Course content

Fundamental terms in chemistry: amount of substance, concentration, and stoichiometry. Nomenclature of chemical compounds. Fundamental results from quantum chemistry: atomic orbitals and the principle behind the periodic table of the elements. Properties of gasses: units of pressure, vapour pressure, ideal gas, Daltons law. Chemical equilibrium: law of mass action, acid- and base equilibrium, buffer solutions, solubility and precipitation reactions. Formation of complexes. Fundamental thermochemistry and chemical thermodynamics: work and heat, internal energy, enthalpy, entropy, and Gibbs' energy. Electrochemistry: Galvanic cells, standard electrode potential, Nernst equation, and the relationship between electrochemistry and chemical thermodynamics, corrosion, and an introduction to Pourbaix diagrams, Faradays law, and speed of corrosion.

The course emphasises general aspects of chemistry, and form the basis for further studies in engineering study programs.

Part 1:

• Gas (ideal gas law and Daltons law)
• Mole
• How to balance chemical reactions
• The periodic table of the elements, basics and trends
• Chemical compounds
• Nomenclature
• The atom
• Chemical bonds, inter- and intra molecular), including electronegativity and Lewis structures, polarity and VSEPR.
• Organic chemistry
• Environmental chemistry

Part 2:

• Chemical equilibrium
  • Law of mass action, and the equilibrium constant
  • Acid and base (including pH and buffer solutions) as a special case of chemical equilibrium
  • Coordination complex equilibrium
  • Solubility
• Thermochemistry and thermodynamics
  • Heat capacity and calorimetry
  • Spontaneous reactions, enthalpy, entropy, and Gibbs' energy
  • The Clausius-Clapeyron and van't Hoff equations
• Electrochemistry
  • Galvanic cells, concentration cells, electrolysis
  • Nernst equation
  • Pourbaix diagrams, speed of corrosion
  • Batteries

Learning outcome

After completing the course, the candidate is able to:

• Use roles for chemical nomenclature to name chemical compounds.
• Balance chemical equations, and stoichiometry
• Explain what chemical equilibrium, and use the law of mass action to determine equilibrium constants, and compositions at equilibrium for different types of reactions, including solubility, solubility products, and pH for acid/base reactions.
• Determine changes in enthalpy, entropy and Gibbs' energy for a chemical reaction, and relate this to chemical equilibrium and spontaneous reactions.
• Understand the principle of galvanic cells, concentration cells, and electrolysis. Understand the relationship between chemical equilibrium constant, changes in Gibbs' energy, and cell potential for electrochemical cells. See the relationship between electrochemistry, thermodynamics, and work.
• Use Pourbaix diagrams to predict corrosion.
• Know the principles of green chemistry, and apply these to understand the role of chemistry in a sustainable society.

Learning methods and activities

Lectrues (56 hours) and exercises (48 hours). 96 hours selfstudy. There will be 12 exercises in the course, where four (4) of the six (6) first, and five (5) of the six (6) last has to be approved to get access to the exam.

Compulsory assignments

• Exercise

Required previous knowledge

Emnet krever opptak til siv.ing og fysikk 1 fra vgs.

Course materials

Material will be public at start of semester.

Course material must be read.

Credit reductions