$K_{f}$ (water) $= 1.86 \ K \ kg \ mol^{-1}$. The temperature at which ice begins to separate from a mixture of $10$ mass $\%$ ethylene glycol is (in $^{\circ} C$)

The freezing point depression constant $(K_{f})$ of benzene is $5.12 \ K \ kg \ mol^{-1}$. The freezing point depression for the solution of molality $0.078 \ m$ containing a non-electrolyte solute in benzene is..........$K$ (rounded off up to two decimal places).

During the freezing of a solution at its freezing point,which of the following equilibria exists?

Given below are two statements $:$
Statement $(I) : NaCl$ is added to the ice at $0^{\circ} C$,present in the ice cream box to lower the freezing point of the mixture,which helps in keeping the ice cream frozen.
Statement $(II) :$ On addition of $NaCl$ to ice at $0^{\circ} C$,there is a depression in freezing point.
In the light of the above statements,choose the correct answer from the options given below $:$

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

Ethylene glycol is used as an anti-freezing agent. Calculate the amount of ethylene glycol to be added to $4 \ kg$ of water to prevent it from freezing at $-6 \ ^{\circ}C$. ($K_f$ for water $= 1.85 \ K \ kg \ mol^{-1}$) (molar mass of $(CH_2OH)_2 = 62 \ g \ mol^{-1}$) .......... $g$.