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In: Computers and Technology

Submitted By meme72
Words 840
Pages 4
Matter exists in three different states depending on how much energy they have (measured by temperature). solid liquid gas

Pressure – continual bombardment on the walls of a container by gas molecules in rapid, random motion
Two units used to measure pressure:
1. millimeters of mercury (mm Hg)
2. atmospheres (atm)
1 atm = 760 mm Hg barometer – instrument used to measure atmospheric pressure

manometer – instrument used to measure pressure of a gas in a container

Boyle’s Law – for a fixed mass of an ideal gas at constant temperature, the volume of the gas is inversely proportional to the applied pressure.

P1V1 = P2V2

Charles’s Law – the volume of a fixed mass of an ideal gas at a constant pressure is directly proportional to the temperature in kelvins (K). V1 = V2 T1 = T2
Gay-Lussac’s Law – for a fixed mass of a gas at constant volume, the pressure is directly proportional to the temperature in kelvins (K). P1 = P2
Combined Gas Law – P1V1 = P2V2 T1 T2

Avogadro’s Law – equal volumes of gases at the same temperature and pressure contain equal numbers of molecules. standard temperature and pressure (STP) = 0 °C (273 K) and 1 atm
One mole of any gas at STP occupies a volume of 22.4 L.
Ideal Gas Law: PV = nRT P = pressure of gas (atm) V = volume of gas (L) n = amount of gas (moles) T = temperature of gas (K) R = ideal gas constant (0.0821 L x atm/mole x K
Dalton’s law of partial pressures:
The partial pressure of a gas in a mixture is the pressure that gas would exert if it were alone.
The total pressure (PT) of a mixture of gases is the sum of the partial pressures of each individual gas:
PT = P1 + P2 + P3 + . . .

Kinetic molecular theory:
1. Gases consist of particles…...

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