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23 Cards in this Set
- Front
- Back
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Pressure |
Force exerted per unit of surface area |
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Barometer |
Device used to measure atmospheric pressure |
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Manometer |
Device used to measure the pressure of gas in an experiment |
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Standard atmosphere |
The average atmospheric pressure measured at sea level and 0'C |
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Ideal gas |
A gas that exhibits linear relationships among volume, pressure, temperature, and amount |
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Boyle's law |
At constant temperature, the volume occupied by a fixed amount of gas is inversely proportional to the applied (external) pressure |
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Charles's law |
At constant pressure, the volume occupied by a fixed amount of gas is directly proportional to its absolute (Kelvin) tempurature |
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Avogadro's law |
At fixed temperature and pressure, equal volumes of any ideal gas contain equal numbers (or moles) of particles |
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Standard temperature and pressure (STP) |
A baseline of standard conditions (0'C and 1 atm) |
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Standard molar volume |
The volume of one mole of an ideal gas (22.4L) |
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Ideal gas law |
PV=nRT |
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Partial pressure |
The pressure of a gas in a mixture |
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Dalton's law of partial pressures |
In a mixture of unreacting gases, the total pressure is the sum of the partial pressures of the individual gases |
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Mole fraction (X) |
A fraction of the total number of moles in a mixture for each component |
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Kinetic-molecular theory |
A model that accounts for macroscopic gas behavior at the level of individual particles 1. particle volume is essentially deep 2. Particles are in constant, random, straight-line motion except when they collide 3. Collisions are elastic (frictionless, total kinetic energy remains constant) |
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Root-mean-square speed (rms speed) |
A particle moving at this speed has the average kinetic energy |
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Effusion |
The process by which a gas escapes through a tiny hole in its container into an evacuated space |
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Graham's law of effusion |
The rate of effusion of a gas is inversely proportional to the square root of its molar mass |
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Diffusion |
The movement of one gas through another |
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Mean free path |
The average distance a particle travels between collisions at a given temperature and pressure |
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Collision frequency |
The average number of collisions per second that each particle undergoes |
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Can see Waals equation |
Accounts for the behavior of real gases, at ordinary conditions it becomes the ideal gas equation |
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Van der Waals constants |
Experimentally determined and specific for a given gas, (a and b) |
