BATTERIES AND ELECTROLYTIC CELLS. Practical Electrochemistry
|
|
- Joshua Bishop
- 5 years ago
- Views:
Transcription
1 BATTERIES AND ELECTROLYTIC CELLS Practical Electrochemistry
2 How Batteries Work One of the most practical applications of spontaneous redox reactions is making batteries. In a battery, a spontaneous electron transfer from a reducer to an oxidizer is forced to occur through an external wire. As the electrons crowd through the wire, they give up their energy to do work.
3 Spontaneous Electron Transfer Zinc atoms will give up their 2 valence electrons to copper ions easily. 2+ Zn Cu 0 (s) Cu 2+
4 Remote Transfer If a barrier is placed between Zn and Cu 2+, the transfer can still take place, but through a wire. Zn
5 Electrochemical Cells Electrochemical cells are those in which spontaneous electron transfer takes place through a wire. They are also called voltaic or galvanic cells. You probably know them best by their practical name: batteries. We think of batteries as electrical, but they are really chemical devices that produce electricity.
6 Batteries Batteries are really quite simple devices that contain 2 half-cells with electrodes and solutions. Each half-cell is usually made of a metal electrode and a solution containing a salt of the same metal. There is an external wire connecting the 2 electrodes. The electrodes are the negative anode and the positive cathode.
7 Batteries An electrical power using device (resistor) is placed in the wire, and as the electrons crowd through the device, they give up their energy to make it operate: ex, a light bulb in a flashlight. The circuit must however be complete for electrons to flow, so a salt bridge or porous barrier between half-cells is also necessary.
8 Basic Battery Zinc metal atoms with 2 electrons Copper atoms with 2 electrons Zn 2+ aqueous ions 2+ Cl- 2+ Hungry Cu 2+ ions Cl- Zn Cu Anions move across the 2+ Cl- Cl- barrier to Cl- Cl- complete the circuit. Anode half-cell (-) Cathode half-cell (+) Zn Zn e - Cu e - Cu
9 Disclaimer Unlike the animations, electrons do not really zip through a wire from one end to the other. It s actually more like a tube full of ping-pong balls. If you push a new ball into one end, they all move down a little, and the one on the other end pops out. Electrons in a real electric circuit actually move quite slowly.
10 Basic Battery The anode is slowly dissolving away as the atoms become soluble ions. The cations of the cathode compartment are becoming metal atoms, so the cathode is getting more massive. When either the anode is completely gone or the cathode cations are gone, the battery is dead.
11 Why batteries die on the shelf Cl- Cl- Cl- Cl- - Cl- + Zn Cu Cl- All the energy is released as heat and no work is done. However, the barrier must be porous for the battery to function normally.
12 Rechargeable Batteries Zn Generator: electron pump Cl- 2+ Cl- Cl- Cl- Cu Cl- Cl- Cl- Cl- With a rechargeable battery, a generator pushes the electrons backwards in the circuit. Even though the electrons don t want to go in this direction, the generator forces them. The electrons are restored to the anode and the battery can be used again.
13 Electromotive Force (emf) What is electromotive force? Emf is symbolized E. It is the pressure with which electrons flow through a circuit. Emf is measured in volts. So, how does one go about measuring the voltage produced by a battery? Or, are all batteries the same except for size?
14 Half-Cell Potentials Years ago, scientists agreed on a standard reference half-cell, against which to measure all other halfreactions. The reference they chose was a halfcell with H + in the solution, and a platinum electrode. The reaction occurring in the cell is: 2H + (aq) + 2 e - H 2 (g) Hydrogen ions are reduced. (The Pt is an inert electrode.)
15 Half-Cell Potentials The hydrogen half-cell was assigned a voltage of E = 0.0Volts. Various reactions were used for the other half-cell and the voltages recorded. If an element is easier to reduce than hydrogen, the voltage is a positive value. For example, when the hydrogen half cell is hooked up to a copper half-cell, the voltage is +0.34V.
16 Half-Cell Potentials So, a copper/hydrogen battery has an overall voltage (E cell ) of volts. If the element is more difficult to reduce than hydrogen, the recorded voltage is negative. Ex. Cr e - Cr E = -0.74V All such half-cell voltages are recorded in a table of Standard Electrode Reduction Potentials.
