This is a direct consequence of Boyle's Law, which states that the pressure of a gas is inversely proportional to its volume, assuming constant temperature.
Here's why:
* More frequent collisions: As the volume decreases, the gas molecules are squeezed closer together. This means they collide with the walls of the container more frequently.
* Increased force: Each collision exerts a force on the container walls. With more frequent collisions, the total force exerted on the walls increases.
* Higher pressure: Pressure is defined as force per unit area. Since the force increases and the area remains the same, the pressure of the gas increases.
Example:
Imagine a balloon filled with air. If you squeeze the balloon, you're decreasing its volume. The air inside the balloon will become more compressed, leading to a higher pressure. This is why the balloon feels harder to squeeze.
