11.4 Dependence of the Cell Potential on Concentration
Click on the title of a resource to view it. To save screen space, only the first 3 resources are shown. You can display more resources by scrolling down and clicking on “View all xx results”.
For the textbook, chapter, and section you specified we found
Electrolysis of several aqueous solutions is carried out using a 9-V battery and pencil leads as electrodes. Because only the electrodes are shown in the videos, it is important to show these still images
or describe how the reactions were performed if students are to make sense of the videos. In each case the anode is on the left and a 9-V battery has been connected to the lead of each of the pencils near the eraser end with an alligator clip.
Introducing Undergraduate Students to Electrochemistry: A Two-Week Discovery Chemistry ExperimentKenneth 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
Redox Titration of Ferricyanide to Ferrocyanide with Ascorbic Acid: Illustrating the Nernst Equation and Beer–Lambert LawTina H. Huang, Gail Salter, Sarah L. Kahn, and Yvonne M. Gindt In this simple experiment, which illustrates the Nernst equation and BeerLambert law, students monitor the reduction of ferricyanide ion to ferrocyanide electrochemically and spectrophoto-metrically upon titration with ascorbic acid. The Nernst equation is used to calculate the standard reduction potential of the redox couple at pH 7 and the number of electrons transferred. Huang, Tina H.; Salter, Gail; Kahn, Sarah L.; Gindt, Yvonne M. J. Chem. Educ.2007, 84, 1461.
Coordination Compounds |
Electrochemistry |
Potentiometry |
Spectroscopy |
UV-Vis Spectroscopy
Textbook Error: Short Circuiting an Electrochemical CellJudith 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.
Coulomb's LawEd Vitz, John W. Moore A section of ChemPrime, the Chemical Educations Digital Library's free General Chemistry textbook.
Electrochemistry
Potential EnergyEd Vitz, John W. Moore A section of ChemPrime, the Chemical Educations Digital Library's free General Chemistry textbook.
Electrochemistry
Electron Density and Potential EnergyEd Vitz, John W. Moore A section of ChemPrime, the Chemical Educations Digital Library's free General Chemistry textbook.
Go for the oxidation of 2 mole of silver in the following balanced reaction. 
Ca(s) + 2AgI(s) 
