TU Delft
Education Type
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2016/2017 Civil Engineering and Geosciences Bachelor Applied Earth Sciences
Chemical Thermodynamics
Responsible Instructor
Name E-mail
Dr. W.A. Smith    W.Smith@tudelft.nl
Name E-mail
Dr.ir. D.A. Vermaas    D.A.Vermaas@tudelft.nl
Contact Hours / Week x/x/x/x
47 contact hours in total
Lectures = 36 hrs (over 9 weeks: week 10 exam)
Exercise hours = 11 hrs (over 9 weeks: week 10 exam)
Test = 3 hrs
Education Period
Start Education
Exam Period
Course Language
Expected prior knowledge
Introduction to Chemistry (AESB1120)
Course Contents
Fundamental concepts, heat, work and internal energy, he importance of state functions, hermochemistry, entropy and the second and third law of thermodynamics, chemical equilibrium, the properties of real gases, phase diagrams and the relative stability of solids, liquids and gases, ideal and real solutions
Study Goals
At the end of the course the student should be able to:
- link in practice observed phenomena to the laws of thermodynamics that control the phenomena
- quantitatively predict the behavior of simple thermodynamic systems based on the laws of thermodynamics
- understand the way the thermodynamic theory is set up
Study Goals continuation
Knowledge, at the end of this course, the student is able to:
- give a qualitative description of the four laws of thermodynamics
- describe the difference between an ideal and non-ideal gas
- determine the relationship between pressure, volume, and temperature for real gases
- describe how work, internal energy, and temperature are related
- evaluate the properties of a material in terms of enthalpy, Gibb’s free energy, and entropy
- describe the internal energy and enthalpy changes during chemical reactions
- illustrate solid-liquid-gas phase diagrams for a particular material
- evaluate the differences between the Gibbs free energy and the Helmholtz energy of a system

Skills, at the end of this course, the student is able to:
- classify matter
- apply the law of conservation of energy
- differentiate between heat, temperature, and energy
- qualitatively describe internal energy and entropy
- predict the properties of a gas based on pressure, volume, and temperature changes
- calculate the conditions for a material to undergo a phase change
- apply simple structure-property relationships for elements, ions, and molecules to predict or explain their chemical and physical behavior

Attitude, at the end of this course, the student is familiar with:
- application of a scientific method for problem solving
- solid-liquid-gas phase diagrams
- ideal and real solutions
- converting energies
- the laws of thermodynamics
Education Method
The course will consist of lectures and exercises, using a text book and computer-aided assignments.
Most lectures will cover one particular topic, although larger topics will require 2 lectures to discuss.
From students it is expected that they have studied the lecture topic from the book in advance of the lecture, and complete the assigned exercises for each week before start of the following week’s lecture.
Literature and Study Materials
Physical Chemistry, Chapter 1-11, 3rd edition, Engel and Reid, Pearson Publishers, including the electronic set of tutorials/questions “Mastering Chemistry”
2 mid-term exams and 1 final exam
Permitted Materials during Tests
Pen or pencil, paper, basic (non-graphing) calculator. The necessary tables will be provided at the exam. The use of own books with tables (e.g. ‘BINAS’) is not allowed.
W.A. Smith
Expected prior Knowledge
Basic Chemistry, Calculus, Physics
Academic Skills
Differential equations, problem solving, group work
Literature & Study Materials
Engel and Reid, Physical Chemistry
Average of midterm exams (40%)
Average of homework exercises (20%)
Final exam (40%)
Permitted Materials during Exam
Non-graphing calculator