If an aqueous solution of glucose is allowed to freeze,then crystals of which substance will be separated out first?

....... $g$ will be the amount of ice separated on cooling a solution of $40 \ g$ ethylene glycol in $400 \ g$ water up to $-9.3 \ ^oC$. ($K_f$ for water is $1.86 \ K \ kg \ mol^{-1}$)

$1.8 \ g$ of glucose (molar mass $180 \ g \ mol^{-1}$) is dissolved in $0.1 \ kg$ of water. The freezing point of the solution (in $^{\circ}C$) is ($K_f$ for water $= 1.86 \ K \ kg \ mol^{-1}$)

The freezing point of a $0.05 \ molal$ solution of a non-electrolyte in water is $(K_f = 1.86 \ K \ kg \ mol^{-1})$:

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

When a solute is dissolved in a solvent,the freezing point decreases by $0.184 \ ^oC$. What will be the molality of the solution? (Given $K_f = 18.4 \ K \ kg \ mol^{-1}$)