Redox Reactions

HINT: Oxidation occurs at anode.

Explanation: 

For the given cell : ${\mathrm{Zn}}_{\left(\mathrm{s}\right)<mspace\; width="1em"></mspace>}<mspace\; width="1em"></mspace>+<mspace\; width="1em"></mspace>2{{\mathrm{Ag}}^{+}}_{\left(\mathrm{aq}\right)}<mspace\; width="1em"></mspace>\to {{\mathrm{Zn}}^{+2}}_{\left(\mathrm{aq}\right)}<mspace\; width="1em"></mspace>+<mspace\; width="1em"></mspace>{\mathrm{Ag}}_{\left(\mathrm{s}\right)}<mspace\; width="1em"></mspace>$

Zn electrode is negatively charged because at this electrode, Zn oxidizes to ${\mathrm{Zn}}^{+2}$ and the leaving electrons accumulate on this electrode. Ions are the carriers of current in the cell.

The reaction taking place at the zinc electrode is : ${\mathrm{Zn}}_{\left(\mathrm{s}\right)\hspace{0.17em}}\to <mspace\; width="1em"></mspace>{{\mathrm{Zn}}^{+2}}_{\left(\mathrm{aq}\right)}<mspace\; width="1em"></mspace>+<mspace\; width="1em"></mspace>2{\mathrm{e}}^{–}$