An aqueous solution containing one mole per litre of each $\mathrm{Cu}{\left({\mathrm{NO}}_3\right)}_2,{\mathrm{AgNO}}_3.\mathrm{Hg}{\left({\mathrm{NO}}_3\right)}_2$ $\mathrm{Mg}{\left({\mathrm{NO}}_3\right)}_2$ is being electrolyzed using inert electrodes. The values of standard electrode potential in volts (reduction potential) are $\mathrm{Ag}/{\mathrm{Ag}}^{+}=+0.80 \mathrm{V};\mathrm{Hg}/{\mathrm{Hg}}^{2+}=+0.79 \mathrm{V}; \mathrm{Cu}/{\mathrm{Cu}}^{2+}=+0.34 \mathrm{V};\mathrm{Mg}/{\mathrm{Mg}}^{2+}=-2.37\mathrm{V}$ With increasing voltage, the sequence of deposition of metals on cathode will be