17 Standard Reduction Potentials Reduction Half-Reaction E F 2 + 2e - 2 F V Au e - Au +1.42V Ag + + e - Ag +0.80V I 2 + 2e - 2I V Cu e - Cu +0.34V 2 H e - H 2 (g) 0.0 0V Pb e - Pb -0.13V Ni e - Ni -0.28V Cd e - Cd -0.41V Zn e - Zn -0.76V Li + + e - Li -3.04V
18 Battery Voltages In order for an electrochemical cell to work as a battery, the overall cell voltage must be positive. Remember that a reduction cannot occur without an oxidation. The table we just saw shows only reductions. So, one of the half-cell reactions will need to be turned around to become an oxidation.
19 Battery Voltages Guess what happens to the symbol on the voltage if we turn the equation around. The +/- symbol changes! Let s examine our Cu/Zn battery again with a look at the voltage it generates.
20 Cu/Zn Battery Here are the 2 half-reactions from the table: Cu e - Cu +0.34V Zn e - Zn -0.76V One of the reactions will have to be turned around to show an oxidation. Which one will it be to leave a positive voltage? Right! The Zn reaction must be reversed.
21 Cu/Zn Battery Cu e - Cu Zn Zn e V +0.76V Notice that the voltage became positive. To calculate battery voltage, simply add the 2 equations together. Cu e - Cu +0.34V Zn Zn e V Cu 2+ + Zn Zn 2+ + Cu +1.10V
22 Battery Electrodes In an earlier slide, we said that a battery has an anode and a cathode. How can you tell which is which? Do you know the legend of Paul Bunyan? Paul, the giant lumberjack had a well known pet: Babe, the blue ox. But Paul had another, less famous pet: Fritz, the red cat.
23 Battery Electrodes So, when you think of batteries, think of Paul Bunyan. He had 2 pets: an ox and a red cat. The anode is where oxidation happens, and reduction is at the cathode. The cathode is the + electrode, and the anode is the electrode. Electron flow is always from anode to cathode.
24 Try This Example A battery is composed of a silver half-cell and a cadmium half-cell. Write the reduction and oxidation half reactions. Draw the battery. Calculate the voltage. Label the anode and cathode. Draw the direction of electron flow.
25 Silver-Cadmium Battery e - flow: Cd to Ag Cd is oxidized: anode Ag is reduced: cathode Ag Cathode + Cd Ag + Cd 2+ NO 3 - Cl - Write half-reactions and voltages. Ag + + e - Ag E = 0.80V Cd Cd 2+ Cd + 2e eCd - Anode - E = +0.41V -0.41V Total Voltage = 1.21V Put in the porous barrier. Add the electrodes. Put cations in the solution. We also need some anions. Connect the external circuit. Reverse the Cd equation to be an oxidation.
26 Alternate Battery Diagrams Sometimes a simple battery diagram is shown as 2 separate half-cells. Instead of a porous barrier, there is a salt bridge. The bridge is usually some sort of tube that is filled with salt solution. It allows transfer of ions from one half-cell to the other.
27 Electrolysis Electrolysis involves using electric current and energy to force a nonspontaneous redox reaction to go. It is the opposite of an electrochemical cell. So, the overall cell voltage (E ) is negative rather than positive. This is the minimum voltage needed to make the cell operate.
28 Electrolysis The rechargeable battery we saw earlier is an example of an electrolytic reaction. We use a direct current generator for force the electron flow to go in reverse. Electrolysis is also used extensively for electroplating one metal onto another.
29 Electrolytic Cell Example An easy example of an electrolysis reaction would be the decomposition of NaCl. First the NaCl must be melted (around 1500 C). Then inert metal electrodes are placed in the liquid and the current is turned on. An electron is removed from Cl - and transferred to Na +.
30 Electrolytic Cell Example + Na + ion Na atom At the anode, Cl - ions lose electrons and are oxidized to Cl 2 molecules. - Cl - ion electrons Cl atom Electrons still flow from anode to cathode. At the cathode, Na + ions are reduced to Na atoms A - + C
31 Electrolytic Cell The key differences between the electrolytic cell and the electrochemical cell are: 1. Generator rather than a resistor in the circuit. 2. Lack of a porous barrier or salt bridge. 3. Polarities of the electrodes are reversed. The anode is positive and the cathode is negative A - + C
32 Aluminum Production Another very important industrial electrolysis reaction is the Hall- Heroult process for making aluminum from bauxite ore. Al 2 O 3 (l) + 3 C(s) 2 Al(l) + 3 CO(g) Al e - Al metal (reduction) C(s) + O CO (oxidation of C) The production of aluminum metal takes about 1% of all the electricity used in the U. S. each year.
