For an electrochemical cell, $\mathrm{Sn}(\mathrm{s})\left|\mathrm{Sn}^{2+}(\mathrm{aq}, 1 \mathrm{M}) \| \mathrm{Pb}^{2+}(\mathrm{aq}, 1 \mathrm{M})\right| \mathrm{Pb}(\mathrm{s})$ the ratio $\frac{\left[\mathrm{Sn}^{2+}\right]}{\left[\mathrm{Pb}^{2+}\right]}$ when this cell attains equilibrium is $\_\_\_\_$ .
(Given:
$
\begin{aligned}
& \mathrm{n}: \mathrm{E}_{\mathrm{Sn}^{2+} \mid \mathrm{Sn}}^0=-0.14 \mathrm{~V} \\
& \left.\mathrm{E}_{\mathrm{Pb}^{2+}+\mathrm{Pb}}^0=-0.13 \mathrm{~V} \cdot \frac{2.303 \mathrm{RT}}{\mathrm{~F}}=0.06\right)
\end{aligned}
$
