ChemistryDifference Between Galvanic Cells and Electrolytic Cells – Working and Process

Difference Between Galvanic Cells and Electrolytic Cells – Working and Process

An introduction to Galvanic Cells and Electrolytic Cells

A galvanic cell, or battery, is a device that uses two different metals to create an electrical current. The two metals are placed in a solution of electrolyte. This solution contains ions that can move freely between the two metals. When the metals are connected by a wire, the ions move from the metal with the most ions (the anode) to the metal with the least ions (the cathode). This creates a flow of electrons. The electrons flow through the wire and create an electrical current.

An electrolytic cell is a device that uses electricity to create a chemical reaction. The cell has two metal plates. One plate is made of a metal that is soluble in the electrolyte. The other plate is made of a metal that is insoluble in the electrolyte. When the cell is connected to a battery, the electrons flow from the battery to the metal with the most ions. This causes the metal with the most ions to dissolve. The dissolved metal then travels to the metal with the least ions and forms a metal plate on that plate.

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    What are Galvanic Cells?

    In a galvanic cell, two different metals are placed in an electrolyte solution. The metals react with the electrolyte to form an electrical current. The electrical current can be used to power devices or to produce metals.

    Working of Galvanic Cells

    When two different metals are placed in contact with each other in the presence of an electrolyte, a galvanic cell is formed. The electrolyte provides a path for electrons to flow between the metals. This electron flow produces a current, and the cell produces electrical energy.

    The two metals in a galvanic cell are called the anode and the cathode. The anode is the metal that loses electrons, and the cathode is the metal that gains electrons. The anode is typically the more reactive metal, and the cathode is typically the less reactive metal.

    The anode and the cathode are separated by an electrolyte. The electrolyte is a substance that dissolves in water to form ions. Ions are atoms or molecules that have lost or gained electrons, and they carry an electrical charge. The electrolyte provides a path for electrons to flow between the anode and the cathode.

    In a galvanic cell, the anode is the negative electrode, and the cathode is the positive electrode. The anode is always the metal that is more reactive than the cathode. The cathode is always the metal that is less reactive than the anode.

    The anode and the cathode are connected to a battery, and the battery supplies the electricity that powers the cell. The battery forces electrons to flow from the anode to the cathode. This electron flow produces a current, and the cell produces electrical energy.

    What are Electrolytic Cells?

    An electrolytic cell is a type of electrochemical cell that uses electricity to produce chemical reactions. In an electrolytic cell, a current is passed through a liquid or molten electrolyte, causing chemical reactions to occur. These reactions can produce metals, salts, or other chemicals.

    Working of Electrolytic Cells

    In an electrolytic cell, a current is passed through a liquid or molten electrolyte, causing oxidation of one or more species at the anode and reduction of one or more species at the cathode.

    This can be represented by the following equation:

    Anode: Oxidation reaction
    Cathode: Reduction reaction

    In an electrolytic cell, the anode is the electrode where oxidation takes place, and the cathode is the electrode where reduction takes place.

    The anode is usually made of a metal that is more reactive than the species that is being oxidized. The cathode is usually made of a metal that is less reactive than the species that is being reduced.

    Process of Electrolysis

    The process of electrolysis is the separation of an element from a compound by passing an electric current through it.

    For example, in the electrolysis of water, hydrogen gas is produced at the cathode and oxygen gas is produced at the anode.

    What is an Electrochemical Cell?

    An electrochemical cell is a device that uses electricity to produce a chemical reaction.

    Difference Between Galvanic Cells and Electrolytic cells

    The main difference between galvanic cells and electrolytic cells is that galvanic cells produce electricity through a chemical reaction, while electrolytic cells consume electricity to produce a chemical reaction.

    From the above differences between galvanic and electrolytic cells, we can conclude that a galvanic cell produces an electric current with a chemical reaction that happens spontaneously in it, whereas an electrolytic cell does the opposite. This means it brings about the chemical reaction using an electric current from an external source.

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