Terms : Hide Images
| 174051160 | pressure | 1)the force applied to a unit area of surface 2)the amount of force exerted per unit area of a surface | |
| 174051161 | newton | 1)a unit of force equal to the force that imparts an 2)acceleration of 1 m/sec/sec to a mass of 1 kilogram the SI unit of force | |
| 174051162 | barometer | 1)an instrument that measures atmospheric pressure, 2)measures air pressure | |
| 174051163 | millimeters of mercury | 1)a unit of pressure, 2)a common unit of pressure | |
| 174051164 | atmosphere of pressure | 1)the pressure of Earth's atmosphere at sea level;exactly equivalent to 760 mm Hg, 2)exactly equivalent to 760 mm Hg | |
| 174051165 | pascal | 1)a unit of pressure equal to one newton per square meter, 2)the SI unit of pressure | |
| 174051166 | partial pressure | 1)the pressure of each gas in a mixture, 2)the contribution each gas in a mixture of gases makes to the total pressure | |
| 174051167 | dalton's law of partial pressures | 1)states that the total pressure of a mixture of gases is equal to the sum of the pressures of all the gases in the mixture, 2)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 | |
| 174051168 | boyle's law | 1)The relationship between the pressure and volume of a gas at constant temperture; when volume increase, pressure decreases., 2)describes the inversely proportional relationship between the absolute pressure and volume of a gas, if the temperature is kept constant within a closed container | |
| 174051169 | absolute zero | 1)The coldest temperature, 0 Kelvin, that can be reached. It is the hypothetical temperature at which all molecular motion stops., 2)the temperature at which no more energy can be removed from matter | |
| 174051170 | Charles's law | 1)the law that states that for a fixed amount of gas at a constant pressure, the volume of the gas increases as the temperature of the gas increases and the volume of the gas decreases as the temperature of the gas decreases, 2)A principle that describes the relationship between the temperature and volume of a gas at constant pressure | |
| 174051171 | Gay-Lussac's law | 1)the pressure of a fixed mass of gas at constant volume varies directly with the Kelvin temperature, 2)P1/T1=P2/T2 | |
| 174051172 | combined gas law | 1)P1V1/T1=P2V2/T2, 2)the relationship between the pressure, volume, and temperature of a fixed amount of gas | |
| 174051173 | Gay-Lussac's law of combining volumes of gases | 1)at constant temperature and pressure, the volumes of gaseous reactants and products can be expressed as ratios of small whole numbers, 2)the law that states that the volumes of gases involved in a chemical change can be represented by a ratio of small whole numbers | |
| 174051174 | Avogadro's Law | 1)the law that states that equal volumes of gases at the same temperature and pressure contain equal numbers of molecules, 2)Equal volumes of gases contain the same number of molecules | |
| 174051175 | standard molar volume of a gas | 1)the volume occupied by one mole of a gas at STP 2)22.4 L | |
| 174051176 | ideal gas law | 1)PV = nRT, 2)law that states the math relationship of pressure (P), volume (V), temperature (T), the gas constant (R), and the number of moles of a gas (n) | |
| 174051177 | ideal gas constant | 1)the constant in the ideal gas law with the symbol R and the value is 8.31 (L*kPa)/(K*mol), 2)an experimentally determined constant whose value in the ideal gas equation depends on the units that are used for pressure | |
| 174051178 | Graham's law of effusion | 1)states that the rate of effusion for a gas is inversely proportional to the square root of its molar mass, 2)The rate of effusion for a gas is inversely proportional to the square root of its molar mass |
