Why do ideal gases not show Joule Thomson effect?
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Well, one definition of an ideal gas is that it doesn’t cool on free expansion.
The molecular origin of the cooling effect is cohesive forces between the molecules, which always exist in a real gas. Heat is absorbed as energy goes into breaking these attractions, sort of the way heat is absorbed from the surroundings when a liquid evaporates.
If the cohesive forces between gas molecules are zero, as postulated for a perfect gas, the phenomenon disappears.
The molecular origin of the cooling effect is cohesive forces between the molecules, which always exist in a real gas. Heat is absorbed as energy goes into breaking these attractions, sort of the way heat is absorbed from the surroundings when a liquid evaporates.
If the cohesive forces between gas molecules are zero, as postulated for a perfect gas, the phenomenon disappears.
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Ideal gases do not show the Joule-Thomson effect because there is no intermolecular force of attraction present in them.
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