States of Matte...

$$P_A \, = \, X_AP_A$$ and $$P_B \, = \, X_BP_B$$
$$P_T \, = \, X_AP_A \, + \, X_BP_B$$
Vapour pressure of mixtures of Benzene $$(C_6H_6)$$ and toluene $$(C_7H_8)$$ at $$50^{\circ}C$$ are given by $$P_M \, = \, 179X_B \, + \, 92$$ where $$X_B$$ is mole fraction of $$C_6H_6$$.
What is the vapour pressure of pure liquids?

If $${ PCl }_{ 5 }$$ is 80% dissociated at $$250$$ then its vapour density at room temperature will be:

The vapour pressure of two pure liquids $$A$$ and $$B$$, that form an ideal solution are $$100$$ and $$900$$ torr respectively at temperature $$T$$. This liquid solution of $$A$$ and $$B$$ is composed of $$1\ mole$$ of $$A$$ and $$1\ mole$$ of $$B$$. What will be the pressure, when $$1$$ mole of mixture has been vapourized?

Two containers, X and Y at 300K and 350K with water vapour pressures 22 mm and 40 mm respectively a are connected, initially closed with a valve. If the valves opened.

The vapour pressure of two pure liquids A and B which form an ideal solution are 1000 and 1600 torr respectively at 400 K. A liquid solution of A and B for which the mole fraction of A is 0.60 is contained in a cylinder by a piston on which the pressure can be varied. The solution use slowly vapourised at 400 K by decreasing the applied pressure. What is the composition of last droplet of liquid remaining in equilibrium with vapour?

Which of the following is a correct graph?

Two glass bulbs $$A$$ (of $$100\ mL$$ capacity), and $$B$$ (of $$150\ mL$$ capacity) containing same gas are connected by a small tube of negligible volume. At particular temperature, the pressure in $$A$$ was found to be $$20$$ times more than that in bulb $$B$$. The stopcock is opened without changing the temperature. The pressure in $$A$$ will :

Two liquids $$X$$ and $$Y$$ are perfectly immiscible. If $$X$$ and $$Y$$ have molecular masses in ration $$1 : 2$$, the total vapour pressure of a mixture of $$X$$ and $$Y$$ prepared in weight ratio $$2 : 3$$ should be:$$(P_{X}^{0} = 400\ torr, P_{Y}^{0} = 200\ torr)$$.

A nitrogen-hydrogen mixture initially in the molar ratio 1:3 reached equilibrium to form ammonia when 25% of the $$H_{2}$$ and $$N_{2}$$ had reacted. If the total pressure of the system was 21 atm, the partial pressure of ammonia at the equilibrium was: 

Two liquids X and Y are perfectly immiscible. If X and Y have molecular masses in ratio 1 : 2, the total vapour pressure of a mixture of X and Y prepared in weight ratio 2 : 3 should be ($$Px^0 = 400 torr, Py^0 = 200 torr$$)