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What is the difference between ideal gas and real gas?

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An ideal gas is a theoretical gas with a certain set of properties that allow it to obey the ideal gas laws. A real gas is an existing gas (such as oxygen or hydrogen) that follows a different set of laws due to variations in its properties compared to ideal gases.

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What is the difference between ideal gas and real gas?
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Full Answer

An ideal gas is composed of particles that have a point mass. A particle of point mass has a mass that is low enough to be considered almost zero. This also means that the theoretical particles of an ideal gas do not occupy any volume. A real gas is composed of particles that have a finite mass, and due to this mass, they also occupy a finite volume.

An ideal gas is compressible under extremely high pressures; that is, it is infinitely compressible. A real gas has limitations to the pressure it can be compressed to before it condenses into a liquid.

The collisions between ideal gas particles are completely elastic. The particles do not exert attractive or repulsive forces on each other and do not lose kinetic energy in the collisions. The collisions between real gas particles are nonelastic. Some attractive and repulsive forces exist, and some of the kinetic energy is lost as heat.

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