Interesting Fact about Boyle's Law

What is Boyle's Law and how does it relate to the pressure of a gas in a hot air balloon?

Boyle's Law states that at a constant temperature, the pressure and volume of a gas are inversely proportional. How does this law explain the pressure change in a hot air balloon when its volume decreases?

Boyle's Law and Hot Air Balloon Pressure

Boyle's Law is a fundamental principle in the study of gases. It explains the relationship between the pressure and volume of a gas when the temperature remains constant. According to Boyle's Law, if the volume of a gas decreases, its pressure will increase, and vice versa.

In the case of a hot air balloon, when the balloon is filled with 25 liters of air and exerts a pressure of 500 atm against the walls, this is the initial state where the volume and pressure are related. As the balloon drops to 20 liters of air, the volume decreases, causing the pressure of the hot air inside the balloon to increase.

This pressure increase is a direct application of Boyle's Law, as the volume decrease leads to a higher pressure to maintain the relationship between the two variables. In this scenario, the pressure of the hot air in the balloon would be 625 atm after the volume drops to 20 liters.

Understanding Boyle's Law is crucial in various scientific fields, including chemistry, physics, and engineering. It provides insights into how gases behave under different conditions and helps in analyzing systems involving gas pressure and volume.