Electrochemical System
|
|
- Dennis McBride
- 6 years ago
- Views:
Transcription
1 Electrochemical System Topic Outcomes Week Topic Topic Outcomes 8-10 Electrochemical systems It is expected that students are able to: Electrochemical system and its thermodynamics Chemical reactions in electrochemical cells and the Nernst equation The relationship between the cell emf and the equilibrium constant, Gibbs energies and reaction entropies Thermodynamics of Galvanic cells and Fuel cell Define the electrochemical system. Explain about electrochemical cell and differentiate galvanic cell and electrolyte cell Apply Nernst equation of thermodynamic principles to electrochemical cells. Determine G o, K o, S o, H o, Cp o activity coefficient and ph of cell s chemical reaction. Understand the cell emf in IUPAC convention. Estimate the liquid junction potential from emf measurement..
2 Quick Review Redox: Reduction-Oxidation, an electron transfer process Oxidation: loss one or more e - Reduction: gain one or more e - Oxidation number: the charge of the atom or molecule would have Pure element and neutral compound 0 Mono- and poly-atomic ions sum of oxidation number is ionic charge Check your understanding CaBr 2 ; Ca = +2, Br = -1, Oxidation number (pure element), =(+2)+2(-1)=0 HCO 3 - O = -2 H = +1 C =? K 2 Cr 2 O 7 O = -2 K = +1 Cr =?
3
4 Quick Review (Cont d) Electrochemistry: study of the interchange between chemical change and electrical work Electrochemical cells: systems utilizing a redox reaction to produce or use electrical energy
5 Becomes smaller Becomes larger Zn anode Cu cathode Cell and Cell Notation Anode: Electrode site of oxidation Cathode: Electrode site of reduction Electrons flow from anode to cathode Salt bridge: Maintains electrical neutrality, allows current to flow, prevent solutions mixing Positive ion migrates to cathode Negative ion migrates to anode Cell notation: Anode Salt Bridge Cathode
6 The difference in electrical potential between the anode and cathode is called: cell voltage electromotive force (emf) cell potential E + 0 Cell 0 0 = Eoxidation E (Unit: Volts) reduction Note: Volt (V) = Joule (J) Coulomb (C) Cell Potential
7
8 Standard Electrode Potentials Standard reduction potential (E 0 ) is the voltage associated with a reduction reaction at an electrode when all solutes are 1 M and all gases are at 1 atm. Reduction Reaction 2e - + 2H + (1 M) H 2 (1 atm) E 0 = 0 V Reference electrode Standard hydrogen electrode (SHE)
9 (Cathode) (Anode) Note: Copper reduction potential, E o = (If copper is reduced (at cathode), voltmeter can give a reading- positive) Note: Zn reduction potential is negative. Change Zn as anode
10 E 0 is for the reaction as written The half-cell reactions are reversible; the sign of E 0 changes when the reaction is reversed Changing the stoichiometric coefficients of a half-cell reaction does not change the value of E 0 The more positive E 0 the greater the tendency for the substance to be reduced Spontaneity of Redox Reaction E = E + 0 Cell 0 oxidation E 0 reduction E o reduction=-e o oxidation + E CELL : spontaneous reaction E CELL = 0 :equilibrium -E CELL : non-spontaneous reaction More positive E CELL means stronger oxidizing agent or more likely to be reduced
11 Balance the Half-Cell Reactions Write separate equations (half-reactions) for oxidation and reduction For each half-reaction Balance elements involved in e - transfer Balance number e - lost and gained To balance e - multiply each half-reaction by whole numbers Add half-reactions/cancel like terms (e - ) Check that all atoms and charges balance Check your understanding?? e e e e Zn(s) Zn 2+ SO M Zn 2+ solution Cu 2+ SO M Cu 2+ solution Cu(s)?? Anode Cathode??
