Depict the galvanic cell in which the reaction $Zn_{(s)} + 2Ag_{(aq)}^{+} \to Zn_{(aq)}^{2+} + 2Ag_{(s)}$ takes place. Further show:
$(i)$ Which electrode is negatively charged?
$(ii)$ The carriers of the current in the cell.
$(iii)$ Individual reaction at each electrode.

(A) The given redox reaction is: $Zn_{(s)} + 2Ag_{(aq)}^{+} \to Zn_{(aq)}^{2+} + 2Ag_{(s)}$
Representation of the galvanic cell: $Zn_{(s)} | Zn_{(aq)}^{2+} || Ag_{(aq)}^{+} | Ag_{(s)}$
$(i)$ The $Zn$ electrode acts as the anode where oxidation occurs $(Zn \to Zn^{2+} + 2e^-)$,so it is the negatively charged electrode.
$(ii)$ In the external circuit,electrons are the carriers of current (flowing from $Zn$ to $Ag$),while in the internal circuit (electrolyte),ions are the carriers of current.
$(iii)$ Individual reactions:
Anode (Oxidation): $Zn_{(s)} \to Zn_{(aq)}^{2+} + 2e^-$
Cathode (Reduction): $2Ag_{(aq)}^{+} + 2e^- \to 2Ag_{(s)}$