It's not enough to know what Boyle's law is; you also have to learn how to calculate Boyle's law. We created this calculator to help you in that endeavor.
We can use Boyle's law to calculate constant temperature processes (also known as isothermal processes), which are present in many real-life systems or situations, such as Carnot heat engines, the process of breathing, or even when pulling the plunger of an injection syringe.
To know how to calculate that gas law manually, you can look at Boyle's law equation in the following sections. You can also click on the advanced mode of the calculator to find the temperature or pressure using the ideal gas law.
💡 Boyle's law only is one within a list of gas laws. You can study those laws using our combined gas law calculator.
What is Boyle's law?
Boyle's law definition says that at constant temperature (or constant thermal energy), the absolute pressure exerted by a constant amount of mass of an ideal gas is inversely proportional to the volume occupied.
Boyle's law formula
We can derive Boyle's law equation from the ideal gas law. Boyle's law states that the product of the pressure and temperature of an ideal gas is constant for isothermal processes:
P₁V₁ = P₂V₂
P₁— First pressure, in Pa;
P₂— Second pressure, in Pa;
V₁— First volume, in m3; and
V₂— Second volume, in m3.
Other experimental gas laws
Boyle's law is not the only experimental gas law derived from the ideal gas law. Other two similar fundamental laws describe other thermodynamic processes:
- Charles' law: While we use Boyle's law to calculate constant pressure processes, we can use Charles' gas law to calculate constant pressure processes through the formula
V₁/T₁ = V₂/T₂. Learn more about it in our Charles' law calculator.
- Gay-Lussac's law: With Charles' gas law, we can calculate constant volume processes through the formula
P₁/T₁ = P₂/T₂. Learn more about it in our Gay-Lussac's law calculator.
Hopefully, now you know how to calculate Boyle's law formula and its importance 🎉. Thanks for reading this article!