The galvanic cell in which the given reaction takes place is depicted as: $$\\displaystyle Zn(s)| Zn^{2+} (aq) || Ag^+ (aq) |Ag(s)$$(i) The negatively charged electrode is the zinc electrode. It acts as an anode.(ii) In the external circuit, the current will flow from silver to zinc. (iii) Oxidation at anode: $$\\displaystyle Zn(s) \\rightarrow Zn^{2+}(aq) +2e^-$$Reduction at cathode: $$\\displaystyle Ag^+(aq) + e^- \ o Ag(s) $$