What does Boyle's Law state regarding the relationship between pressure and volume of a gas?

Boyle's Law states that the pressure of a gas is inversely proportional to its volume when the temperature and the quantity of gas remain constant. This means that if the volume of a gas decreases, the pressure increases, provided the temperature does not change, and vice versa. Mathematically, this relationship can be expressed as ( P \times V = k ), where ( P ) is pressure, ( V ) is volume, and ( k ) is a constant for a given amount of gas at a specific temperature.

At a constant temperature, if the volume is halved, for example, the pressure will double, demonstrating the inverse relationship. This principle is fundamental in understanding how gases behave under varying conditions, particularly in processes like respiration in biology or in various industrial applications.

The other options do not accurately reflect Boyle's Law: the direct proportionality of pressure and volume is contradicted by this law; volume independence does not hold true when pressure changes; and the assertion that pressure and volume are unrelated misrepresents the established gas behavior described by Boyle's Law.