Boyle’s law is a gas law that states that for a fixed amount of an ideal gas kept at a fixed temperature, pressure and volume are inversely proportional. This means that if pressure increases, volume decreases, and vice versa.
The law was first published by Irish natural philosopher and chemist Robert Boyle in 1662. Boyle’s law is one of the three gas laws that form the basis of the ideal gas law. The other two gas laws are Charles’s law and Gay-Lussac’s law.
Boyle’s law can be expressed mathematically as:
$P_1V_1 = P_2V_2$
where $P_1$ is the initial pressure, $V_1$ is the initial volume, $P_2$ is the final pressure, and $V_2$ is the final volume.
Boyle’s law can be used to explain a number of phenomena, such as the compression of air in a bicycle pump or the expansion of air in a
hot air balloon.Option A: Pressure and volume are inversely proportional. This means that if pressure increases, volume decreases, and vice versa.
Option B: Volume and temperature are directly proportional. This means that
if temperature increases, volume increases, and vice versa.Option C: Volume and density are inversely proportional. This means that if volume increases, density decreases, and vice versa.
Option D: Pressure and temperature are directly proportional. This means that if pressure increases, temperature increases, and vice versa.