When a gas is under pressure, its volume decreases.
This relationship is described by Boyle's Law, which states that for a fixed amount of gas at a constant temperature, the pressure and volume are inversely proportional. In simpler terms, if you increase the pressure on a gas, the volume will decrease proportionally, and vice versa.
Here's a breakdown:
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Boyle's Law: Mathematically expressed as P₁V₁ = P₂V₂, where:
- P₁ = Initial Pressure
- V₁ = Initial Volume
- P₂ = Final Pressure
- V₂ = Final Volume
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Inverse Relationship: This means if you double the pressure, you halve the volume. If you halve the pressure, you double the volume.
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Constant Temperature and Amount of Gas: Boyle's Law is only applicable when the temperature and the amount of gas remain constant.
Example:
Imagine a balloon filled with air. If you squeeze the balloon (increase the pressure), the balloon's size (volume) decreases. Conversely, if you release some of the pressure on the balloon, it will expand, increasing in volume.
Summary:
The fundamental principle is that gases are compressible. Applying pressure forces the gas molecules closer together, leading to a reduction in volume. This inverse relationship between pressure and volume is a cornerstone of gas behavior.
