Study Guides/Chemistry/Faraday's Second Law of Electrolysis
Study Guide · Chemistry

Faraday's Second Law of Electrolysis

Faraday's Second Law of Electrolysis describes the relationship between the quantities of different substances deposited at electrodes when the same amount of charge is passed through different electrolytic solutions.

Question (Click to Flip)

What is the practical application of Faraday's Second Law?

Answer

It is used in electroplating industries to precisely calculate how much of a metal (like gold or silver) will be deposited on an object for a given amount of current and time.

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Key Facts

Faraday's First Law states that the mass of a substance deposited is directly proportional to the charge passed. Faraday's Second Law compares different substances at the same charge.

Statement of the Law

"When the same quantity of electricity is passed through different electrolytes connected in series, the masses of substances deposited at the respective electrodes are directly proportional to their equivalent masses (chemical equivalents)."

Mathematically:

m₁/m₂ = E₁/E₂

Where:

  • m₁ and m₂ = Masses of substances deposited
  • E₁ and E₂ = Equivalent masses of the respective substances

Equivalent Mass

The Equivalent Mass (or Chemical Equivalent) is calculated as:

Equivalent Mass = Molar Mass / Valency (n-factor)

Example: If you pass the same charge through aqueous CuSO₄ and AgNO₃:

  • Equivalent mass of Cu = 64/2 = 32 g/mol
  • Equivalent mass of Ag = 108/1 = 108 g/mol
  • Therefore, the ratio of masses deposited = 32:108 = 8:27

For every 32 g of copper deposited, 108 g of silver will be deposited simultaneously.

Questions and Answers

What is the practical application of Faraday's Second Law?+

It is used in **electroplating** industries to precisely calculate how much of a metal (like gold or silver) will be deposited on an object for a given amount of current and time.

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