Experimental Verification of Boyle’s Law

Gas laws were created around the end of the 18th century by various scientists. Each gas rule is identified by the names of the scientists who proposed the law. As a result, we now identify five key gas laws, wherein Boyle’s Law describes the link between a gas’s pressure and volume. On the other hand, the connection between the volume filled by a particular gas and its absolute temperature is comprehended through Charles’ Law. 

Gay-Lussac’s law sheds light on the connection between the pressure exerted by a gas on the walls of its container and the absolute temperature associated with the gas. The link between the volume occupied by a gas and the amount of gaseous material is given by Avogadro’s Law. By combining the preceding four rules presented by four different scientists, the Combined Gas Law, often known as the ideal gas law, may be created. 

What is Boyle’s law?

In 1662, the Anglo-Irish chemist Robert Boyle proposed Boyle’s Law. Boyle’s law says that the pressure exerted by gasses (of a given mass and temperature) is inversely proportional to the volume occupied by the gas. In other words, as long as the temperature and amount of gas remain constant, the pressure and volume of a gas are inversely proportional.

The connection between volume and pressure in a gas may be stated as Boyle’s law mathematically as follows (at constant mass and temperature).

P ∝ (1/V)

The pressure exerted by the gas is P, and the volume occupied by it is V. By adding a constant, k, to this proportionality, we can convert it into an equation.

P = k*(1/V) ⇒ PV = k

Experimental Verification of Boyle’s Law

The mathematical expression of Boyle’s Law is constant pressure and constant volume, which can be expressed as P V = k, where P is pressure, V is volume and k is a constant. This means that for continuous pressure, a constant volume must be maintained. This law can be seen in the illustration of a column of air, where the pressure at the base increases as the column expands, while the pressure at the top remains constant. This demonstrates that as the volume of a substance increases, the pressure within the substance also increases.

Boyle’s Law is a statement of the relationship between the pressure and volume of a gas, which can be written as the constant pressure of gas multiplied by the constant volume of gas. The law is often written as P1V1 = P2V2, where P1 is the pressure, V1 is the volume, P2 is the pressure of the gas, V2 is the volume of the second gas, and n is the constant of proportionality. 

Derivation and Boyle’s Law Formula

According to Boyle’s law, any change in the volume filled by a gas (at constant quantity and temperature) results in a difference in its pressure. Put another way, the product of a gas’s initial pressure and initial volume equals the product of the gas’s final pressure and final volume (at constant temperature and number of moles). This law can be mathematically represented as follows:

P1V1 = P2V2

Here, P1 refers to the gas’s starting pressure. V1 is the gas’s initial volume of occupancy. P2 refers to the gas’s ultimate pressure. The final volume filled by the gas is V2.

Boyle’s law formula suggests a pressure-volume connection, which may be used to get this phrase. PV = k for a certain quantity of gas at constant temperatures. 

Therefore, P1V1 = k (initial pressure × initial volume)

P2V2 = k (final pressure × final volume)

∴ P1V1 = P2V2

When a gas’s container volume decreases, the equation can be used to predict the increase in pressure exerted by the gas on the container walls (and its quantity and absolute temperature remain unchanged).

Example of Boyle’s Law 

Our lungs use Boyle’s Law during breathing. Inhaling causes the lungs to expand because they are filled with air. As the volume grows, the pressure level decreases. Similarly, when the lungs are emptied of air, they contract, reducing the volume and increasing the pressure. The change in pressure and volume is both instantaneous and periodic.

Conclusion

Experiments and observations in physics have led to the development of four fundamental principles that describe how gases behave: the law of Boyle, the law of Charles, Avogadro’s law and the law of Gay-Lussac. The experiments and observations described in this section have led to the development of gas laws. These laws are most useful in explaining the behaviour of gases under constant pressure and constant temperature. We’ve further discussed Boyle’s law and its mathematical expression that is P1V1 = P2V2.