Terms : Hide Images
| 384344493 | pressure | force per unit area on a surface | |
| 384344494 | barometer | device used to measure atmospheric pressure | |
| 384344495 | pascal | force exerted by force of one newton acting on an area of one square meter; 1.013x10^4 Pa = 1 atm | |
| 384344496 | kilopascal | 101.325 kPa = 1 atm | |
| 384344497 | millimeters of mercury | common unit of pressure; mm Hg; also called 1 torr in honor of Torricelli for his invention of the barometer; 760 mm Hg = 1 atm | |
| 384344498 | atmosphere of pressure | atm | |
| 384344499 | STP | standard temperature and pressure; 1 atm and 0 degrees Celsius | |
| 384344500 | Dalton's law of partial pressures | total pressure of a gas mixture is the sum of the partial pressures of the component gases; PT=P1+P2+P3... | |
| 384344501 | partial pressure of dry gas | Patm=Pgas+PH2O | |
| 384344502 | Boyle's Law, P1V1=P2V2 | volume of a fixed mass of gas varies inversely w/the pressure at constant temperature | |
| 384344503 | Charles' Law, V1/T1=V2/T2 | volume of a fixed mass of gas at constant pressure varies directly w/Kelvin temp | |
| 390171747 | K=273+degrees C | conversion from kelvin to degrees Celsius | |
| 384344504 | Gay-Lussac's Law, P1/T1=P2/T2 | pressure of a fixed mass of gas at constant volume varies directly w/the Kelvin temp | |
| 384344505 | combined gas law, P1V1/T1=P2V2/T2 | relationship between pressure, volume, and temp of fixed amount of gas | |
| 384344506 | Gay-Lussac's law of combining volumes of gases | at constant and temperature, volumes of gaseous reactants and products can be expressed as ratios of small whole numbers | |
| 384344507 | Avogadro's Law, V1/n1=V2/n2 | equal volumes of gases at the same temperature and pressure contain equal numbers of molecules | |
| 384344508 | molar volume of a gas | volume occupied by one mole of gas at STP; 22.4 L | |
| 390171748 | gas stoichiometry | coefficients of gases in chemical equations indicate molar amounts, mole ratios, and volume ratios | |
| 384344509 | ideal gas law, PV=nRT | mathematical relationship among pressure, volume, temp, number of moles of a gas | |
| 390573584 | number of moles | n=mass/molar mass | |
| 384344510 | ideal gas constant; 0.0821 L atm/mol K, 62.4 L mm Hg/mol K, 8.314 L kPa/mol K | R |
