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.
$(iii)$ Individual reaction at each electrode.

(N/A) The galvanic cell in which the given reaction takes place is represented as:
$Zn_{(s)} | Zn^{2+}_{(aq)} || Ag^{+}_{(aq)} | Ag_{(s)}$
$(i)$ The $Zn$ electrode (anode) is negatively charged.
$(ii)$ Ions are the carriers of current inside the cell,while electrons are the carriers in the external circuit.
$(iii)$ The reaction at the anode (oxidation) is:
$Zn_{(s)} \longrightarrow Zn^{2+}_{(aq)} + 2e^-$
The reaction at the cathode (reduction) is:
$Ag^{+}_{(aq)} + e^- \longrightarrow Ag_{(s)}$