According to Boyle's Law, what happens to the volume of a gas when the pressure increases, assuming the temperature remains constant?

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 pressure exerted on a gas increases, its volume decreases.

This relationship can be represented mathematically as PV = k, where P stands for pressure, V stands for volume, and k is a constant for a given amount of gas at a specific temperature. When the pressure increases (P goes up), the volume (V) must decrease to keep the product PV constant.

Thus, if the pressure of a gas is raised while maintaining a constant temperature, the result is a decrease in volume. This is a fundamental principle in understanding how gases behave under varying pressure conditions, showcasing the gas's response to external pressures without changing temperature.