One litre flask contains air, water vapour and a small amount of liquid water at a pressure of 200 mmHg. If this is connected to another one-litre evacuated flask, what will be the final pressure of the gas mixture at equilibrium?Assume the temperature to be 50°C.Aqueous tension at 50°C = 93 mm Hg.

1 mole of N2 and 3 moles of H2 are mixed in 8.21 lit. container at 300 K to form NH3 . If at equilibrium, average molecular mass was found to be 34/3, then find partial pressure of each component.

A vessel of 2 lit. capacity contains hydrogen at 380 mm pressure at 27°C. 16 gm of O2 is added to the container at constant temperature, then find the final total pressure and final partial pressure of H2 . Sol. As partial pressure of a gas is independent from the pressure of other gas, initial as well as final partial pressue of H2 gas,

A mixture of CO and CO2 is found to have a density of 1.50 g/litre at 30oC and 730 mm. The mole percent of CO in the mixture is

The density of methane at 2.0 atmosphere pressure and 27°C is