| Lectures and exercises |
hours |
| Topics |
Specific contents |
|
| Mass balances |
Mass balances in simple systems, with ricycle and purge; conversion, yield and selectivity of reactions |
6
|
| Thermodynamics |
The first law: energy, heat and work; internal energy and enthalpy, standard states, heat capacity at costant pressure and volume, reaction enthalpies, laws of Hess and Kirchhoff. The second law: entropy and spontaneous reactions, isothermal reversible expansion of a perfect gas, entropy in a irreversible process, entropy variation with temperature and pressure, standard entropy e third law of thermodynamics; free energies (Gibbs and Helmholtz), maximum non-expansion work, standard free energy, formation free energy; free energy variation with composition, van't Hoff law, Gibbs free energy variation with pressure. Operating conditions evaluation. Hydrocarbon stability and Frances diagram. Chemical potential, real gases, fugacity and coefficient of fugacity. Physical transformation of pure substances: phase diagrams, stability and phase transitions at constant temperature or pressure, phase boundaries. Mixtures: Gibbs-Duhem equation; properties of simply mixtures, partial molar volume and partial molar free energy. Free energy, entropy and enthalpy of mixing of gases. Chemical potential of liquids, laws of Henry and Raoult, solutions properties, free energy, entropy and enthalpy of mixing of solutions, colligative properties, solvent and solute activity (ideal and real solutions). |
16
|
| Phase equilibria |
Phase diagrams: pressure-composition diagrams, the phase rule, 1 or 2 component systems, the lever rule; temperature-composition diagrams; azeotropes, immiscible and partially immiscible liquids. Liquid-liquid diagrams: phase separation, upper and lower critical temperature, distillation of partially miscible liquids. Solid-liquid phase diagrams: eutectics, reacting systems, incongruent melting. 3 component systems, partially miscible liquids. |
4
|
| Chemical kinetics |
The rate of reactions, rate laws and rate costant, reaction order, isolation method, differential and integrated methods. One component irreversible reactions: 1, 2 e 0 orders. Half lives, e second order bimolecular reactions. Transition state theory and the Arrhenius law. Reactions approaching equilibrium, consecutive and parallel irreversible reactions, steady state approximation, reactions with pre-equilibria and homogeneous catalysts. in Batch, CSTR and PFR reactor kinetics: mass balance and conversion; basic reactor sizing and in series reactors. |
11
|
| Catalysis |
Catalytic phenomenon and steps, catalysts classification, synthesis, selectivity, promoters, dopants and poisons. |
3
|
| Total hours for lectures and exercises |
40 |
| for exercises only |
40 |
|
Further educational activities
|
hours
|
| Labs |
|
| Tutorials / Seminars |
|
| Workshops |
|
| Guided tours |
|
| |
|
| Total hours for further educational activities |
0 |
| Total hours |
40
|