12 Check your understanding A half-cell reduction reaction is Fe(OH) 2 (s) + 2e - Fe (s) + 2OH - (aq) E o = V Is to combine with another half-cell, which the reduction reaction is given as: a) Al 3+ (aq) + 3e - Al (s) E o = V b) AgBr (s) + e - Ag (s) + Br - (aq) E o = V Determine E o cell, and whether Fe is oxidized or reduced. Nernst Equation G = G 0 + RTlnQ G 0 = -nfe 0 cell the emf for an electrochemical cell to be calculated if the activity and E are known. -nfe cell =-nfe 0 cell +RTlnQ E cell =E 0 cell - RTln Q nf E cell = E 0 cell ln Q n E cell =E 0 cell log Q n Note: At equilibrium, G=0, thus E cell =0
13 G o = -nfe o cell Faraday, F: charge on 1 mole e - F = C/mole n= moles of balanced e - ΔG 0 = -RT ln K -RT ln K = -nfe 0 cell ΔG 0 = -nfe 0 cell 0 E Cell = RT nf ln K RT F J 8.31 molk = C mole ( 298K ) = E Cell = ln K n = logk n
14 Entropy Change The reaction entropy related to ΔG R pprrtenftgs = Δ = Δ o o o Measurement of the T dependence of E can be used to determine ΔS R To obtain the entropy change for the cell reaction The reaction entropy related to ΔG R PTEnFTnFEH + = Δ o o o Enthalpy Change H o = G o + T S o
15 Example (from text book) The half-cell reduction reactions, Fe 3+ (aq) + e - Fe 2+ (aq) Fe 2+ (aq) + 2e - Fe (s) E o = V E o = V Calculate E o for half-cell reduction reaction Fe 3+ (aq) + 3e - Fe (s) Example Calculate ΔG o r and the equilibrium constant at K for two half-cell reduction reactions: Cr 2 O 7 2- (aq) + 14H + (aq) + 6e - 2Cr 3+ (aq) + 7H 2 O(l) Eº = V 2H + (aq) + 2e - H 2 (g) Eº = 0.00 V
16 Example The standard potential E for a given cell in which a two electron transfer takes place is 1.10 V at K and ( E / T) = V K 1. Calculate ΔG rxn, ΔS rxn, ΔH rxn. Assume that n = 2. Check your understanding Calculate the equilibrium constant at K for the following half-cell reactions a) Cathode: NO H + + 3e - NO + 2H 2 O Eº = V Anode: 2H 2 O O 2 + 4H + + 4e - Eº = V b) Anode: Cd(OH) 2 + 2e - Cd + 2OH - Eº = 0.809V Cathode: O 2 + 2H 2 O + 4e - 4OH - Eº = V
17 Example Calculate the equilibrium constant at 25 C for the reaction occurring in the Daniell cell, if the standard EMF is 1.10 V. Calculate the equilibrium constant for the reaction H 2 + 2Fe 3+ 2H + + 2Fe 2+ Galvanic cell vs. Electrolytic cell
18
19 Galvanic cell vs. Electrolytic cell Electrochemical cell (Galvanic Cell) Converts chemical energy into electrical energy Redox reaction is spontaneous and is responsible for the production of electrical energy The two half-cells are set up in different containers, being connected through the salt bridge or porous partition Anode is negative and cathode is the positive electrode. The reaction at the anode is oxidation and that at the cathode is reduction. The electrons are supplied by the species getting oxidized. They move from anode to the cathode in the external circuit. Electrolytic cell Converts electrical energy into chemical energy Redox reaction is not spontaneous and electrical energy has to be supplied to initiate the reaction Both the electrodes are placed in a same container in the solution of molten electrolyte Here, the anode is positive and cathode is the negative electrode. The reaction at the anode is oxidation and that at the cathode is reduction. The external battery supplies the electrons. They enter through the cathode and come out through the anode.
17.1 Redox Chemistry Revisited
Chapter Outline 17.1 Redox Chemistry Revisited 17.2 Electrochemical Cells 17.3 Standard Potentials 17.4 Chemical Energy and Electrical Work 17.5 A Reference Point: The Standard Hydrogen Electrode 17.6
More informationElectrochemistry objectives
Electrochemistry objectives 1) Understand how a voltaic and electrolytic cell work 2) Be able to tell which substance is being oxidized and reduced and where it is occuring the anode or cathode 3) Students
More informationELECTROCHEMISTRY OXIDATION-REDUCTION
ELECTROCHEMISTRY Electrochemistry involves the relationship between electrical energy and chemical energy. OXIDATION-REDUCTION REACTIONS SPONTANEOUS REACTIONS Can extract electrical energy from these.
More informationOxidation-Reduction Review. Electrochemistry. Oxidation-Reduction Reactions. Oxidation-Reduction Reactions. Sample Problem.
1 Electrochemistry Oxidation-Reduction Review Topics Covered Oxidation-reduction reactions Balancing oxidationreduction equations Voltaic cells Cell EMF Spontaneity of redox reactions Batteries Electrolysis
More informationElectrochemistry. The study of the interchange of chemical and electrical energy.
Electrochemistry The study of the interchange of chemical and electrical energy. Oxidation-reduction (redox) reaction: involves a transfer of electrons from the reducing agent to the oxidizing agent. oxidation:
More informationReview: Balancing Redox Reactions. Review: Balancing Redox Reactions
Review: Balancing Redox Reactions Determine which species is oxidized and which species is reduced Oxidation corresponds to an increase in the oxidation number of an element Reduction corresponds to a
More informationChapter 18 Electrochemistry. Electrochemical Cells
Chapter 18 Electrochemistry Chapter 18 1 Electrochemical Cells Electrochemical Cells are of two basic types: Galvanic Cells a spontaneous chemical reaction generates an electric current Electrolytic Cells
More informationOxidation number. The charge the atom would have in a molecule (or an ionic compound) if electrons were completely transferred.
