To observe an elevation of boiling point of $0.05^{\circ} C$, the amount of a solute (mol. wt. $= 100$) to be added to $100 \ g$ of water $(K_{b} = 0.5)$ is (in $g$)

$x \ g$ of urea (molar mass $60 \ g \ mol^{-1}$) is completely dissolved in $y \ g$ of pure water and the solution boiled at $373.202 \ K$. If the boiling point of pure water at $1.013 \ bar$ is $373.15 \ K$, then $x:y$ is $(K_b(H_2O) = 0.52 \ K \ kg \ mol^{-1})$

$18 \, g$ of glucose $(C_{6}H_{12}O_{6})$ dissolved in $1 \, kg$ of water is heated to boiling. The boiling point (in $K$) measured at $1 \, atm$ pressure is closest to: [Ebullioscopic constant,$K_{b}$ for water is $0.52 \, K \, kg \, mol^{-1}$. Consider the boiling point of pure water to be $373.15 \, K$]

Calculate the amount of solute dissolved in $160 \ g$ of solvent that boils at $85^{\circ}C$. The molar mass of the solute is $120 \ g \ mol^{-1}$. $(K_{b}$ for solvent $= 2.7^{\circ}C \ kg \ mol^{-1}$ and boiling point of pure solvent $= 76^{\circ}C)$ (in $g$)

$A$ solution of $1$ molal concentration of a solute will have maximum boiling point elevation when the solvent is

When a substance is dissolved in a solvent,the vapour pressure of the solvent decreases. It brings: