According to Boyle's Law, what is the relationship between pressure and volume of a gas at constant temperature?

Boyle's Law states that the pressure of a gas is inversely proportional to its volume when the temperature is held constant. This means that as the volume of a gas decreases, its pressure increases, and conversely, as the volume increases, the pressure decreases. The relationship can be expressed mathematically as (P \times V = k), where (P) represents pressure, (V) represents volume, and (k) is a constant for a given amount of gas at constant temperature.

This principle underlies many practical applications, such as the operation of syringes and scuba diving regulations. For instance, when a diver ascends, the volume of air in their lungs expands as the surrounding pressure decreases, which must be regulated to avoid barotrauma.

The correct choice accurately reflects this fundamental principle of gas behavior under constant temperature conditions.