Oxidation number The charge the atom would have in a molecule (or an ionic compound) if electrons were completely transferred. 1. Free elements (uncombined state) have an oxidation number of zero. Na,
More informationChapter 19: Electrochemistry
Chapter 19: Electrochemistry Overview of the Chapter review oxidation-reduction chemistry basics galvanic cells spontaneous chemical reaction generates a voltage set-up of galvanic cell & identification
More informationOxidation-reduction (redox) reactions
Oxidation-reduction (redox) reactions Reactions in which there are changes in oxidation state (oxidation number) between reactants and products 2 MnO 4- + 10 Br - + 16 H + 2 Mn 2+ + 5 Br 2 + 8 H 2 O One
More informationLecture 14. Thermodynamics of Galvanic (Voltaic) Cells.
Lecture 14 Thermodynamics of Galvanic (Voltaic) Cells. 51 52 Ballard PEM Fuel Cell. 53 Electrochemistry Alessandro Volta, 1745-1827, Italian scientist and inventor. Luigi Galvani, 1737-1798, Italian scientist
More informationHg2 2+ (aq) + H2(g) 2 Hg(l) + 2H + (aq)
The potential difference between two electrodes in a cell is called the electromotive force, or The EMF of a voltaic cell is called the The cell voltage of a voltaic cell will be a Note: We are used to
More informationCHAPTER 17: ELECTROCHEMISTRY. Big Idea 3
CHAPTER 17: ELECTROCHEMISTRY Big Idea 3 Electrochemistry Conversion of chemical to electrical energy (discharge). And its reverse (electrolysis). Both subject to entropic caution: Convert reversibly to
More informationLecture Presentation. Chapter 20. Electrochemistry. James F. Kirby Quinnipiac University Hamden, CT Pearson Education, Inc.
Lecture Presentation Chapter 20 James F. Kirby Quinnipiac University Hamden, CT is the study of the relationships between electricity and chemical reactions. It includes the study of both spontaneous and
More informationElectrode Potentials and Their Measurement
Electrochemistry Electrode Potentials and Their Measurement Cu(s) + 2Ag + (aq) Cu(s) + Zn 2+ (aq) Cu 2+ (aq) + 2 Ag(s) No reaction Zn(s) + Cu 2+ (aq) Cu(s) + Zn 2+ (aq) In this reaction: Zn (s) g Zn 2+
More informationChapter 20. Electrochemistry
Chapter 20. Electrochemistry 20.1 Oxidation-Reduction Reactions Oxidation-reduction reactions = chemical reactions in which the oxidation state of one or more substance changes (redox reactions). Recall:
More informationElectrochemistry. Chapter 18. Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display.
Electrochemistry Chapter 18 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. 1 Electrochemical processes are oxidation-reduction reactions in which: the energy
More informationSection Electrochemistry represents the interconversion of chemical energy and electrical energy.
Chapter 21 Electrochemistry Section 21.1. Electrochemistry represents the interconversion of chemical energy and electrical energy. Electrochemistry involves redox (reduction-oxidation) reactions because
More informationChapter 20. Electrochemistry
Chapter 20. Electrochemistry 20.1 OxidationReduction Reactions Oxidationreduction reactions = chemical reactions in which the oxidation state of one or more substance changes (redox reactions). Recall:
More informationPart One: Introduction. a. Chemical reactions produced by electric current. (electrolysis)
CHAPTER 19: ELECTROCHEMISTRY Part One: Introduction A. Terminology. 1. Electrochemistry deals with: a. Chemical reactions produced by electric current. (electrolysis) b. Production of electric current
More informationElectrochem: It s Got Potential!
Electrochem: It s Got Potential! Presented by: Denise DeMartino Westlake High School, Eanes ISD Pre-AP, AP, and Advanced Placement are registered trademarks of the College Board, which was not involved
More informationCh 20 Electrochemistry: the study of the relationships between electricity and chemical reactions.
