Concluded that the concentration of electrolytes

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concluded that the concentration of electrolytes contributes to the change in the value of voltage produced and to the standard reduction potential. It was also known that carbon electrodes do not affect the electrolysis reaction and that copper, when oxidized, turns into solid and in this particular experiment, coats itself in a copper electrode making it bigger and heavier. Due to lack of resources, some of the objectives were not met since the construction of both voltaic and electrolytic cells were made by the instructors. However, through the experiment, the students were able to recall and use concepts such as the Nernst equation and Faraday’s Law of Electrolysis.
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VII. Literature Cited/Bibliography Amateis, P., & Silberberg, M. (2018). An Overview of Electrochemical Cells. In P. Amateis, & M. Silberberg, Chemistry: The Molecular Nature of Matter and Change (pp. 944-948). New York: McGraw-Hill Education. Chang, R. (2010). Electrochemistry. In R. Chang, Chemistry 10th Edition (pp. 871- 874). New York: McGraw-Hill. Electrochemical Cells . (2019, April 28). Retrieved from Chemistry Libre Texts: %3A_Principles_of_Modern_Chemistry_(Oxtoby_et_al.)/UNIT_4%3A_EQ UILIBRIUM_IN_CHEMICAL_REACTIONS/17%3A_Electrochemistry/17. 1%3A_Electrochemical_Cells Key, J. (2019). Introduction to Chemistry - 1st Canadian Edition . Retrieved from Rate Laws: Labrake, Mccord, & Vandenbout. (2013). Electrochemical Cells . Retrieved from Chemistry 302: - all.php Standard Reduction Potential . (2019, June 6). Retrieved from Chemistry Libre Texts: Modules_(Analytical_Chemistry)/Electrochemistry/Redox_Chemistry/Standa rd_Reduction_Potential
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VIII. Appendix Figure 3. Standard reduction potential of half-reactions at 25˚C.
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