The vapour pressure of 2-propanol is 50.00 kPa at 338.8 °C, but it fell to 49.62 kPa when 8.69 g of a non-volatile organic compound was dissolved in 250 g of 2-propanol. Calculate the molar mass of the compound.

Calculate the vapour pressure of water at 75 °C. Take the enthalpy of vaporization of water as 40.66 kJ/mol and its boiling point as 100 °C. Calculate the change in chemical potential for a substance X with a molar mass of 100 g/mol, a density of 2 g/cm, when the pressure on it is increased by 10 bar at its melting point temperature of 25 °C.

. The vapor pressure of benzene is 10 kPa while methylbenzene is 2.8 kPa. Determine the total pressure of an equimolar solution.

A certain dilute solution has an osmotic pressure of 11.1 atm at 25°C. Calculate the difference between the chemical potential of the solvent in the solution and that of pure water. Assume that the density is the same as that of water at 25°C, 0.99705 g-cm-3. (Hint: Express the chemical potential in terms of mole fraction, x1, and rewrite the osmotic pressure equation as OV = n2RT, where n2 is the number of moles of the solute and V = 1.00 L.)