The purpose of this experiment is to determine how the concentration of the galvanic cell affected the voltage of the galvanic cell. An experiment was performed in class that examined the voltage of the galvanic cell at various concentrations of 0.1M, 0.3M, 0.5M, 0.7M and 1M of Both Copper Sulfate (CuSO4) and Zinc Sulfate (ZnSO4). What is a galvanic cell? A galvanic cell is an electrochemical cell in which oxidation-reduction reactions generate electrical energy (opentextbc, 2021). https://opentextbc.ca/chemistry/chapter/17-2-galvanic-cells/ How is voltage related to current? Galvanic cells harness the electrical energy available from the electron transfer in a redox reaction to perform electrical work. https://www.sparknotes.com/chemistry/electrochemistry/galvanic/section2/ What is happening in the wire? Galvanic cells transform chemical energy into electrical energy that can be used to generate electricity. The electrons that are released at the anode flow through the wire, therefore creating an electrical current. https://chem.libretexts.org/Courses/University_of_California_Davis/UCD_Chem_002C/UCD_Chem_2C_(Larsen)/Text/02%3A_Electrochemistry/2.01%3A_Galvanic_Cells#:~:text=The%20electrons%20that%20are%20released,Ions%20in%20a%20Galvanic%20Cell. The experiment was modified by using various concentrations of the same metals and solutions; being Copper Sulfate (CuSO4) and Zinc Sulfate (ZnSO4) instead of various metals to investigate the voltage. Explain the theory of the relationship.
