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Chemistry · L4 · Why Real Gases Deviate from Ideal

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The two causal chains — high pressure and low temperature — that push a real gas away from PV = nRT, ending in the compressibility factor Z.

by @openstemUpdated Chemistry
Ideal gas law:no particle volume,no intermolecular forcesHigh pressure:molecules pushedclose togetherLow temperature:particles moveslowlyMolecules' own volumeis now a significantfraction of VReal gas resists compression:takes up MORE space thanideal predicts (Z > 1)Intermolecular attractions(van der Waals forces)dominate kinetic energyReal gas is MORE compressiblethan ideal predicts (Z < 1)Cooled or compressedfurther: gas condensesto a liquid

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