# Phys. Char. of gases

 Kinetic-molecular theory
 the idea that particles of matter are always in motion
 ideal gas
 an imaginary gas that perfectly fits all the assumptions of the kinetic-molecular theory
 elastic collision
 one in which there is no net loss of kinetic energy
 fluid
 the flow of liquids and gases
 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
 real gas
 a gas that does not behave to the assumptions of the kinetic-molecular theory
 pressure
 the force per unit area on a surface
 newton(N)
 the force that will increase the speed of a one kilogram mass by one meter per second each second it is applied
 millimeters of meucury(mm Hg)
 common unit of pressure
 torr
 1 mm Hg
 atmosphere of pressure(atm)
 760 mm Hg
 pascal(Pa)
 the pressure exerted by a force of one newton (1 N) acting on an area of one square meter
 standard temperature and pressure(STP)
 for purposes of comparision standard conditions of exactly 1 atm and 0 degrees
 gas laws
 simple mathematical relationships between the volume, temperture, pressure,and the amount of a gas
 boyle’s law
 states the volume that the volume of a fixed mass of gas varies inversely with the pressure at cconstant temperture
 absolute zero
 the temperture -273.15degrees
 charles’s law
 the volume of a fixedmass of gas at constant pressure varies directly with the kelvin temperture
 barometer
 a device used to measure atmospheric pressure
 gay-lussac’s law
 pressure of a fixed mass of a gas at constant volume varies directly with the kelvin temperture
 combined gas law
 the relationship between pressure, volume, and temperture of a fixed amount of gas
 partial pressure
 pressure of gas in each mixture
 daltons law of partial pressures
 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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