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| 8348937276 | Kinetic Theory | particles are always in motion | 0 | |
| 8348937278 | vacuum | space void of matter | 1 | |
| 8348937279 | atmospheric pressure | when there you are at a higher elevation then there is less atmosphere so less pressure | 2 | |
| 8348937280 | Diffusion | movement of gas from high to low | 3 | |
| 8348937281 | Effusion | high gas to low gas | 4 | |
| 8348937282 | barometer | instrument to measure atmospheric pressure | 5 | |
| 8348937283 | pressure | is caused by the collisions of molecules with the walls of a contaiter | 6 | |
| 8348937284 | Pressure increases | if you decrease the size of the container then what happens to the pressure | 7 | |
| 8348937285 | Boyles law | P1V1=P2V2 if the pressure increases then the volume will decrease | 8 | |
| 8348937286 | Charles law | V1/T1=V2/T2 The volume increases then the temperature will increase | 9 | |
| 8348937287 | Gay Lussac law | P1/T1=P2/T2 if the volume stays the same then if the pressure increases so will the temperature | 10 | |
| 8348937288 | Combined gas law | P1V1/T1=P2V2/T2 | 11 | |
| 8348937289 | Daltons law of partial pressure | Total pressure of a gas is equal to the sum of the partial pressure of the component gases | 12 | |
| 8348937290 | Ideal gas law | PV=nRT | 13 | |
| 8348937291 | avagadros gas law | at stp 1 mole of any gas will occupy 22.4 L of space | 14 | |
| 8348937293 | Temperature, Volume, Moles | The three factors that affect gas pressure | 15 | |
| 8348937294 | Graham's law of effusion | if the temperatures and pressures are the same then the rates of effusion are inversely proportional to the square root of their molar mass | 16 | |
| 8348937295 | equation of graham's law of effusion | A is always the lighter gas |  | 17 |
