Question

A gas that follows Boyle's law, Charles law and Avogadro's law is called an ideal gas. Under what conditions a real gas would behave ideally?
(A) High pressure and low temperature
(B) Low pressure and high temperature
(C) Low pressure and low temperature
(D) High pressure and high temperature

Answer 1

Hint :Real gases are those gases that do not behave ideally like an ideal gas. The intermolecular force of interaction between the particles is the reason that these gases do not behave like the ideal gas. Real gases are also called non-ideal gases.

Complete Step By Step Answer:
In ideal gases the collision is intermolecular. The molecules are perfectly elastic and also there is no intermolecular force of attraction between them. An ideal gas is represented by four variables $ P,{ }V\,and\,T $ as well as $ n $ constant. Here $ P $ represents pressure, $ V $ volume, $ T $ temperature as well as $ n $ the number of moles. The equation represented with these variables is given by:
 $ PV = nRT $
In Ideal gas, the gas molecules are allowed to move uniformly in all directions, and the collision between them is said to be perfectly elastic which means there is no loss in the kinetic energy of the molecule. It always remains conserved.
Compressibility, van der waal force of attraction, specific heat capacities. These are some of the factors that are kept in mind while dealing with real gas.
At high temperature and low pressure, the real gases behave like ideal gases because two postulates of the kinetic theory of gases are true under these conditions. These are
The volume of a molecule of a gas is negligible with respect to the total volume.
The force of attraction between the molecules of gas is negligible.
Hence, Option (A) is correct.

Note :
The PV-graph of real gases shows a deviation from the behavior of real gases. This deviation is of two types- positive deviation and negative deviation At high temperature and low pressure, real gases show ideal behavior.