33 Aluminum Production Although aluminum is relatively inexpensive, (about $1.50-$2.00 per pound), it is MUCH cheaper to melt and recycle aluminum than it is to smelt new metal. In the early 1800 s, when only a small amount of metal could be produced, Al cost $250,000 per pound ($545/gram) while silver was only $17/gram!
34 Calculating Voltage Voltage for electrolytic cells is calculated the same way that it is for batteries, except that the value will be negative rather than positive for this non-spontaneous cell. 2Cl - Cl e - E = -1.36V 2Na e - 2Na E = -2.71V Total voltage: E cell = -4.07V 4.07V is the minimum voltage needed to decompose NaCl(l).
35 Uses for Electrolysis Electrolysis of seawater is used to make Cl 2, H 2 and NaOH, three very useful and important materials. Electrolysis is also used extensively for electroplating one metal onto another (sometimes called anodizing. ) For example silver flatware is really silver plated flatware.
36 Electroplating Silverware is not solid silver. It is made of some cheaper, harder metal, like nickel. Then the nickel piece is coated with silver in an electrolysis cell. A bar of solid silver acts as the anode, and the nickel piece is the cathode. The cell simply transfers silver atoms from anode to cathode.
37 Electroplating Silver bar anode: Ag atoms change to ions and dissolve into the solution. e - The generator pulls electrons from the anode and pushes them into the cathode. e - e - e - e - e - e - e - e - Knife and threek cathode: Ag + ions change back to atoms and stick to, or plate the metal. Ag + Ag anode Ag AgNO 3 (aq)
38 Schematic Symbols Here are some symbols commonly used in electronic schematics: Generator Resistor Battery Voltmeter V Ammeter A Switch
Aim: What are electrochemical cells?
Aim: What are electrochemical cells? Electrochemistry Electrochemistry- involves a redox reaction and a flow of electrons TWO TYPES of ELECTROCHEMICAL CELLS 1.Voltaic (similar to a battery) 2.Electrolytic
More information11.3. Electrolytic Cells. Electrolysis of Molten Salts. 524 MHR Unit 5 Electrochemistry
11.3 Electrolytic Cells Section Preview/ Specific Expectations In this section, you will identify the components of an electrolytic cell, and describe how they work describe electrolytic cells using oxidation
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 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 informationElectrochemistry. Electrochemical Process. The Galvanic Cell or Voltaic Cell
Electrochemistry Electrochemical Process The conversion of chemical energy into electrical energy and the conversion of electrical energy into chemical energy are electrochemical process. Recall that an
More informationElectrochemistry C020. Electrochemistry is the study of the interconversion of electrical and chemical energy
Electrochemistry C020 Electrochemistry is the study of the interconversion of electrical and chemical energy Using chemistry to generate electricity involves using a Voltaic Cell or Galvanic Cell (battery)
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 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 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 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 informationChemistry 1011 TOPIC TEXT REFERENCE. Electrochemistry. Masterton and Hurley Chapter 18. Chemistry 1011 Slot 5 1
Chemistry 1011 TOPIC Electrochemistry TEXT REFERENCE Masterton and Hurley Chapter 18 Chemistry 1011 Slot 5 1 18.5 Electrolytic Cells YOU ARE EXPECTED TO BE ABLE TO: Construct a labelled diagram to show
More informationIntroduction to electrochemistry
Introduction to electrochemistry Oxidation reduction reactions involve energy changes. Because these reactions involve electronic transfer, the net release or net absorption of energy can occur in 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 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 informationElectrochemical Cells
CH302 LaBrake and Vanden Bout Electrochemical Cells Experimental Observations of Electrochemical Cells 1. Consider the voltaic cell that contains standard Co 2+ /Co and Au 3+ /Au electrodes. The following
More informationWhat is the importance of redox reactions? Their importance lies in the fact that we can use the transfer of electrons between species to do useful
What is the importance of redox reactions? Their importance lies in the fact that we can use the transfer of electrons between species to do useful work. This is accomplished by constructing a voltaic
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 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 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 informationOxidation & Reduction (Redox) Notes
Oxidation & Reduction (Redox) Notes Chemical Activity (or Chemical Reactivity) is the measure of the reactivity of elements. If an element has high activity, then it means that the element is willing to
More informationELECTROCHEMICAL CELLS
ELECTROCHEMICAL CELLS Electrochemistry 1. Redox reactions involve the transfer of electrons from one reactant to another 2. Electric current is a flow of electrons in a circuit Many reduction-oxidation
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 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 informationElectrochemical Cells
Electrochemical Cells There are two types: Galvanic and Electrolytic Galvanic Cell: a cell in which a is used to produce electrical energy, i.e., Chemical energy is transformed into Electrical energy.
