Depict the galvanic cell in which the reaction $Zn_{(s)} + 2Ag^{+}_{(aq)} \rightarrow Zn^{2+}_{(aq)} + 2Ag_{(s)}$ takes place,further show:
$(i)$ which of the electrode is negatively charged,
$(ii)$ the carriers of the current in the cell,and
$(iii)$ individual reaction at each electrode.

(N/A) The galvanic cell corresponding to the given redox reaction is represented as:
$Zn_{(s)} | Zn^{2+}_{(aq)} || Ag^{+}_{(aq)} | Ag_{(s)}$
$(i)$ The $Zn$ electrode is negatively charged because oxidation occurs here $(Zn \rightarrow Zn^{2+} + 2e^-)$,leaving behind electrons.
$(ii)$ The carriers of current in the cell are ions in the electrolyte and electrons in the external circuit.
$(iii)$ The individual reactions are:
At anode: $Zn_{(s)} \rightarrow Zn^{2+}_{(aq)} + 2e^-$
At cathode: $Ag^{+}_{(aq)} + e^- \rightarrow Ag_{(s)}$