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# Jade Davis Ch 10 voc

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diffusion   spontaneous mixing of the particles of two substances caused by their random motion
effusion   a process by which gas particles pass through a tiny opening
elastic collision   a collision between gas particles and between gas particles and container walls in which there is no net loss of kinetic energy
fluid   a substance that can flow and therefore take the shape of its container, a liquid or a gas
ideal gas   an imaginary gas that perfectly fits all the assumptions of the kinetic molecular theory
kinetic-molecular theory   a theory based on the idea that particles of matter are always in motion
real gas   a gas that does not behave completely according to the assumption os the kinetic molecular theory
atmosphere of pressure (atm)   exactly equivalent to 760 mm Hg
barometer   a device used to measure atmospheric pressure
millimeter of mercury (mm of Hg)   a common use of pressure
newton   the SI unit for force, the force that will increase the speed of a one kilogram mass by one meter per second each second it is applied
pascal   the pressure exerted by a force of one newton acting on an are of one square meter
kilopascal   equal to 1.013 x 10 ^5
pressure   the force per unit area on a surface
standard temperature and pressure (STP)   the agreed upon standard conditions of exactly 1 atm pressure and 0 degrees cecius
standard ambient temperature and pressure (SATP)   equal to one bar
torr   equal to 1 mm Hg
absolute zero   the temperature -273.15 degree Celsius given a value of 0 in the kelvin scale
Kelvin   the temperature at which all thermal motion ceases
Boyle’s Law   the volume of a fixed mass of gas varies inversely with pressure at constant temperature
Charles’s Law   the volume of a fixed mass of gas at constant pressure varies directly with the kelvin temperature
Combined gas law   the relationship between the pressure, volume, and temperature of a fixed amount of gas
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
Gay-Lusscac’s Law   the pressure of a fixed mass of gas at constant volume varies directly with the kelvin temperature
Ideal gas law   the mathmatical relationship of pressure volume temperature and the number of moles of a gas
Partial pressure   the pressure of each gas in a mixture
Avogadro’s Law   equal volumes of gases at the same temperature and pressure contain equal numbers of molecules
van der Waals equation   equation that relates the behavior of real gases to those of ideal gases
bar
Gas Constant

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