Boyles Law
| Item | Formula / Note | Source / Standard |
|---|---|---|
| Boyle law | pV = const at fixed T | Boyle 1662 |
| Isothermal condition | Constant temperature and amount | Ideal gas law |
| Ideal gas | Special case of pV = nRT | Clapeyron 1834 |
| Deviation | Real gas correction at high p/low T | van der Waals 1873 |
| Units | Consistent units required | Calculation note |
| Compressibility | Z = pV/(nRT) measures deviation | Real gas theory |
Constants used on this page and their authoritative sources, for verification and citation
| Constant | Value | Unit | Source |
|---|---|---|---|
| Molar gas constant R | 8.314462618 | J·mol⁻¹·K⁻¹ | New SI (derived from exact N_A·k) |
| Standard atmosphere | 101 325 | Pa | ISO 2533 defining value (exact) |
| Molar volume of an ideal gas (0 ℃, 1 atm) | 22.41396954 | L·mol⁻¹ | Derived from RT/p (same value in CODATA 2018) |
| Celsius scale zero point T_0 | 273.15 | K | SI / ITS-90 defining value (exact) |
Note: Boyle's law P₁V₁ = P₂V₂ holds only at constant temperature and fixed amount of gas, and is an ideal-gas approximation; use a real-gas equation of state (e.g. van der Waals / IAPWS) at high pressure or near liquefaction.