What does Boyle's Law state regarding gas volume and pressure?

Boyle's Law describes the relationship between the volume and pressure of a gas, stating that the volume of a gas is inversely proportional to the pressure exerted on it, assuming the temperature is kept constant. This means that as the pressure increases, the volume decreases, and vice versa. This relationship can be mathematically represented as PV = k, where P is pressure, V is volume, and k is a constant for a given quantity of gas at a constant temperature.

When pressure is applied to a gas, its particles are forced closer together, resulting in a decrease in volume. Conversely, if the pressure decreases, the gas expands and the volume increases. This principle is fundamental in understanding gas behavior in various situations, such as in aviation and medical contexts, where changes in altitude can affect pressure and, consequently, gas volume in the human body and in aircraft systems.

The other options do not accurately reflect Boyle's Law. For instance, the notion that volume decreases with increased temperature pertains to Charles's Law, while the idea that volume increases with an increase in pressure contradicts the established relationship described by Boyle's Law. Similarly, stating that volume is directly proportional to the pressure surrounding it misrepresents the inverse relationship that Boyle's Law specifically highlights.