Lecture #11 Corrosion 1-Corrosion in metals.

Slides:

Advertisements

Similar presentations

Fig. 22-1a (p.629) A galvanic electrochemical cell at open circuit

Advertisements

Electrochemistry Chapter 20.

Failures of Materials 1. Environmental Effects on the Materials There are significant impacts of environmental factors on Engineering Materials. 2.

Chapter 20: Electrochemsitry A.P. Chemsitry Oxidation-Reduction Reactions Oxidation-reduction reactions (or redox reactions) involve the transfer.

Electrochemistry. Remember… Anode: electrode in the half-cell where oxidation takes place Metal electrode atoms are oxidized and become aqueous ions Anions.

Lecture 15 CM1001.

STANDARD REDUCTION POTENTIAL. STANDARD REDUCTION (ELECTRODE) POTENTIAL (E O ) Is a measurement that indicates how easily a half cell undergoes reduction.

Cell Voltages To compare cells compare voltages of cells in their standard state. Standard States For solids and liquids: the state of the pure solid or.

ELECTROCHEMISTRY Chapter 17. W HAT IS ELECTROCHEMISTRY Electrochemistry is the science that unites electricity and chemistry. It is the study of the transfer.

ELECTROCHEMISTRY. During electrolysis positive ions (cations) move to negatively charged electrode (catode) and negative ions (anions) to positively charged.

Galvanic Cells What will happen if a piece of Zn metal is immersed in a CuSO 4 solution? A spontaneous redox reaction occurs: Zn (s) + Cu 2 + (aq) Zn 2.

Types of Electrochemical Cells Electrolytic Cells: electrical energy from an external source causes a nonspontaneous reaction to occur Voltaic Cells (Galvanic.

Thermodynamics in Corrosion Engineering

Lecture 14 CM1001. Oxidation Numbers Positive or negative numbers decided using agreed rules. Help us work out whether a substance is oxidized or reduced.

Password Lectures 1-9: Falcon10 Password Lectures 10-16: Wryneck Lecture 16 CM1001.

The Study of the Interchange of Chemical and Electrical Energy

Chapter 19 Electrochemistry

Electrochemistry Chapter 20.

Chapter 20 Notes Electrochemistry.

ELECTROCHEMISTRY Chapter 17. W HAT IS ELECTROCHEMISTRY Electrochemistry is the science that unites electricity and chemistry. It is the study of the transfer.

Lecture 9. Chemistry of Oxidation-Reduction Processes Prepared by PhD Halina Falfushynska.

Electrochemistry Chapter 21. Electrochemistry and Redox Oxidation-reduction:“Redox” Electrochemistry: study of the interchange between chemical change.

Electrochemistry AP Chapter 20. Electrochemistry Electrochemistry relates electricity and chemical reactions. It involves oxidation-reduction reactions.

TO CATCH LOTS OF FISH, YOU MUST FIRST GO TO THE WATER. -ANON-

Electrochemistry. Electrochemical Cells  Electrons are transferred between the particles being oxidized and reduced  Two types –Spontaneous = Voltaic.

Using and Controlling Reactions Assign oxidation numbers and balance atom whose oxidation number changes 2. Balance oxygen by adding water 3. Balance.

Chapter 23 Corrosion.

An Introduction to Electroanalytical Chemistry Electrochemistry: The study of the interchange of chemical and electrical energy Oxidation is the loss of.

 Deals with the relation of the flow of electric current to chemical changes and the conversion of chemical to electrical energy (Electrochemical Cell)

Chapter 21.  Two types: ◦ Voltaic cell: electrons flow spontaneously ◦ Electrolytic cell: electrons are forced to flow.

Chapter 21 Electrochemistry 21.2 Half-Cells and Cell Potentials

Chapter 20 Electrochemistry and Oxidation-Reduction.

6/2/20161 CHAPTER 2 CORROSION PRINCIPLES Chapter Outlines 2.1 Oxidation and Reduction Reactions 2.2 Standard Electrode Half- Cell Potentials 2.3 Standard.

Chapter 26 – Electricity from Chemical Reactions.

CHM Lecture 23 Chapt 14 Chapter 14 – Fundamentals of Electrochemistry Homework - Due Friday, April 1 Problems: 14-4, 14-5, 14-8, 14-12, 14-15, 14-17,

CHAPTER 11 ELEMENTS OF ELECTROCHEMISTRY Introduction to Analytical Chemistry.

Chapter 17 Corrosion and Degradation of Materials.

