| Journal Articles: 47 results |
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Introducing Undergraduate Students to Electrochemistry: A Two-Week Discovery Chemistry Experiment Kenneth V. Mills, Richard S. Herrick, Louise W. Guilmette, Lisa P. Nestor, Heather Shafer, and Mauri A. Ditzler,
Within the framework of a laboratory-focused, guided-inquiry pedagogy, students discover the Nernst equation, the spontaneity of galvanic cells, concentration cells, and the use of electrochemical data to calculate equilibrium constants.
Mills, Kenneth V.; Herrick, Richard S.; Guilmette, Louise W.; Nestor, Lisa P.; Shafer, Heather;Ditzler, Mauri A. J. Chem. Educ. 2008, 85, 1116.
Electrochemistry |
Electrolytic / Galvanic Cells / Potentials |
Equilibrium
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Metal Electrodeposition on an Integrated, Screen-Printed Electrode Assembly Yieu Chyan and Oliver Chyan
Screen-printed, carbon strip electrodes illustrate the essential concepts of electrochemistry and electrodeposition; their light weight facilitates sensitive measurements of electrodeposited metal, allowing for the exploration of Faraday's law and electrodeposition efficiency.
Chyan, Yieu; Chyan, Oliver. J. Chem. Educ. 2008, 85, 565.
Electrochemistry |
Metals |
Oxidation / Reduction |
Quantitative Analysis
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Electrochemical Polishing of Silverware: A Demonstration of Voltaic and Galvanic Cells Michelle M. Ivey and Eugene T. Smith
Using a battery and a graphite electrode, an electrolytic cell is constructed to generate a layer of tarnish on silverware. Students then determine that the tarnish can be removed by electrochemically converting it back to silver using aluminum foil and baking soda.
Ivey, Michelle M.; Smith, Eugene T. J. Chem. Educ. 2008, 85, 68.
Consumer Chemistry |
Electrochemistry |
Electrolytic / Galvanic Cells / Potentials
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Textbook Error: Short Circuiting an Electrochemical Cell Judith M. Bonicamp and Roy W. Clark
Reports a serious error in the electrochemical diagrams in eight, 21st century texts and offers an analogy to electrical potential energy and a diagram to clarify the interrelationships between electromotive force E, reaction quotient Q, and Gibbs free energy G.
Bonicamp, Judith M.; Clark, Roy W. J. Chem. Educ. 2007, 84, 731.
Electrochemistry |
Electrolytic / Galvanic Cells / Potentials
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Small-Scale and Low-Cost Electrodes for "Standard" Reduction Potential Measurements Per-Odd Eggen, Lise Kvittingen, and Truls Grønneberg
This article describes how to construct three simple and inexpensive, microchemistry electrodes: hydrogen, chlorine, and copper.
Eggen, Per-Odd; Grønneberg, Truls; Kvittingen, Lise. J. Chem. Educ. 2007, 84, 671.
Electrochemistry |
Electrolytic / Galvanic Cells / Potentials |
Laboratory Equipment / Apparatus |
Microscale Lab |
Student-Centered Learning
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A Lemon Cell Battery for High-Power Applications Kenneth R. Muske, Christopher W. Nigh, and Randy D. Weinstein
This article discusses the development of a lemon cell battery for high-power applications such as radios, portable cassette or CD players, and battery-powered toys.
Muske, Kenneth R.; Nigh, Christopher W.; Weinstein, Randy D. J. Chem. Educ. 2007, 84, 635.
Applications of Chemistry |
Electrochemistry |
Electrolytic / Galvanic Cells / Potentials
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Isolation of Copper from a 5–Cent Coin. An Example of Electrorefining Steven G. Sogo
The United States 5cent coin, commonly known as a "nickel", is made of an alloy containing 75% copper and 25% nickel. The experiment is a visually appealing illustration of the process of electrorefining using selective reduction.
Sogo, Steven G. J. Chem. Educ. 2004, 81, 530.
Electrochemistry |
Oxidation / Reduction |
Metals
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Lithium Batteries: A Practical Application of Chemical Principles Richard S. Treptow
In recent years batteries have emerged in the marketplace that take advantage of the unique properties of lithium. Lithium metal is an attractive choice to serve as a battery anode because it is easily oxidized and it produces an exceptionally high amount of electrical charge per unit-weight.
