The relative lowering of vapour pressure produced by dissolving $18 \text{ g}$ of urea (molar mass = $60 \text{ g mol}^{-1}$) in $100 \text{ g}$ of water is

The vapour pressures of pure liquids $A$ and $B$ are $400$ and $600\, mm\, Hg$,respectively at $298\, K$. On mixing the two liquids,the sum of their initial volumes is equal to the volume of the final mixture. The mole fraction of liquid $B$ is $0.5$ in the mixture. The vapour pressure of the final solution,the mole fractions of components $A$ and $B$ in vapour phase,respectively are

The following graph is obtained for an ideal solution containing a non-volatile solute. The $x$- and $y$-axes represent,respectively:

What is the relationship between vapor pressure and temperature? What will be the vapor pressure at $373 \, K$?

The vapor pressure of a pure liquid solvent $(X)$ decreases from $0.80 \ atm$ to $0.60 \ atm$ upon the addition of a non-volatile solute $(Y)$. What is the mole fraction of $(Y)$ in the solution?

Vapour pressure of a solution containing $18 \ g$ of glucose and $178.2 \ g$ of water at $100^{\circ} C$ is (Vapour pressure of pure water at $100^{\circ} C = 760 \ torr$) (in $torr$)