The common unit of pressure, symbolized mm Hg
a unit of pressure: the pressure that will support a column of mercury 760 mm high at sea level and 0 degrees centigrade
a unit of pressure that is nearly, but not quite equal to an atmosphere; 1.013bar = 1atm = 760mm Hg
Ideal Gas Law
Volume is directly proportional to amount. Volume is directly proportional to absolute temperature.Volume is inversly proportional to pressure.
Ideal Gas Equation
Gas constant; 0.0821 (L atm/ mol K), 8.31 (J/ mol K), 8.31x10³ (g m²/ s² mol K)
standard temperature and pressure; EX: At STP, one mole of gas occupies 22.4 L.
the pressure exerted by a vapor over a liquid
The ratio of the moles of the substance to the total moles.
the pressure of each gas in a mixture
passage of a gas through a small hole
Combined Gas Law
P₁V₁/ T₁ = P₂V₂/ T₂
held temperature constant; Equation: P₁V₁ = P₂V₂ (Chickens Go Bawk)
held pressure constant; Equation: V₁/ T₁ = V₂/ T₂ (Chickens Go Bawk)
held volume constant; Equation: P₁/ T₁ = P₂/ V₂ (Chickens Go Bawk)
Equal volumes of gases at the same temperature and pressure contain the same number of particles.
the spreading of a gas through a room.
the total pressure is equal to the sum of its parts.
velocity of gas varies inversley with mass.
the theory that gases are made up of a large sum of small particles.
the gaseous form of any substance
the distance traveled per unit time
a pressure gauge for comparing pressures of a gas
an instrument that measures atmospheric pressure
Kinetic Molecular Theory
-KE is directly proportional to the absolute temperature. -The volume of s gas particle is negligible relative to the volume in which the gas is contained. -Attractive and repulsive forces between gas molecules are negligible. -Gases consist of atoms or molecules in constant, random motion. -At a given temperature, all gases will have the same average KE. -Collisions between gas particles and their container are elastic.