq}\right)\Vert {\mathrm{Ag}}^{+}\left(\mathrm{aq}\right)\right|\mathrm{Ag}$

(i) Zn electrode is negatively charged because of the oxidation of Zn to ${\mathrm{Zn}}^{2+}$ions, electrons are accumulated on zinc electrode.

(ii) The ions carry current in the cell. Current flows from Ag electrode to Zn electrode, while electrons flow from Zn electrode to Ag electrode.

(iii) Individual reaction at each electrode

$\text{ Anode }\mathrm{Zn}\left(s\right)⟶{\mathrm{Zn}}^{2+}\left(aq\right)+2e^{-}$

$\text{ Cathode }{\mathrm{Ag}}^{+}\left(\mathrm{aq}\right)+{\mathrm{e}}^{-}⟶\mathrm{Ag}\left(\mathrm{s}\right)$