Treptow, Richard S. J. Chem. Educ. 2003, 80, 1015.
Consumer Chemistry |
Electrochemistry |
Oxidation / Reduction |
Electrolytic / Galvanic Cells / Potentials |
Applications of Chemistry
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A Copper-Sulfate-Based Inorganic Chemistry Laboratory for First-Year University Students That Teaches Basic Operations and Concepts Emilio Rodríguez and Miguel Angel Vicente
A 10-hour integrated experiment that covers all the inorganic chemistry topics in first-year chemistry and chemical engineering courses.
Rodríguez, Emilio; Vicente, Miguel Angel. J. Chem. Educ. 2002, 79, 486.
Oxidation / Reduction |
Solutions / Solvents
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The Lead-Acid Battery: Its Voltage in Theory and in Practice Richard S. Treptow
Lead-acid battery fundamentals, cell voltage and the Nernst equation, and an analysis of actual battery performance.
Treptow, Richard S. J. Chem. Educ. 2002, 79, 334.
Electrochemistry |
Oxidation / Reduction |
Thermodynamics |
Electrolytic / Galvanic Cells / Potentials |
Acids / Bases |
Applications of Chemistry
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Observations on Lemon Cells Jerry Goodisman
The lemon cell, consisting of pieces of two different metals stuck into a lemon or other fruit, is pictured in many general chemistry textbooks without being discussed; manuscript describes simple experiments, suitable for the general chemistry laboratory, which elucidate how this kind of cell works.
Goodisman, Jerry. J. Chem. Educ. 2001, 78, 516.
Electrochemistry |
Metals |
Electrolytic / Galvanic Cells / Potentials
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The Household Chemistry of Cleaning Pennies Laurence D. Rosenhein
Although it is well known that solutions of vinegar and table salt are effective in removing tarnish from pennies, chemical explanations of this behavior are not included in sources of this "household chemistry" and erroneous explanations have crept into popular literature on this subject; this article provides some relevant empirical information on the system.
Rosenhein, Laurence D. J. Chem. Educ. 2001, 78, 513.
Consumer Chemistry |
Coordination Compounds |
Oxidation / Reduction
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Understanding Electrochemical Thermodynamics through Entropy Analysis Thomas H. Bindel
This discovery-based activity involves entropy analysis of galvanic cells. The intent of the activity is for students to discover the fundamentals of electrochemical cells through a combination of entropy analysis, exploration, and guided discovery.
Bindel, Thomas H. J. Chem. Educ. 2000, 77, 1031.
Electrochemistry |
Thermodynamics |
Electrolytic / Galvanic Cells / Potentials
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An Analysis of College Chemistry Textbooks As Sources of Misconceptions and Errors in Electrochemistry Michael J. Sanger and Thomas J. Greenbowe
The oxidation-reduction and electrochemistry chapters of 10 introductory college chemistry textbooks were reviewed for misleading or erroneous statements, using a list of student misconceptions. As a result of this analysis, we provide suggestions for chemistry instructors and textbook authors.
Sanger, Michael J.; Greenbowe, Thomas J. J. Chem. Educ. 1999, 76, 853.
Electrochemistry |
Oxidation / Reduction |
Learning Theories
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The Nernst Equation: Determination of Equilibrium Constants for Complex Ions of Silver Martin L. Thompson and Laura J. Kateley
The experiment requires a voltmeter capable of recording millivolts (or a good pH meter) and inexpensive chemicals. It allows students to check the validity of the Nernst equation and compare their experimental Kform values to reported ones.
Thompson, Martin L.; Kateley, Laura J. J. Chem. Educ. 1999, 76, 95.
Equilibrium |
Coordination Compounds |
Electrochemistry |
Oxidation / Reduction
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Redox Challenges (the author replies) Stout, Roland
Algebraic solution to balancing a redox equation.
Stout, Roland J. Chem. Educ. 1996, 73, A227.
Stoichiometry |
Oxidation / Reduction |
Oxidation State
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Redox Challenges (2) Zaugg, Noel S.
Algebraic solution to balancing a redox equation.
Zaugg, Noel S. J. Chem. Educ. 1996, 73, A226.
Stoichiometry |
Oxidation / Reduction |
Oxidation State
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Redox Challenges (1) Hart, David M.
