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Boyle's law says that for a fixed amount of gas at constant temperature, pressure and volume are inversely proportional: squeeze a gas into half the volume and its pressure doubles. Mathematically, P₁V₁ = P₂V₂.
Choose whether you want the final volume or the final pressure. Any units work as long as both pressures use the same unit and both volumes use the same unit.
| Find | Final volume (V₂) |
| Initial pressure (P₁) | 1 |
| Initial volume (V₁) | 6 |
| Final pressure (P₂) | 3 |
| Final volume V₂ | 2 |
| Final pressure P₂ | 3 |
| P × V (constant) | 6 |
Tripling the pressure shrinks 6 mL of air to 2 mL.
Try this example →| Find | Final volume (V₂) |
| Initial pressure (P₁) | 1 |
| Initial volume (V₁) | 5 |
| Final pressure (P₂) | 0.5 |
| Final volume V₂ | 10 |
| Final pressure P₂ | 0.5 |
| P × V (constant) | 5 |
At half the pressure the 5 L balloon expands to 10 L.
Try this example →At constant temperature, the pressure of a fixed amount of gas is inversely proportional to its volume: PV = constant.
P₁V₁ = P₂V₂.
Temperature and the amount (moles) of gas.
No. Any units work as long as P₁ and P₂ match and V₁ and V₂ match.