States of Matte...

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?

A mixture (by weight) of hydrogen and helium is enclosed in a two-litre flask at $$27^o C$$. Assuming ideal kept behaviour, the partial pressure of helium is found to be 0.2atm. Then the concentration of hydrogen would be:

If $$0.2\ mol$$ of $$H_{2}(g)$$ and $$2\ mol$$ of $$S(s)$$ are mixed in a $$1\ dm^{3}$$ vessel at $$90^{\circ}C$$, the partial pressure of $$H_{2}S(g)$$ formed according to the reaction, $$H_{2}(g) + S(s)\rightleftharpoons H_{2}S, K_{P} = 6.8\times 10^{-2}$$ would be:

Two moles of pure liquid 'A' $$(P_{A}^{0} =80mm$$ of Hg) and $$3$$ moles of pure liquid 'B' ($$P_{B}^{0} = 120mm$$ of Hg) are mixed. Assuming ideal behaviour?

The virial equation for 1 mole of a real gas is written as:
PV=RT

Vapour pressure of $$CCl_4$$ at $$25^0$$C is $$143$$mm Hg. $$0.5$$ gm of a non-volatile solute (mol.wt.$$65$$) is dissolved in $$100$$ ml of $$CCl_4$$. Find the vapour pressure of the solution. (Density of CCl_4 = $$1.58 gm/cm^3$$)

Which of the following relationships between partial pressure, volume and temperature is correct?
(i) $$P = \dfrac {nRT}{V}$$
(ii) $$P_{total} = p_{1} + p_{2} + p_{3}$$
(iii) $$P_{total} = (n_{1} + n_{2} + n_{3}) \dfrac {RT}{V}$$.

A rigid and insulated tank of 3 $$m^3$$ volume is divided into two components. One compartment of volume of 2 $$m^3$$ contains an ideal gas at 0.8314 MPa and 400 K and while the second compartment of volume 1 $$m^3$$ contains the same gas 8.314 MPa and 500 k. If the partition between the two compartments is ruptured, the final temperature of the gas is:

The pressure of a mixture of equal weights of two gases $$X$$ and $$Y$$ with molecular weight $$4$$ and $$40$$ respectively is $$1.1\ atm$$. The partial pressure of the gas $$X$$ in the mixture is :

An open flask contains air at $$27^{\circ}C$$. At what temperature should it be heated so that $$1/3rd$$ of air present in it goes out?