Question

According to kinetic theory how are gases compared with liquids and solids?

Answer 1

Hint: The actual properties of a substance rely on its actual state. Water fume, fluid water, and ice all have similar substance properties, however their actual properties are extensively unique.

Complete answer:
The dynamic atomic hypothesis of the issue says that particles of gases go through more prominent rotational, translational, and vibrational movement than the particles solids and fluids. That is the reason gases don't have fixed volumes; their atoms simply move around "imprudently" for as much space is accessible; practically zero intermolecular powers are included, besides in a crash.
What's more, we can likewise see that there are a greater number of impacts between gas atoms than there are in fluid and none in solids. We can likewise take note of that the pressing factor of a gas is in this manner a consequence of the crashes that the gas particles make with the holder encasing the gas or some other item in contact. The active atomic hypothesis of gases portrays this condition of issue as made out of minuscule particles in steady movement with a great deal of distance between the particles.
Since the majority of the volume involved by a gas is unfilled space, gas has a low thickness and can grow or contract under the suitable impact. The way that gas particles are in consistent movement implies that at least two gases will consistently blend as the particles from the individual gases move and crash into one another. The quantity of crashes the gas particles make with the dividers of their holder and the power with which they impact decide the size of the gas pressure.

Note: At the point when the volume of an encased gas is diminished, the gas particles have less space in which to move and consequently they impact all the more frequently with one another, subsequently making the pressing factor of the encased gas increment.