{"id":447,"date":"2017-08-22T12:20:01","date_gmt":"2017-08-22T16:20:01","guid":{"rendered":"https:\/\/ac.fiu.edu\/?page_id=447"},"modified":"2025-12-16T22:28:34","modified_gmt":"2025-12-16T22:28:34","slug":"ema5305-4303","status":"publish","type":"page","link":"https:\/\/www.engr.colostate.edu\/laboratories\/ceramics\/teaching\/ema5305-4303\/","title":{"rendered":"Electrochemical Engineering"},"content":{"rendered":"\t\t
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Course Information<\/span><\/h1>

An introduction to the fundamental principles of electrochemistry and its applications in different engineering systems for energy, chemical, biomedical, and electronics industries.<\/span><\/p>

Course Objective<\/span><\/h1>

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.<\/span><\/p>

Course Syllabus<\/span><\/h1>

TENTATIVE Syllabus<\/a><\/span><\/p>

Lecture Slides & Videos<\/span><\/h1>
Lecture Slides (PDF)<\/strong><\/span><\/td>Videos on YouTube w\/ closed caption (CC)<\/strong><\/span><\/td><\/tr>
Lecture 00_Course Information<\/a><\/td>Introduction<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Objectives and outcome<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Topics and schedule<\/a><\/span><\/td><\/tr>
Lecture 01_Basic concepts_voice over<\/a><\/td>Electrochemistry<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Electrochemistry application examples<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Solution<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Electrolyte and electrolyte solution<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Different definitions for solution concentration<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Molten electrolyte and solid electrolyte<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Electrode and electrode materials<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Electrochemical cell and cell potential<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Half cell reaction and full cell reaction<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Examples for half cell and full cell reactions<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Active electrode vs inert electrode<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Geometric separation of oxidation and reduction half cell reactions<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Transition between electronic and ionic conduction at interfaces<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Other features for electrochemical reactions<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Equilibrium cell potential<\/a><\/span><\/td><\/tr>
\u00a0<\/span><\/td>Galvanic cell<\/a><\/span><\/td><\/tr>
\u00a0<\/span><\/td>Electrolytic cell<\/a><\/span><\/td><\/tr>
\u00a0<\/span><\/td>Faraday constant and Faraday’s law<\/a><\/span><\/td><\/tr>
\u00a0<\/span><\/td>Faraday’s law example<\/a><\/span><\/td><\/tr>
Lecture 02_Equilibrium electrochemistry_voice over<\/a><\/td>Equilibrium cell potential and cell construction<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Standard hydrogen electrode<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Standard electrode potential<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Standard electrode potential series<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Standard cell potential<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Two examples for standard cell potential<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Notes for standard electrode potential<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Standard cell potential – positive vs negative<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Reference electrodes other than SHE<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Nernst equation for full cell reaction<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Activity<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Nernst equation for half cell reaction<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Nernst equation notes<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Example of cell potential from Nernst equation<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Cell potential and direction of reaction<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Example of reaction equilibrium constant from Nernst equation<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Example of solubility product from Nernst equation<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Concentration cell<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Introduction to Pourbaix diagram<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Hydrogen evolution line in Pourbaix diagram<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Oxygen evolution line in Pourbaix diagram<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Pure redox reactions in Pourbaix diagram<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Pure acid-base reaction in Pourbaix diagram<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Acid-base reactions with charge transfer in Pourbaix diagram<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Gibbs free energy change<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Standard Gibbs formation energy<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Reaction Gibbs free energy change<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Gibbs free energy change example on methanol oxidation<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Cell potential and Gibbs free energy change<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Gibbs free energy change to cell potential – methanol fuel cell example<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Cell potential to Gibbs free energy change – hydrogen fuel cell example<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Gibbs free energy to cell potential example involving aqueous ions<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Gibbs free energy and cell potential example at non-standard condition<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Reaction equilibrium constant<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Cell potential vs temperature example on hydrogen fuel cell<\/a><\/span><\/td><\/tr>
