1. komponenta

Lecture type	Total
Lectures	60
Seminar	30

* Load is given in academic hour (1 academic hour = 45 minutes)

COURSE CONTENT:
Thermodynamics and temperature. First low: heat and work. Enthalpy. Extent of chemical reactions and stoichiometry. Reaction enthalpy. Thermochemistry. Calorimetry. Temperature dependency of enthalpy. Adiabatic isothermal work. Irreversibility and entropy. Probability and entropy. Entropy of mixing. Thermodynamic potentials. Gibbs energy. G(p) i G(T) functions. Phase equilibrium. Phase diagrams. Partial molar quantities. Chemical potential. Colligative properties: cryoscopy and ebullioscopy. Osmosis. Mixtures. Standard states. Relative activity. Chemical equilibrium. Solutions. Electrochemistry. Electrolyte solutions. Conductivity. Electrochemical cells. Nernst equation. Chemical kinetics. Rate lows and rate constants. Reaction mechanisms. Temperature dependency of reaction rates. Theory of reaction rates. Catalysis. Enzymes.

LEARNING OUTCOMES:
- Describe and explain changes of energy during chemical reactions and physical processes
- Explain the criteria for a chemical reaction and physical process to be classified as spontaneous
- Apply the chemical thermodynamics on chemical equilibrium and quantitatively describe chemical equilibrium
- Describe the general features of the ion-ion interactions in aqueous electrolyte solutions
- Explain the molar conductivity of electrolyte solutions
- Describe the processes in galvanic and electrolytic cells
- Define the rate of chemical reaction and rate laws
- List and explain the parameters influencing the rate of chemical reactions
- Use the physical and chemical models to describe the state od systems and changes occurred during chemical reactions
- Apply the standard mathematical methods for solving physical-chemical problems and data analysis

1. P. W. Atkins i J. De Paula, Physical Chemistry, 8. izd., W H Freeman & Co, 2014., ili prijašnja izdanja.
2. T. Cvitaš, I. Planinić, N. Kallay, Rješavanje računskih zadataka u kemiji II dio, Hrvatsko kemijsko društvo, Zagreb, 2014.
3. T. Cvitaš, I. Planinić, N. Kallay, Rješavanje računskih zadataka u kemiji I dio, Hrvatsko kemijsko društvo, Zagreb, 2014.
4. T. Cvitaš, Fizikalna kemija, rukopis u pripremi.
5. T. Cvitaš i N. Kallay, Fizičke veličine i jedinice međunarodnog sustava, Školska knjiga, Zagreb, 1980.
6. V. Simeon, Termodinamika, rukopis u pripremi.
7. P. W. Atkins, J. de Paula: Atkins' Physical Chemistry, 10. izd., Oxford University Press, Oxford, 2014.
8. I. N. Levine: Physical Chemistry, 6. izd., McGraw Hill, New York 2009.
9. R. J. Silbey, R. A. Alberty, M. G. Bawendi: Physical Chemistry, 4. izd., Wiley, New York 2004.
10. N. Kallay, T. Preočanin, V. Tomišić, Osnove fizikalne kemije (predavanja), skripta za internu upotrebu, Zagreb, 2012.

Enrollment :
Passed : Mathematics 2
Passed : Physics 2
Attended : Physical Chemistry 1

Examination :
Passed : Physical Chemistry 1

Mandatory course - Regular study - Biology and Chemistry Education