Question

Benzene (C6H6) and toluene (C6H5CH3) form an ideal solution. At 313K, the vapour pressures of pure benzene and toluene are 160 mm Hg and 60 mm Hg respectively. Calculate the partial pressures of benzene and toluene, and the total pressure of the solution when

Methanol and ethanol form a nearly ideal solution at 300K. A solution is made by mixing 32 g of methanol and 23 g of ethanol at 300 K. Calculate the partial pressures of constituents and the total pressure of the solution. (At 300K, P°CH3OH = 90 mm Hg, P°C2H5OH = 51 mm Hg)

At 25°C, the vapour pressure of water is 22.75 mm Hg. Calculate the vapour pressure at the same temperature of 5% aqueous solution of urea (NH2CONH2).

Solutions of two volatile liquids A and B obey Raoult's law. At a certain temperature, it is found that when the total pressure above a given solution is 400 mm Hg, the mole fraction of A in the vapour is 0.45 and in the liquid is 0.65. What are the vapour pressures of the two liquids in the pure state at the given temperature?