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.

Two liquid A and B have vapour pressure in the ratio P_A^(@) : P_B^(@) =1.3 at a certain temperature.Assume A and B from an ideal solution and the ratio of mole fractions of A to B in the vapour phase is 4 : 3, then the mole fraction of B in the solution at the same tempreature is :

P_A and P_B are the vapour pressure of pure liquid components A and B respectively of an ideal binary solution. If X_A represent the mole fraction of component A, then the total pressure of the solution will be

Two solutions A and B have pH of 6 and 9 respectively. Which solution will be basic in nature?

The temperature at which the vapour pressure of a liquid becomes equal to external pressure is

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.

The liquids X and Y from ideal solution having vapour pressures 200 and 100mm Hg respectively. Calculate the mole fraction of component X in vapour phase in equilibrium with an equimolar solution of the two.

The vapour pressure of pure liquid A at 310^@C is 0.158bar. The vapour pressure of this liquid in solution with liquid B is 0.095 bar. Calculate the mole fraction of A in the solution if the mixture obeys Raoult's law.

The vapour presure of a pure liquid 'A' is 70 torr at 27^@C . It forms an ideal solutons with another liquid B. the mole fraction of B in the solutin is 0.2 and total pressure of solution is 84 torr at 27^@C . The vapour pressure of pure liquid is B at 27^@C :

Two metals A and B have reduction potentials values -0.76V and +0.34V respectively. Which of these will liberate H_2 from dil H_2SO_4 ?