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Gases consist of tiny particles (atoms/molecules)Particles are so small, relative to the distances between them, that the volume of the individual particles is assumed to be negligible (zero)Particles are in constant, random motion, colliding with the walls of the container. These collisions cause the pressure exerted by the gasParticles are assumed not to attract or to repel each otherAvg kinetic energy of gas particles is directly proportional to the Kelvin temperature of the gas

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