When $0.01 \ mol$ of nonvolatile solute is dissolved in a certain solvent,calculate the mass of the solvent in $kg$ if $\Delta T_{b} = 0.6 \ K$ and $K_{b}$ for the solvent $= 2 \ K \ kg \ mol^{-1}$. (in $kg$)

$A$ solution of $6 \ g$ of solute in $100 \ g$ of water boils at $100.52^{\circ} C$. The molal elevation constant of water is $0.52 \ K \ kg \ mol^{-1}$. What is the molar mass of the solute?

When $3.3 \ g$ of an unknown substance is dissolved in $125 \ g$ of benzene (boiling point $80^\circ \text{C}$),the boiling point of the resulting solution is $80.66^\circ \text{C}$. What is the molar mass of the unknown substance? $(K_b = 3.28 \ \text{K kg mol}^{-1})$

$A$ solution of non-volatile solute has boiling point elevation $0.5 \ K$. Calculate molality of solution $[K_{b} = 2.40 \ K \ kg \ mol^{-1}]$.

The normal boiling point of ethyl acetate is $77^{\circ}\text{C}$. $A$ solution of a non-volatile, non-electrolyte solute in ethyl acetate boils at $78^{\circ}\text{C}$. The $K_b$ for ethyl acetate is $2.77^{\circ}\text{C kg mol}^{-1}$. What is the molality of the solution (in $\text{ m}$)?

When a substance is dissolved in a solvent,the vapour pressure of the solvent is decreased. This results in: