Which of the following graphs correctly represents the changes in thermodynamic properties during the formation of $1 \, mol$ of an ideal binary solution?

If ethanol dissolves in water,then which of the following would be done?

Match the following.

List-$I$	List-$II$
$(A)$ Azeotrope	$(I)$ $\Delta T_b = i K_b m$
$(B)$ Henry's law	$(II)$ $p = K_H x$
$(C)$ Cryoscopic constant	$(III)$ $\Delta T_f / m$
$(D)$ Van't Hoff factor	$(IV)$ Deviation from Raoult's law
	$(V)$ $\pi = CRT$

The correct answer is

When a solute is added to a solvent,the freezing point of the solution decreases to $1.86 \ K$. What is the value of $\Delta T_b$? $[K_f = 1.86, K_b = 0.512]$

$A$ cylinder containing an ideal gas ($0.1 \; mol$ in $1.0 \; dm^{3}$) is in thermal equilibrium with a large volume of $0.5 \; m$ (molal) aqueous solution of ethylene glycol at its freezing point. If the stoppers $S_{1}$ and $S_{2}$ (as shown in the figure) are suddenly withdrawn,the volume of the gas in litres after equilibrium is achieved will be ............ $litre$.
(Given: $K_{f}$ (water) $= 2.0 \; K \; kg \; mol^{-1}$,$R = 0.08 \; dm^{3} \; atm \; K^{-1} \; mol^{-1}$,freezing point of water $= 273 \; K$)

Statement $1$: The cold pack used by athletes to treat injuries on the field works by dissolving a solute in water,which causes the temperature to decrease. Statement $2$: Adding a non-volatile solute to a solvent decreases its freezing point.