Ch 10 Vocab - Gases
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diffusion | spontaneous mixing of the particles of two substances caused by their random motion.
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effusion | a process by which gas particles pass through a tiny opening.
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elastic collision | a collision between gas particles and container walls in which there are no net loss of kinetic energy.
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fluid | a substance that can flow and therefore take the shape of its container; a liquid or a gas.
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ideal gas | an imaginary gas that perfectly fits all the assumptions of the kinetic-molecular theory.
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kinetic-molecular theory | a theory based on the idea that particles of matter are always in motion.
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real gas | a gas that does not behave completely according to the assumptions of the kinetic-molecular theory.
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atmosphere of pressure (atm) | exactly equivalent to 760 mm Hg.
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barometer | a device used to measure atmospheric pressure.
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millimeter of mercury (mm of Hg) | a common unit of pressure.
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newton | the SI unit for force; the force that will increase the speed of a one kilogram mass by one meter per second it is applied.
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pascal | the pressure exerted by a force of one newton acting on an area of one square meter.
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kilopascal | 1,000 pascals.
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pressure | the force per unit area on a surface.
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standard temperature and pressure (STP) | the agreed-upon standard conditions of exactly 1 atm pressure and 0oC.
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standard ambient temperature and pressure (SATP) | corresponds to 25oC, 1 bar.
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torr | a pressure equal to 1 mm Hg in honor of Torricelli for his invention of the barometer.
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absolute zero | the temperature -273.15oC, given a value of zero in the Kelvin scale.
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Kelvin | equal to 273.15 + oC.
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Boyle’s Law | states that the volume of a fixed mass of gas varies inversely with the pressure at constant temperature.
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Charles’s Law | the volume of a fixed mass of gas at constant pressure varies directly with the Kelvin temperature.
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Combined gas law | the relationship between the pressure, volume, and temperature of a fixed amount of gas.
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Dalton’s Law of partial pressure | the total pressure of a mixture of gases is equal to the sum of the partial pressures of the component gases.
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Gay-Lusscac’s Law | the pressure of a fixed mass of gas at constant volume varies directly with the Kelvin temperature.
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Ideal gas law | the mathematical relationship of pressure, volume, temperature, and the number of moles of gas.
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Partial pressure | the pressure of each gas in a mixture.
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Avogadro’s Law | 6.0221367x1023; the number of particles in exactly one mole of a pure substance.
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van der Waals equation | the equation that relates real gases to the ideal gas.
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bar | 100kPa or 25oC.
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Gas Constant | R equals 0.082 liter-atmospheres per mole-degree.
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