Calculate final pressure or volume using Boyle's Law (P₁V₁ = P₂V₂). Supports kPa, atm, psi, bar, mmHg with isothermal work and compression ratio.
**Boyle's Law Calculator** applies the foundational gas law P₁V₁ = P₂V₂, which states that for a fixed amount of gas at constant temperature, pressure and volume are inversely proportional. Enter any three of the four variables (P₁, V₁, P₂, V₂) and the calculator solves for the fourth, along with the compression ratio, isothermal work, and a pressure–volume table.
Robert Boyle published his observation in 1662, and it remains one of the most widely taught relationships in chemistry and physics. It applies to ideal gases and is a good approximation for real gases at moderate pressures and temperatures. Common applications include scuba diving (gas compression at depth), syringe mechanics, weather balloons, pneumatic systems, and engine compression analysis.
Choose a pressure unit (kPa, atm, psi, bar, mmHg), select a preset scenario, and explore the inverse PV curve in the reference table. The visual bar compares V₁ and V₂ at a glance. Keeping the solved variable, the units, and the curve together makes the inverse relationship easier to interpret without reworking the algebra by hand. It also makes it easier to compare one compression setup with another while keeping the constant-temperature assumption visible.
Boyle's law is easy to write down, but the inverse pressure-volume relationship is more intuitive when the selected units and the solved variable are shown together. This calculator is useful for quick checks, classroom work, and comparison of compression scenarios before you move on to a more detailed gas-model calculation. It also helps keep the unit choice visible when you move between kPa, atm, psi, bar, and mmHg.
Boyle's Law: P₁V₁ = P₂V₂ (constant T, constant n) Compression Ratio: CR = V₁ / V₂ Isothermal Work: W = P₁V₁ ln(V₂/V₁)
Result: V₂ = 5.0 L
Doubling the pressure at constant temperature halves the volume: 101.325 × 10 = 202.65 × 5.
Boyle's law is an ideal-gas relationship for a fixed amount of gas at constant temperature. That makes it useful for clean textbook problems, basic compression estimates, and many moderate-pressure situations where real-gas effects are still small.
The law explains why reducing volume raises pressure so quickly in sealed systems. It is the core idea behind syringes, pistons, hand pumps, and many diving pressure intuitions.
The relation becomes less reliable when temperature changes materially during compression or when the gas departs from ideal behavior. If the process is rapid, adiabatic effects can dominate and the final pressure may not match an isothermal estimate.
At constant temperature and fixed amount of gas, pressure and volume vary inversely so that the product `PV` stays constant. If one goes up, the other must go down to preserve the same product.
At very high pressures or low temperatures, real-gas effects (intermolecular forces, molecular volume) cause deviations. Use the van der Waals equation for those conditions, especially when the gas is no longer behaving close to ideally.
A diver's lungs compress with depth; at 10 m (2 atm total), lung volume halves. This underpins equalization and ascent safety rules, and it shows why pressure changes matter so quickly underwater.
It is the work associated with a slow constant-temperature compression or expansion. For an ideal gas, it depends on the logarithm of the volume ratio.
Engine compression ratio is V_max / V_min of the cylinder. Higher CR means more efficient combustion but requires higher-octane fuel.
It is the constant-temperature special case of `PV = nRT`. When `n` and `T` do not change, the product `PV` remains constant.