kinetic molecular theory
1 – The particles are so small compared with the distances between them that the volume of the individual particles can be assumed to be negligible (zero).
2 – The particles are in constant motion. The collisions of the particles with the walls of the container are the cause of the pressure exerted by the gas.
3 – The particles are assumed to exert no forces on each other; they are assumed neither to attract nor to repel each other.
4 – The average kinetic energy of a collection of gas particles is assumed to be directly proportional to the Kelvin temperature of the gas.
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