500 ml oxygen at a pressure of 700 mm, 300 ml hydrogen at a pressure of 750 mm and 700 ml of nitrogen at a pressure of 600 mm are enclosed in a vessel of 1 litre capacity at `25^@C`. Calculated the total pressure of the gas mixture.

If a mixture of gas has a total pressure of 100 cm Hg and the partial pressure of nitrogen in the mixture is 25 mm Hg, then the per cent of nitrogen in the mixture is :

Aclosed vessel contains equal number of nitrogen and oxygen molecules at a pressure of P mm. If nitrogen is removed from the system, then the pressure will be :

A vessel has nitrogen gas and water vapours at a total pressure of 1 atm. The partial pressure of water vapours is 0.3 atm. The contents of this vessel are transferred to another vessel havig one third of the capacity of original volume, completely at the same temperature, the total pressure of the system in the new vessel is :

A gas occupies a volume of 400 mL at800 mm pressure and at 27^@C . Calculate the volume occupied by the same gas at 600 mm pressure and at 127^@ C.

In an experiment 300 ml of a gas was collected at 22^@C and 720 mm pressure. What will be the volume of the gas at NTP ?

Define Boyle's law and Charle's law. Define the combined gas equation from the two laws. Temperature remaining constant, 100 mL of oxygen at 100 mm pressure is transferred to a container of 25 mL capacity. What is the pressure of oxygen in the new container.

Air cotains 79 % N_2 and 21% O_2 by volume.If the barometric pressure is 750 mm Hg the partial pressure of oxygen is :

2.5 g of pure calcium carbonate, when strongly heated left a residue of 1.400 g. The evolved gas was found to occupy 624 mL at 27^@ C and 755 mm pressure. Calculate the molecular weight of the gas.

200 Ml of a gas had a temperature 27^@ C and pressure 750 mm. Find the pressure at which the gas will have a volume 175mL if the temperature is 77^@ C .

Calculate the volume of 4 gm molecule of hydrogen at 27^@C and 750 mm pressure.