Module Notes
Faculty Member (Members):
Undergraduate, 10th Semester (5th Year, Spring)
Module Category: Thematic Unit Electives, Group B
Module Type: Core Chemical Engineering
Teaching Language: Greek
Course Code: CHM_E_Β5
Credits: 3
ECTS Credits: 4
Teaching Type: Lectures (3h/W) Project/Homework (4/Semester)
Module Availability on Erasmus Students: No
Course URL: E-Class (CMNG2149)
Student's office hours: Monday, 16:00-17:00
Module Details

Ability to describe the modes of operation of electrochemical systems, the different types of ionic conductors, the interactions between ions in electrolytic solutions and the fundamental parameters and laws which concern ion transfer and electrical conduction in a homogeneous electrolyte phase.

Ability to describe the structure of an electrode/electrolyte interphase and explain the appearance of potential difference across it, as well as to formulate the condition of thermodynamic equilibrium for an electrode/electrolyte interphase or an electrochemical reaction.

Ability to describe the factors and mechanisms which determine the rate of an electrochemical reaction and control the operation of electrochemical systems under non-equilibrium conditions, as well as to express the rate of a multistep electrochemical reaction as a function of measurable parameters.

Ability to explain and implement equations for calculation of the ionic strength, activity coefficients, conductivity and related parameters in electrolyte solutions, as well as of the conductivity temperature dependence in electrolyte melts and solid electrolytes.

Ability to explain and implement equations for calculation of the standard emf of an electrochemical cell using standard electrode potentials data or thermodynamic data, for correlation of the equilibrium electrode potential or the emf with the activities of the electroactive species, and for prediction of the spontaneous direction of a redox reaction using electrochemical data.

Ability to explain and implement equations for calculation of the overpotentials developing during operation of an electrochemical cell as well of the operating potential of the cell, for a given current density.

Ability to clearly present in written as well as discuss solutions to homework exercises and problems related to electrochemical processes.

The students should have basic knowledge of Physical Chemistry, with focus on Chemical Thermodynamics and Chemical Kinetics.

Introduction to electrochemistry: Electrochemical vs. purely chemical reactions. Electrolytic and galvanic cells.

Ions and electrolytes: Activities of ions in electrolyte solutions - Activity coefficients -
Debye-Hückel theory. Mechanisms of ion transfer and electrical conduction in electrolyte solutions.  Electrolyte melts. Solid electrolytes.

Electrode/electrolyte interphases and electrochemical cells: The structure of the electrode/electrolyte interphase and the potential difference across it. Polarizable and
non-polarizable interphases. Reference electrodes. The electrochemical series. The IUPAC conventions for electrochemical cells and for the sign of electromotive force. Prediction of the spontaneous direction of redox reactions using electrode potential data.

Thermodynamics of electrochemical reactions: Electrochemical potential and electrochemical Gibbs free energy. Electrochemical equilibrium. The Nernst equation.

Electrode kinetics: The relation of current density to electrochemical reaction rate. Exchange current density. Faraday’s laws of electrolysis. Effect of potential on the rate of an electrochemical reaction. Definition and measurement of electrode overpotential. Activation overpotential. The
Butler-Volmer equation. The Tafel equation. Concentration overpotential and limiting current density. Ohmic overpotential. Operating potential of an electrochemical cell.  Kinetic models for multistep electrochemical reactions.

Electrocatalysis and Electrochemical Promotion of Catalysis: Basic concepts

Teaching Organization

PROJECT / HOMEWORK: 3-4/semester

Total Module Workload (ECTS Standards):

108 Hours

1.  Final written exam

The written exams comprise mainly theoretical questions (part of them in the form of multiple-choice questions) but also solving of simple exercises.   

2.  Mid-term written exam (on volunteer basis)

The mid-term exam grade is taken into account only if it is higher than that of the final exam.

3.  Homework assignments (3-4  homework sets), on volunteer basis. 

  1. Ι. Α. Μουμτζής και Δ. Π. Σαζού, “Ηλεκτροχημεία”, Eκδόσεις Ζήτη, Θεσσαλονίκη, 1997
  2. Ν. Κουλουμπή, “Ηλεκτροχημεία”, Εκδόσεις Συμεών, Αθήνα, 2005
  3. Ν.-Ε. Κυρατζής,  “ Εισαγωγή στην ηλεκτροχημεία ”, Eκδόσεις Ζήτη Π. & Σια , Θεσσαλονίκη, 2005
  4. Σ. Μπεμπέλης, “Ηλεκτροχημεία”, Β’ Έκδοση, Εκδόσεις ΕΑΠ, Πάτρα, 2008
  5. E. Gileadi, “Electrode Kinetics for Chemists, Chemical Engineers, and Materials Scientists”, VCH, New York, 1993
  6. J. O' M. Bockris and A. K. N. Reddy, “Modern electrochemistry”, Vol.1 (Ionics), 2nd Edition, Kluwer Academic/Plenum Publishers, New York, 1998
  7. J. O'M. Bockris, A. K. N. Reddy and M. Gamboa-Aldeco, “Modern electrochemistry”, Vol.2 (Fundamentals of Electrodics), 2nd Edition, Kluwer Academic/Plenum Publishers, New York, 2000
  8. D. Pletcher, “A First Course in Electrode Processes”, The Electrochemical Consultancy, Romsey, U.K., 1991