Question

For a gas deviation from ideal behaviour is maximum at:
(A) 0$^0C$ and 1.0 atm
(B) 100$^0C$ and 2.0 atm
(C) -13$^0C$ and 1.0 atm
(D) -13$^0C$ and 2.0 atm

Answer 1

Hint : An ideal gas is a theoretical gas made up of a large number of randomly moving point particles with no interparticle interactions. Because it obeys the ideal gas law, a simplified equation of state, and is susceptible to statistical mechanics analysis, the ideal gas notion is helpful. If the interaction is fully elastic or viewed as point-like collisions, the criterion of zero interaction can frequently be waived.

Complete Step By Step Answer:
We suppose that individual gas molecules take up very little space in comparison to the entire volume of the gas and that there is no attraction between them. Ideal gases are gases whose behaviour is consistent with these assumptions under all situations. In practise, however, none of these assumptions holds true under all circumstances. The fact that gases may be liquefied, for example, demonstrates the existence of an attraction force between molecules. Under some situations, actual gases tend to approach ideal behaviour. As a result, it is obvious that actual gases behave like ideal gases at low pressure and high temperature.
At low temperatures and high pressures, a gas acts like an ideal gas.
When we compare the two alternatives, we can see that option B is the better ideal gas since it has a low temperature and a high pressure.
As a result, option D differs from ideal gas behaviour.

Note :
When intermolecular interactions and molecular size become relevant at lower temperatures or greater pressures, the ideal gas model tends to collapse. Most heavy gases, such as many refrigerants, and gases with high intermolecular interactions, such as water vapour, also fail. The volume of a real gas is typically much bigger than that of an ideal gas at high pressures.