General Chemistry (KJE150)
The aim of the course is to provide basic chemistry knowledge including thermodynamics, chemical thermodynamics, chemical kinetics, electrochemistry, properties of solutions, acid and bases, titrations techniques, buffer solutions and reactions in aqueous solution.
Course description for study year 2024-2025. Please note that changes may occur.
Course code
KJE150
Version
1
Credits (ECTS)
10
Semester tution start
Autumn
Number of semesters
1
Exam semester
Autumn
Language of instruction
Norwegian
Content
Learning outcome
On completion of the General Chemistry course, KJE150, 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 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 colligative properties (vapor-pressure lowering, boiling-point elevation, freezing point depression, and osmose) and explain the role of entropy change in such physical properties of solutions.
- 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.
- 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.
- carry out simple and safe laboratory experiments
- write lab reports
Required prerequisite knowledge
Recommended prerequisites
Exam
| Form of assessment | Weight | Duration | Marks | Aid |
|---|---|---|---|---|
| Written exam | 1/1 | 4 Hours | Letter grades | All calculators |
The exam is digital.
Coursework requirements
Compulsory course attendance that must be completed and approved before access to the laboratory: Electronic Course in Health, Safety and Environment (HMS - kurs).
Compulsory attendance at the laboratory course with exercises 4 hours per week for 8 weeks. The laboratory work includes 6-7 exercises which must be approved on a pass/fail basis in order to get access to the final exam.
Valid absence due to illness or other reasons must be communicated as soon as possible to teaching staff.
Course teacher(s)
Course coordinator:
Kåre Bredeli JørgensenCourse coordinator:
Emil LindbackCourse teacher:
Ingebret FjeldeTutor:
Lyudmyla NilsenTutor:
Hong LinCoordinator laboratory exercises:
Xiaoping ZhangHead of Department:
Päivi Annele Teivainen-LædreCoordinator laboratory exercises:
Liv Margareth AkslandMethod of work
Overlapping courses
| Course | Reduction (SP) |
|---|---|
| General chemistry (BIK230_1) | 10 |
| General Chemistry w/o Laboratory Exercises (KJE155_1) | 5 |
Open for
Due to limited capacity in the laboratory, the course will only be available to students enrolled in study programs where the course is included as compulsory, or as a recommended elective, in the education plan.
Students who do not have the course in their original education plan, but wish to follow the course, can apply for admission.