$\mathrm{Sn}(\mathrm{s})+\mathrm{Pb}^{+2}(\mathrm{aq}) \rightarrow \mathrm{Sn}^{+2}(\mathrm{aq})+\mathrm{Pb}(\mathrm{s})\dots (1)$

Apply Nernst equation:

$\mathrm{E}_{\text {cell}}=\mathrm{E}_{\text {cel }}^{0}-\frac{0.06}{2} \log \frac{\left[\mathrm{Sn}^{+2}\right]}{\left[\mathrm{Pb}^{+2}\right]}$

$\mathrm{E}_{\mathrm{cell}}^{0}=-0.13+0.14=0.01 \mathrm{V}$

At equilibrium : $E_{\text {cell}}=0$

Substituting in $( 1)$

$0=0.01-\frac{0.06}{2} \log \frac{\left[\mathrm{Sn}^{+2}\right]}{\left[\mathrm{Pb}^{+2}\right]}$

$\Rightarrow \quad \frac{1}{3}=\log \frac{\left[\mathrm{Sn}^{+2}\right]}{\left[\mathrm{Pb}^{+2}\right]}$

$\Rightarrow\; \frac{\left[\mathrm{Sn}^{+2}\right]}{\left\lceil\mathrm{Pb}^{+2}\right\rceil}=2.15$