Gases

Boyles Law
Pressure X Volume = Constant
At constant temperature and moles, the volume of a gas is inversely proportional to its pressure.
Charles Law
Volume / Temperature = Constant
At constant pressure the volume of a gas is directly proportional to the temperature in kelvin.
Avogadros Law
Volume / Moles = Constant
At constant temperature and pressure the volume of a gas is directly proportional to the number of its moles.
Ideal Gas Law
Pressure X Volume = Moles X Universal Gas Constant X Temperature
Daltons Law
Mole Fraction of a Gas = Partial Pressure
Kinetic Molecular Theory
1. Gas is tiny particles. 2. The volume of the particles is assumed to be zero. 3. The particles are in random motion, colliding with the walls causing the pressure. 4. The particles do not attract or repel each other. 5. Average kinetic energy is directly proportional to the kelvin temperature of the gas.
Gay-Lussacs Law
Pressure / Temperature = Constant
At constant temperature and pressure, the volumes of gaseous reactants and products can be expressed as ratios of small whole numbers
Avogadros Hypothesis
Different gases at same volume, pressure and temperature contain same number of moles.
Universal Gas Constant (R)
.0821 L X atm / mole X temperature
Ideal Gas
A hypothetical gas that obeys the ideal gas equation is said to be an ideal gas. An ideal gas should have zero volume and have no attraction for each other.
Real Gases
A real gas is opposite of an ideal gas. However, a real gas can behave as an ideal gas at low pressures and high temperature, thus obeying PV = nRT.
A real gas differs from an ideal gas when a real gas is compressed or cooled.
Combined Gas Law
Pressure X Volume / Temperature = Moles X Universal Gas Constant OR Constant
x

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