Ch 20 Electrochemistry: the study of the relationships between electricity and chemical reactions. In electrochemical reactions, electrons are transferred from one species to another. Learning goals and
More informationChapter Nineteen. Electrochemistry
Chapter Nineteen Electrochemistry 1 Electrochemistry The study of chemical reactions through electrical circuits. Monitor redox reactions by controlling electron transfer REDOX: Shorthand for REDuction-OXidation
More informationChapter 18. Electrochemistry
Chapter 18 Electrochemistry Section 17.1 Spontaneous Processes and Entropy Section 17.1 http://www.bozemanscience.com/ap-chemistry/ Spontaneous Processes and Entropy Section 17.1 Spontaneous Processes
More informationTopic 19 Redox 19.1 Standard Electrode Potentials. IB Chemistry T09D04
Topic 19 Redox 19.1 Standard Electrode Potentials IB Chemistry T09D04 19.1 Standard Electrode Potentials 19.1.1 Describe the standard hydrogen electrode. (2) 19.1.2 Define the term standard electrode potential,
More informationCh 18 Electrochemistry OIL-RIG Reactions
Ch 18 Electrochemistry OIL-RIG Reactions Alessandro Volta s Invention Modified by Dr. Cheng-Yu Lai Daily Electrochemistry Appliactions Electrochemistry: The area of chemistry that examines the transformations
More informationChapter 20. Electrochemistry. Chapter 20 Problems. Electrochemistry 7/3/2012. Problems 15, 17, 19, 23, 27, 29, 33, 39, 59
Chemistry, The Central Science, 11th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten Chapter 20 John D. Bookstaver St. Charles Community College Cottleville, MO Chapter 20 Problems
More informationA + B C +D ΔG = ΔG + RTlnKp. Me n+ + ne - Me. Me n n
A + B C +D ΔG = ΔG + RTlnKp Me n+ + ne - Me K p a a Me Me n a n e 1 mol madde 6.2 x 1 23 atom elektron yükü 1.62 x 1-19 C FARADAY SABİTİ: 6.2 x 1 23 x 1.62 x 1-19 = 96485 A.sn (= coulomb) 1 Faraday 965
More informationLecture Presentation. Chapter 20. Electrochemistry. James F. Kirby Quinnipiac University Hamden, CT Pearson Education
Lecture Presentation Chapter 20 James F. Kirby Quinnipiac University Hamden, CT is the study of the relationships between electricity and chemical reactions. It includes the study of both spontaneous and
More informationChapter 17. Electrochemistry
Chapter 17 Electrochemistry Contents Galvanic cells Standard reduction potentials Cell potential, electrical work, and free energy Dependence of cell potential on concentration Batteries Corrosion Electrolysis
More informationREVIEW QUESTIONS Chapter 19
Chemistry 10 ANSWER KEY REVIEW QUESTIONS Chapter 19 1. For each of the following unbalanced equations, (i) write the half-reactions for oxidation and reduction, and (ii) balance the overall equation in
More informationChapter 20 Electrochemistry
Chapter 20 Electrochemistry Learning goals and key skills: Identify oxidation, reduction, oxidizing agent, and reducing agent in a chemical equation Complete and balance redox equations using the method
More informationChemistry 102 Chapter 19 OXIDATION-REDUCTION REACTIONS
OXIDATION-REDUCTION REACTIONS Some of the most important reaction in chemistry are oxidation-reduction (redox) reactions. In these reactions, electrons transfer from one reactant to the other. The rusting
More informationElectrochemistry. Remember from CHM151 G E R L E O 6/24/2014. A redox reaction in one in which electrons are transferred.
Electrochemistry Remember from CHM151 A redox reaction in one in which electrons are transferred Reduction Oxidation For example: L E O ose lectrons xidation G E R ain lectrons eduction We can determine
More informationELECTROCHEMISTRY. Oxidation/Reduction
ELECTROCHEMISTRY Electrochemistry involves the relationship between electrical energy and chemical energy. OXIDATION-REDUCTION REACTIONS SPONTANEOUS REACTIONS Examples: voltaic cells, batteries. NON-SPONTANEOUS
More informationAnnouncements. Comprehensive Final Exam: March 24 7:30AM - 9:30 C114 2,9,10,11,13,17,22,29,31,38,40,44,46,50,53,58,62,64,65,70, 72,73,82,85,87
Announcements Exam 3 March 17 Comprehensive Final Exam: March 24 7:30AM - 9:30 C114 Problems Chapter 21: 2,9,10,11,13,17,22,29,31,38,40,44,46,50,53,58,62,64,65,70, 72,73,82,85,87 Up to but not including
More informationRedox reactions & electrochemistry
Redox reactions & electrochemistry Electrochemistry Electrical energy ; Chemical energy oxidation/reduction = redox reactions Electrochemistry Zn + Cu 2+ º Zn 2+ + Cu Oxidation-reduction reactions always
More informationDr. Anand Gupta
By Dr Anand Gupta Mr. Mahesh Kapil Dr. Anand Gupta 09356511518 09888711209 anandu71@yahoo.com mkapil_foru@yahoo.com Electrochemistry Electrolysis Electric energy Chemical energy Galvanic cell 2 Electrochemistry
More informationChapter 20. Electrochemistry Recommendation: Review Sec. 4.4 (oxidation-reduction reactions) in your textbook
Chapter 20. Electrochemistry Recommendation: Review Sec. 4.4 (oxidation-reduction reactions) in your textbook 20.1 Oxidation-Reduction Reactions Oxidation-reduction reactions = chemical reactions in which
More informationElectron Transfer Reactions
ELECTROCHEMISTRY 1 Electron Transfer Reactions 2 Electron transfer reactions are oxidation- reduction or redox reactions. Results in the generation of an electric current (electricity) or be caused by
More informationChapter 17 Electrochemistry
Chapter 17 Electrochemistry 17.1 Galvanic Cells A. Oxidation-Reduction Reactions (Redox Rxns) 1. Oxidation = loss of electrons a. the substance oxidized is the reducing agent 2. Reduction = gain of electrons
More informationElectrochem 1 Electrochemistry Some Key Topics Conduction metallic electrolytic Electrolysis effect and stoichiometry Galvanic cell Electrolytic cell Electromotive Force (potential in volts) Electrode
More informationChemistry: The Central Science. Chapter 20: Electrochemistry
Chemistry: The Central Science Chapter 20: Electrochemistry Redox reaction power batteries Electrochemistry is the study of the relationships between electricity and chemical reactions o It includes the
More informationElectrochemistry. Review oxidation reactions and how to assign oxidation numbers (Ch 4 Chemical Reactions).
