Chemistry - Electrochemistry Question with Solution | TestHub

The tendency of a metal ion to undergo reduction and deposit on the electrode is directly proportional to its standard reduction potential ($E^{\circ }$).

Higher the standard reduction potential, greater is the tendency of the metal ion to get reduced and deposited.

The given standard reduction potentials are:
$E_{{\mathrm{Ag}}^{+}/\mathrm{Ag}}^{\circ }=0.80\mathrm{V}$
$E_{{\mathrm{Cu}}^{2+}/\mathrm{Cu}}^{\circ }=0.337\mathrm{V}$
$E_{{\mathrm{Sn}}^{2+}/\mathrm{Sn}}^{\circ }=-0.136\mathrm{V}$
$E_{{\mathrm{Cd}}^{2+}/\mathrm{Cd}}^{\circ }=-0.403\mathrm{V}$

Arranging the standard reduction potentials in decreasing order:
$0.80\mathrm{V}>0.337\mathrm{V}>-0.136\mathrm{V}>-0.403\mathrm{V}$

Therefore, the decreasing order of deposition of the metals is $\mathrm{Ag}>\mathrm{Cu}>\mathrm{Sn}>\mathrm{Cd}$.

Answer: $\mathrm{Ag}>\mathrm{Cu}>\mathrm{Sn}>\mathrm{Cd}$