The kinetic molecular theory of gases
The kinetic molecular theory explains how gases behave using a few assumptions about their particles: gas particles are in constant, random, straight-line motion; the particles are tiny compared with the distances between them, so a gas is mostly empty space; collisions between particles and with the container walls are elastic, so no energy is lost overall; an ideal gas has no attractive or repulsive forces between its particles; and the average kinetic energy of the particles is proportional to the gas's absolute (Kelvin) temperature. Gas pressure is the result of particles colliding with the container walls. Real gases behave most like ideal gases at high temperatures and low pressures.
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