Electrolysis and Faraday's Law Worksheet
Explore the principles of electrolysis and Faraday's Law with this comprehensive worksheet for Grade 11 Chemistry students.
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Electrolysis and Faraday's Law
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Read each question carefully and answer to the best of your ability. Show all work for calculations.
1. Which of the following is NOT a necessary component for an electrolytic cell?
Electrolyte
Salt bridge
External power source
Electrodes
2. Faraday's first law of electrolysis states that:
The mass of a substance produced at an electrode is directly proportional to the quantity of electricity passed.
The mass of a substance produced is inversely proportional to the quantity of electricity passed.
The mass of different substances produced by the same quantity of electricity is directly proportional to their equivalent masses.
Electrolysis always produces hydrogen and oxygen gas.
3. The process of using electrical energy to drive a non-spontaneous chemical reaction is called .
4. In an electrolytic cell, oxidation occurs at the , which is the electrode.
5. According to Faraday's second law, if the same quantity of electricity is passed through different electrolytes, the masses of the substances deposited are proportional to their masses.
6. Explain the difference between an electrolytic cell and a galvanic (voltaic) cell.
7. Calculate the mass of copper deposited at the cathode when a current of 5.0 A is passed through a solution of CuSO₄ for 30 minutes. (Molar mass of Cu = 63.55 g/mol, Faraday's constant = 96485 C/mol)
8. Electrolysis is a spontaneous process.
True
False
9. In the electrolysis of molten NaCl, chlorine gas is produced at the anode.
True
False