Duration
Thermodynamics : 20h Th, 20h Pr, 15h Mon. WS
Electrochemistry : 20h Th, 10h Pr, 10h Mon. WS
Number of credits
| Bachelor in chemistry | 8 crédits |
Lecturer
Thermodynamics : Loïc Quinton
Electrochemistry : Loïc Quinton
Coordinator
Language(s) of instruction
French language
Organisation and examination
Teaching in the first semester, review in January
Schedule
Units courses prerequisite and corequisite
Prerequisite or corequisite units are presented within each program
Learning unit contents
1. Classical Thermodynamics, including te microscopic description
Introduction
First Principle: Internal Energy, Work, Heat, State Function, Equilibrium and Thermodynamic Reversibility, Enthalpy
Second and Third Principles
Free Energy and Free Enthalpy.
The chemical potential
2. Changes in the state of pure substances
Introduction
Conditions of equilibrium between phases
Phase equilibria and phase diagrams: solid-liquid transition, liquid-vapor transition, Trouton's rule and Clapeyron's diagram, solid-vapor transition, solid-solid transition (allotropy)
The phase rule: variance
3. State changes of mixtures
Introduction
Thermodynamics of gas mixtures
Thermodynamics of liquid mixtures: chemical potential of liquids, Raoult's law, Henry's law, chemical activities of solvent and solute
Colligative properties: ebullioscopic elevation, lowering of melting point, osmosis and osmotic pressure.
Solubility
Coefficient of partition
Vapor pressure of ideal binary solutions
Thermodynamic quantities of real binary solutions
Vapor pressure of a real binary solution
4. Diagram of free enthlapie and phase diagrams of binary systems
Stability of solutions
Liquid-vapor, liquid-solid binary systems
5. Diagram of the phases of ternary systems
6. Chemical equilibria
7. Electrochemistry
Potentiometry
Redox reactions
Thermodynamic description of electrode reactions (Nernst equation)
Normal electrode potentials
Activities in ionic solution (Debye-Huckel)
The types of electrodes
Conductometry
The phenomenon of electrical conduction in solution (Ohm's law in solution)
The law of independent migration of ions
Strong electrolytes, weak electrolytes
Transport numbers
Batteries and accumulators
Electrochemical titrations (optional)
Thermodynamics
1. Classical Thermodynamics, including te microscopic description
Introduction
First Principle: Internal Energy, Work, Heat, State Function, Equilibrium and Thermodynamic Reversibility, Enthalpy
Second and Third Principles
Free Energy and Free Enthalpy.
The chemical potential
2. Changes in the state of pure substances
Introduction
Conditions of equilibrium between phases
Phase equilibria and phase diagrams: solid-liquid transition, liquid-vapor transition, Trouton's rule and Clapeyron's diagram, solid-vapor transition, solid-solid transition (allotropy)
The phase rule: variance
3. State changes of mixtures
Introduction
Thermodynamics of gas mixtures
Thermodynamics of liquid mixtures: chemical potential of liquids, Raoult's law, Henry's law, chemical activities of solvent and solute
Colligative properties: ebullioscopic elevation, lowering of melting point, osmosis and osmotic pressure.
Solubility
Coefficient of partition
Vapor pressure of ideal binary solutions
Thermodynamic quantities of real binary solutions
Vapor pressure of a real binary solution
4. Diagram of free enthlapie and phase diagrams of binary systems
Stability of solutions
Liquid-vapor, liquid-solid binary systems
5. Diagram of the phases of ternary systems
6. Chemical equilibria
Electrochemistry
1. Classical Thermodynamics, including te microscopic description
Introduction
First Principle: Internal Energy, Work, Heat, State Function, Equilibrium and Thermodynamic Reversibility, Enthalpy
Second and Third Principles
Free Energy and Free Enthalpy.
