The molal depression constant for a liquid is $2.77^{\circ} C \ kg \ mol^{-1}$. What is its value on the Kelvin scale?

During the depression of freezing point in a solution,which of the following are in equilibrium?

Calculate the molal depression constant of a solvent, which freezes at $15^{\circ}C$. The latent heat of fusion is $180.7 \ Jg^{-1}$.

Calculate $\Delta T_f$ of $0.15 \ m$ solution of nonvolatile solute $\left[K_f = 1.5 \ K \ kg \ mol^{-1}\right]$ (in $K$)

$1.80 \ g$ of solute $A$ was dissolved in $62.5 \ cm^{3}$ of ethanol and the freezing point of the solution was found to be $155.1 \ K$. The molar mass of solute $A$ is $.......... \ g \ mol^{-1}$.
[Given: Freezing point of ethanol is $156.0 \ K$,Density of ethanol is $0.80 \ g \ cm^{-3}$,Freezing point depression constant of ethanol is $2.00 \ K \ kg \ mol^{-1}$]

In cold countries,ethylene glycol is added to water in the radiators to: