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Electrochemistry Lab Report

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Experiment 5- Electrochemistry: Voltaic cells, Electrolysis and Faraday's law. Name: Christian Miranda Student#: 169019008 Date conducted: Friday March 10th Date submitted: Thursday March 16th Lab section: L16 2:30-5:20 Lab IA: Jaymie Abstract: In this experiment, the objective was to set up a voltaic cell and use it to carry out two electrolysis processes to determine the equivalent weights of zinc and copper. The procedure involved using zinc strips, copper strips, zinc wire, copper wire, a zinc plating solution, a CuSO4 solution, an ammeter, wooden blocks, alligator clamps, and beakers. However, the main findings of the experiment showed that the equivalent weights for both copper and zinc were not as expected. Copper had over 300 …show more content…

In this experiment no deviations were made. Wilfrid Laurier University Chemistry Department. Winter 2023. Electrochemistry. Pages 79-82 in Chemistry 111 Lab Manual. Wilfrid Laurier University, ON, Canada. Observation Results: Table 1: Qualitative Observations of all reactants and products in experiment Reactant/ Product Before During …show more content…

No file sharing websites were used or other students' assignments. I did not share this work with anyone else. I understand the academic integrity policies at laurier and its consequences for violating them. Application Questions: Valence refers to the number of electrons an atom can donate or accept when forming chemical bonds , Equivalent weight on the other hand refers to is a measure of ions that can combine with a fixed weight of a substance in a chemical reaction. So valence is a measure of forming chemical bonds while equivalent weight is how much an ion can replace another in a chemical reaction. In the experiment many chemical reactions took place, in the voltaic cell there was a spontaneous reaction between Zinc and copper (Oxidation and reduction). In the zinc electrolytic cell it was a oxidation reaction losing electrons in the equation Zn(s)--> Zn(aq)^2+2e^- For copper in it;s cathode there is the reduction reaction Cu(aq)^2+ + 2e^--> Cu(s) The flow of electrons will move from zinc ( anode electrolytic cell) to copper (cathode electrolytic cell). The overall reaction looks like

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