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
- Boyle's Law applies only to ideal gases and assumes the temperature remains constant (isothermal process).
- The product of pressure and volume ($PV$) remains constant for a given amount of gas.
- If the volume of a gas doubles, its pressure will be halved, provided the temperature is kept constant.
- Boyle's Law can be derived from the Ideal Gas Law when temperature and number of moles are held constant.
- 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.
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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.