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 informationELECTROCHEMICAL CELLS NAME ROW PD
4-26-12 NAME ROW PD (1) Which statement describes the redox reaction that occurs when an object is electroplated? The diagram below shows the electrolysis of fused KCl. A) It is spontaneous and requires
More informationElectrochemistry: Voltaic Cells
Name: Band: Date: An Overview and Review Electrochemistry: Voltaic Cells Electrochemistry is the field of chemistry that focuses on reactions involving electrical energy. All electrochemical reactions
More informationUnit 8 Redox 8-1. At the end of this unit, you ll be able to
8-1 Unit 8 Redox At the end of this unit, you ll be able to Define and identify oxidation reactions Define and identify reduction reactions Assign oxidation numbers to elements in a compound Write and
More informationOxidation numbers are charges on each atom. Oxidation-Reduction. Oxidation Numbers. Electrochemical Reactions. Oxidation and Reduction
Oxidation-Reduction Oxidation numbers are charges on each atom. 1 2 Electrochemical Reactions Oxidation Numbers In electrochemical reactions, electrons are transferred from one species to another. In order
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 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 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 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 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 information18.3 Electrolysis. Dr. Fred Omega Garces. Chemistry 201. Driving a non-spontaneous Oxidation-Reduction Reaction. Miramar College.
18.3 Electrolysis Driving a non-spontaneous Oxidation-Reduction Reaction Dr. Fred Omega Garces Chemistry 201 Miramar College 1 Electrolysis Voltaic Vs. Electrolytic Cells Voltaic Cell Energy is released
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 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 informationElectrochem 1 Electrochemistry Some Key Topics Conduction metallic electrolytic Electrolysis effect and stoichiometry Galvanic cell Electrolytic cell Electromotive Force (potential in volts) Electrode
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 informationOXIDATION-REDUCTIONS REACTIONS. Chapter 19 (From next years new book)
OXIDATION-REDUCTIONS REACTIONS Chapter 19 (From next years new book) ELECTROCHEMICAL REACTIONS: What are electrochemical reactions? Electrons are transferred from one species to another ACTIVATING PRIOR
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 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 informationCHAPTER 5 REVIEW. C. CO 2 D. Fe 2 O 3. A. Fe B. CO
CHAPTER 5 REVIEW 1. The following represents the process used to produce iron from iron III oxide: Fe 2 O 3 + 3CO 2Fe + 3CO 2 What is the reducing agent in this process? A. Fe B. CO C. CO 2 D. Fe 2 O 3
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 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 informationmccord (pmccord) HW11 Electrochemistry I mccord (51520) 1
mccord (pmccord) HW11 Electrochemistry I mccord (51520) 1 This print-out should have 27 questions. Multiple-choice questions may continue on the next column or page find all choices before answering. 001
More informationChapter 19: Oxidation - Reduction Reactions
Chapter 19: Oxidation - Reduction Reactions 19-1 Oxidation and Reduction I. Oxidation States A. The oxidation rules (as summarized by Mr. Allan) 1. In compounds, hydrogen has an oxidation # of +1. In compounds,
More informationZn + Cr 3+ Zn 2+ + Cr. 9. neutrons remain the same: C. remains the same. Redox/Electrochemistry Regents Unit Review. ANSWERS
Redox/Electrochemistry Regents Unit Review. ANSWERS 1. ½ red = Cr 3+ + 3e Cr 2. ½ ox = Zn Zn +2 + 2e 3. Balanced = 3Zn + 2Cr 3+ 3Zn +2 + 2Cr 4. Zn loses electrons, 2Cr 3+ gains electrons Zn + Cr 3+ Zn
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 informationElectrochemical Cells Homework Unit 11 - Topic 4
Electrochemical Cell Vocabulary Electrochemical Cells Homework Unit 11 - Topic 4 Electrode Anode Voltaic Cell Oxidation Electrolytic Cell Cathode Salt Bridge Reduction Half Reaction Refer to Table J: For
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 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 Worksheets
Electrochemistry Worksheets Donald Calbreath, Ph.D. Say Thanks to the Authors Click http://www.ck12.org/saythanks (No sign in required) To access a customizable version of this book, as well as other interactive
More informationFind the oxidation numbers of each element in a reaction and see which ones have changed.
