Final answer:
Boyle's Law states that the volume of a gas is inversely proportional to its pressure at a constant temperature. This means if pressure increases, volume decreases, and vice versa, maintaining the product of pressure and volume as a constant.
Step-by-step explanation:
Understanding the Relationship Between Pressure and Volume of a Gas
The relationship between the pressure and volume of a given amount of gas at a constant temperature is described by Boyle's Law. This law states that the volume is inversely proportional to pressure. When the temperature is held constant, increasing the pressure on a gas will decrease its volume, and conversely, decreasing the pressure will increase the gas's volume. This relationship is quantified by the equation PV = k, where P is the pressure, V is the volume, and k is a constant for a given amount of gas at a specific temperature.
Robert Boyle, an English natural philosopher, first published this relationship more than 300 years ago. It is an essential principle in the field of chemistry and physics, particularly within the study of gases, and it lays the foundation for understanding how gases behave under different pressures and volumes at a constant temperature.
It's critical to note that Boyle's Law only applies under the condition of constant temperature. If the temperature changes, other gas laws, such as Charles's Law, may be applied. Charles's Law states that at constant pressure, the volume of a gas is directly proportional to its temperature in kelvins.