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 $$ \sqrt{x} $$ times slower:

$$ \frac{v_2}{v_1} = \sqrt{\frac{MM_1}{MM_2}} $$

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.