Find the oxidation numbers of each element in a reaction and see which ones have changed. Rules for oxidation numbers: An element that is not in a compound has an oxidation number of zero (0) Group 1 Metals
More informationReview. Chapter 17 Electrochemistry. Outline. Voltaic Cells. Electrochemistry. Mnemonic
Review William L Masterton Cecile N. Hurley Edward J. Neth cengage.com/chemistry/masterton Chapter 17 Electrochemistry Oxidation Loss of electrons Occurs at electrode called the anode Reduction Gain of
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 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 informationElectrochemistry. Chapter 19. Concept Check Concept Check Solution. Solution
Chapter 19 Electrochemistry Concept Check 19.1 If you were to construct a wet cell and decided to replace the salt bridge with a piece of copper wire, would the cell produce sustainable current? Explain
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 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 informationOxidation-Reduction Reactions and Introduction to Electrochemistry
ADVANCED PLACEMENT CHEMISTRY Oxidation-Reduction Reactions and Introduction to Electrochemistry Students will be able to: identify oxidation and reduction of chemical species; identify oxidants and reductants
More informationIntroduction to Electrochemical reactions. Schweitzer
Introduction to Electrochemical reactions Schweitzer Electrochemistry Create and or store electricity chemically. Use electricity to drive a reaction that normally would not run. Plating metal onto a metal
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 informationSCHOOL YEAR CH- 19 OXIDATION-REDUCTION REACTIONS SUBJECT: CHEMISTRY GRADE: 12
SCHOOL YEAR 2017-18 NAME: CH- 19 OXIDATION-REDUCTION REACTIONS SUBJECT: CHEMISTRY GRADE: 12 TEST A Choose the best answer from the options that follow each question. 1. During oxidation, one or more electrons
More informationWhat is a Voltaic Cell? Voltaic Cells a.k.a. Electrochemical cells. May 25, Voltaic Cells 2018.notebook
What is a? s a.k.a. Electrochemical cells Aim: To analyze the process of a spontaneous chemical reaction that produces electricity. Voltaic cell: an electrochemical cell where chemical energy is spontaneously
More informationChemistry 213. Electrochemistry I
1 Chemistry 213 Electrochemistry I Electrochemical Cells Objective Oxidation/reduction reactions find their most important use in the construction of voltaic cells (chemical batteries). In this experiment,
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 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 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 informationChemistry 30 Review Test 3 Redox and Electrochemistry /55
Chemistry 30 Review Test 3 Redox and Electrochemistry /55 Part I Multiple choice / Numerical Response Answer the following multiple choice questions on the scantron sheet. Answer the numerical response
More information11.1. Galvanic Cells. The Galvanic Cell
Galvanic Cells 11.1 You know that redox reactions involve the transfer of electrons from one reactant to another. You may also recall that an electric current is a flow of electrons in a circuit. These
More informationElectrochemistry. (Hebden Unit 5 ) Electrochemistry Hebden Unit 5
(Hebden Unit 5 ) is the study of the interchange of chemical energy and electrical energy. 2 1 We will cover the following topics: Review oxidation states and assigning oxidation numbers Redox Half-reactions
More informationRedox Reactions and Electrochemistry
Redox Reactions and Electrochemistry Redox Reactions and Electrochemistry Redox Reactions (19.1) Galvanic Cells (19.2) Standard Reduction Potentials (19.3) Thermodynamics of Redox Reactions (19.4) The
More informationOxidation-Reduction (Redox) Reactions (4.4) 2) The ox. state of an element in a simple ion is the charge of the ion. Ex:
Redox reactions: Oxidation-Reduction (Redox) Reactions (4.4) Oxidation & reduction always occur simultaneously We use OXIDATION NUMBERS to keep track of electron transfers Rules for Assigning Oxidation
More informationChapter 7. Oxidation-Reduction Reactions
Chapter 7 Oxidation-Reduction Reactions Chapter Map Oxidation Historically oxidation meant reacting with oxygen. 2Zn(s) + O 2 (g) 2ZnO(s) Zn Zn 2+ + 2e or 2Zn 2Zn 2+ + 4e O + 2e O 2 or O 2 + 4e 2O 2 Oxidation
More informationBatteries. How does a battery (voltaic cell) work? Time Passes
Why? Batteries How does a battery (voltaic cell) work? When we use portable devices like MP3 players and cell phones we need a ready source of electricity to provide a flow of electrons. Batteries are
More informationChapter 9 Oxidation-Reduction Reactions. An Introduction to Chemistry by Mark Bishop
Chapter 9 Oxidation-Reduction Reactions An Introduction to Chemistry by Mark Bishop Chapter Map Oxidation Historically, oxidation meant reacting with oxygen. 2Zn(s) + O 2 (g) 2ZnO(s) Zn Zn 2+ + 2e or 2Zn
More information17.1 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 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. Outline
Electrochemistry Outline 1. Oxidation Numbers 2. Voltaic Cells 3. Calculating emf or Standard Cell Potential using Half-Reactions 4. Relationships to Thermo, Equilibrium, and Q 5. Stoichiometry 6. Balancing
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 informationElectrochemical Cells Intro
Electrochemical Cells Intro Outcomes: Outline the historical development of voltaic (galvanic) cells. Explain the operation of a voltaic cell at the visual, particulate and symbolic levels. Vocabulary:
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 informationReducing Agent = a substance which "gives" electrons to another substance causing that substance to be reduced; a reducing agent is itself oxidized.
