Boyle’s law

Definition

Boyle’s Law states that the pressure of a given mass of gas is inversely proportional to its volume at constant temperature. Mathematically, it is expressed as $P \propto \frac{1}{V}$ or $PV = k$, where $k$ is a constant.

5 Must Know Facts For Your Next Test

1. Boyle's Law applies only to ideal gases and assumes the temperature remains constant (isothermal process).
2. The product of pressure and volume ($PV$) remains constant for a given amount of gas.
3. If the volume of a gas doubles, its pressure will be halved, provided the temperature is kept constant.
4. Boyle's Law can be derived from the Ideal Gas Law when temperature and number of moles are held constant.
5. Graphically, Boyle’s Law can be represented by a hyperbolic curve on a $P-V$ diagram where each point on the curve represents a state with equal product $PV$.

Review Questions

• What happens to the pressure of a gas if its volume is reduced to one-third while keeping temperature constant?
• How can Boyle's Law be derived from the Ideal Gas Law?
• Describe how you would graphically represent Boyle's Law on a $P-V$ diagram.

Related terms

Ideal Gas Law: $PV = nRT$, which relates pressure ($P$), volume ($V$), number of moles ($n$), universal gas constant ($R$), and temperature ($T$).

Isothermal Process: A thermodynamic process in which the temperature remains constant.

Charles's Law: $V \propto T$, stating that at constant pressure, the volume of an ideal gas is directly proportional to its absolute temperature.