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Physical chemistry 2

Code: 41014
ECTS: 8.0
Lecturers in charge: prof. dr. sc. Vladislav Tomišić - Lectures
Lecturers: Nikola Bregović - Seminar
Take exam: Studomat

1. komponenta

Lecture typeTotal
Lectures 60
Seminar 45
* Load is given in academic hour (1 academic hour = 45 minutes)
Chemical thermodynamics: Postulates of phenomenological thermodynamics (laws: 0, I, II). Isothermal thermodynamic potentials: Helmholtz (A) and Gibbs (G) energies. Heat capacity. Temperature dependence of U, H, S and G. Experimental methods of phenomenological thermodynamics: thermometry, calorimetry. Multicomponent systems. Chemical potential. Standard states of components; relative activity. Dependence of the activity on chemical composition: activity coefficients. Partial pressure, fugacity. Partial molar quantities. Gibbs-Duhem equation. Dependence of Gibbs energy on the extent of reaction. Standard and empirical equilibrium constant. Temperature dependence of equilibrium constant. Phase change; phase equilibrium; transition enthalpy; dependence of chemical potential on p and T; Gibbs phase rule. Ideal and real liquid mixtures. Equilibrium of binary liquid mixture with its vapour. Ideal dilute solution, Henry's law. Real solutions. Colligative properties. Electrochemistry: Electrolytes. Electrical conductivity of strong and weak electrolytes. Conductometry. Ion migration in electrical field; ionic mobility; transference number. Electroneutrality principle: average ionic activities. Debye & Hückel theory of dilute electrolyte solutions. Equilibria in the solutions of weak electrolytes. Galvanic cells. Electromotivity and work of a galvanic cell. Nernst equation. Standard electromotivity. Electrode potential. Electrodes of first and second kinds, redox electrodes, glass electrode. Definition and measurement of pH. Potentiometric titration. Chemical kinetics: Simple radioactive decay. Rate of chemical change; order of reaction, rate coefficient. Molecularity of an elementary reaction. Simple reaction mechanisms: consecutive, parallel and reversible reactions; preequilibrium. Temperature dependence of reaction rate coefficients; Arrhenius' equation. Collision theory. Transition-state theory. Primary salt effect. Catalysis; heterogeneous, homogeneous. Enzyme catalysis.

1. To qualitatively and quantitatively describe isotermic thermodynamic potentials (Helmholtz and Gibbs energies) and their pressure and temperature dependence (Gibbs-Helmholtz equation).
2. To define partial molar quantities and chemical potential. To desribe dependence of the reaction Gibbs energy on the extent of reaction.
3. To define relative activity, activity coefficient, as well as thermodynamic and stoichiometric equilibrium constants. To describe and explain temperature dependence of the equilibrium constant (van't Hoff equation).
4. To qualitatively and quantitatively describe phase changes and coligative properties.
5. To state the laws which define electrical conductivities of strong and weak electrolyte solutions. To describe how the electrical mobility and molar conductivity of ions depends on ionic and medium properties. To describe and explain basic principles of Debye-Hückel theory of electrolyte solutions.
6. To explain the principles of the working of Galvanic cells. To derive Nernst equations and apply it to different electrochemical cells.

7. To define the electrode potential and to state the types of electrodec and their applications.
8. To define the rate of chemical reaction and rate law (order of reaction, rate coefficient). To describe temperature dependence of reaction rate coefficient (Arrhenius equation).
9. To qualitatively and quantitatively describe simple reaction mechanisms, basic principles of collision and transition-state theories and catalysis.
10. To solve numerical problems from the fields of Chemical Thermodynamics, Electrochemistry and Chemical Kinetics.
  1. 1. P. W. Atkins, J. de Paula, Atkins' Physical Chemistry, 7. izd., Oxford University Press, Oxford 2002.
    2. R.J. Silbey, R. A. Alberty, M. G. Bawendi, Physical chemistry, 4. izd., Wiley, New York 2004.
    3. I. N. Levine, Physical chemistry, 4. izd., McGraw Hill, New York 1995.
    4. G. M. Barrow, Physical chemistry, 6. izd., McGraw Hill, New York 1996.
    5. T. Cvitaš, Fizikalna kemija, rkp. (primjerak za studentsku uporabu nalazi se u CKB).
    6. Vl. Simeon, Termodinamika, Školska knjiga, Zagreb 1980.
    7. Vl. Simeon, Kemijska termodinamika, 2. izd., rkp. (primjerak za studentsku uporabu nalazi se u CKB)
    8. Vl. Simeon, V. Tomišić, Kem. Ind. 45 (1996) 61.
  2. T. Cvitaš, Fizikalna kemija, rkp. {primjerak za studentsku uporabu nalazi se u CKB [c/o Branka Maravić]}
  3. Vl. Simeon, Termodinamika, Školska knjiga, Zagreb, 1980.
  4. Vl. Simeon, Kemijska termodinamika, 2. izd. [st80], rkp. {primjerak za studentsku uporabu nalazi se u CKB [c/o Branka Maravić]}
  5. Vl. Simeon i V. Tomišić, Kem. Ind. 45 (1996) 61.
  6. S. Ašperger: Chemical Kinetics and Inorganic Reaction Mechanisms, 2. izd., Kluwer Academic / Plenum, New York 2003.
  7. R. S. Berry, S. A. Rice, J. Ross: Physical Chemistry, 2. izd., Oxford University Press, New York ? Oxford 2000.
Prerequisit for:
Examination :
Passed : Physical chemistry 1
4. semester
Mandatory course - Mandatory studij - Chemistry
Consultations schedule: