Question

Write differences between real gas and ideal gas.

Answer 1

Hint: Real gas is the different gases around us. Ideal gas is an imaginary concept developed to enhance our thinking on how gases behave. In reality, no gas is ideal.

Complete step by step answer:
Ideal gas: Ideal gas can be defined as a gas that obeys all gas laws at all conditions of pressure and temperature. Ideal gases do not condense. They also do not have a triple point. Ideal gases have mass and velocity.
Real gas: Real gases are defined as the gases that do not obey gas laws at all standard pressure and temperature. Real gases condense when cooled to their boiling point. They have velocity, mass and volume.
To understand the difference between ideal gas and real gas more precisely, the points of difference can be jot down in a tabular form.

Ideal gas	Real gas
Ideal gas obeys all gas laws under all conditions of pressure and temperature.	Real gas obeys gas laws only at conditions of low pressure and high temperature. They obey Vanderwaal’s real gas equation
The molecules collide with each other elastically.	The molecules collide with each other inelastically.
The volume occupied by the molecules is negligible as compared to the total volume.	The volume occupied by molecules is not negligible as compared to total volume.
There are no intermolecular forces of attraction.	Either attractive or repulsive forces are present between the particles.
It is a hypothetical gas.	It exists in nature around us.
It has high pressure	It has a pressure correction term in its equation and the actual pressure is less than ideal gas.
Obeys PV = nRT	Obeys $(P + \dfrac{{a{n^2}}}{{{V^2}}})(V - nb) = nRT$

Note: A student can confuse between ideal gas and real gas when solving a numerical. Remember nothing is said about the gas, consider it to be ideal. Also, remember to use the right equations in the questions of ideal and real gas.