AP Chemistry/Gases

=Kinetic Molecular Theory Ideal gases don't exist, but if they did, they would fit the following descriptions: Full of tiny particles that are far apart Neither attract nor repel each other Are constantly and randomly moving, creating pressure Do not lose energy when colliding. Pressure Pressure is measured with a barometer (for atmospheric pressure) or a manometer (for sealed containers of gases). Avogadro's Law One mole of gas particles at STP takes up 22.4L Ideal Gas Equation PV=nRT, where R = 0.0821 L*atm/K*mol = ideal gas constant. Note how if P is in atm, V is in L, n is in moles, and T is in Kelvin, the units cancel out. Remember that these gas laws only work in Kelvin. Graham's Law For every x times heavier a gas is, it travels times slower: Non-Ideal Gases When gases are polar, massive, at high pressure and low temperature, they do not behave like ideal gases. They may even condense into liquids or freeze into solids.