Which postulate of the kinetic molecular theory best explains why gases can be compressed?

Answer in explanation

Step-by-step explanation:

When we talk of compression of gases, what we are talking about is simply the reduction in the volume of the gases. When we compress a volume of a gas, we are looking at reducing the volume of the gas in question.

Now, let's work through this. The postulate that works in this scenario is that postulate about the interaction between the gas molecules whether attractive or repulsive are negligible. This is the driving force that dictates the compressibility of gases.

Gases are termed compressible because the the negligible force of attraction or repulsion between them confers a kind of fluidity to these gases. It is this fluidity that makes it possible for gases to be compressible.

If it was that the attractive or repulsive forces are not negligible, they would have posed a difficulty that would be dependent on the strength of the compressive forces to overcome

Step-by-step explanation:

Gases are compressible because most of the volume of a gas is composed of the large amounts of empty space between the gas particles.

The kinetic molecular theory postulate: "These particles are much smaller than the distance between particles". Most of the volume of a gas is therefore empty space.