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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