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Chemistry
Chapter 14 Definitions
| Term | Definition |
|---|---|
| Boyle's Law | For a given mass of gas at constant temperature, the volume of the gas caries inversely with pressure |
| Charle's Law | The volume of a fixed mass of gas is directly proportional to its Kelvin temperature if the pressure is kept constant |
| Combined Gas Law | The law that describes the relationship among the pressure, temperature of an enclosed gas |
| Compressibility | A measure of how much the volume of matter decreases under pressure |
| 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 |
| Diffusion | The tendency of molecules to move toward areas of lower concentration until the concentration is uniform throughout |
| Effusion | The process that occurs when a gas escapes through a tiny hole in its container |
| Gay-Lussac's Law | The pressure of a gas is directly proportional to the kelvin temperature if the volume is constant |
| Graham's Law of Effusion | The rate of effusion of a gas is inversely proportional to the square root of its molar mass |
| Ideal Gas Constant | The constant in the ideal gas law with the symbol R and the value 8.31 (L*kPa)/ (K*mol) |
| Ideal Gas Law | The relationship PV=nRT, which describes the behavior of an ideal gas |
| Partial Pressure | The contribution each gas in a mixture of gases makes to the total pressure |
| Kinetic Theory | A theory explaining the states of matter, based on the concept that all matter consists of tiny particles that are in constant motion |
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