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23 Cards in this Set
- Front
- Back
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Pressure
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force per unit are, that is, a force divided by the area over which the force is distributed
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Pascal(Pa)
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a pressure of one newton per square meter
pressure(Pa) = F(N) / A(m^2) |
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Kilopascal(kPa)
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larger pressure unit than the pascal
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Barometer
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Torricelli, measures the pressure exerted by the atmosphere
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Barometric Pressure
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height of mercury in a barometer, varies with atmospheric conditions and altitude
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Standard Atmosphere(atm)
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the pressure exerted by a mercury column of exactly 760 mm in height when the density of mercury - 13.5951 g/cm3 and the acceleration due to gravity = 9.80665 m s-2
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Torr
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1/760 of a standard atmosphere
1 atm = 760 Torr |
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Manometer
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pressure of the gas to be measured can be compared with barometric pressure using a manometer
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Boyle's Law
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for a fixed amount of gas at a constant temperature, the gas volume is inversely proportional to the gas pressure
V alpha 1/P |
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Charle's Law
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the volume of a fixed amount of gas at constant pressure is directly proportional to the Kelvin (absolute) temperature
V alpha T |
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Avogadro's Law
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at a fixed temperature and pressure, the volume of a gas is directly proportional to the amount of gas
V alpha n |
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Ideal Gas Equation
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those three laws combined into a single equation
V alpha (nT/P) and V = (RnT/P) PV = nRT |
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Ideal/Perfect Gas
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a gas whose behavior conforms to the ideal gas equation
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Gas Constant
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the constant, R
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General Gas Equation
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PiVi / Ti = PfVf / Tf
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Law of Combining Volumes
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the volume of gases involved in a reaction are in the ration of small whole number, which are the stoichiometric coefficients in the balances equation
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Partial Pressure
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each gas expands to fill the container and exerts the same pressure that it would if it were alone in the container
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Dalton's Law of Partial Pressure
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the total pressure of a mixture of gases is the sum of the partial pressures of the components of the mixture
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Mole Fraction
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the fraction of all the molecules in the mixture contributed by that component, the sum of all the mole fractions in a mixture is one
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Kinetic-Molecular Theory of Gases
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1. big # of small particles, move in straight line, random, constant motion
2. mostly empty space 3. most of the time not engaged in collisions 4. no forces, except during collisions, act independently 5. may gain or lose energy in collisions, the total energy remains constant though |
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Root-Mean-Square Speed
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square root of the average of the squares of the speeds of all the molecules in a sample
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Diffusion
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the migration of molecules as a result of random molecular motion
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Effusion
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the escape of gas molecules from their container through a tiny orifice or pinhole
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