Question #44224

Calculate the boiling point elevation ($\Delta T_b$) of a $2.00\text{ molal}$ aqueous solution of a non-volatile, non-electrolyte solute.

Given data: Standard enthalpy of vaporization of water at $298\text{ K}$, $\Delta H_{vap}^\circ(298\text{ K}) = 44.0\text{ kJ mol}^{-1}$ Molar heat capacities at constant pressure: $C_{p,m}(\ce{H2O}, l) = 75.0\text{ J K}^{-1}\text{mol}^{-1}$, $C_{p,m}(\ce{H2O}, g) = 35.0\text{ J K}^{-1}\text{mol}^{-1}$ Boiling point of pure water, $T_b^\circ = 373\text{ K}$ Universal gas constant, $R = 8.314\text{ J K}^{-1}\text{mol}^{-1}$ Molar mass of water, $M = 18.0\text{ g mol}^{-1}$

Assume $C_{p,m}$ values are independent of temperature.