Question

Under what condition real gases obey ideal gas behavior?

Answer 1

Hint: Real gases are the gases that experience an intermolecular force of attraction between the molecules, whereas, ideal gases are the gases that do not experience any force of attraction between the molecules. However, in reality, ideal gases do not exist.

Complete step by step answer:
Real gases occupy the entire volume available to them, whereas ideal gases do not occupy any volume.
When gas is at a high temperature, the kinetic energy of the molecules increases and they start moving faster. As the molecules move faster, they collide more rapidly with each other and also with the walls of the container. Due to this rapid collision, the molecules move away from each other and overcome their force of attraction, which is a condition of an ideal gas.
Also, when the pressure of a gas is decreased, the volume of the gas increases as pressure and volume are inversely proportional to each other. When the volume of a gas increases, the molecules move far apart from each other and are not held together by the intermolecular force of attraction. As a result, a real gas starts behaving as an ideal gas with no volume and no force of attraction.
Therefore, to conclude, it can be said that real gases obey ideal gas behavior at high temperatures and low pressure.

Note: The equation for an ideal gas is called an ideal gas equation. It can be represented as follows:
$PV = nRT$, Where $P$ are the pressure of the gas, $V$ is the volume of the gas, $n$ is the number of moles of the gas, $R$ is the ideal gas constant, $T$ is the temperature of the gas.