Electrochemistry Oxidation-Reduction: Review oxidation reactions and how to assign oxidation numbers (Ch 4 Chemical Reactions). Half Reactions Method for Balancing Redox Equations: Acidic solutions: 1.
More information25. A typical galvanic cell diagram is:
Unit VI(6)-III: Electrochemistry Chapter 17 Assigned Problems Answers Exercises Galvanic Cells, Cell Potentials, Standard Reduction Potentials, and Free Energy 25. A typical galvanic cell diagram is: The
More informationChapter 20. Electrochemistry
Chemistry, The Central Science, 10th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten Chapter 20 John D. Bookstaver St. Charles Community College St. Peters, MO 2006, Prentice Hall,
More informationZn+2 (aq) + Cu (s) Oxidation: An atom, ion, or molecule releases electrons and is oxidized. The oxidation number of the atom oxidized increases.
Oxidation-Reduction Page 1 The transfer of an electron from one compound to another results in the oxidation of the electron donor and the reduction of the electron acceptor. Loss of electrons (oxidation)
More informationSpontaneous Redox Between Zinc Metal and Copper(II) Ions. Zn 2+ Zn + 2e- Cu 2+ NO 3
Spontaneous Redox Between Zinc Metal and Copper(II) Ions Zn 2+ Cu 2+ NO 3 _ Zn + 2e- Cu Zn 0 + Cu 2+ º Zn 2+ + Cu 0 spontaneous red 1 ox 2 ox 1 red 2 Spontaneous Redox Between Copper Metal and Silver Ions
More information18.2 Voltaic Cell. Generating Voltage (Potential) Dr. Fred Omega Garces. Chemistry 201. Miramar College. 1 Voltaic Cell.
18.2 Voltaic Cell Generating Voltage (Potential) Dr. Fred Omega Garces Chemistry 201 Miramar College 1 Voltaic Cell Redox Between If Zn (s) and Cu 2+ (aq) is in the same solution, then the electrons transfer
More informationChapter 20 Electrochemistry
Chapter 20 Electrochemistry Electrochemical Cell Consists of electrodes which dip into an electrolyte & in which a chem. rxn. uses or generates an electric current Voltaic (Galvanic) Cell Spont. rxn. -
More informationElectrochemistry Pearson Education, Inc. Mr. Matthew Totaro Legacy High School AP Chemistry
2012 Pearson Education, Inc. Mr. Matthew Totaro Legacy High School AP Chemistry Electricity from Chemistry Many chemical reactions involve the transfer of electrons between atoms or ions electron transfer
More informationChapter 18 Electrochemistry
Chapter 18 Electrochemistry Definition The study of the interchange of chemical and electrical energy in oxidation-reduction (redox) reactions This interchange can occur in both directions: 1. Conversion
More informationLecture 27 Chapter 19, Sections 3-4 Galvanic Cells Electrochemical Potential
Lecture 27 Chapter 19, Sections 3-4 Galvanic Cells Electrochemical Potential Galvanic Cells Defined Standard Hydrogen Electrode Standard Reduction Potentials Redox Balancing One More Example This time
More informationChapter 19: Redox & Electrochemistry
Chapter 19: Redox & Electrochemistry 1. Oxidation-Reduction Reactions Definitions Oxidation - refers to the of electrons by a molecule, atom or ion Reduction - refers to the of electrons by an molecule,
More informationLecture Presentation. Chapter 18. Electrochemistry. Sherril Soman Grand Valley State University Pearson Education, Inc.
