According to Boyle's Law, the pressure of a gas in a closed container would decrease when the volume of the container increases. Use the kinetic molecular theory of gases to explain this relationship between volume and pressure. Provide a unique example wherein this relationship is applied. 

 

The Kinetic Molecular Theory (KMT) of Gases define pressure as the measure of the frequency of collision between the gas molecules and the walls of their container. If you increase the volume of the container, your gas molecules would have to travel farther lengths for them to be able to collide with the walls of your container. Thus, when you increase the container volume, the frequency of collision with the walls decreases. Therefore, the pressure, as defined by the KMT, decreases.

A unique example of this is when you go SCUBA diving. As you go deeper in the water, you know that the ambient pressure increases as well. Thus, the volume of gases in your lungs decrease, which is why you need SCUBA gear and diving tanks to maintain the volume of gases in your lungs at a steady state. When you're done with your diving, you do not just rush to go towards the sea level, because when you suddenly drop the ambient pressure by doing so, the volume of gases in your lungs would expand suddenly, which may cause the rupturing of your lungs.