which assumption of kinetic molecular theory of gases explain the compressibility of gases ?
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Answer:
The kinetic molecular theory of gases explains the laws that describe the behavior of gases. Developed during the mid-19th century by several physicists, including the Austrian Ludwig Boltzmann (1844–1906), the German Rudolf Clausius (1822–1888), and the Englishman James Clerk Maxwell (1831–1879), who is also known for his contributions to electricity and magnetism, this theory is based on the properties of individual particles as defined for an ideal gas and the fundamental concepts of physics. Thus the kinetic molecular theory of gases provides a molecular explanation for observations that led to the development of the ideal gas law. The kinetic molecular theory of gases is based on the following five postulates:
A gas is composed of a large number of particles called molecules (whether monatomic or polyatomic) that are in constant random motion.
Because the distance between gas molecules is much greater than the size of the molecules, the volume of the molecules is negligible.
Intermolecular interactions, whether repulsive or attractive, are so weak that they are also negligible.
Gas molecules collide with one another and with the walls of the container, but these collisions are perfectly elastic; that is, they do not change the average kinetic energy of the molecules.
The average kinetic energy of the molecules of any gas depends on only the temperature, and at a given temperature, all gaseous molecules have exactly the same average kinetic energy.
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