Which of the following best explains why real gases do not behave exactly like ideal gases?

• A. Real gases consist of particles that move in perfectly straight lines without collisions.
• B. Real gases always have zero pressure at absolute zero temperature.
• C. Real gases have intermolecular forces and occupy a finite volume.
• D. Real gases are composed of atoms that never interact with each other.

Answer: (C)

Verified step by step guidance

1. Recall the assumptions of the ideal gas law: ideal gases are composed of point particles with no volume and no intermolecular forces, moving randomly and colliding elastically.
2. Understand that real gases deviate from ideal behavior because these assumptions are not perfectly true in reality.
3. Recognize that real gas particles have a finite volume, meaning they occupy space, which affects how they move and interact.
4. Acknowledge that real gases experience intermolecular forces (attractive and repulsive), which influence their pressure and volume, especially at high pressures and low temperatures.
5. Conclude that the best explanation for why real gases do not behave exactly like ideal gases is that real gases have intermolecular forces and occupy a finite volume.