General Chemistry w/o Laboratory Exercises (KJE155)
The aim of the course is to provide the students with fundamental knowledge in chemistry.
Course description for study year 2024-2025. Please note that changes may occur.
Facts
Course code
KJE155
Version
1
Credits (ECTS)
5
Semester tution start
Autumn
Number of semesters
1
Exam semester
Autumn
Language of instruction
Norwegian
Offered by
Time table
Content
The course includes reactions in aqueous solutions (redox, precipitation, and neutralization reactions), thermodynamics, acids and bases, properties of solutions (solubility and osmosis), acid-base titrations, factors that affect solubility, buffers, chemical kinetics and electrochemistry.
Learning outcome
On completion of the General Chemistry w/o laboratory exercises, the students should be able to:
- classify reactions in aqueous solution into neutralization reactions, precipitation reactions, and redox reactions.
- define enthalpy change and explain how it can be measured in a coffee-cup calorimeter and how we apply the first law of thermodynamics in such measurements.
- explain when a reaction has reached its chemical equilibrium and recognize the role of chemical equilibrium in the La Châtelier’s principle.
- explain the difference between a spontaneous and nonspontaneous reaction and how to use the reaction free energy or the reaction quotient to decide whether a reaction occurs spontaneously or not.
- define change in entropy and recognize how it is used in the second law of thermodynamics to decide whether a process is spontaneous or nonspontaneous.
- define a solution and recognize the parameters that affect the solubility of a solute in a solvent.
- define osmosis and explain the role of entropy change in such physical property of a solution.
- describe the difference between a galvanic cell and electrolytic cell and explain the role of redox reactions in such cells.
- use the Nernst equation to calculate the cell potential.
- explain the corrosion process and give examples of how to protect objects from corrosion.
- define a base and acid by using the Brønsted-Lowry and Arrhenius acid-base theory, respectively, and to define pH. The students will be able to employ the acid and base definitions to calculate the pH of a solution.
- define a buffer and being able to explain why its pH changes only little when a small amount of strong acid or base is added.
- give examples of parameters that affect the rate of a reaction.
- explain the difference between first and second order reactions.
Required prerequisite knowledge
None
Recommended prerequisites
Chemistry 1 and 2 from high school.
Exam
| Form of assessment | Weight | Duration | Marks | Aid |
|---|---|---|---|---|
| Written exam | 1/1 | 3 Hours | Letter grades | Compendium of tables and formulae, Optional calculator, |
Course teacher(s)
Course coordinator:
Emil LindbackHead of Department:
Ingunn Westvik JolmaMethod of work
Two lectures per week and one exercise class.
Overlapping courses
| Course | Reduction (SP) |
|---|---|
| General Chemistry (KJE150_1) | 5 |