Electrolysis of a 0.1 M sulfuric acid solution with copper electrodes: an interactive lab experiment.
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As it is known, electrolytic processes use up electrical energy to bring about redox reactions. In this exercise, the electrolysis of a 0.1 M sulfuric acid solution is carried out using copper electrodes and a simple experimental setup. This consists of a 500 mL beaker containing the electrolyte solution into which an inverted burette filled up with the same solution is dipped. The copper anode is weighed before and after the experiment to find the amount of this metal dissolved as Cu(II) ions. The volume of H released at the cathode is also measured and the moles of this gas calculated using the ideal gas equation. From these data, the equivalents of both copper and hydrogen are calculated. Finally, the average current intensity is obtained according to the equation Eq.F=I.t (Eq: equivalents generated in the process; F, the Faraday; I, the current intensity and t, the electrolysis time). The cc source supplies 10 volts, enough for the oxidation of copper at the anode and the reduction of protons at the cathode. Data of the experiment are randomly generated and the atmospheric variables as well as the water vapor pressure must be entered accordingly. The reactions that occur at both the cathode and the anode are shown by means of 3D animations, as well as the charge movement throughout the electrolytic system. The interactive file is completed with a true-false test that must be solved by the user.
Subjectselectrochemistry; electrolysis; electrolysis of a 0.1 molar sulfuric acid solution; electrolysis with copper electrodes; interactive lab experiment; redox reactions in electrolysis
- Material Docente Quim. Ana. 
- Objetos de Aprendizaje 
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