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

View course schedule

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 Lindback

Head of Department:

Ingunn Westvik Jolma

Method of work

Two lectures per week and one exercise class.

Overlapping courses

Course Reduction (SP)
General Chemistry (KJE150_1) 5

Open for

Battery and Energy Engineering - Bachelor in Engineering

Literature

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