Algebraic solution to balancing a redox equation.
Hart, David M. J. Chem. Educ. 1996, 73, A226.
Stoichiometry |
Oxidation / Reduction |
Oxidation State
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A Simple Method for Determining the Temperature Coefficient of Voltaic Cell Voltage Alfred E. Saieed, Keith M. Davies
This article describes a relatively simple method for preparing voltaic cells, and through their temperature coefficient, ?E/?T, it explores relationships between ?G, ?H,and ?S for the cell reactions involved.
Saieed, Alfred E.; Davies, Keith M. J. Chem. Educ. 1996, 73, 959.
Electrochemistry |
Calorimetry / Thermochemistry |
Thermodynamics |
Electrolytic / Galvanic Cells / Potentials |
Laboratory Equipment / Apparatus |
Laboratory Management |
Oxidation / Reduction
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The "Golden Penny" Demonstration: An Explanation of the Old Experiment and the Rational Design of the New and Simpler Demonstration. Szczepankiewicz, Steven H.; Bieron, Joseph F.; Kozik, Mariusz
An explanation and simpler/safer design for the classical "gold penny" demonstration.
Szczepankiewicz, Steven H.; Bieron, Joseph F.; Kozik, Mariusz J. Chem. Educ. 1995, 72, 386.
Electrochemistry |
Electrolytic / Galvanic Cells / Potentials
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Use of Electrochemical Concentration Cells to Demonstrate the Dimeric Nature of Mercury(I) in Aqueous Media Bhattacharya, Deepta; Peters, Dennis G.
Experimental procedure for demonstrating that divalent mercury is monovalent in aqueous solution; includes data and analysis.
Bhattacharya, Deepta; Peters, Dennis G. J. Chem. Educ. 1995, 72, 64.
Atomic Properties / Structure |
Electrochemistry |
Electrolytic / Galvanic Cells / Potentials |
Aqueous Solution Chemistry
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Using the Biological Cell in Teaching Electrochemistry Merkel, Eva Gankiewicz
How electricity is produced in a simple cell is correlated with how commercial batteries work; this concept can then be related to how living cells send electrical impulses.
Merkel, Eva Gankiewicz J. Chem. Educ. 1994, 71, 240.
Electrochemistry |
Electrolytic / Galvanic Cells / Potentials |
Equilibrium
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Redox demonstrations and descriptive chemistry: Part 3. Copper (I)-copper(II) equilibria Ophardt, Charles E.
The unusual redox properties of copper (I) and copper (II) ions explained and illustrated.
Ophardt, Charles E. J. Chem. Educ. 1991, 68, 248.
Descriptive Chemistry |
Oxidation State |
Oxidation / Reduction
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Electrochemical conventions: Responses to a provocative opinion (6) Martin-Sanchez, M.; Martin-Sanchez, MaT
The solution may be to use the etymological meaning of anode and cathode.
Martin-Sanchez, M.; Martin-Sanchez, MaT J. Chem. Educ. 1990, 67, 992.
Electrochemistry |
Nomenclature / Units / Symbols |
Electrolytic / Galvanic Cells / Potentials
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Electrochemical conventions: Responses to a provocative opinion (5) Sweeting, Linda M.
The chemical potential of the electrons, not their "richness" determines direction of flow.
Sweeting, Linda M. J. Chem. Educ. 1990, 67, 992.
Electrochemistry |
Nomenclature / Units / Symbols |
Electrolytic / Galvanic Cells / Potentials
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Electrochemical conventions: Responses to a provocative opinion (4) Fochi, Giovanni
It is sufficient to show what part of the circuit is the electric generator.
Fochi, Giovanni J. Chem. Educ. 1990, 67, 992.
Electrochemistry |
Nomenclature / Units / Symbols |
Electrolytic / Galvanic Cells / Potentials
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Electrochemical conventions: Responses to a provocative opinion (3) Woolf, A. A.
There are no shortcuts in teaching the electrochemistry of galvanic cells; the process in each cell must be treated holistically.
Woolf, A. A. J. Chem. Educ. 1990, 67, 992.
Electrochemistry |
Nomenclature / Units / Symbols |
Electrolytic / Galvanic Cells / Potentials
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Electrochemical conventions: Responses to a provocative opinion (2) Castellan, Gilbert W.
