According to Boyle's Law, what happens to the pressure of a gas when its volume is reduced at a constant temperature?

Boyle's Law states that at a constant temperature, the pressure of a gas is inversely proportional to its volume. This means that when the volume of a gas decreases, the pressure inside the container increases, assuming there is no change in temperature.

When you compress a gas (reducing its volume), the molecules have less space to move around, which leads to an increase in collisions between gas molecules and the walls of the container. As these collisions become more frequent, the pressure exerted by the gas rises. Therefore, when interpreting Boyle's Law within this context, the correct understanding is that reducing the volume results in an increase in pressure—reflecting the inverse relationship between these two variables.

The incorrect options suggest that pressure either decreases, remains constant, or fluctuates unpredictably, which doesn’t align with the established principles of gas behavior as outlined by Boyle's Law. This law is a fundamental relationship in thermodynamics and gas physics that illustrates how pressure and volume interact at a stable temperature.