ideal gas law

Up to what pressure a gas will follow the ideal gas law depends upon the nature of the gas and its temperature . The temperature at which a real gas obeys the ideal gas law over an appreciable range of pressure is called

One mole of nitrogen is contained in a vessel of volume V = 1.00 1 . Find : (a) the temperature of the nitrogen at which the pressure can be calculated from an ideal gas law with an error eta = 10 % (as compared with the pressure calculated from the Van der Walls equation of state) , (b) the gas pressure at this temperature.

We have 0.5 g of hydrogen gas in a cubic chamber of size 3 cm kept at NTP. The gas in the chamber is compressed keeping the temperature constant till a final pressure of 100 atm. Is one justified in assuming the ideal gas law in the final state ? (Hydrogen molecules can be consider as spheres of radius 1Å ).

A 0.109 g sample of a pure gaseous compound occupies 112 mL at 100^(@) C and 750 torr. What is the molecular mass of the compound ? Strategy : We first use the ideal gas law , pV = nRT , to find the number of moles of the gas . Then knowing the mass of that number of moles of the gas , we calculate the molar mass which is numerically equal to the molecular mass . Alternatively , we use Eq.(5.21) directly to get the molar mass.

An ideal gas has adiabatic exponenty. It expands according to the law P = alpha V, where is alpha constant. For this process, the Bulk modulus of the gas is

The law describing realtionship between P and V of ideal gas at constant temperature is called..........

Which law states that the volume of an ideal gas at constant pressure is directly proportional to the absolute temperature?

One mole of an ideal gas at temperature T_(1) expends according to the law (P)/(V^(2))=a (constant). The work done by the gas till tempereature of gas becomes T_(2) is