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22 Cards in this Set
- Front
- Back
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Based on the idea that particles of matter are always in motion
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Kinetic-molecular theory
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An imaginary gas that perfectly fits all the assumptions of the kinetic-molecular theory.
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Ideal gas
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A collision between gas particles and between particles and container walls are elastic collisions where there is no net loss of kinetic energy.
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Elastic collision
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Spontaneous mixing of the particles of two substances caused by their random motion.
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diffusion
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A gas that does not behave completely according to the assumptions of the kinetic-molecular theory.
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real gas
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The force per unit area on a surface.
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pressure
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The force that will increase the speed of a one kilogram mass by one meter per second each second it is applied. abbreviated N.
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Newton.
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A device used to measure atmospheric pressure. Invented by Torricelli.
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barometer
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Common unit of pressure. symbolized mm Hg. Pressure that supports a 1 mm mercury column in a barometer.
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millimeters of mercury
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being exactly equivalent to 760 mm Hg
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Atmosphere of pressure (atm)
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The pressure exerted by a force of one newton acting on an area of one square meter.
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pascal (Pa)
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1 atm pressure and 0 degrees celcius. Standard conditions are agreed upon by scientists for comparison.
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Standard temperature and pressure
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simple mathematical relationships between the volume, temperature, pressure, and quantity of a gas
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gas laws
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The volume of a fixed mass of gas varies inversely with the pressure at constant temperature.
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Boyle's law
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-273 degrees celcius. 0 degrees in Kelvins.
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absolute zero
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The volume of a fixed mass of gas at constant pressure varies directly with the Kelvin temperature.
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Charles's law
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The pressure of a fixed mass of gas at constant volume varies directly with the Kelvin temperature.
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Gay-Lussac's Law
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Expresses the relationship between pressure, volume, and temperature of a fixed amount of gas.
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Combined gas law
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The pressure of each gas in a mixture.
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Partial Pressure
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The total pressure of a mixture of gases is equal to the sum of the partial pressure of the component gases.
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Dalton's law of partial pressures.
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Gasses and liquids because they both flow
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fluids
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A process by which gas particles under pressure pass through a tiny opening
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effusion
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