A thermally insulted vessel contains $150\, g$ of water at $0\,^oC$. Then the air from the vessel is pumped out a adiabatically. A fraction of water turns into ice and the rest evaporates at $0\,^oC$ itself. The mass of evaporated water will be closes to ....... $g$ (Latent heat of vaporization of water $= 2.10 \times10^6\, Jkg^{-1}$ and Laten heat of Fusion of water $ = 3.36 \times10^5\,Jkg^{-1}$ )
$35$
$150$
$130$
$20$
The point on the pressure temperature phase diagram where all the phases co-exist is called
Match the following according to conversion by heat :
Column $-I$ | Column $-II$ |
$(a)$ Required heat to convert solid into gaseous. | $(i)$ Latent heat of fusion |
$(b)$ Required heat to convert solid into liquid. | $(ii)$ Latent heat of vaporization. |
What is the effect of pressures on boiling point of water ?
Two different liquids of same mass are kept in two identical vessels, which are placed in a freezer that extracts heat from them at the same rate causing each liquid to transform into a solid. The schematic figure below shows the temperature $T$ versus time $t$ plot for the two materials. We denote the specific heat in the liquid states to be $C_{L 1}$ and $C_{L 2}$ for materials 1 and 2, respectively and latent heats of fusion $U_1$ and $U_2$, respectively. Choose the correct option.
The variation of density of water with temperature is represented by the