Boyle's law states that the pressure of a gas is inversely proportional to its volume when the temperature and the amount of gas are held constant. Mathematically, it can be expressed as:
\[ P \propto \frac{1}{V} \]
or
\[ PV = k \]
where:
- \( P \) is the pressure of the gas,
- \( V \) is the volume of the gas, and
- \( k \) is a constant for a given amount of gas at a constant temperature.
This means that if the volume of a gas decreases, its pressure increases, provided that the temperature remains constant, and vice versa. Boyle's law is applicable to ideal gases and is a foundational principle in the study of gas behavior.
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