Kinetic Theory of Gases and Radiation

Gas molecules are in continuous random

Gas molecules are in continuous random motion, behaving as point masses with negligible intermolecular forces except during collisions. Collisions are

PV = nRT (or PV =

PV = nRT (or PV = NkₐT) derived from kinetic theory gives P = (1/3)(N/V)mv̄². This connects pressure to molecular motion where v̄² represents mean squ

vᵣₘₛ = √(3RT/M₀) = √(3kₐT/m) shows

vᵣₘₛ = √(3RT/M₀) = √(3kₐT/m) shows that molecular speed increases with temperature and decreases with molecular mass. Average kinetic energy per molec

λ = 1/[√2πd²(N/V)] represents average distance

λ = 1/[√2πd²(N/V)] represents average distance traveled by molecules between collisions. Depends inversely on gas density and molecular diameter. High

Each quadratic degree of freedom contributes

Each quadratic degree of freedom contributes (1/2)kₐT to average molecular energy. Monatomic gases have 3 translational DOF, diatomic gases have 5 DOF