$2.5 \mathrm{~g}$ of a non-volatile, non-electrolyte is dissolved in $100 \mathrm{~g}$ of water at $25^{\circ} \mathrm{C}$. The solution showed a boiling point elevation by $2^{\circ} \mathrm{C}$. Assuming the solute concentration is negligible with respect to the solvent concentration, the vapor pressure of the resulting aqueous solution is $\underline{\hspace{2cm}}\mathrm{mm}$ of $\mathrm{Hg}$(nearest integer) [Given : Molal boiling point elevation constant of water $\left(\mathrm{K}_{\mathrm{b}}\right)=0.52 \mathrm{~K} . \mathrm{kg} \mathrm{mol}^{-1}$, $1 \mathrm{~atm}$ pressure $=760 \mathrm{~mm}$ of $\mathrm{Hg}$, molar mass of water $=18 \mathrm{~g} \mathrm{~mol}^{-1}]$