${\mathrm{E}}^0{\mathrm{Sn}}^{2+}\left|\mathrm{Sn}=-1.14\mathrm{V},{\mathrm{E}}^0{\mathrm{Pb}}^{2+}\right|\mathrm{Pb}=-0.126{\mathrm{V}}^{ }$. The cell reaction of the cell constructed from these two electrodes is

$$\begin{gathered} {\mathrm{E}}_{\mathrm{Sn}2+/\mathrm{Sn}}^{\mathrm{o}}=-1.14\mathrm{V} \\ {\mathrm{E}}_{\mathrm{Pb}2+/\mathrm{Pb}}^{\mathrm{o}}=-0.126\mathrm{V} \end{gathered}$$

Higher the SRP. metal can oxidize easily and behaves as reducing agent.

$\mathrm{Sn}+{\mathrm{Pb}}^{2+}⟶{\mathrm{Sn}}^{2+}+\mathrm{Pb}$