{"id":6517,"date":"2026-03-13T11:28:12","date_gmt":"2026-03-13T05:58:12","guid":{"rendered":"https:\/\/www.tutoroot.com\/blog\/?p=6517"},"modified":"2026-03-13T11:28:12","modified_gmt":"2026-03-13T05:58:12","slug":"electrochemical-cell-diagram-working-principle-examples","status":"publish","type":"post","link":"https:\/\/www.tutoroot.com\/blog\/electrochemical-cell-diagram-working-principle-examples\/","title":{"rendered":"Electrochemical Cell \u2013 Diagram, Working Principle & Examples"},"content":{"rendered":"

Electrochemical cells\u00a0<\/span><\/b>are significant in the study of chemistry as it is a device that converts chemical energy into electrical energy. The concept of electrochemical cells is usually taught in the study of chemistry for students of\u00a0<\/span>Class 12 CBSE, IIT-JEE, and NEET.<\/span><\/b>\u00a0<\/span><\/p>\n

Studying about\u00a0electrochemical cells will give you an idea of how battery\u00a0operates\u00a0how electricity\u00a0generated\u00a0from a chemical reaction and how scientists use it to\u00a0observe\u00a0<\/span>oxidation-reduction<\/span><\/b>\u00a0reactions.<\/span>\u00a0<\/span><\/p>\n

In this whole blog, you will learn the definition, principle, diagram, half-reactions, and examples of electrochemical cells.<\/span>\u00a0<\/span><\/p>\n

What is an Electrochemical Cell?\u00a0<\/span><\/b>\u00a0<\/span><\/h2>\n

An\u00a0<\/span>electrochemical cell<\/a>\u00a0<\/span><\/b>is a device used to produce electricity through a chemical reaction.\u00a0<\/span>\u00a0<\/span><\/p>\n

Two electrodes are dipped into two different solutions within an\u00a0<\/span>electrochemical cell<\/span><\/b>. A chemical reaction takes place between these electrodes. This chemical reaction causes electrons to flow through an external source to produce electricity.\u00a0<\/span>\u00a0<\/span><\/p>\n

This is achieved through redox reactions. In these reactions, one compound loses electrons, and another compound gains electrons.\u00a0<\/span>\u00a0<\/span><\/p>\n

This flow of electrons causes chemical energy to convert into electrical energy.<\/span>\u00a0<\/span><\/p>\n

Electrochemical Cell Diagram\u00a0<\/span><\/b>\u00a0<\/span><\/p>\n

It consists of several key components. <\/span>\u00a0<\/span><\/p>\n

Main Parts of an Electrochemical Cell <\/span><\/b>\u00a0<\/span><\/h3>\n
    \n
  1. Anode\u00a0<\/span><\/b><\/li>\n<\/ol>\n

    Oxidation occurs at the anode. Electrons are released during this reaction.\u00a0<\/span>\u00a0<\/span><\/p>\n

      \n
    1. Cathode\u00a0<\/span><\/b><\/li>\n<\/ol>\n

      Reduction occurs at the cathode. Electrons are accepted here.\u00a0<\/span>\u00a0<\/span><\/p>\n

        \n
      1. Electrolyte\u00a0<\/span><\/b><\/li>\n<\/ol>\n

        The electrolyte allows ions to move between electrodes.\u00a0<\/span>\u00a0<\/span><\/p>\n

          \n
        1. Salt Bridge\u00a0<\/span><\/b><\/li>\n<\/ol>\n

          The salt bridge\u00a0maintains\u00a0electrical neutrality by transferring ions from the solutions.\u00a0<\/span>\u00a0<\/span><\/p>\n

          These parts make sure that the flow of electrons in the circuit is continuous.\u00a0<\/span>\u00a0<\/span><\/p>\n

          Working Principle of an Electrochemical Cell\u00a0<\/span><\/b>\u00a0<\/span><\/h2>\n

          The working principle is based on oxidation and reduction. <\/span>\u00a0<\/span><\/p>\n

          First, oxidation takes place at the\u00a0<\/span>anode<\/span><\/b>. The electrons are released during oxidation. These electrons are then passed through the external circuit to the cathode.\u00a0<\/span>\u00a0<\/span><\/p>\n

          Then reduction takes place at the\u00a0<\/span>cathode.\u00a0<\/span><\/b>\u00a0<\/span><\/p>\n

          This flow of electrons through the circuit is called an electric current.\u00a0<\/span>\u00a0<\/span><\/p>\n

          Half Reactions in an Electrochemical Cell\u00a0<\/span>\u00a0<\/span><\/p>\n

          It consists of two half reactions. <\/span>\u00a0<\/span><\/p>\n

          H3: Oxidation Reaction\u00a0<\/span><\/b>\u00a0<\/span><\/p>\n

          Oxidation happens when a substance loses electrons.\u00a0<\/span>\u00a0<\/span><\/p>\n

          Example\u00a0<\/span><\/b>\u00a0<\/span><\/p>\n

          Zn \u2192 Zn\u00b2\u207a + 2e\u207b\u00a0<\/span>\u00a0<\/span><\/p>\n

          Reduction Reaction\u00a0<\/span>\u00a0<\/span><\/p>\n

          Reduction occurs when a substance gains electrons.\u00a0<\/span>\u00a0<\/span><\/p>\n

          Example\u00a0<\/span><\/b>\u00a0<\/span><\/p>\n

          Cu\u00b2\u207a + 2e\u207b \u2192 Cu\u00a0<\/span>\u00a0<\/span><\/p>\n

          Together, these two half reactions generate electrical energy in the electro<\/span><\/p>\n

          Difference Between Electrochemical Cell and Electrolytic Cell\u00a0<\/span><\/b>\u00a0<\/span><\/h2>\n\n\n\n\n\n\n\n
          Feature<\/span><\/b>\u00a0<\/span><\/td>\nElectrochemical Cell<\/span><\/b>\u00a0<\/span><\/td>\nElectrolytic Cell<\/span><\/b>\u00a0<\/span><\/td>\n<\/tr>\n
          Energy Conversion<\/span>\u00a0<\/span><\/td>\nChemical \u2192 Electrical<\/span>\u00a0<\/span><\/td>\nElectrical \u2192 Chemical<\/span>\u00a0<\/span><\/td>\n<\/tr>\n
          Power Source<\/span>\u00a0<\/span><\/td>\nGenerates electricity<\/span>\u00a0<\/span><\/td>\nRequires electricity<\/span>\u00a0<\/span><\/td>\n<\/tr>\n
          Reaction Type<\/span>\u00a0<\/span><\/td>\nSpontaneous<\/span>\u00a0<\/span><\/td>\nNon-spontaneous<\/span>\u00a0<\/span><\/td>\n<\/tr>\n
          Example<\/span>\u00a0<\/span><\/td>\nBatteries<\/span>\u00a0<\/span><\/td>\nElectroplating<\/span>\u00a0<\/span><\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n

          Students preparing for\u00a0JEE\u00a0and NEET exams must clearly understand this difference.\u00a0<\/span>\u00a0<\/span><\/p>\n

          Real Life Examples of Electrochemical Cells\u00a0<\/span><\/b>\u00a0<\/span><\/h2>\n

          Electrochemical cells appear in many real-world applications.\u00a0<\/span>\u00a0<\/span><\/p>\n

          Examples include:\u00a0<\/span><\/b>\u00a0<\/span><\/p>\n