Course content

Stoichiometry, gass law, chemical equilibria, aqueous equilibria. Acid-base and redox equilibria. Basic chemical thermodynamics, energy, work, heat, entropy, enthalpy, Gibbs energy. Calculations of equilibria from thermodynamical data. Electrochemistry: Reduction potential series, cell voltage, electrolysis, galvanic cells, corrosion and use of Pourbaixdiagrams. Chemical bond. Basic organic chemistry and polymer chemistry. Laboratory exercises give further insight into the following topics: Chemical principles: Stoichiometry, chemical equilibria, chemical kinetics, acids and bases, reduction and oxidation. Quantitative methods: Titration, instrumental methods: pH-electrode, redox reactions, spectrophotometer. A compulsory safety course, including fire prevention and first aid has to be passed in order for admission to the laboratory course. Mandatory exercises where several tasks are related to sustainability from a chemical perspective.

Learning outcome

The most important learning outcomes in this course is associated with quantitative treatment of aqueous equilibria and the relation between Gibbs energy and equilibrium constants and electrode potentials, as well as the ability to combine theory with concrete issues. The student can upon successful course completion: - Identify the most important inorganic acids, bases, salts and ions and know the most important reactions between these. - Describe different types of chemical bonding, how they occur and connections with the properties of the substances. - Explain the shape and name of the atom orbitals, and be able to see properties in relation to the periodic table. -Be able to explain important environmental problems related to inorganic chemistry. - Balance chemical reactions and perform stoichiometric calculations. - Perform calculations with reaction equilibria, including calculation of pH, solubility, complex ion formation and other heterogeneous reactions. - Carry out simple thermodynamic calculations founded on knowledge on entropy, enthalpy and Gibbs energy and be able to relate these to chemical equilibrium - Account for the relation between equilibrium constant, Gibbs' free energy, and electrode potential, and for a simplified derivation of these relations. - Principles for galvanic cells (batteries, fuel cells) and electrolysis and recognize industrial electrolysis processes. - Calculate cell potentials in electrochemical cells from Gibbs' free energy, from standard electrode potential and from the Nernst equation, including concentration cells. - Explain the connection, and perform calculations of potential/voltage for electrochemical cells from Gibbs energy, from standard electrode potential and from Nernst equation, including concentration cells and potentiometric sensors. - Explain basic reaction kinetics - Explain the basic principles, compounds and reactions in organic chemistry. - In the laboratory work, the students are supposed to obtain a deeper understanding of the principles through the experiments, and be trained in working accurately.

Learning methods and activities

Lectures, written exercises and laboratory work.

Expected time consumption:

Lectures: 56 hours

Exercises: 40 hours

Laboratory: 50 hours

Self study: 56 hours

Total: 202 hours

Compulsory assignments

• Laboratory couse
• Exercises

Specific conditions

Recommended previous knowledge

Knowledge of the more important elements and chemical compounds is expected. Also the understanding of chemical formulas and equations, the concepts of atoms, molecules, and moles. Calculations with logarithms and exponents should be mastered.

Course materials

R. H. Petrucci, G. G. Herring, J. D. Madura and C. Bissonnette, "General Chemistry. Principles and Modern Applications", 12. ed., Pearson, Toronto (2024).

A. Blackman and L. R. Gahan, Aylward & Findlay's SI Chemical Data, 7. utg., Wiley, 2014.

"TMT4110/TMT4115 Laboratoriekurs i generell kjemi" will be made available to the students.

Credit reductions