$1 \mathrm{gm}$ of water at ${100}^{o}C$ is completely converted into steam at ${100}^{o}C$ . $1 \mathrm{gm}$ steam occupies a volume of $1650 \mathrm{cc}$. (Neglect the volume of $1 \mathrm{gm}$ of water at ${100}^{o}C$). At the pressure of ${10}^5$$\raisebox{1ex}{$\mathrm{N}$}\!\left/ \!\raisebox{-1ex}{${\mathrm{m}}^2$}\right.$, latent heat of steam is $540 \raisebox{1ex}{$\mathrm{cal}$}\!\left/ \!\raisebox{-1ex}{$\mathrm{gm}$}\right.$ $\left(1 \mathrm{calorie}=4.2 \mathrm{Joule}\right)$. The increase in the internal energy in Joules is