Lecture Presentation Chapter 18 Electrochemistry Sherril Soman Grand Valley State University Harnessing the Power in Nature The goal of scientific research is to understand nature. Once we understand the
More informationAssigning Oxidation Numbers:
Assigning Oxidation Numbers: 1. Oxidation number of a free element or diatomic molecule is zero. Ex: Na(s), Cu(s), H 2 (g), F 2 (g) 2. In most cases the oxidation number of hydrogen is +1, oxygen is -2,
More informationElectrochemistry 1 1
Electrochemistry 1 1 Half-Reactions 1. Balancing Oxidation Reduction Reactions in Acidic and Basic Solutions Voltaic Cells 2. Construction of Voltaic Cells 3. Notation for Voltaic Cells 4. Cell Potential
More informationOxidation (oxidized): the loss of one or more electrons. Reduction (reduced): the gain of one or more electrons
1 of 13 interesting links: Battery Chemistry Tutorial at http://www.powerstream.com/batteryfaq.html Duracell Procell: Battery Chemistry at http://www.duracell.com/procell/chemistries /default.asp I. Oxidation
More informationChapter 18. Electrochemistry
Chapter 18 Electrochemistry Oxidation-Reduction Reactions Review of Terms Oxidation-reduction (redox) reactions always involve a transfer of electrons from one species to another. Oxidation number - the
More informationElectrochemistry. Galvanic Cell. Page 1. Applications of Redox
Electrochemistry Applications of Redox Review Oxidation reduction reactions involve a transfer of electrons. OIL- RIG Oxidation Involves Loss Reduction Involves Gain LEO-GER Lose Electrons Oxidation Gain
More informationLecture 30 Chapter 19, Sections 3-4 Galvanic Cells Electrochemical Potential
Lecture 30 Chapter 19, Sections 3-4 Galvanic Cells Electrochemical Potential Galvanic Cells Defined Standard Hydrogen Electrode Standard Reduction Potentials Redox Balancing One More Example OK, then here
More informationCHM 213 (INORGANIC CHEMISTRY): Applications of Standard Reduction Potentials. Compiled by. Dr. A.O. Oladebeye
CHM 213 (INORGANIC CHEMISTRY): Applications of Standard Reduction Potentials Compiled by Dr. A.O. Oladebeye Department of Chemistry University of Medical Sciences, Ondo, Nigeria Electrochemical Cell Electrochemical
More informationChapter 19 ElectroChemistry
Chem 1046 General Chemistry by Ebbing and Gammon, 9th Edition George W.J. Kenney, Jr, Professor of Chemistry Last Update: 11July2009 Chapter 19 ElectroChemistry These Notes are to SUPPLIMENT the Text,
More informationAP CHEMISTRY NOTES 12-1 ELECTROCHEMISTRY: ELECTROCHEMICAL CELLS
AP CHEMISTRY NOTES 12-1 ELECTROCHEMISTRY: ELECTROCHEMICAL CELLS Review: OXIDATION-REDUCTION REACTIONS the changes that occur when electrons are transferred between reactants (also known as a redox reaction)
More information2013 AP CHEMISTRY FREE-RESPONSE QUESTIONS
2013 AP CHEMISTRY FREE-RESPONSE QUESTIONS 2. Answer the following questions involving the stoichiometry and thermodynamics of reactions containing aluminum species. 2 Al 2 O 3 (l) + 3 C(s) 4 Al(l) + 3
More informationChapter 19 - Electrochemistry. the branch of chemistry that examines the transformations between chemical and electrical energy
Chapter 19 - Electrochemistry the branch of chemistry that examines the transformations between chemical and electrical energy 19.1 Redox Chemistry Revisited A Spontaneous Redox Reaction Znº(s) + Cu 2+
More information9/19/2018. Corrosion Thermodynamics 2-3. Course Outline. Guiding Principles. Why study thermodynamics? Guiding Principles
Kwame Nkrumah University of Science & Technology, Kumasi, Ghana Week 1 Course Outline Topic Introduction: Reactivity types, corrosion definition, atmospheric corrosion, classification, effects, costs,
More informationLecture Presentation. Chapter 20. Electrochemistry. James F. Kirby Quinnipiac University Hamden, CT Pearson Education
Lecture Presentation Chapter 20 James F. Kirby Quinnipiac University Hamden, CT is the study of the relationships between electricity and chemical reactions. It includes the study of both spontaneous and
More informationChapter 18: Electrochemistry
Chapter 18: Electrochemistry Oxidation States An oxidation-reduction reaction, or redox reaction, is one in which electrons are transferred. 2Na + Cl 2 2NaCl Each sodium atom is losing one electron to
More informationlect 26:Electrolytic Cells
