According to Boyle's Law, what is 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 amount of gas are held constant. This means that if the pressure of a gas increases, the volume must decrease to maintain the balance defined by the law, and similarly, if the volume increases, the pressure must decrease. This inverse relationship is often simplified to the statement that as pressure increases, volume decreases.

The concept behind this law can be understood through the movement and spacing of gas molecules. When you compress a gas by applying pressure, the molecules are forced closer together, reducing the volume. Conversely, if you allow the gas to expand without applying pressure, the molecules will spread apart, resulting in an increased volume.

Other options may misstate the relationship described by Boyle's Law. For instance, asserting that as volume increases, pressure also increases would contradict the fundamental inverse relationship established by this principle, as both cannot rise simultaneously under constant temperature conditions. The notion that pressure decreases while volume remains constant misrepresents the interaction between these two variables. Thus, the correct interpretation of Boyle's Law is that there is a decrease in volume corresponding to an increase in pressure, affirming the correct answer.