The chemical potential
2. Changes in the state of pure substances
Introduction
Conditions of equilibrium between phases
Phase equilibria and phase diagrams: solid-liquid transition, liquid-vapor transition, Trouton's rule and Clapeyron's diagram, solid-vapor transition, solid-solid transition (allotropy)
The phase rule: variance
3. State changes of mixtures
Introduction
Thermodynamics of gas mixtures
Thermodynamics of liquid mixtures: chemical potential of liquids, Raoult's law, Henry's law, chemical activities of solvent and solute
Colligative properties: ebullioscopic elevation, lowering of melting point, osmosis and osmotic pressure.
Solubility
Coefficient of partition
Vapor pressure of ideal binary solutions
Thermodynamic quantities of real binary solutions
Vapor pressure of a real binary solution
4. Diagram of free enthlapie and phase diagrams of binary systems
Stability of solutions
Liquid-vapor, liquid-solid binary systems
5. Diagram of the phases of ternary systems
6. Chemical equilibria
7. Electrochemistry
Potentiometry
Redox reactions
Thermodynamic description of electrode reactions (Nernst equation)
Normal electrode potentials
Activities in ionic solution (Debye-Huckel)
The types of electrodes
Conductometry
The phenomenon of electrical conduction in solution (Ohm's law in solution)
The law of independent migration of ions
Strong electrolytes, weak electrolytes
Transport numbers
Batteries and accumulators
Electrochemical titrations (optional)<br /><br /> 1. Classical Thermodynamics, including te microscopic description
Introduction
First Principle: Internal Energy, Work, Heat, State Function, Equilibrium and Thermodynamic Reversibility, Enthalpy
Second and Third Principles
Free Energy and Free Enthalpy.
The chemical potential
2. Changes in the state of pure substances
Introduction
Conditions of equilibrium between phases
Phase equilibria and phase diagrams: solid-liquid transition, liquid-vapor transition, Trouton's rule and Clapeyron's diagram, solid-vapor transition, solid-solid transition (allotropy)
The phase rule: variance
3. State changes of mixtures
Introduction
Thermodynamics of gas mixtures
Thermodynamics of liquid mixtures: chemical potential of liquids, Raoult's law, Henry's law, chemical activities of solvent and solute
Colligative properties: ebullioscopic elevation, lowering of melting point, osmosis and osmotic pressure.
Solubility
Coefficient of partition
Vapor pressure of ideal binary solutions
Thermodynamic quantities of real binary solutions
Vapor pressure of a real binary solution
4. Diagram of free enthlapie and phase diagrams of binary systems
Stability of solutions
Liquid-vapor, liquid-solid binary systems
5. Diagram of the phases of ternary systems
6. Chemical equilibria
Learning outcomes of the learning unit
This course of scond year deepens the subjects seen in the 1st year course of General Chemistry and opens to more conceptual subjects.
It covers the following subjects:
Thermodynamics: introduction of concepts and quantities
Change of state of pure and mixed substances.
Phase diagram of simple, binary and ternary systems.
Electrochemistry and kinetics: introductions and bases
Thermodynamics
This course of scond year deepens the subjects seen in the 1st year course of General Chemistry and opens to more conceptual subjects.
It covers the following subjects:
Thermodynamics: introduction of concepts and quantities
Change of state of pure and mixed substances.
Phase diagram of simple, binary and ternary systems.
Electrochemistry
This course of scond year deepens the subjects seen in the 1st year course of General Chemistry and opens to more conceptual subjects.
It covers the following subjects:
Thermodynamics: introduction of concepts and quantities
Change of state of pure and mixed substances.
Phase diagram of simple, binary and ternary systems.
Electrochemistry and kinetics: introductions and bases<br /><br /> This course of scond year deepens the subjects seen in the 1st year course of General Chemistry and opens to more conceptual subjects.
It covers the following subjects:
Thermodynamics: introduction of concepts and quantities
Change of state of pure and mixed substances.
Phase diagram of simple, binary and ternary systems.