lect 26:Electrolytic Cells Voltaic cells are driven by a spontaneous chemical reaction that produces an electric current through an outside circuit. These cells are important because they are the basis
More informationElectrochemistry. Slide 1 / 144. Slide 2 / 144. Slide 3 / 144. Electrochemistry. Electrochemical Reactions
Slide 1 / 144 Electrochemistry Electrochemistry Slide 2 / 144 Electrochemistry deals with relationships between reactions and electricity In electrochemical reactions, electrons are transferred from one
More informationEMA4303/5305 Electrochemical Engineering Lecture 02 Equilibrium Electrochemistry
EMA4303/5305 Electrochemical Engineering Lecture 02 Equilibrium Electrochemistry Dr. Junheng Xing, Prof. Zhe Cheng Mechanical & Materials Engineering Florida International University 2 Equilibrium Electrochemistry
More informationCHEM J-14 June 2014
CHEM1101 2014-J-14 June 2014 An electrochemical cell consists of an Fe 2+ /Fe half cell with unknown [Fe 2+ ] and a Sn 2+ /Sn half-cell with [Sn 2+ ] = 1.10 M. The electromotive force (electrical potential)
More informationTypes of Cells Chemical transformations to produce electricity- Galvanic cell or Voltaic cell (battery)
Electrochemistry Some Key Topics Conduction metallic electrolytic Electrolysis effect and stoichiometry Galvanic cell Electrolytic cell Electromotive Force Electrode Potentials Gibbs Free Energy Gibbs
More informationCHEM J-8 June /01(a)
CHEM1001 2012-J-8 June 2012 22/01(a) A galvanic cell has the following cell reaction: D(s) + 2Zn 2+ (aq) 2Zn(s) + D 4+ (aq) Write the overall cell reaction in shorthand cell notation. E = 0.18 V 8 D(s)
More informationQ1. Why does the conductivity of a solution decrease with dilution?
Q1. Why does the conductivity of a solution decrease with dilution? A1. Conductivity of a solution is the conductance of ions present in a unit volume of the solution. On dilution the number of ions per
More informationElectrochemical Cells
Electrochemistry Electrochemical Cells The Voltaic Cell Electrochemical Cell = device that generates electricity through redox rxns 1 Voltaic (Galvanic) Cell An electrochemical cell that produces an electrical
More informationΔG = -nfe cell. Electrode Potentials. The cell potential E cell is related to the free energy of the reaction ΔG by:
Electrode Potentials Ahmad Aqel Ifseisi Assistant Professor of Analytical Chemistry College of Science, Department of Chemistry King Saud University P.O. Box 2455 Riyadh 11451 Saudi Arabia Building: 05,
More informationCHEMISTRY - CLUTCH CH.18 - ELECTROCHEMISTRY.
!! www.clutchprep.com CONCEPT: OXIDATION-REDUCTION REACTIONS Chemists use some important terminology to describe the movement of electrons. In reactions we have the movement of electrons from one reactant
More information20.1 Consider the Brønsted-Lowry acid-base reaction and the redox reaction below. + A
20 Electrochemistry Visualizing Concepts 20.1 Consider the Brønsted-Lowry acid-base reaction and the redox reaction below. HA + B BH + + A HA H + + A B + H + BH + X(red) + Y + (ox) X + (ox) + Y(red) X(red)
More informationChapter 18 problems (with solutions)
Chapter 18 problems (with solutions) 1) Assign oxidation numbers for the following species (for review see section 9.4) a) H2SO3 H = +1 S = +4 O = -2 b) Ca(ClO3)2 Ca = +2 Cl = +5 O = -2 c) C2H4 C = -2
More informationChemistry 2000 Lecture 15: Electrochemistry
Chemistry 2000 Lecture 15: Electrochemistry Marc R. Roussel February 21, 2018 Marc R. Roussel Chemistry 2000 Lecture 15: Electrochemistry February 21, 2018 1 / 33 Electrochemical cells Electrochemical
More informationGalvanic Cells Spontaneous Electrochemistry. Electrolytic Cells Backwards Electrochemistry
Today Galvanic Cells Spontaneous Electrochemistry Electrolytic Cells Backwards Electrochemistry Balancing Redox Reactions There is a method (actually several) Learn one (4.10-4.12) Practice (worksheet)
More informationGeneral Chemistry I. Dr. PHAN TẠI HUÂN Faculty of Food Science and Technology Nong Lam University
General Chemistry I Dr. PHAN TẠI HUÂN Faculty of Food Science and Technology Nong Lam University Module 7: Oxidation-reduction reactions and transformation of chemical energy Oxidation-reduction reactions
More informationUnit 12 Redox and Electrochemistry
Unit 12 Redox and Electrochemistry Review of Terminology for Redox Reactions OXIDATION loss of electron(s) by a species; increase in oxidation number. REDUCTION gain of electron(s); decrease in oxidation
