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Chapter 6 — Chapter 6 — Heat and Thermodynamics
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📘Easy summary
Postulates of kinetic theory: a gas consists of a very large number of tiny molecules in constant random motion; their size is negligible compared with the distance between them; collisions with each other and the walls are perfectly elastic; there are no intermolecular forces except during collisions; the time of collision is negligible; the average K.E. of molecules is proportional to the absolute temperature. Gas laws: Boyle's law PV = constant (T constant); Charles's law V/T = constant (P constant); pressure law P/T = constant (V constant). Combined: PV/T = constant → PV = nRT = Nk_BT, where k_B = R/N_A = 1.38 × 10⁻²³ J K⁻¹. Real gases deviate from ideal at high pressure and low temperature because molecular volume and intermolecular attractions become significant.
⭐Key points
- Elastic collisions, random motion.
- PV = nRT = Nk_BT.
- k_B = 1.38 × 10⁻²³ J K⁻¹.
🔬Diagram
🌿Real-life example
6.0 L at 12 atm → 14 atm: V = 72/14 = 5.14 L.
💡Exam tip
- Always use kelvin in gas law calculations.
✅Quick check
1. Boltzmann constant:
2. Real gases deviate at:
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