Prerequisite knowledge and skills
Good knowledge of general chemistry (fisrt year)
Thermodynamics
Good knowledge of general chemistry (fisrt year)
Electrochemistry
Good knowledge of general chemistry (fisrt year)<br /><br /> Good knowledge of general chemistry (fisrt year)
Planned learning activities and teaching methods
Mode of delivery (face to face, distance learning, hybrid learning)
Thermodynamic part: classroom teaching
20h of theory, 20h of sessions of exercice and 15h of laboratory
Electrochemistry part: face-to-face teaching
20h of theory, 10h of of sessions of exercice and 10h of laboratory
Thermodynamics
Thermodynamic part: classroom teaching
20h of theory, 20h of sessions of exercice and 15h of laboratory
Electrochemistry
Thermodynamic part: classroom teaching
20h of theory, 20h of sessions of exercice and 15h of laboratory
Electrochemistry part: face-to-face teaching
20h of theory, 10h of of sessions of exercice and 10h of laboratory<br /><br /> Thermodynamic part: classroom teaching
20h of theory, 20h of sessions of exercice and 15h of laboratory
Recommended or required readings
Chimie générale Partim II, , Loïc Quinton
reference book: Physical Chemistry, P. Atkins,
Lectures notes progressively desposited on eCampus
Thermodynamics
Chimie générale Partim II, , Loïc Quinton
reference book: Physical Chemistry, P. Atkins,
Lectures notes progressively desposited on eCampus
Electrochemistry
Chimie générale Partim II, , Loïc Quinton
reference book: Physical Chemistry, P. Atkins,
Lectures notes progressively desposited on eCampus<br /><br /> Chimie générale Partim II, , Loïc Quinton
reference book: Physical Chemistry, P. Atkins,
Lectures notes progressively desposited on eCampus
Assessment methods and criteria
The final evaluation concerns all the parts of the course (theory, problems, laboratory)
The successful completion of the course will be awarded to any student with a minimum overall score of 10,00 / 20.
Thermodynamics
The final evaluation concerns all the parts of the course (theory, problems, laboratory)
The successful completion of the course will be awarded to any student with a minimum overall score of 10,00 / 20.
Electrochemistry
The final evaluation concerns all the parts of the course (theory, problems, laboratory)
The successful completion of the course will be awarded to any student with a minimum overall score of 10,00 / 20.<br /><br /> The final evaluation concerns all the parts of the course (theory, problems, laboratory)
The successful completion of the course will be awarded to any student with a minimum overall score of 10,00 / 20.
Work placement(s)
Organisational remarks and main changes to the course
Contacts
Enseignants :
Prof. Loïc Quinton, loic.quinton@uliege.be
Laboratory of Mass Spectrometry
MolSys Research Unit
Allée du six Aout 11 - Quartier Agora - Liège Université
B4000 -Liège 1 - Belgium
Tel +0032 4 366 3679
Assistant:
Wendy Muller, wmuller@student.uliege.be
Vincent Natalis, vincent.natalis@uliege.be
Thermodynamics
Enseignants :
Prof. Loïc Quinton, loic.quinton@uliege.be
Laboratory of Mass Spectrometry
MolSys Research Unit
Allée du six Aout 11 - Quartier Agora - Liège Université
B4000 -Liège 1 - Belgium
Tel +0032 4 366 3679
Assistants :
Wendy Muller, wmuller@student.uliege.be
Vincent Natalis, vincent.natalis@uliege.be
Electrochemistry
Teacher:
Prof. Loïc Quinton, loic.quinton@uliege.be
Laboratory of Mass Spectrometry
MolSys Research Unit
Allée du six Aout 11 - Quartier Agora - Liège Université
B4000 -Liège 1 - Belgium
Tel +0032 4 366 3679
Assistants :
Wendy Muller, wmuller@student.uliege.be
Vincent Natalis, vincent.natalis@uliege.be