Depict the galvanic cell in which the reaction $\mathrm{Zn}(\mathrm{s})+2 \mathrm{Ag}^{+}(\mathrm{aq}) \rightarrow \mathrm{Zn}^{2+}(\mathrm{aq})+2 \mathrm{Ag}(\mathrm{s})$ 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.
The galvanic cell corresponding to the given redox reaction can be represented as:
$\mathrm{Zn}\left|\mathrm{Zn}_{\left(a_{q}\right)}^{2+}\right|\left|\mathrm{Ag}_{\left(a_{q}\right)}^{+}\right| \mathrm{Ag}$
(i) $\mathrm{Zn}$ electrode is negatively charged because at this electrode, $\mathrm{Zn}$ oxidizes to $\mathrm{Zn}^{2+}$ and the leaving electrons accumulate on this electrode.
(ii) Ions are the carriers of current in the cell.
(iii) The reaction taking place at Zn electrode can be represented as:
$\mathrm{Zn}_{(s)} \longrightarrow \mathrm{Zn}_{(a q)}^{2+}+2 \mathrm{e}^{-}$
And the reaction taking place at Ag electrode can be represented as:
$\mathrm{Ag}_{(\text {aq })}^{+}+\mathrm{e}^{-} \longrightarrow \mathrm{Ag}_{(s)}$
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