| A | B |
|---|
| Boyle's Law | PV = PV |
| Charles's Law | V/T = V/T |
| inverse | relationship between pressure and volume |
| direct | relationship between volume and temperature |
| ideal gas law | takes into account pressure, volume, temperature, and moles present |
| Dalton's law | deals with partial pressures |
| partial pressure | amount of pressure exerted by a gas in a mixture of gases |
| Avogadro's hypothesis | equal volumes of a gas at the same temp. and pressure contain equal numbers of particles |
| 22.4 Liters | volume a gas occupies at STP |
| STP | standard temperature and pressure |
| 1 atmosphere | = 760 mm Hg |
| 2 atmospheres | = 202.6 kPa |
| 1 mm Hg | = 1 torr |
| ideal gas constant | 8.31 L*kPa/K*mol |
| diffusion | the tendency of molecules to move from areas of higher concentration to areas of lower concentration |
| effusion | the process of a gas escaping through a small opening |
| temperature | measure of the average kinetic energy of gas particles |
| Kelvin temperature | degrees celsius + 273 |
| absolute zero | where volume of a gas is zero |
| combined gas law | PV/T = PV/T |
| ideal gas | gas whose particles have no volume and no attraction to one another |
| kinetic molecular theory | based on the concept that particles of all forms of matter are in constant motion |
