Electrochemical Reactors

Slides:



Advertisements
Similar presentations
Chemistry 21.3.
Advertisements

Electrochemistry Chapter 20.
THE CHLOR-ALKALI INDUSTRY
Electrolysis Electrolysis breaks down ionic substances into simpler substances by using electricity!
6. Electrochemistry Candidates should be able to: (a)Describe and explain redox processes in terms of electron transfer and/or of changes in oxidation.
Oxidation-Reduction Reactions LEO SAYS GER. Oxidation and Reduction (Redox)  Electrons are transferred  Spontaneous redox rxns can transfer energy 
Electrolysis project Electrode: Is an electrical conductor that is used to pass current through an electrolyte.
Chemistry 1011 Slot 51 Chemistry 1011 TOPIC Electrochemistry TEXT REFERENCE Masterton and Hurley Chapter 18.
CLASS PRACTICE 3 a. What four ions are present in sodium chloride solution? Na+(aq), Cl-(aq), H+(aq), OH-(aq) b. In Figure 21.3, write the ionic equation.
Yr 10 Electrolysis project. Yr 10 Electrolysis project.
Option C12.  The chlor-alkali industry refers to the production of chlorine, sodium hydroxide and sodium carbonate.  Cl2 and NaOH are made from the.
Electrochemistry Chapter 20.
Electrolysis. –A redox reaction that is made to occur by passing a direct electric current through an electrolyte Electrolyte –is a liquid that conducts.
1 Lec. 2 Faraday’s Laws Lec. 2 Faraday’s Laws Industrial Electrolytic Processes “Electrolysis”
Explain the process of electrolysis and its uses
Ions in Solution. Electrolysis During electrolysis ions move towards the electrodes. At the anode (+) Negatively charged ions are oxidised and lose electrons.
CHEMISTRY World of Zumdahl Zumdahl DeCoste. Copyright© by Houghton Mifflin Company. All rights reserved. Chapter 18 Oxidation-Reduction Reactions and.
Electrolysis Process by which an electric current is passed through a substance to cause a chemical change. The chemical change is one in which the substance.
An Introduction to Electroanalytical Chemistry Electrochemistry: The study of the interchange of chemical and electrical energy Oxidation is the loss of.
Chapter 21.  Two types: ◦ Voltaic cell: electrons flow spontaneously ◦ Electrolytic cell: electrons are forced to flow.
 Learners must be able to define galvanic cell in terms of electrode reaction. e.g. salt bridge.(N.B. anode and cathode)  Learners must be able to do.
Salt Power Chloe Shreve and Helen Row.  It uses an electrochemical cell. In the cell there are anodes, cathodes and electrolytes that concert chemical.
Copyright©2000 by Houghton Mifflin Company. All rights reserved. 1 Electrochemistry The study of the interchange of chemical and electrical energy.
Chapter 18: Introduction to Electrochemistry CHE 321: Quantitative Chemical Analysis Dr. Jerome Williams, Ph.D. Saint Leo University.
18.8 Electrolysis 2 Types of electrochemistry 1.Battery or Voltaic Cell – Purpose? 2.Electrolysis - forces a current through a cell to produce a chemical.
Oxidation-Reduction Dr. Ron Rusay Fall 2001 © Copyright 2001 R.J. Rusay.
Electrochemical Cells in Actions Batteries and Fuel Cells Chapter 15.
Electrochemistry Oxidation-Reduction Dr. Ron Rusay Spring 2004 © Copyright 2004 R.J. Rusay.
Electrolytic Cells Section 9.2. Vocabulary Electrolysis: electrical energy used to bring about a non-spontaneous redox reaction Electrolyte: any substance.
Electrolysis  Section Electrolysis Occurs in an electrolytic cell Can be the molten salt, or ions in solution Cations are attracted to the cathode.
Electrolysis. What is electrolysis? Electrolysis means “breaking up a compound with electricity” From the Greek Electro – electricity Lysis – breaking.
Electrochemical Cells
How to predict a Product. Synthesis Acid anhydride + water  acid Base anhydride + water  base Nonmetallic oxide is acid anhydride Metallic oxide is.
Electrolytic Cells Chemistry Chapter 19 E.
9.5 Electrolytic Cells. Match up the words with their descriptions Test for Oxygen Test for Hydrogen Electrolyte Relights a glowing splint Makes a ‘popping’
Electrolytic Cells. An electrolytic cell is an electrochemical cell that undergoes a redox reaction when electrical energy is applied. It is most often.
Chapter Menu Electrochemistry Section 20.1Section 20.1Voltaic Cells Section 20.2Section 20.2 Batteries Section 20.3Section 20.3 Electrolysis Exit Click.
Chapter  The electrochemical cells require the INPUT of energy rather than creating energy.
Electrochemistry Oxidation-Reduction Dr. Ron Rusay Spring 2004 © Copyright 2004 R.J. Rusay.
Teknik Elektrokimia Instructor: Rama Oktavian
Oxidation-Reduction Reactions
CHEMISTRY CHAPTER 19 LEO SAYS GER
Chemical energy from electrical energy
Electrolytic Cells.
The membrane keeps the chlorine gas away
Electrochemistry and The Chemical Cells.
The following slides should help you with your revision, but should not be your only form of revision. Remember to use your notes, a textbook, websites.
Images.
Cells.
Redox Reactions and Electrolysis
Chemistry AS – Redox reactions
From Chemistry to Electricity
Oxidation-Reduction Reactions
ELECTROCHEMISTRY JEOPARDY: THE GAME
20/11/2018 nrt.
Make sure you revise the following:
Chemistry 21.3.
The Chlor-alkali Industry
An electrolytic cell uses electricity to do a chemical reaction.
Electrochemistry Chapter 20.
Aim # 36: What is the difference between a
Extraction from Dolomite CaMg(CO3)2 and Magnesite Ore MgCO3.
Oxidation-Reduction Reactions
from a battery or other external energy source
Voltaic Cells/Electrochemical Cells/Spontaneous Reactions
C4 – Chemical changes Key Concepts.
1. What is the reaction between acid and alkalis called?
Chemistry 4: Chemical Changes
A. Oxidation-Reduction Reactions
Redox in Electrochemistry
Presentation transcript:

