Kinetic Theory

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All things are made of atoms - little particles that move around in perpetual motion, attracting each other when they are a little distance apart, but repelling upon being squeezed into one another. T

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Avogadro's hypothesis states that equal volumes of all gases at equal temperature and pressure have the same number of molecules. Avogadro's number (NA) = 6.02 × 10²³ molecules, which is the number of

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1) PV = μRT (where μ = number of moles, R = universal gas constant) 2) PV = kBNT (where N = number of molecules, kB = Boltzmann constant) 3) P = ρRT/M₀ (where ρ = mass density, M₀ = molar mass)

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Universal gas constant: R = 8.314 J mol⁻¹ K⁻¹ Boltzmann constant: kB = 1.38 × 10⁻²³ J K⁻¹ Relation: R = NA × kB

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Boyle's Law: At constant temperature, PV = constant (pressure varies inversely with volume) Charles' Law: At constant pressure, V ∝ T (volume is proportional to absolute temperature) Both laws are der

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The total pressure of a mixture of ideal gases is the sum of partial pressures: P = P₁ + P₂ + P₃ + ... Where P₁ = μ₁RT/V is the pressure that gas 1 would exert alone at the same temperature and volume

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For a molecule hitting a wall with velocity vₓ: - Momentum change = 2mvₓ - Force on wall = rate of momentum transfer - Considering all molecules: P = (1/3)nm⟨v²⟩ Where n = number density, m = molecula

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The average kinetic energy of a molecule is proportional to absolute temperature: ⟨½mv²⟩ = (3/2)kBT This means temperature is a measure of average molecular kinetic energy, independent of pressure, vo