What is the value of $K_{f}$ if $30 \ g$ urea (molar mass $60$) dissolved in $0.5 \ dm^{3}$ of water decreases the freezing point by $0.15^{\circ}C$?

Identify the correct relation between depression in freezing point and the freezing point of a pure solvent.

The addition of $0.643 \,g$ of a compound to $50 \,mL$ of benzene (density $= 0.879 \,g \,mL^{-1}$) lowers the freezing point from $5.51^{\circ}C$ to $5.03^{\circ}C$. If the freezing point constant,$K_f$ for benzene is $5.12 \,K \,kg \,mol^{-1}$,the molar mass of the compound is approximately $..... \,g \,mol^{-1}$.

The solution containing $6 \ g$ urea (molar mass $60$) per $dm^3$ of water and another solution containing $9 \ g$ of solute $A$ per $dm^3$ water freeze at the same temperature. What is the molar mass of $A$?

Ethylene glycol is used as an antifreeze in cold climates. The mass of ethylene glycol $(C_2H_6O_2)$ that should be added to $4 \ kg$ of water to prevent it from freezing at $-6 \ ^oC$ is ......... $g$.
($K_f$ for water $= 1.86 \ K \ kg \ mol^{-1}$,and molar mass of ethylene glycol $= 62 \ g \ mol^{-1}$)

Which of the following solutions has the maximum freezing point?