| A | B |
|---|
| Dalton's law of partial pressures | At constant volume and temperature, the total pressure exerted by a mixture of gases is equal to the sum of the partial pressures of the component gases |
| Charles's law | The volume of a fixed mass of gas is directly proportional to its Kelvin temperature if the pressure is kept constant |
| Graham's law of effusion | The rate of effusion of a gas is inversely proportional to the square root of its molar mass |
| partial pressure | the contribution each gas in a mixture makes to the total pressure of that mixture |
| compressibility | a measure of how much the volume of matter decreases under pressure |
| Boyle's law | For a given mass of gas at constant temperature, the volume of the gas varies inversely with pressure |
| diffusion | the tendency of molecules to move toward areas of lower concentration until the concentration is uniform throughout |
| effusion | the escape of a gas through a tiny hole in a container of gas |
| ideal gas constant (R) | 8.31 (L•kPa)/(K•mol) |
| Gay-Lussac’s Law | the pressure of a gas is directly proportional to the Kelvin temperature if the volume remains constant |
| P1 x V1 = P2 X V2 | mathematical representation of Boyle’s law |
| V1/T1 = V2/T2 | mathematical representation of Charles’s law |
| P1/T1 = P2/T2 | mathematical representation of Gay-Lussac’s law |
| (P1 x V1)/T1 = (P2 x V2)/T2 | mathematical representation of the combined gas law |
| PV = nRT | mathematical representation of the ideal gas law |
