At `27^(@)C` a sample of ammonia gas exerts a pressure of 5.3 atm. What is the pressure when the volume of the gas is reduced to one-tenth of the original value at the same temperature ?

A vessel has nitrogen gas and water vapour in equilibrium with liquid water at a total pressure of 1 atm. The partial pressure of water vapours is 0.3 atm. The volume of this vessel is reduced to one third of the original volume, at the same temperature, then total pressure of the system is: (Neglect volume occupied by liquid water)

If the pressure of 2 litres of an ideal gas is 4 atm then what will be the pressure of the gas if the volume is reduced to one- fourth of its present value?

The pressure of a gas of volume 22.4 l is 3 atm at certain temperature. Then find the pressure of the gas of volume 44.8 l at the same temperature.

A gas occupies a volume of 250 ml at 700 mm Hg pressure and 25^(@)C . What additional pressure is required to reduces the gas volume to its 4//5 th value at the same temperature ?

A gas occupied a volume of 50 ml at 700 mm Hg pressure atn 250^(@)C . What additional pressure is required to reduce the gas volume to its 4/5 th value at the same temperature?

A sample of an ideal gas has a volume of 0.5 litres at 27^@C and 750mm pressure. The number of moles of gas are