The difficulty is not so much confusion over conventions as the actual wrong use of terminology.
Castellan, Gilbert W. J. Chem. Educ. 1990, 67, 991.
Electrochemistry |
Nomenclature / Units / Symbols |
Electrolytic / Galvanic Cells / Potentials
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A bromate clock reaction: The formation of purple tris(diphosphato)manganate(III) Rich, Ronald L.; Noyes, Richard M.
Bromate is used to oxidize nearly colorless Mn(II) to a deep purple complex of Mn(III).
Rich, Ronald L.; Noyes, Richard M. J. Chem. Educ. 1990, 67, 606.
Reactions |
Oxidation / Reduction |
Kinetics
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Construction and evaluation of an inexpensive reference electrode with internal electrolyte in agar matrix Victoria, Leandro; Ortega, M. Gloria; Ibanez, Jose A.
In this paper the authors show how to construct a reference electrode of Ag/AgCl with an internal electrolyte in agar matrix.
Victoria, Leandro; Ortega, M. Gloria; Ibanez, Jose A. J. Chem. Educ. 1990, 67, 179.
Electrolytic / Galvanic Cells / Potentials |
Electrochemistry |
Laboratory Equipment / Apparatus
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Alleviating the common confusion caused by polarity in electrochemistry Moran, P. J.; Gileadi, E.
The issue of polarity encountered in electrochemistry and relevant to a variety of electrochemical concepts often confuses students and is an unnecessary deterrent to the study of electrochemistry.
Moran, P. J.; Gileadi, E. J. Chem. Educ. 1989, 66, 912.
Electrochemistry |
Electrolytic / Galvanic Cells / Potentials
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Using a projecting voltmeter to introduce voltaic cells Solomon, Sally; Lee, Jeffrey; Schnable, Joseph; Wirtel, Anthony
Using a transparent "projecting" voltmeter and assembling a zinc versus copper cell one component at a time allows students to develop a more concrete notion of the nature of a voltaic cell and the potential it produces.
Solomon, Sally; Lee, Jeffrey; Schnable, Joseph; Wirtel, Anthony J. Chem. Educ. 1989, 66, 510.
Electrochemistry |
Electrolytic / Galvanic Cells / Potentials
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Electrochemical cells using sodium silicate Rapp, Bernard, FSC
A procedure of assembly and execution of a demonstration of an electrochemical cell using sodium silicate.
Rapp, Bernard, FSC J. Chem. Educ. 1988, 65, 358.
Electrochemistry |
Electrolytic / Galvanic Cells / Potentials
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Redox demonstrations and descriptive chemistry: Part 1. Metals Ophardt, Charles E.
The oxidation states of iron, tin, and mercury.
Ophardt, Charles E. J. Chem. Educ. 1987, 64, 716.
Metals |
Descriptive Chemistry |
Oxidation / Reduction |
Oxidation State
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Estimating the one electron reduction potential for vanadium (V) by chemical techniques: An experiment for general chemistry Wentworth, R. A. D.
Procedure requires no electrochemical equipment because the method depends solely upon observations of the spontaneity of the reactions of V(V) with a series of potential reducing agents and V(IV) with a series of potential oxidizing agents.
Wentworth, R. A. D. J. Chem. Educ. 1985, 62, 440.
Oxidation State |
Oxidation / Reduction |
Electrochemistry
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Drug stabilization against oxidative degradation Akers, Michael J.
Describes the process of oxidation and ways in which pharmaceutical preparations can be protected from oxidative degredation.
Akers, Michael J. J. Chem. Educ. 1985, 62, 325.
Drugs / Pharmaceuticals |
Oxidation / Reduction |
Medicinal Chemistry |
Nonmajor Courses
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Electrochemistry in the general chemistry curriculum Chambers, James Q.
Students in introductory chemistry courses at large universities do not develop sufficient understanding of electrochemical phenomenon. From State-of-the-Art Symposium: Electrochemistry, ACS meeting, Kansas City, 1982.
Chambers, James Q. J. Chem. Educ. 1983, 60, 259.
Electrochemistry |
Electrolytic / Galvanic Cells / Potentials
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Reduction potentials and hydrogen overvoltage: An overhead projector demonstration Ramette, Richard W.
Relates the scale of standard reduction potentials to the observed behavior of metals in their reactions with hydrogen ion to produce hydrogen gas.
