A sample of an ideal gas occupies `20` L under a pressure of "0.5" atm and under isothermal condition.On increasing its pressure to `1.0` atm. Its volume will be

A sample of gas occupies 10 litre under a pressure of 1 atmosphere. What will be its volume if the pressure is increased to 2 atmosphere? Assume that the temperature of the gas sample does not change

1 mole of a ciatomic gas present in 10 L vessel at certain temperature exert a pressure of 0.96 atm. Under similar conditions an ideal gas exerted 1.0 atm pressure. If volume of gas molecule is negligible, then find the value of van der Waals' constant ''a'' (in atm L^(2)//mol^(2) ).

5 mole of an ideal gas expand isothermally and irreversibly from a pressure of 10 atm to 1 atm against a constant external pressure of 1 atm. w_(irr) at 300 K is :

A sample of gas at 20^(@)C occupies a volume of 2 L at a pressure of 0.867xx10^(5)Pa . Calculate its volume at 100 kPa atmospheric pressure.

How much heat is absorbed and how much work is done in the expansion?2L of an ideal gas at a pressure of 10 atm expansion isothermally into a vacuum until its total volume is 10L.

How many moles of Helium gas occupy 22.4 L at 0^(@)C at 1 atm pressure?