EMA5305-4303 Electrochemical Engineering

Course Information

An introduction to the fundamental principles of electrochemistry and its applications in different engineering systems for energy, chemical, biomedical, and electronics industries.

Course Objective

To introduce to undergraduate and junior graduate students the basic concepts, physical/chemical principles, and engineering practices of electrochemistry and its applications in various electrochemical systems for energy, chemical, biomedical, and electronics industries.

Course Syllabus

EMA4303-5305 online – TENTATIVE Syllabus

Lecture Slides & Videos

Lecture Slides (PDF) Videos on YouTube w/ closed caption (CC)
Lecture 0 Course Info Introduction
Objectives and outcome
Topics and schedule
Lecture 1 Basic Concepts Electrochemistry
Electrochemistry application examples
Electrolyte and electrolyte solution
Different definitions for solution concentration
Molten electrolyte and solid electrolyte
Electrode and electrode materials
Electrochemical cell and cell potential
Half cell reaction and full cell reaction
Examples for half cell and full cell reactions
Active electrode vs inert electrode
Geometric separation of oxidation and reduction half cell reactions
Transition between electronic and ionic conduction at interfaces
Other features for electrochemical reactions
Equilibrium cell potential
  Galvanic cell
  Electrolytic cell
  Faraday constant and Faraday’s law
  Faraday’s law example
Lecture 2 Equilibrium Electrochemistry Equilibrium cell potential and cell construction
Standard hydrogen electrode
Standard electrode potential
Standard electrode potential series
Standard cell potential
Two examples for standard cell potential
Notes for standard electrode potential
Standard cell potential – positive vs negative
Reference electrodes other than SHE
Nernst equation for full cell reaction
Nernst equation for half cell reaction
Nernst equation notes
Example of cell potential from Nernst equation
Cell potential and direction of reaction
Example of reaction equilibrium constant from Nernst equation
Example of solubility product from Nernst equation
Concentration cell
Introduction to Pourbaix diagram
Hydrogen evolution line in Pourbaix diagram
Oxygen evolution line in Pourbaix diagram
Pure redox reactions in Pourbaix diagram
Pure acid-base reaction in Pourbaix diagram
Acid-base reactions with charge transfer in Pourbaix diagram
Gibbs free energy change
Standard Gibbs formation energy
Reaction Gibbs free energy change
Gibbs free energy change example on methanol oxidation
Cell potential and Gibbs free energy change
Gibbs free energy change to cell potential – methanol fuel cell example
Cell potential to Gibbs free energy change – hydrogen fuel cell example
Gibbs free energy to cell potential example involving aqueous ions
Gibbs free energy and cell potential example at non-standard condition
Reaction equilibrium constant
Cell potential vs temperature example on hydrogen fuel cell
Lecture 3 Electrochemical Kinetics Introduction to electrochemical kinetics
Cell potential for galvanic cell and electrolytic cell
Cell potential and current relationship
Cell voltage loss from equilibrium potential
Definition of overpotential for an electrode reaction
Contributing factors to overpotential for an electrode reaction
Polarization curve and example for an electrode reaction
Butler Volmer equation without mass transport limitation
Butler Volmer equation under anodic or cathodic bias or at equilibrium
Butler Volmer equation to polarization curve
Exchange current density on Butler Volmer equation
Symmetry factor on Butler Volmer equation
Experimental data for exchange current density and symmetry factor
Linear approximation of B-V equation near equilibrium
Tafel equation at large overpotential
Tafel vs B-V equation
Overpotential measurement using reference electrode
Fitting data to B-V equation
Fitting Cl2 production anode polarization data to Tafel equation
Fitting Cl2 production anode polarization data to B-V equation
Comparing Tafel and BV fittings with experiment for Cl2 production
Three voltage loss mechanisms in electrochemical cell
Parameters in Zn NiOOH electrochemical cell
Overpotential from current in Zn NiOOH electrochemical cell
Zn NiOOH electrochemical cell potential at a given current density
Potential profile in Zn NiOOH electrochemical cell
Current from cell voltage in Zn NiOOH electrochemical cell
Concentration overpotential from Nernst equation
Limiting current density and mass transfer overpotential
Generalized B-V equation
Current vs overpotential plots from generalized B V equation
Lecture 4 Electroanalytical Techniques Classification of electrochemical techniques
Configuration for electrochemical measurements
Potentiometry at zero current and activity example
Potential measurement at constant current
Amperometry with fixed potential step and Cottrell equation
Cyclic voltammetry introduction
CV for capacitor
CV for reversible electrode reaction
Kinetic information from CV for reversible electrode reaction
CV for quasi-reversible and irreversible electrode reactions
From resistance to impedance
AC voltage and current
Impedance as a complex number
Impedance for resistor capacitor inductor
Impedance for elements in series and in parallel
Impedance spectra for R C RC in series and RC in parallel
Impedance spectrum for electrode without diffusion
Impedance for constant phase element CPE
Impedance for Warburg element for diffusion
Impedance for electrode with mixed control
Lecture 5 Electrochemical Engineering Applications Basic battery components
  Basic classifications and requirements for batteries
  Lead acid battery
  Lithium ion battery
  OCV, specific capacity, and specific energy for batteries
  Battery state of charge and discharge and their impacts
  Voltage current relationships and voltage loss mechanisms for batteries
  C rate for batteries and its impacts
  Side reactions in battery charging & discharging
  Battery efficiencies
  Fuel cell introduction
  Fuel cell classification
  Fuel cell OCV
  pO2 from fuel cell OCV
  Fuel cell j-V curves
  Temperature effect on fuel cell performance