Chemistry 2014 Electroplating Lab Essay

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Abstract The first part of our experiment analyzed the flow of electricity between two solid pieces of different metals, immersed in solutions containing cations of said metals connected by a salt bridge. The direction and voltage of the reaction was then measured. The second part of the investigation utilized the electrolytic cell. This cell was used to electroplate different pieces of metal with the application of DC electricity. The aim of these experiments was to determine the causes of the reactions and to determine the differences in how they come about. Report on Reactions in Electrochemical and Electrolytic Cells Voltaic, or, electrochemical cells, produce an electric current through a redox reaction. In these reactions, reduction takes place at the cathode, and oxidation taking place at the anode, as shown by (Singh & Gho, 2013). This transfer of electrons is what created the current that was measured. Why it travelled in a certain direction, such as from Zn to Cu, was a mystery. We predicted that it was due to the electronegativity of the metals being used in the experiment. Elements with a higher electronegativity are more likely to gain electrons, as electronegativity is the measure of an element’s ability to attract bonding electrons to it. The second part of this experiment was an investigation of the electrolytic cell, which uses an external source of electricity to start the reaction. Despite this, a redox reaction still takes place (Mittal, 2013). As the anode is connected to the positive terminal and the cathode to the negative, oxidation and reduction take place, respectively. We predicted that the cations from the oxidized metal associate with the anions in the solution, which is composed of CuCl2. The Cu2+ will then be reduced at the cathode,

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