the system it can already be connected to the copper half cell to produce a

The system it can already be connected to the copper

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the system, it can already be connected to the copper half-cell to produce a galvanic cell. It now acts as the cathode because of the high amount of Cl 2 which tend to be reduced to Cl - . Conclusions The three main objectives of the experiment, namely to (1) relate and apply the concepts of electrochemistry to actual experiments, (2) understand the processes and elements of an electrochemical cell and (3) determine the spontaneity of reduction-oxidation (redox) reactions based on standard reduction potential, were all achieved in the experiment. From the read voltages, the spontaneity of the reactions was measured. It can be concluded based on the data gathered and values calculated that the spontaneity of the reactions with respect to a copper half- cell in decreasing order is: Set-up # 2 > # 4 > # 3 > # 5 > # 6 > # 1 This was concluded using the knowledge that a higher potential difference or E cell produces a more spontaneous reaction and more work that can be done by the system. This means that the farther the value of the standard reduction potential (SRP) of the half-cell is from the SRP of copper, the more spontaneous the reaction would be. Individually, the standard reduction potentials of the half-cells, when at a higher value, also indicate a higher tendency to be reduced and serve as a cathode in the voltaic cell and as an anode in an electrolytic cell. To further understand the concepts of electrochemistry, it is recommended that in the second part of the experiment, the change in concentration due to electrolysis is taken into account. This can be done by measuring the amperes and recording the time of the duration of electrolysis. Also, the effect of concentration differences between the half-cells can also be investigated by setting up two half-cells containing the same solutions but in different concentrations. References [1] Belcher, R. Quantitative Inorganic Analysis, 1970 [2] Christian, G.D. Analytical Chemistry, 1986 [3] Day, Underwood, et al. Quantitative Analysis, 1967 [4] Haenisch, Pierce, et al. Quantitative Analysis, 1958 [5] Skoog, et al., Fundamentals of Analytical Chemistry, Eighth edition, 2004 8
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