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 $= 0.52 \ K \ kg \ mol^{-1}$)

Calculate $\Delta T_b$ of a $0.45 \text{ m}$ solution of a nonvolatile solute in a solvent if the molal elevation constant of the solvent is $3.0 \text{ K kg mol}^{-1}$. (in $\text{ K}$)

If $0.15 \ g$ of a solute dissolved in $15 \ g$ of solvent is boiled at a temperature higher by $0.216 \ ^oC$ than that of the pure solvent,what is the molecular weight of the substance? (Given: molal elevation constant for the solvent is $2.16 \ ^oC \ kg \ mol^{-1}$)

When $0.5143 \ g$ of anthracene is dissolved in $35 \ g$ of $CHCl_3$,the boiling point of $CHCl_3$ increases by $0.323 \ K$. Calculate the molar mass of anthracene. ($K_b$ for $CHCl_3 = 3.9 \ K \ kg \ mol^{-1}$)

When a substance is dissolved in a solvent,the vapour pressure of the solvent decreases. It brings:

Calculate the molar mass of a nonvolatile solute if a solution containing $0.35 \ g$ of solute in $100 \ g$ of water has a boiling point elevation of $0.01 \ K$ $\left[K_{b}=0.50 \ K \ kg \ mol^{-1}\right]$.