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

A current of 0.2 A is passed through a solution of AgNO₃ for 1 hour. Calculate the mass of silver deposited. (Ag = 108, n = 1, 1 F = 96500 C)

A current of 0.5 A is passed through molten NaCl for 1930 seconds. Calculate the mass of sodium deposited. (Na = 23 g/mol, n = 1, 1 F = 96500 C)

A current of 2 A is passed through a solution of ZnSO₄ for 40 minutes. Calculate the mass of zinc deposited. (Zn = 65, n = 2, 1 F = 96500 C)

A current of 3 A is passed through an electrolytic cell for 10 minutes. How many coulombs of charge have passed?

A current of 5 A is passed through an electrolytic cell for 10 minutes. Calculate the total charge passed.

A solution of CuSO₄ is electrolyzed using a current of 1.5 A for 20 minutes. Calculate the mass of copper deposited. (Cu = 63.5, n = 2, 1 F = 96500 C)

Calculate the mass of copper deposited when a current of 2 A is passed through copper(II) sulfate solution for 30 minutes. (Cu = 63.5 g/mol, n = 2, 1 F = 96500 C)

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.

If 0.27 g of a divalent metal is deposited by passing 1.5 A for 15 minutes, calculate its molar mass. (1 F = 96500 C)

If 0.5 g of a metal is deposited by passing 2 A for 10 minutes, what is its electrochemical equivalent (Z)?

If 0.54 g of a metal (M) is deposited by passing 1 A for 30 minutes, calculate the electrochemical equivalent (Z) of the metal.

If 1 Faraday of electricity is passed through molten MgCl₂, how many grams of magnesium will be deposited? (Mg = 24, n = 2)

If 96500 coulombs of charge deposit 1 mole of silver (Ag) from AgNO₃ solution, what is the equivalent mass of silver?

If the same quantity of electricity is passed through solutions of AgNO₃ and CuSO₄, and 1.08 g of silver is deposited, what mass of copper will be deposited? (Ag = 108, n = 1; Cu = 63.5, n = 2)

State Faraday’s First Law of Electrolysis.

State Faraday’s Second Law of Electrolysis.