Real gas behavior differs from ideal gas behavior primarily for two reasons, the volume of the particles in themselves and their intermolecular forces.
In a real gas, the molecules occupy a minimum volume beyond which the gas cannot be further compressed. This volume is different than the volume corresponding the thermodynamic state of the gas.
Furthermore, real molecules exhibit intermolecular force, which becomes especially significant the more time the molecules spend close together. The greater the opportunity for intermolecular force to play a part in determining the behavior of the system, the greater the deviation of the behavior of the gas from the ideal gas model. For this reason, gases deviate from ideal gas behavior at low temperature and volume.
In a real gas, the molecules occupy a minimum volume beyond which the gas cannot be further compressed. This volume is different than the volume corresponding the thermodynamic state of the gas.
Furthermore, real molecules exhibit intermolecular force, which becomes especially significant the more time the molecules spend close together. The greater the opportunity for intermolecular force to play a part in determining the behavior of the system, the greater the deviation of the behavior of the gas from the ideal gas model. For this reason, gases deviate from ideal gas behavior at low temperature and volume.
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