Thermodynamics of Equilibrium Systems - Revision Sheet

1. 📌 Essentials

• System types: closed (no matter exchange), open (matter exchange), isolated (no energy or matter exchange).
• Equilibrium: no mac change; requires uniform pressure and temperature.
• State variables: extensive (U, V), intensive (p, T); path-independent.
• Equation of State: ideal gas: pV = nRT; Van der Waals: (p + a(n/V)^2)(V - nb) = nRT.
• Transformations: quasi-static, reversible, adiabatic, isenthalpic, isobaric, isochoric.
• Phase transitions: latent heat, critical point, triple point; phases: solid, liquid, gas.
• First law: ΔU = W + Q; energy conservation.
• Cycle: initial and final states identical; net energy change zero.
• Maximum efficiency: Carnot cycle: η = 1 - Tf/Tc.
• Latent heat: energy absorbed/released during phase change (e.g., vaporization ≈ 2257 kJ/kg---

2. 🧩 Key Structures & Components

• System boundary — separates system from surroundings.
• States of matter — solid, liquid, gas.
• Phase diagram — shows phases, coexistence lines, critical point, triple point.
• Equation of State — relates p, V, T for gases.
• Latent heat — energy during phase change at constant T and P.
• Energy forms — internal energy (U), enthalpy (H), kinetic, potential.
• Process types — isothermal, adiabatic, isobaric, isochoric.
• Cycle components — heat source, heat sink, work output.

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