A snorkeler with a lung capacity of \(6.3 \mathrm{~L}\) inhales a lungful of air at the surface, where the pressure is \(1.0\) atm. The snorkeler then descends to a depth of \(25 \mathrm{~m}\), where the pressure increases to \(3.5 \mathrm{~atm}\). What is the capacity of the snorkeler's lungs at this depth? (Assume constant temperature.)

Understanding the fundamental concepts of gas laws is crucial for students as it forms the basis for explaining how gases behave under different conditions of temperature, volume, and pressure. These laws allow us to predict the behavior of gases in various scenarios, from everyday occurrences like inflating a balloon to the more complex processes involved in respiratory physiology and scuba diving.

• Boyle's Law, one of the most essential gas laws, deals specifically with the pressure-volume relationship of a gas at constant temperature.
• Charles's Law, another important gas law, focuses on the relationship between volume and temperature at constant pressure.
• The Combined Gas Law integrates both Boyle's and Charles's laws to describe the simultaneous change in pressure, volume, and temperature.

These principles are foundational in fields such as chemistry, physics, environmental science, and various engineering disciplines. They provide a framework for understanding gas behavior and are represented by mathematical equations that predict how a change in one variable affects others.

The pressure-volume relationship, as defined by Boyle's Law, is an inverse relationship that expresses how, for a given mass of a gas at a constant temperature, as pressure increases, volume decreases, and vice versa. To visualize this concept, imagine a syringe filled with air: If you push on the plunger to decrease the syringe's volume, the pressure of the air inside increases.

The mathematical expression for Boyle's Law is given by: \[PV = k\] where:\

• \