More informationAP Chemistry Readiness Thermodynamics and Electrochemistry Review Page 1 of 15. AP Chemistry Review Session UCLA April 23, 2016
AP Chemistry Readiness Thermodynamics and Electrochemistry Review Page 1 of 15 AP Chemistry Review Session UCLA April 23, 2016 Michael A. Morgan Richard Erdman Larry Walker mmorgan@lausd.net xchemteach@yahoo.com
More informationElectrochemistry (Galvanic and Electrolytic Cells) Exchange of energy in chemical cells
Electrochemistry (Galvanic and Electrolytic Cells) Exchange of energy in chemical cells Oxidation loss of electrons (oxidation number increases) OIL RIG Reduction gain of electrons (oxidation number decreases)
More informationChapter 20. Electrochemistry
Chapter 20. Electrochemistry Sample Exercise 20.1 (p. 845) The nickelcadmium (nicad) battery, a rechargeable dry cell used in batteryoperated devices, uses the following redox reaction to generate electricity:
More informationCHEMISTRY 13 Electrochemistry Supplementary Problems
1. When the redox equation CHEMISTRY 13 Electrochemistry Supplementary Problems MnO 4 (aq) + H + (aq) + H 3 AsO 3 (aq) Mn 2+ (aq) + H 3 AsO 4 (aq) + H 2 O(l) is properly balanced, the coefficients will
More informationElectrochemistry Pulling the Plug on the Power Grid
Electrochemistry 18.1 Pulling the Plug on the Power Grid 18.3 Voltaic (or Galvanic) Cells: Generating Electricity from Spontaneous Chemical Reactions 18.4 Standard Electrode Potentials 18.7 Batteries:
More informationHow to Assign Oxidation Numbers. Chapter 18. Principles of Reactivity: Electron Transfer Reactions. What is oxidation? What is reduction?
Chapter 18 Principles of Reactivity: Electron Transfer Reactions What is oxidation? When a molecule/ion loses electrons (becomes more positive) Whatever is oxidized is the reducing agent What is reduction?
More informationCh. 13 Fundamentals of Electrochemistry
Ch. 13 Fundamentals of Electrochemistry 13.1 13-1. Basic Concepts of electrochemistry redox reaction : reactions with electron transfer oxidized : loses electrons reduced : gains electrons Fe 3+ + V 2+
More informationIntroduction. can be rewritten as follows: Oxidation reaction. H2 2H + +2e. Reduction reaction: F2+2e 2F. Overall Reaction H2+F2 2H + +2F
Electrochemistry is the study of chemical processes that cause electrons to move. This movement of electrons is called electricity, which can be generated by movements of electrons from one element to
More informationWe can use chemistry to generate electricity... this is termed a Voltaic (or sometimes) Galvanic Cell
Unit 6 Electrochemistry Chemistry 020, R. R. Martin Electrochemistry Electrochemistry is the study of the interconversion of electrical and chemical energy. We can use chemistry to generate electricity...
More informationELECTROCHEMISTRY Chapter 14
ELECTROCHEMISTRY Chapter 14 Basic Concepts: Overview of Electrochemical Process at Constant T, P (14-1) ΔG = ΔG o + RT ln Q = w elec (maximum) = qe = ItE (exp) (E intensive parameter, q extensive) = nfe
More information12.05 Galvanic Cells. Zn(s) + 2 Ag + (aq) Zn 2+ (aq) + 2 Ag(s) Ni(s) + Pb 2+ (aq) «Ni 2+ (aq) + Pb(s)
12.05 Galvanic Cells 1. In an operating voltaic cell, reduction occurs A) at the anode B) at the cathode C) in the salt bridge D) in the wire 2. Which process occurs in an operating voltaic cell? A) Electrical
More informationRedox and Electrochemistry
Redox and Electrochemistry 1 Electrochemistry in Action! 2 Rules for Assigning Oxidation Numbers The oxidation number of any uncombined element is 0. The oxidation number of a monatomic ion equals the
More informationCHEM J-12 June 2013
CHEM1101 2013-J-12 June 2013 In concentration cells no net chemical conversion occurs, however a measurable voltage is present between the two half-cells. Explain how the voltage is produced. 2 In concentration
More informationCHAPTER 17 ELECTROCHEMISTRY
Advanced Chemistry Approximate Timeline Students are expected to keep up with class work when absent. CHAPTER 17 ELECTROCHEMISTRY Day Plans for the day Assignment(s) for the day 17.1 Galvanic Cells Assignment
More informationChemistry 132 NT. Electrochemistry. Oxidation-Reduction Reactions
Chemistry 132 NT If you ever catch on fire, try to avoid seeing yourself in the mirror, because I bet that s what really throws you into a panic. Jack Handey 1 Chem 132 NT Electrochemistry Module 1 HalfReactions
More information