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ELECTROLYSIS

Electrolysis

1. Definition

Electrolysis is the process of using an electric current to drive a non-spontaneous chemical reaction. It typically involves the decomposition of a compound into its elements or simpler compounds.

2. Basic Setup

  • Electrolyte: A liquid or solution that conducts electricity (usually an ionic compound dissolved in water or molten form).

  • Electrodes: Two conductors inserted into the electrolyte.

    • Anode: Positive electrode where oxidation occurs.

    • Cathode: Negative electrode where reduction occurs.

  • Power source: Provides the electric current.

3. How It Works

  • When current passes through the electrolyte:

    • Positive ions (cations) move to the cathode to gain electrons (reduction).

    • Negative ions (anions) move to the anode to lose electrons (oxidation).

4. Electrolysis of Molten Ionic Compounds

  • Example: Electrolysis of molten sodium chloride (NaCl)

    • Na⁺ moves to cathode → Na (metal) is formed.

    • Cl⁻ moves to anode → Cl₂ gas is released.

5. Electrolysis of Aqueous Solutions

  • Water can also be electrolyzed, producing H₂ and O₂ gases.

  • The products depend on:

    • The ions present in the solution.

    • The electrode materials.

    • The relative reactivity of the ions.

6. Faraday’s Laws of Electrolysis

  • The amount of substance produced at each electrode is proportional to:

    • The quantity of electric charge passed through the electrolyte.

  • First Law: Mass of substance produced ∝ charge.

  • Second Law: Masses of different substances produced by the same charge are proportional to their chemical equivalents.

7. Applications

  • Extraction of metals (e.g., aluminum, copper).

  • Electroplating (coating objects with a metal layer).

  • Purification of metals.

  • Production of chemicals (chlorine, hydrogen, sodium hydroxide).

8. Important Terms

  • Electrolyte: The ionic conductor.

  • Electrode: The conductor where electrons enter or leave.

  • Oxidation: Loss of electrons (at anode).

  • Reduction: Gain of electrons (at cathode).