Gas Laws

Boyles Law:

• Temperature must be constant

• Pressure and volume have an inverse relationship

• Equation: P₁V₂ = P₁V₂

Charles Law:

• Pressure must be constant

• Temperature and volume have a direct relationship

• Equation: V₁/T₁ = V₂/T₂

Gay-Lussac Law:

• Volume must be constant

• Temperature and p[pressure have a direct relationship

• Equation: P₁/T₂ = P₂/T₂

Combined Gas Law:

• Equation: P₁V₁/T₁ = P₂V₂/T₂

Avogadro Law:

• Moles and volume have a direct relationship

• n = moles

• Equation: V₁/n₁ = V₂/n₂

Daltons Law:

• The total pressure is the pressure of all the gasses added together

• Equation: P_total = P₁ + P₂ + P₃ + …

Ideal Gas Law:

• Pv = nRT

  • P: atm

  • v: L

  • n: moles

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

  • T: kelvin

• With stoichiometry

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

STP:

• T: 273 K

• P: 1.00 atm

• 1 mole of a gas occupies 22.4 L

The Barometer is used to measure pressure. It was invented by Evangelista Torricelli. Torr was named after him.

Kinetic Molecular Theory;

• Gases consist of tiny particles

• These particles are so small compared with the distance between them, that the volume of the individual particles can be assumed to be zero.

• These particles are in constant random motion, colliding with the walls of the container. These collisions with the walls cause the pressure exerted by the gas.

• The particles are assumed not to attract or repel each other

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