Boyles Law
Calculator
Results
- Final volume (L)
- 1.6
- Volume change (L)
- -2.4
Chemistry results
| Final volume (L) | 1.6 |
| Volume change (L) | -2.4 |
formula-map diagram
- Final volume (L)
- 1.6
- Volume change (L)
- -2.4
Formula breakdown
Formula
P₁ × V₁ = P₂ × V₂= 1.6
Note
Simplified model: these results assume ideal behaviour (ideal gases, dilute solutions, complete reactions) and standard textbook constants. Real laboratory values vary with temperature, pressure, purity and activity coefficients. Do not rely on this for safety-critical or analytical work.
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See all →Frequently asked questions
What does Boyle's law state?+
Boyle's law says that for a fixed amount of gas at constant temperature, pressure and volume are inversely proportional: P1V1 = P2V2. As you compress a gas into a smaller volume, its pressure increases proportionally, and vice versa.
Why does compressing a gas increase its pressure?+
Squeezing gas molecules into a smaller volume means they collide with the container walls more frequently in a given time, and pressure is essentially a measure of that collision rate, so more frequent collisions mean higher pressure. Temperature must stay constant for this relationship to hold exactly.
What real-world situations use Boyle's law?+
Boyle's law explains how a syringe works (pulling the plunger increases volume and drops pressure, drawing in fluid), how scuba diving affects lung volume with depth, and how a bicycle pump compresses air to inflate a tire. It's one of the most directly observable gas laws in daily life.
What happens to Boyle's law calculation if temperature changes during the process?+
Boyle's law strictly assumes constant temperature, so if temperature also changes, you need the combined gas law instead, which accounts for simultaneous pressure, volume, and temperature changes. Using Boyle's law when temperature isn't held constant will give an inaccurate result.
Does it matter what pressure and volume units I use in Boyle's law?+
You can use any consistent units for pressure (atm, kPa, mmHg) and any consistent units for volume (L, mL) as long as both sides of the equation use the same units, since the law is a ratio and the units cancel out. Just don't mix atm on one side with kPa on the other.