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Unit 5: Gases

3U Chemistry

inversely proportional as the independent variable increases, the dependent variable decreases
bombarding gases exert pressure on the sides of their container because they have high kinetic energy
weak IMFs gases are separated by a lot of space, so have weak intermolecular forces. All this space also makes gases highly compressible.
Intermolecular forces solids are separated by very small amount of space, so have strong intermolecular forces.
Boyle's Law Pressure and volume are inversely proportional .
Charles' Law Volume and temperature are proportional to each other. As KE increases, the particles take up more space!
-273.15 K = Absolute Zero The temperature at which a gas theoretically takes up zero volume. OR the temperature at which all molecular movement stops.
Gay-Lussac's Law Pressure and temperature are proportional to each other
Avogadro’s Law Moles of gas and volume of gas are proportional to each other
STP 101.325 kPa; 0 oC; 22.4 L per mole
SATP (room conditions): 100 kPa; 25 oC; 24.8 L per mole
Ideal Gas Law P and V are directly proportional to n, R and T as they are on opposite sides of the equation
Dalton's Law The total pressure exerted by a mixture is equal to the sum of the partial pressures each gas in the mixture (Ptotal=P1+P2+...)
barometer device that measures air pressure (in Canada, our weather reports include air pressure in kPA).
Combined Gas Law The combined gas law analyses pressure, temperature and volume when none are held constant
solubility of gases is inversely proportional to temperature. Cold water holds more dissolved gases because their KE is lower so they don't pop out of solution as readily.
Created by: jcepella