Electrochemical Reactors Quak Foo Lee Department of Chemical and Biological Engineering The University of British Columbia

Introduction In electrochemical reactions, electrons are supplied to a reactant in the electrolyte or removed from it with the aid of an electric current. A minimum voltage called the decomposition voltage must be applied to the electrodes for this purpose. In addition to the electrochemical reactions occurring on the electrode surface, transport processes and chemical reactions in the electrolyte both are important.

Reactors for Electrochemical Processes A) Metal winning by fused-salt electrolysis; B) Electrolytic metal refining; C) Electrolysis of inorganic material; D) Electrolysis of organic material; E) Mercury amalgam process; F) Diaphragm-cell process; G) Membrane process a) Water; b) Chlorine; c) Sodium chloride; d) Hydrogen; e) Sodium; f) Sodium hydroxide; g) Anode; h) Cathode; i) Membrane; j) Product; k) Amalgam; l) Recycle brine +  chlorine; m) Mercury; n) Graphite; o) Diaphragm; p) Electrolytic salt solution of metal to be refined; q) Anode slime; r) Electrolyte removal; s) Organic feed solution; t) Oxygen

Advantages High product purity (no secondary reactions) Low reaction temperature (except for fused-salt electrolysis) Easy control of reaction rate through variation of electrode voltage

Disadvantages High energy losses in the system Large space requirement High investment costs

When to Use Electrochemical Reactor? Electrochemical processes are used only when no available thermal or catalytic process can accomplish the same purpose, which is especially true in the production of chlorine, aluminum, and copper.

Applications Chlorine production by chlor – alkali electrolysis Mercury amalgam process Diaphragm-cell process Membrane process Metal winning by fused-salt electrolysis Aluminum Magnesium Sodium Metal refining Copper Nickel

Applications Electrolysis of inorganic materials Electrolysis of water Fluorine production by electrolysis of hydrogen fluoride Production of sodium chlorate by electrolysis of sodium chloride Electrochemical oxidation of sodium chlorate to perchlorate Recovery of persulfuric acid Production of ozone Electrolysis of organic materials Production of adiponitrile from acrylonitride Production of dimenthyl sebacate Reduction of nitrobenzene to aniline