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Q1: What is the role of the anode and cathode in an electrolytic cell?
In an electrolytic cell, the anode is oxidized by the power source, releasing ions that travel through the solution to the cathode. At the cathode, these ions are reduced and plated onto the surface. The copper anode oxidizes to produce copper(2+) ions, which are then reduced and deposited as solid copper on the brass cathode.
Q2: How does electroplating work in this experiment?
Electroplating occurs when copper(2+) ions from the copper anode migrate through the copper sulfate solution and are reduced at the brass cathode, forming a thin layer of solid copper. The power source drives this nonspontaneous redox reaction, transferring electrons that reduce the ions into metal plating on the cathode surface.
Q3: What does the Faraday constant represent in electrochemistry calculations?
The Faraday constant represents the magnitude of electric charge per mole of electrons, calculated by multiplying the charge of an electron by Avogadro's constant. It is used to convert total charge transferred in coulombs into moles of electrons, enabling calculation of moles of metal plated during electroplating.
Q4: How do you calculate the total charge transferred during electroplating?
Total charge is calculated using the equation Q = I × t, where Q is charge in coulombs, I is average current in amperes, and t is time in seconds. The current probe measures current over time, and averaging these values allows you to determine the total charge transferred throughout the electroplating process.
Q5: Why must the copper electrode and brass key be polished before the experiment?
Polishing with emery paper removes surface oxidation and contaminants from both the copper electrode and brass key, ensuring clean electrode surfaces. This preparation improves electrical contact and allows accurate measurement of mass changes during electroplating, since only the intended copper deposition is measured.
Q6: What is the relationship between moles of electrons transferred and moles of copper plated?
The reduction of one mole of copper(2+) ions requires two moles of electrons to produce one mole of solid copper. By calculating moles of electrons from total charge using the Faraday constant, you can predict the expected moles of copper plated and verify this matches the measured mass change of the cathode.
Q7: How should you handle the current data if it drops to zero during electroplating?
If current drops to zero or near zero during a trial, electrons have stopped flowing and the plating process has halted. Only use current values recorded before the drop occurs when calculating average current and total charge. If current drops early, repeat the trial to ensure sufficient electroplating occurs.