States of Matte...

A vessel has $$6 \ g$$ of oxygen at pressure $$P$$ and temperature $$400 \ K$$. A small hole is made in it so that oxygen $$O_2$$ leaks out. How much oxygen leaks out if the final pressure is $$P/2$$ and temperature $$300 \ K$$?

Dalton's law of partial pressure will not apply to which of the following mixture of gases?

Equal mass of $$H_2$$, $$He$$ and $$CH_4$$ are mixed in empty container at $$300$$K, when total pressure is $$2.6$$ atm. The partial pressure of $$H_2$$ in the mixture is:

A gaseous mixture contains $$56\ g\ N_{2}. 44\ g\ CO_{2}$$ and $$16\ g\ CH_{4}$$. The total pressure of the mixture is $$720\ mm\ Hg$$. The partial pressure of $$CH_4$$ in mm Hg is:

The vapour pressure of pure benzene at a certain temperature is $$640\ mm\ Hg$$. A non-volatile solute weighing $$2.175\ g$$ is added to $$39.0\ g$$ of benzene. The vapour pressure of solution is $$600\ mm\ Hg$$. What is the molar mass of the solute?

A solution containing 30 g of non-volatile solute exactly in 90 g of water has a vapour  pressure of 2.8 kPa at 298 K. Further 18 g  of water is then added to the solution and the new vapour pressure becomes 2.9 kPa at 298 k Calculate vapour pressure of water at 298K?

Calculate (in mm) Vapour pressure of liquid mixture obtained by mixing $$936 \, g\ C_6H_6 \, $$ and $$736\ g$$ toluene is:

Pressure of the gas in column (1) is :

Vapour pressure of $$CC{l}_{4}$$ at $$25^{O}C$$ is 143mm Hg. 0.5gm of a non-volatile solute (mol. wt. 65) is dissolved in 100ml of $$CC{l}_{4}$$. Find the vapour pressure of the solution.

A sample of pure $$NO_{2}$$ gas healed lo 1000 K decomposes.

$$NO_{2}(g) \leftrightharpoons 2NO(g) + O_{2}(g)$$

The equillibrium constant $$K_{P}$$ is 100atm. Analysis shows that the partial pressure of $$O_{2}$$ is 0.25 atm at equillibrium. The partial pressure of $$NO_{2}$$ at equillibrium is: