An application of Boyle's Law states that when the pressure on a gas increases at constant temperature, what happens to the volume?

Boyle's Law describes the inverse relationship between the pressure and volume of a gas when the temperature is held constant. According to this law, if the pressure on a gas increases, the volume must decrease to maintain equilibrium, provided that the temperature does not change.

Mathematically, Boyle's Law is represented as ( P_1 V_1 = P_2 V_2 ), where ( P ) represents pressure and ( V ) represents volume. If you increase the pressure (P2 > P1), to satisfy the equation, the volume must decrease (V2 < V1). This is because the amount of gas particles remains constant, and as pressure is applied, the particles are forced closer together, resulting in a smaller volume.

This fundamental principle is supported by numerous real-world observations, such as when squeezing a balloon: as you apply pressure, the balloon's volume decreases. Thus, when the pressure on a gas increases at constant temperature, the volume indeed decreases.