Gas Laws

Boyle's Law

Pressure and volume have an inverse relationship when temperature is constant.

Charles's Law

Volume and temperature have a direct relationship when pressure is constant.

Gay-Lussac's Law

Temperature and pressure have a direct relationship when volume is constant.

Combined Gas Law

Describes the relationship between pressure, volume, and temperature in a gas system.

Avogadro's Law

Moles and volume have a direct relationship in a gas at constant temperature and pressure.

Dalton's Law

The total pressure of a gas mixture is the sum of the partial pressures of each gas in the mixture.

STP

Standard Temperature and Pressure conditions for gases.

Barometer

Instrument used to measure atmospheric pressure, invented by Evangelista Torricelli.

Kinetic Molecular Theory

The average kinetic energy of the gas particles is directly proportional to the kelvin temperature of the gas.

Gas particles description

Gas particles are so small and they are assumed not to attract or repel each other. They are in constant random motion, colliding with the walls of their container. These collisions with the walls cause the pressure exerted by the gas.

Boyle’s Law equation

P₁V₂ = P₁V₁

Charles Law equation

V₁/T₁ = V₂/T₂

Gay-Lussac equation

P₁/T₂ = P₂/T₂

Combined Gas Law equation

P₁V₁/T₁ = P₂V₂/T₂

Avogadro Law equation

V₁/n₁ = V₂/n₂

Dalton’s Law equation

P_total = P₁ + P₂ + P₃ + …

Ideal Gas Law equation

Pv = nRT

R: gas constant = 0.0821 L x atm / mol x K

Stoichiometry

grams A (periodic table) →moles A (coefficients) →moles B (periodic table→grams B

STP measurements

T: 273 K

P: 1.00 atm

How much space does 1 mole of gas occupy at STP

1 mole of a gas occupies 22.4 L