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

In countries nearer to the polar region,the roads are sprinkled with $CaCl_{2}$. This is

The freezing point depression of $645 \ g$ of an aqueous solution of ethylene glycol $(C_2H_6O_2)$ is $2.25 \ K$. Find the weight of ethylene glycol in the solution. $[K_f = 1.86 \ K \ kg \ mol^{-1} ; H = 1, C = 12, O = 16 \ amu]$ (in $g$)

The freezing point of a $1\%$ aqueous solution of calcium nitrate will be:

Elements $X$ and $Y$ form two non-volatile compounds ($XY$ and $XY_3$). When $10 \ g$ of $XY$ is dissolved in $50 \ g$ of ethanol,the depression in freezing point $(\Delta T_{f})$ is $5.333 \ K$. When $10 \ g$ of $XY_3$ is dissolved in $50 \ g$ of ethanol,the $\Delta T_{f}$ is $2.2857 \ K$. What are the atomic weights of $X$ and $Y$ respectively? $(K_{f} = 2 \ K \ kg \ mol^{-1})$

If the $K_f$ value of $H_2O$ is $1.86$,what is the value of $\Delta T_f$ for a $0.1 \ m$ solution of a non-volatile solute?