In regard to gas laws, when volume decreases, what happens to the pressure if temperature remains constant?

When considering gas laws, particularly Boyle's Law, which states that, for a given amount of gas at a constant temperature, the pressure of the gas is inversely proportional to its volume, the correct outcome is that pressure increases when volume decreases, provided the temperature remains constant.

This relationship is significant in diving because as a diver descends and the volume of air in their equipment (like a buoyancy control device or a tank) decreases due to increased external pressure, the pressure of the gas within that volume increases. This principle governs many aspects of diving, including how gas behaves in a tank and how divers manage buoyancy. Understanding this behavior is crucial for safety and effective dive planning.

The other options do not accurately reflect the behavior described by Boyle's Law. Pressure does not decrease or remain constant; instead, it must increase as the volume decreases, illustrating the fundamental behavior of gases under constant temperature conditions.