Electrolytic Cells
Chemistry ⇒ Redox Reactions and Electrochemistry
Electrolytic Cells starts at 11 and continues till grade 12.
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See sample questions for grade 12
A current of 0.5 A is passed through an electrolytic cell containing AgNO3 solution for 1930 seconds. Calculate the mass of silver deposited. (Molar mass of Ag = 108 g/mol, 1 Faraday = 96500 C)
A current of 1.5 A is passed through molten Al2O3 for 2 hours. Calculate the mass of aluminum deposited. (Molar mass of Al = 27 g/mol, 1 Faraday = 96500 C, 3 mol e− per mol Al)
A solution of NiSO4 is electrolyzed using nickel electrodes. Write the half-reactions occurring at the anode and cathode.
Calculate the mass of copper deposited when a current of 2.0 A is passed through a solution of CuSO4 for 30 minutes. (Molar mass of Cu = 63.5 g/mol, 1 Faraday = 96500 C)
Describe the process of electrorefining of copper using an electrolytic cell.
Describe the role of the external power source in an electrolytic cell.
Describe what happens at the anode and cathode during the electrolysis of water.
During the electrolysis of aqueous CuSO4 using copper electrodes, what happens to the mass of the anode and cathode?
Explain the term 'overpotential' in the context of electrolytic cells.
Explain why electrolysis of molten NaCl produces sodium metal and chlorine gas, but electrolysis of aqueous NaCl produces hydrogen gas and chlorine gas.
Explain why inert electrodes such as platinum or graphite are often used in electrolytic cells.
State the main difference between an electrolytic cell and a galvanic cell.
