1. Intermolecular Forces: Real gas particles exhibit attractive and repulsive forces between each other, known as intermolecular forces. These forces influence the behavior of gases, particularly at high pressures when the particles are densely packed.
2. Finite Volume of Gas Particles: Unlike ideal gases, real gas particles have a finite size and occupy some space. This becomes significant at high pressures because the effective volume available for particle movement decreases.
3. Non-Random Molecular Motion: The assumption of completely random molecular motion in ideal gases does not hold true for real gases. Intermolecular forces can introduce correlations and patterns in the movement of real gas particles.
4. Variable Collisions: In real gases, collisions between particles are not perfectly elastic as assumed in the ideal gas model. The interactions between particles result in energy transfer and internal energy changes, affecting the pressure-volume-temperature relationships.
The deviations from ideal behavior are described by equations of state such as the van der Waals equation, which account for the effects of intermolecular forces and finite particle volume. Real gases approach ideal behavior at high temperatures and low pressures, where the influence of these factors becomes negligible.
