Chapter 6. Gases and the States of Matter

Gas laws (temperature in kelvin) [1][5]:

Boyle: P₁V₁ = P₂V₂ (constant n, T)

Charles: V₁/T₁ = V₂/T₂ (constant n, P)

Combined: P₁V₁/T₁ = P₂V₂/T₂

Ideal gas law: PV = nRT, with R = 0.08206 L·atm·mol⁻¹·K⁻¹ or 8.314 J·mol⁻¹·K⁻¹

Dalton: P_total = ΣPᵢ

Kinetic molecular theory. Gas particles are in constant random motion, and average kinetic energy is proportional to absolute temperature. Real gases deviate from ideality at high pressure and low temperature (van der Waals equation) [4].

Liquids and solids. Properties reflect intermolecular forces: viscosity, surface tension, vapor pressure. Solids may be crystalline (ionic, molecular, covalent network, metallic) or amorphous. Phase diagrams show the stable phase at each pressure and temperature, including the triple and critical points [2].

Review: What volume does 1.00 mol of ideal gas occupy at 273.15 K and 1 atm? (About 22.4 L.)