Respuesta :
Answer:
e. All of the above statements are consistent with the Kinetic Molecular Theory.
Explanation:
for a.;
Kinetic molecular theory assumes the collision of particles with each other and walls of container as perfectly elastic, that is why no particle loses energy.
for b.;
Kinetic molecular theory assumes that particles are of very small size in comparison with the size of container and far apart from each other that is why their density is very low. because density is described as
Density = Mass/Volume
So, one can imagine that in a big container, entire mass of all gas particles is very low as compared to the volume of container. So the gas have very low density
For c.;
Gases assume shape of their container because they are freely moving with in a container
For d.;
For statement in "b", one can easily understand that because according to kinetic molecular theory, particles are very small and at great distances, so they are compressible against any external pressure applied.
A kinetic molecular theory is a theory of gases and is a classical model of thermodynamics. It describes the gas as a large number of identical subatomic which are constant, rapid, and have a random motion.
- The gas-particle collides with each other surfaces without losing energy. The gases have a low density and have lots of empty spaces.
- The gas assumes the shape of the container in which they fill. They are compressible and take the entire volume of the open space.
Hence the option E is all of the above.
Learn more about the consistency of the Kinetic Molecular Theory.
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