Lecture 03_Electrochemical Kinetics_voice over<\/a><\/td>Introduction to electrochemical kinetics<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Cell potential for galvanic cell and electrolytic cell<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Cell potential and current relationship<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Cell voltage loss from equilibrium potential<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Definition of overpotential for an electrode reaction<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Contributing factors to overpotential for an electrode reaction<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Polarization curve and example for an electrode reaction<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Butler Volmer equation without mass transport limitation<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Butler Volmer equation under anodic or cathodic bias or at equilibrium<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Butler Volmer equation to polarization curve<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Exchange current density on Butler Volmer equation<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Symmetry factor on Butler Volmer equation<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Experimental data for exchange current density and symmetry factor<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Linear approximation of B-V equation near equilibrium<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Tafel equation at large overpotential<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Tafel vs B-V equation<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Overpotential measurement using reference electrode<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Fitting data to B-V equation<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Fitting Cl2 production anode polarization data to Tafel equation<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Fitting Cl2 production anode polarization data to B-V equation<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Comparing Tafel and BV fittings with experiment for Cl2 production<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Three voltage loss mechanisms in electrochemical cell<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Parameters in Zn NiOOH electrochemical cell<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Overpotential from current in Zn NiOOH electrochemical cell<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Zn NiOOH electrochemical cell potential at a given current density<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Potential profile in Zn NiOOH electrochemical cell<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Current from cell voltage in Zn NiOOH electrochemical cell<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Concentration overpotential from Nernst equation<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Limiting current density and mass transfer overpotential<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Generalized B-V equation<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Current vs overpotential plots from generalized B V equation<\/a><\/span><\/td><\/tr>
Lecture 04_Electrochemical Techniques_voice over<\/a><\/td>Classification of electrochemical techniques<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Configuration for electrochemical measurements<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Potentiometry at zero current and activity example<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Potential measurement at constant current<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Amperometry with fixed potential step and Cottrell equation<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Cyclic voltammetry introduction<\/a><\/span><\/td><\/tr>
\u00a0<\/td>CV for capacitor<\/a><\/span><\/td><\/tr>
\u00a0<\/td>CV for reversible electrode reaction<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Kinetic information from CV for reversible electrode reaction<\/a><\/span><\/td><\/tr>
\u00a0<\/td>CV for quasi-reversible and irreversible electrode reactions<\/a><\/span><\/td><\/tr>
\u00a0<\/td>From resistance to impedance<\/a><\/span><\/td><\/tr>
\u00a0<\/td>AC voltage and current<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Impedance as a complex number<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Impedance for resistor capacitor inductor<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Impedance for elements in series and in parallel<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Impedance spectra for R C RC in series and RC in parallel<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Impedance spectrum for electrode without diffusion<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Impedance for constant phase element CPE<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Impedance for Warburg element for diffusion<\/a><\/span><\/td><\/tr>
\u00a0<\/td>Impedance for electrode with mixed control<\/a><\/span><\/td><\/tr>
Lecture 05_Applications_voice over<\/a><\/td>Basic battery components<\/a><\/span><\/td><\/tr>
\u00a0<\/span><\/td>Basic classifications and requirements for batteries<\/a><\/span><\/td><\/tr>
\u00a0<\/span><\/td>Lead acid battery<\/a><\/span><\/td><\/tr>
\u00a0<\/span><\/td>Lithium ion battery<\/a><\/span><\/td><\/tr>
\u00a0<\/span><\/td>OCV, specific capacity, and specific energy for batteries<\/a><\/span><\/td><\/tr>
\u00a0<\/span><\/td>Battery state of charge and discharge and their impacts<\/a><\/span><\/td><\/tr>
\u00a0<\/span><\/td>Voltage current relationships and voltage loss mechanisms for batteries<\/a><\/span><\/td><\/tr>
\u00a0<\/span><\/td>C rate for batteries and its impacts<\/a><\/span><\/td><\/tr>
\u00a0<\/span><\/td>Side reactions in battery charging & discharging<\/a><\/span><\/td><\/tr>
\u00a0<\/span><\/td>Battery efficiencies<\/a><\/span><\/td><\/tr>
\u00a0<\/span><\/td>Fuel cell introduction<\/a><\/span><\/td><\/tr>
\u00a0<\/span><\/td>Fuel cell classification<\/a><\/span><\/td><\/tr>
\u00a0<\/span><\/td>Fuel cell OCV<\/a><\/span><\/td><\/tr>
\u00a0<\/span><\/td>pO2 from fuel cell OCV<\/a><\/span><\/td><\/tr>
\u00a0<\/span><\/td>Fuel cell j-V curves<\/a><\/span><\/td><\/tr>
\u00a0<\/span><\/td>Temperature effect on fuel cell performance<\/a><\/span><\/td><\/tr><\/tbody><\/table>\t\t\t\t\t\t\t\t<\/div>\n\t\t\t\t<\/div>\n\t\t\t\t\t<\/div>\n\t\t\t\t<\/div>\n\t\t\t\t<\/div>\n\t\t","protected":false},"excerpt":{"rendered":"

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