Heptane and octane form an ideal solution at 373 K, the vapour pressures of the pure liquids at this temperature are 105.2 kPa and 46.8 kPa respectively. If the solution contains 25 g of heptane and 28.5 g of octane, calculate. mole fraction of octane in the vapour phase.

Heptane and octane form ideal solution . At 373K , the vapour pressure of the two liquid components are 105.2k Pa and 46.8k Pa respectively. What will be th vapour pressure of a mixture of 26.0g of heptane and 35.0g of octane?

The vapour pressure of two pure liquids A and B are 5 and 10 torr respectively. Calculate the total pressure of the solution (in torr) obtained by mixing 2 mole of A and 3 mole of B.

Benzene and toluene form nearly ideal solution . At 313 K the vapour pressure of benzene and toluene are 160 mm and 60 mm of Hg respectively. Calculate the total pressure of the solution made by mixing their equal masses at 313 K.

Benzene and toluene form nearly ideal solution. At a certain temperature the vapour pressure of pure benzene and toluene are 150 and 50 torr. respectively. Calculate the vapour pressure of solution containing equal weights of benzene and toluene at this temperature .

Two liquids A and B have vapour pressure of 0.658 bar and 0.264 bar respectively. In an ideal solution of the two, calculate the mole fraction of A at which the two liquids have equal partial pressures.

The vapour pressure of two pure liquids A and B are 50 and 40 torr respectively. If 8 molrs of A is mixed with x moles of B , then vapour pressure of solution obtained is 48 torr. What is the value of x.

The vapour pressure of ethanol and methanol are 44.5 and 88.7 mm of Hg at 298 K. An ideal solution is formed at the same temperature by mixing 60 g of ethanol and 40 g methanol. Calculate the total vapour pressure of the solution and the mole fraction of methanol in the vapour phase.