Boyle’s Law

Summary:

Boyle’s Law states that the pressure and volume of a gas are inversely proportional when temperature and mass are constant. It explains the relationship between the volume and pressure of a gas and sheds light on phenomena like the explosion of a gas-filled balloon when compressed. The law is represented as P ∝ 1/V or PV = k, where P is pressure, V is volume, and k is a constant of proportionality.

According to Boyle’s Law, at a constant temperature and mass, the volume of a gas decreases as the pressure increases. It is one of the fundamental gas laws formulated by English Chemist Robert Boyle in 1662. The law can be mathematically expressed as P = k * (1/V), or PV = k, where the product of pressure and volume remains constant.

A pressure vs. volume diagram illustrates Boyle’s Law as a curve, which becomes a straight line when pressure is plotted on the Y-axis and the inverse of volume on the X-axis.

The formula and derivation of Boyle’s Law show that the initial pressure and volume of a gas multiplied together equal the final pressure and volume, demonstrating the relationship between pressure and volume changes.

Examples of Boyle’s Law include the expansion and contraction of the lungs during breathing and the behaviour of carbonated drinks when the bottle is opened. Medical syringes also illustrate the principles of Boyle’s Law.

Excerpt:

Boyle’s Law

Boyle’s law expresses that the pressure and volume of a gas are inversely corresponding when the temperature and mass of the gas are steady. Boyle’s Law makes sense of the connection between the volume and pressure of a gas. Boyle’s law makes sense of the peculiarity where on the off chance that we crush a gas-filled balloon, it explodes. Thus, when tension is applied to the inflatable, its volume attempts to diminish, and when that isn’t feasible, it explodes.

Boyle’s law is addressed as,
P ∝ 1/V
Or
PV= k

Where,
P is pressure
V is volume
K is constant of proportionality