Ramette, Richard W. J. Chem. Educ. 1982, 59, 866.
Electrochemistry |
Metals |
Oxidation / Reduction
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Electrochemical demonstration: Motor driven by a simple galvanic cell Skinner, J. F.
A Zn / Zn 2+ Cu 2+ / Cu (Daniel) cell operates a small motor.
Skinner, J. F. J. Chem. Educ. 1977, 54, 619.
Electrochemistry |
Electrolytic / Galvanic Cells / Potentials |
Aqueous Solution Chemistry
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Racing car batteries Plumb, Robert C.; Combs, R. E.; Connelly, J. M.
Illustrating the Nernst equation and Faraday's laws using the example of the silver-zinc batteries used in racing cars.
Plumb, Robert C.; Combs, R. E.; Connelly, J. M. J. Chem. Educ. 1973, 50, 857.
Applications of Chemistry |
Electrochemistry |
Electrolytic / Galvanic Cells / Potentials
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The bombardier beetle Plumb, Robert C.; Erickson, Karen L.
The chemistry behind the bombardier beetle's chemical defenses illustrates the principles of reaction rates, catalysis, and laboratory safety.
Plumb, Robert C.; Erickson, Karen L. J. Chem. Educ. 1972, 49, 705.
Applications of Chemistry |
Natural Products |
Rate Law |
Catalysis |
Oxidation / Reduction |
Aromatic Compounds
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Electrochemical reactions in batteries. Emphasizing the MnO2 cathode of dry cells Kozawa, Akiya; Powers, R. A.
The purpose of this article is to make a simplified, but current presentation of the electrochemical reactions in batteries, particularly those of the manganese dioxide cathode of dry cells.
Kozawa, Akiya; Powers, R. A. J. Chem. Educ. 1972, 49, 587.
Electrochemistry |
Electrolytic / Galvanic Cells / Potentials |
Applications of Chemistry
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Chemical queries. Especially for introductory chemistry teachers Young, J. A.; Malik, J. G.; Quagliano, James V.; Danehy, James P.
(1) Why different potential for copper/zinc cells when using nitrates vs. sulfates? Why is neither cell potential as large as predicted by Nerst equation? (2) Do elements in the zinc subgroup belong to the transition series? - answer by Quagliano. (3) How can the 2,4,5-trichloro derivative of phenoxyacetic acid be prepared? - answer by Danehy.
Young, J. A.; Malik, J. G.; Quagliano, James V.; Danehy, James P. J. Chem. Educ. 1969, 46, 227.
Electrochemistry |
Electrolytic / Galvanic Cells / Potentials |
Periodicity / Periodic Table |
Metals |
Synthesis |
Aromatic Compounds
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Verification of the form of the Nernst equation: An experiment for introductory chemistry Evans, James S.
In this experiment, students record data for the concentration dependence of the ferrous-ferric half-cell potential at a platinum electrode, using a silver-silver ion reference electrode, a salt bridge, and a voltmeter.
Evans, James S. J. Chem. Educ. 1968, 45, 532.
Electrochemistry |
Electrolytic / Galvanic Cells / Potentials
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Potentiometer for the general chemistry laboratory Wood, Stanley E.; Anderson, C. B.
A circuit diagram is presented for a potentiometer used to verify the Nernst equation and investigate other electrochemical phenomenon.
Wood, Stanley E.; Anderson, C. B. J. Chem. Educ. 1965, 42, 659.
Laboratory Equipment / Apparatus |
Electrochemistry |
Electrolytic / Galvanic Cells / Potentials
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Recent developments concerning the signs of electrode potentials Licht, Truman S.; deBethune, Andre J.
It is the purpose of this paper to review recent developments concerning the signs of electrode potentials, particularly with respect to single electrode potential, half-reaction potential, and half-cell electromotive force.
Licht, Truman S.; deBethune, Andre J. J. Chem. Educ. 1957, 34, 433.
Electrochemistry |
Nomenclature / Units / Symbols |
Electrolytic / Galvanic Cells / Potentials
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Letters to the editor Campbell, J. A.
The author includes an interpretation of the "Beating Heart Experiment" which was omitted in an earlier Journal article.
Campbell, J. A. J. Chem. Educ. 1957, 34, 362.
Oxidation / Reduction |
Electrochemistry
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