ELECTROCHEMICAL POTENTIALS

ELECTROCHEMICAL POTENTIALS By [Name] Class Name Professor University State and City Date Introduction In particular, distinctive metals have varying electrochemical potentials (EPs). That is why this laboratory experiment was prepared so that it can depict the EP properties of Iron (Fe), Copper (Cu), Magnesium (Mg), Zinc (Zn), and Silver (Ag). The standard EPs of these metals enable them to have different electrolytic characteristics, which is studied in this experiment. Moreover, for this experiment to be successful respective ionic solutions for the above stated metals were used, which include Copper Sulphate (CuSO4), Magnesium Sulphate (MgSO4), Iron Sulphate (FeSO4), Zinc Sulphate (ZnSO4), and Silver Sulphate (Ag(NO3)2). Most importantly, the cell voltage of the complete circuit involving these electrodes and electrolytes were measured, recorded, and the Nernst equation was used to verify them. Experiment’s Primary Objective This experiment’s primary goal was determining the EPs of different metals, such as Iron (Fe), Magnesium (Mg), Copper (Cu), Silver (Ag), and Zinc (Zn), and comparing their relationships. Redox reactions were used to obtain the EP. A sodium chloride salt bridge was used to complete the circuit connecting the two electrolytes from different beakers. In most cases, oxidation occurs in the anode and reduction in the cathode (Nolle et al., 2020). Specifically, reduction involves metal accepting electrons while oxidation entails donating electrons when the circuit is complete. Lessons Obtained For sure, this experiment was beneficial to me since it helped me learn various lessons about the EP properties of distinctive metals. The first lesson obtained was that different metals have distinctive reduction and oxidation properties, which comprises their standard EPs. For instance, by using the Nernst equation to portray the EP of Ag, Mg, Cu, Zn, and Fe, their respective V vs. SHE was +0.8, -2.37, +0.34, -0.76, and -0.44, respectively. Second, I also learned that the capacity of metals to give electrons is significantly affected by the redox reactions between the electrode and electrolyte (Weltin & Kieninger, 2021). Third, I acquired a significant lesson about the relationships between metals and their standard potentials. Besides, the potential entails a system’s quantification to perform work, which in this scenario involves conducting electrochemical reactions. Aspects of the Laboratory Experiment that Were More Difficult There exist two key aspects of this experiment that I thought would be more difficult. The first one was to verify the EP measurements by using the Nernst equation (Dickinson & Wain, 2020). Besides, it was clear that the ionic solutions had different concentrations of 1 M, 0.1 M, 0.01 M, and 0.001 M. The most significant thing was to maintain the accuracy of measurement recordings throughout the experiment. Another thing I thought would be more challenging is to use the salt bridge within the shortest period to avoid contamination. As such, one might be confused, leading to wrong measurements since time should not be wasted in recording these readings. Aspects of the Experiment I Enjoyed Specifically, I enjoyed various aspects of this laboratory experiment. First, I witnessed how the reduction and oxidation of distinctive metals take place. I understood clearly how metal donates electrons, reducing agents, and how electrons go to other metals, oxidizing agents (Cao et al., 2022). Second, I comprehended the equations that show how oxidation and reduction occur. Third, I observed how different electrodes and electrolytes react and what it means by electrochemical potentials. Fourth, I witnessed how the concentrations of electrolytes contribute to electrochemical reactions. Overall, the experiment gave me an idea of how the charging and discharging of batteries happen and the role played by redox reactions. How Can the Experiment Be Improved Although the laboratory experiment invo...