Faraday’s Laws of Electrolysis

Chemistry ⇒ Redox Reactions and Electrochemistry

Faraday’s Laws of Electrolysis starts at 12 and continues till grade 12. QuestionsToday has an evolving set of questions to continuously challenge students so that their knowledge grows in Faraday’s Laws of Electrolysis. How you perform is determined by your score and the time you take. When you play a quiz, your answers are evaluated in concept instead of actual words and definitions used.

See sample questions for grade 12

Define electrochemical equivalent (Z).

Describe the significance of the Faraday constant in electrolysis.

Explain how Faraday’s laws are applied in the extraction of aluminium from bauxite.

Explain why Faraday’s laws are important in electroplating industries.

Explain why the equivalent mass is used in Faraday’s Second Law instead of molar mass.

A current of 0.25 A is passed through an electrolytic cell containing FeSO₄ solution for 40 minutes. Calculate the mass of iron deposited at the cathode. (Fe = 56, n = 2, 1 F = 96500 C)

A current of 1.0 A is passed through three electrolytic cells connected in series containing solutions of AgNO₃, CuSO₄, and AuCl₃ respectively. If 1.08 g of silver is deposited in the first cell, calculate the mass of copper and gold deposited in the other two cells. (Ag = 108, n = 1; Cu = 63.5, n = 2; Au = 197, n = 3)

A solution contains a mixture of NiSO₄ and ZnSO₄. If a current is passed through the solution, which metal will be deposited first and why?

Which of the following is NOT a factor affecting the mass of substance deposited during electrolysis? (1) Current passed (2) Time for which current is passed (3) Temperature of the electrolyte (4) Volume of the electrolyte

Which of the following is NOT a limitation of Faraday’s laws? (1) Side reactions may occur (2) Laws are not applicable to fused electrolytes (3) Current efficiency may be less than 100% (4) Laws assume 100% current efficiency

Which of the following is the correct expression for the mass of substance deposited according to Faraday’s Second Law? (1) m = (E × Q) / F (2) m = (M × Q) / (nF) (3) m = (n × Q) / (M × F) (4) m = (Q × F) / (M × n)

Which of the following is the correct formula for Faraday’s First Law of Electrolysis? (1) m = ZIt (2) m = ZVt (3) m = ZI/t (4) m = Zt/I

Fill in the blank: 1 Faraday is equal to _______ coulombs.

Fill in the blank: The charge required to deposit 1 mole of a univalent metal is _______ coulombs.

Fill in the blank: The mass of a substance deposited is directly proportional to the _______ of electricity passed.

Fill in the blank: The number of moles of electrons required to deposit 1 mole of Al from Al³⁺ ions is _______.

True or False: Faraday’s laws can be used to determine the purity of metals.

True or False: Faraday’s laws of electrolysis are applicable to both molten and aqueous electrolytes.

True or False: The amount of substance deposited during electrolysis depends only on the type of electrolyte used.

True or False: The electrochemical equivalent (Z) is the mass of substance deposited by one coulomb of charge.