Electrochemistry Chapter 20 Preview Image Bank Electrochemical Cells Ion Movement Through a Porous Barrier Electron Pathway in an Electrochemical Cell.

Electrochemistry Ch.19 & 20 Using chemical reactions to produce electricity.

Batteries Electrochemical cells  Terms to know Anode Cathode Oxidation Reduction Salt Bridge Half cell Cell potential Electron flow Voltage.

In the previous videos, we looked at electrochemical cells with reactive metal electrodes and solutions containing their cations. However, some electrochemical.

Copyright©2000 by Houghton Mifflin Company. All rights reserved. 1 Chemistry FIFTH EDITION by Steven S. Zumdahl University of Illinois.

Reduction- Oxidation Reactions (1) 213 PHC 9 th lecture Dr. mona alshehri (1) Gary D. Christian, Analytical Chemistry, 6 th edition. 1.

Electrochemistry Measurement of Electrode Potential Electrode Potential of Galvanic Cell The galvanic cell has two electrode potentials; anode potential.

ELECTROCHEMICAL CELLS. ELECTROCHEMISTRY The reason Redox reactions are so important is because they involve an exchange of electrons If we can find a.

Electrochemistry The Study of the Interchange of Chemical and Electrical Energy.

Electrolytic Cells Chemistry Chapter 19 E.

ELECTROCHEMISTRY Electrochemistry relates electricity and chemical reactions. It involves oxidation-reduction reactions (aka – redox) They are identified.

ENT 487 ENVIRONMENTALLY ASSISTED CRACKING IN METALS

After completing this topic you should be able to : State electricity can be produced in a cell by connecting two different metals in solutions of their.

Chapter Menu Electrochemistry Section 20.1Section 20.1Voltaic Cells Section 20.2Section 20.2 Batteries Section 20.3Section 20.3 Electrolysis Exit Click.

ELECTROCHEMISTRY Presentation by: P.K. CHOURASIA K.V MANDLA, Jabalpur Region.

In voltaic cells, oxidation takes place at the anode, yielding electrons that flow to the cathode, where reduction occurs. Section 1: Voltaic Cells K What.

Electrochemistry - The relationship between chemical processes and electricity oxidation – something loses electrons reduction – something gains electrons.

Definition of Corrosion

Oxidation-Reduction Reactions

Basic Corrosion Theory

Oxidation-Reduction reactions

Electrochemical cells

ELECTROCHEMISTRY JEOPARDY: THE GAME

Harnessing the changes in oxidation and reduction

Electrochemistry.

Corrosion Degradation 0f a metal due to reaction with its environment Impairs function and appearance of component.

Electrochemistry Chapter 17.

Summary of Previous Lecture Development of; Human History → Technology → Population → Current Problems & Changes, Global warming, Urbanization, Aging/Increasing.

Engineering Materials

FACTORS AFFECTING REACTIONS IN CELLS

Voltaic (Galvanic)Cells

Chapter 21 Thanks to D Scoggin Cabrillo College

Redox in Electrochemistry

Presentation transcript:

Lecture #11 Corrosion 1-Corrosion in metals. Learning objective outcomes: 1-Corrosion in metals. 2-Distinguish between oxidation and reduction electrochemical reactions. 3. Describe the following: galvanic couple, standard half-cell, and standard hydrogen electrode. 4. Compute the cell potential and write the spontaneous electrochemical reaction direction for two pure metals that are electrically connected and also submerged in solutions of their respective ions. 5-Corrosin in ceramics. 6- Corrosion in polymers

CORROS ION OF METALS An oxidation reaction: Corrosion is defined as the destructive and unintentional attack of a metal; it is electrochemical and ordinarily begins at the surface. The problem of metallic corrosion is one of significant proportions; in economic terms, it has been estimated that approximately 5% of an industrialized nation’s income is spent on corrosion prevention and the maintenance or replacement of products lost or contaminated as a result of corrosion reactions.. ELECTROCHEMICAL CONSIDERATIONS: An oxidation reaction:

Reduction reaction: A- In acidic medium: B-In basic or neutral medium:

solution of H ions, saturated with hydrogen gas that is bubbled through the solution at a pressure of 1 atm and a temperature of 25C (77F). The platinum itself does not take part in the electrochemical reaction; it acts only as a surface on which hydrogen atoms may be oxidized or hydrogen ions may be reduced.

Degradation of polymers: Polymeric materials deterioration by means of environmental interactions. However an undesirable interaction is specified as degradation rather than corrosion.