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STUDY GUIDE · GKU 4

Thermodynamics study guide (Chemical Engineering)

Thermodynamics tells a chemical engineer how much energy a step needs, how far a separation or a reaction can go, and which design claims are impossible. This guide starts with the properties of real fluids: equations of state, the compressibility factor, steam tables and phase diagrams. It then applies the first and second laws to the processes and cycles found in plants, and computes heats of reaction and of mixing. The second part turns to equilibrium: vapour–liquid equilibrium with Raoult's law, activity coefficients and Henry's law; liquid–liquid splitting; and chemical-reaction equilibrium through the equilibrium constant and the extent of reaction.

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Structured by the official ETEC subject standard for this topic: every listed topic and learning outcome, with formulas, figures and worked examples. The full sections are available to members in the app.

SKU 4.1 · Ideal gases, pure substances and mixtures

  1. Properties of pure fluids and mixtures; equations of state

    The state functions , , , and , the ideal gas and how real gases depart from it (compressibility factor, virial and cubic equations), and how mixing changes the properties of a mixture.

  2. Property data, steam tables and phase diagrams

    Reading phase diagrams and steam tables, the quality of a wet mixture, the phase rule, vapour-pressure equations (Clapeyron, Clausius–Clapeyron, Antoine) and the generalized compressibility chart.

  3. The first and second laws

    Energy balances for closed systems and steady-flow equipment, the entropy balance and entropy generation, and how the volumetric behaviour of a fluid (––) enters the work terms.

  4. Isothermal, adiabatic, isentropic and phase-change processes

    Simple models for the processes met in compressors, expanders, vessels and boilers: work, heat and outlet temperature for ideal gases along isothermal, isentropic and polytropic paths, real machines through an isentropic efficiency, and phase change at constant pressure.

  5. Cycles and their efficiencies

    Heat engines, refrigerators and heat pumps: the Carnot limits, the Rankine steam cycle and the vapour-compression refrigeration cycle, worked from enthalpy data.

  6. Heat of reaction and heat of mixing

    Standard heats of reaction from heats of formation (Hess's law), their correction to the reactor temperature (Kirchhoff), and the heat released or absorbed when liquids are mixed or a solute is dissolved.

SKU 4.2 · Thermodynamic equilibria

  1. Vapour–liquid equilibrium

    The equilibrium criterion (equal fugacities), Raoult's law and its modified form with activity coefficients, Henry's law for dissolved gases, bubble and dew points, the isothermal flash and azeotropes.

  2. Liquid–liquid equilibrium and extraction

    Why some liquids split into two phases, the stability test on the Gibbs energy of mixing, equal activities in the two liquids, the lever rule, and the distribution coefficient used for extraction.

  3. Chemical-reaction equilibrium

    The equilibrium constant from the standard Gibbs energy change, its dependence on temperature (van 't Hoff), the extent of reaction, and how pressure, inerts and feed ratio shift the equilibrium conversion.

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