Oxidation = a loss of electrons; an element which loses electrons is said to be oxidized. Reduction = a gain of electrons; an element which gains electrons is said to be reduced. Oxidizing Agent = a substance
More informationName AP CHEM / / Collected Essays Chapter 17
Name AP CHEM / / Collected Essays Chapter 17 1980 - #2 M(s) + Cu 2+ (aq) M 2+ (aq) + Cu(s) For the reaction above, E = 0.740 volt at 25 C. (a) Determine the standard electrode potential for the reaction
More informationElectrochemistry. A. Na B. Ba C. S D. N E. Al. 2. What is the oxidation state of Xe in XeO 4? A +8 B +6 C +4 D +2 E 0
Electrochemistry 1. Element M reacts with oxygen to from an oxide with the formula MO. When MO is dissolved in water, the resulting solution is basic. Element M is most likely: A. Na B. Ba C. S D. N E.
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 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 informationPractice Packet Unit 13: Electrochemistry (RedOx)
Regents Chemistry: Mr. Palermo Practice Packet Unit 13: Electrochemistry (RedOx) Redox and Batteries? Ain t nobody got time for that!!! 1 Lesson 1: Oxidation States Oxidation numbers are very important
More informationELECTROCHEMISTRY INVOLVES TWO MAIN TYPES OF PROCESSES:
ELECTROCHEMISTRY Terms to Know: Electrochemistry the study of the interchange of chemical and electrical energy OIL RIG oxidation is loss, reduction is gain (of electrons) Oxidation the loss of electrons,
More informationCHEM N-12 November In the electrolytic production of Al, what mass of Al can be deposited in 2.00 hours by a current of 1.8 A?
CHEM161 014-N-1 November 014 In the electrolytic production of Al, what mass of Al can be deposited in.00 hours by a current of 1.8 A? What products would you expect at the anode and the cathode on electrolysis
More informationElectrochemical Cells: Virtual Lab
Electrochemical Cells: Virtual Lab Electrochemical cells involve the transfer of electrons from one species to another. In these chemical systems, the species that loses electrons is said to be oxidized
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 informationthe study of the interchange of and energy reactions are oxidationreduction
the study of the interchange of and energy reactions are oxidationreduction reactions. : oxidation loss of e -, reduction gaining of e - 1. Oxidation = loss of electrons; increase in charge a. the substance
More informationToday s Objectives: and an electrolytic cell. standard cell potentials. Section 14.3 (pp )
Today s Objectives: 1. Identify the similarities and differences between a voltaic cell and an electrolytic cell 2. Predict the spontaneity of REDOX reactions based on standard cell potentials. 3. Recognize
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 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 information5.7 Galvanic Cells. Electrochemical Gizmos
5.7 Galvanic Cells Have you ever accidentally bitten into a piece of aluminum foil? If you have silver amalgam fillings, you may have experienced a bit of a jolt (Figure 1). The aluminium, in contact with
More informationHomework 11. Electrochemical Potential, Free Energy, and Applications
HW11 Electrochemical Poten!al, Free Energy, and Applica!ons Homework 11 Electrochemical Potential, Free Energy, and Applications Question 1 What is the E for Zn(s) Zn (aq) Ce (aq) Ce (aq) + cell + 4+ 3+
More informationCH 223 Friday Sept. 08, 2017 L14B
CH 223 Friday Sept. 08, 2017 L14B Previously: Relationships between E cell, K, and ΔG Concentration and cell potential Nernst equation for non-standard conditions: E cell = E 0 cell - 0.0592 n log Q at
More information