For a $1 \ m$ (molal) aqueous solution of glucose,which of the following is correct?

What is the boiling point of a $0.5 \ m$ aqueous solution of sucrose if a $0.1 \ m$ aqueous solution of glucose boils at $100.16^{\circ} C$ (in $^{\circ} C$)?

Calculate the molar mass of a non-volatile solute when $5 \ g$ of it is dissolved in $50 \ g$ of solvent,which boils at $119.6^{\circ} C$. $[K_{b} = 3.2 \ K \ kg \ mol^{-1}$,boiling point of pure solvent $= 118^{\circ} C]$.

Two different solutions were prepared by dissolving sucrose in water having concentrations of $1 \ m$ and $2 \ m$ respectively. The value of $(T_2 - T_1)$ will be ........... $K$. (Given: $K_b$ for water $= 0.52 \ K \ kg \ mol^{-1}$)

The boiling point of $0.2 \ m$ aqueous urea solution is $....... \ ^oC$. ($K_b$ of water $= 0.52 \ K \ kg \ mol^{-1}$)

The molal elevation boiling point constant for water is $0.513 \ ^{\circ}C \ kg \ mol^{-1}$. Calculate the boiling point of the solution if $0.1 \ mol$ of sugar is dissolved in $200 \ g$ of water. (in $^{\circ}C$)