You must first understand what happens when water is heated along the boiling curve.
Start from the point $\pu{100°C}$and $\pu{1 atm}$. At this point there are two phases, one liquid whose density is nearly $\pu{1 g/cm^3}$ and exactly $\pu{0.96 g/cm3}$. And the vapor has a density of $\ce{0.0006 g/cm^3}$. If now you heat this system in a closed volume, the temperature and the pressure will increase like in a steamer. But the densities of the two phases vary in opposite directions. The liquid expands, and the vapor contracts.
At $\pu{180°C}$ , the liquid has a density of $\pu{0.87 g/cm3}$ and the vapor $\pu{0.0079 g/cm3}$
At $\pu{312°C}$, the liquid has a density of $\pu{0.71 g/cm3}$ and the vapor $\pu{0.046 g/cm3}$
At $\pu{374.8°C}$, both the liquid and the vapor have a density of $\pu{0.32 g/cm3}$
If you look at the surface of the liquid just before $\pu{374.8°C}$, the surface of the liquid gets less and less visible. It is transformed into a sort of haze, and slowly disappears. Of course the pressure is extremely high ($\ce{217 atm}$) and the curve pressure vs temperature stops at $\pu{374.8°C}$.