two pure liquids A and B have vapour pressures in the ratio 1:3. The mole fraction of A in vapour phase, when A and B are mixed in 1:3 molar ratio in a solution will be: a-0.1 b-0.2 c-0.3 d-0.5

Q. Two liquids A and B are mixed in 1 : 4 mole ratio to from an ideal solution. If they exert vapour pressures of 75 mmHg and 22 mmHg respectively, the mole fraction of liquid of A in the vapour phase would be

Q. Two liquids A and B have vapour pressure in the ratio $P_A^0:P_B^0=1:3$ at a certain temperature.Assume A and B form an ideal solution and the ratio of the 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 temperature is :

Q. The vapour pressures of two liquids A and B in their pure states are in the ratio of 1 : 2. A binary solution of A and B contains A and B in the mole proportion of 1 : 2. The mole fraction of A in the vapour phase of the solution will be:

Q. Two liquids $\text{A}$ and $\text{B}$ have ${P^{\circ }}_A:{P^{\circ }}_B=1:3$ at a certain temperature. If the mole fraction ratio of $x_A:x_B=1:3$, the mole fraction of $\text{A}$ in vapour in equilibrium with the solution at a given temperature is

Q. Two liquids 'A' and 'B' have vapour pressure (in pure state) in the ratio $p_A^{\circ }:p_B^{\circ }=1:3$ at a certain temperature. Assume 'A' and 'B' form an ideal solution and the ratio of mole fractions of 'A' to 'B' in the vapour phase is 4 : 3. The the mole fraction of 'B' in the solution at the same temperature is: