Depict the galvanic cell in which the reaction Zn(s) + 2Ag+(aq) → Zn2+(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.
The galvanic cell in which the given reaction takes place is depicted as:
$\mathrm{Zn}_{(s)}\left|\mathrm{Zn}^{2+}{ }_{(a q)} \| \mathrm{Ag}_{(a q)}^{+}\right| \mathrm{Ag}_{(s)}$
(i) Zn electrode (anode) is negatively charged.
(ii) Ions are carriers of current in the cell and in the external circuit, current will flow from silver to zinc.
(iii) The reaction taking place at the anode is given by,
$\mathrm{Zn}_{(s)} \longrightarrow \mathrm{Zn}^{2+}{ }_{((q))}+2 \mathrm{e}^{-}$
The reaction taking place at the cathode is given by,
$\mathrm{Ag}^{+}{ }_{(a q)}+\mathrm{e}^{-} \longrightarrow \mathrm{Ag}_{(s)}$
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