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| 5243268941 | Gas Pressure | the force that a gas exerts on the walls of its container. | 0 | |
| 5243274129 | Boyle's Law | If the number of moles of a gas and temperature are held constant, the pressure and volume of an ideal gas have an inverse relationship. PV = k and P1V1 = P2V2 (Units of volume and pressure must be the same, k is a proportionality constant.) | 1 | |
| 5243286444 | Charles's Law | If the number of moles of a gas and pressure are held constant, the volume of an ideal gas is directly proportional to temperature. V/T = b and V1/T1 = V2/T2 (Temp in Kelvin, b is a proportionality constant.) | 2 | |
| 5243298571 | Avogadro's Law | At constant temperature and and pressure, the volume of an ideal gas is directly proportional to the number of moles of gas. V/n = a and V1/n1 = V2/n2 (n is equal to the number of moles, a is a proportionality constant.) | 3 | |
| 5243310845 | Universal gas constant | 0.08206 (L*atm)/(K*mol) The gas constant will change based on the unit of pressure. | 4 | |
| 5243315714 | Ideal Gas Law | PV = nRT An equation of state for a gas at a given period of time. This is a limiting law, as it is not always true for all gases. | 5 | |
| 5243319259 | Ideal Gas | A gas that follows the ideal gas law. An ideal gas is a hypothetical substance. Real gases behave "ideally" at low pressures (below 1 atm) and high temperatures. | 6 | |
| 5243331976 | Molar Volume of an Ideal Gas | 22.4L | 7 | |
| 5243335197 | STP | Standard Temperature and pressure, 1atm and 0C | 8 | |
| 5243337841 | Dalton's Law of Partial Pressure | For a mixture of gases in a container, the total pressure exerted is the sum of the pressure that each gas would exert if it were alone. Total Pressure = P1 + P2 + P3 + ....Pn | 9 | |
| 5243340625 | Partial Pressure | The pressure that a particular gas would exert if it were alone in the container. | 10 | |
| 5243345506 | Mole Fraction | The ratio of the number of moles of a given component in a mixture to the total number of moles in the mixture. | 11 | |
| 5243350567 | Kinetic Molecular Theory | A simple model that attempts to explain the properties of an ideal gas. | 12 | |
| 5243352482 | Diffusion | term used to describe the mixing of gases | 13 | |
| 5243355100 | Graham's Law of Effusion | (Rate of Effusion for gas 1)/(Rate of effusion for gas 2) = (Square root of the molar mass of gas 2)/(Square root of the molar mass of gas 2) | 14 | |
| 5243360212 | Effusion | term used to describe the passage of gas through a tiny orifice into an evacuated chamber. | 15 | |
| 5243364373 | Real gas | A gas that does not follow the ideal gas law. | 16 |
