The kinetic theory of gases explains how gas behavior arises from the motion of its constituent particles (molecules or atoms). Key concepts include:
Constant Motion: Gas particles are in constant, random motion.
Negligible Volume: Particle volume is tiny compared to the gas volume.
No Intermolecular Forces: No significant forces between particles except during collisions.
Elastic Collisions: Collisions between particles and container walls conserve kinetic energy.
Temperature & Kinetic Energy: Average particle kinetic energy is directly proportional to absolute temperature.
The Ideal Gas Law (PV = nRT) relates pressure (P), volume (V), number of moles (n), ideal gas constant (R), and absolute temperature (T) for ideal gases, derived from the kinetic theory
