Electroplating is the opposite of which of the following?

Explanation:

Electroplating and Its Opposite Process

Definition: Electroplating is a process that uses electrical current to reduce dissolved metal cations so that they form a coherent metal coating on an electrode. This process is commonly used to deposit a layer of material, such as a metal, onto a surface for various purposes including corrosion resistance, aesthetic improvements, and reducing friction.

Working Principle: In electroplating, the object to be plated is made the cathode (negative electrode) in an electrolysis cell. The anode (positive electrode) is typically made of the metal to be plated. A solution containing a salt of the metal to be plated is used as the electrolyte. When an electric current is passed through the cell, metal cations from the electrolyte are reduced at the cathode surface, forming a thin layer of metal. Simultaneously, metal atoms from the anode dissolve into the electrolyte to maintain the concentration of metal cations.

Advantages:

• Provides corrosion resistance to the plated object.
• Enhances the appearance of the object.
• Improves wear resistance and reduces friction.

Disadvantages:

• Requires careful control of the plating process to achieve uniform coating.
• Involves hazardous chemicals that require proper handling and disposal.

Applications: Electroplating is widely used in various industries, including automotive, electronics, jewelry, and manufacturing, to enhance the properties and appearance of products.

Galvanic cell:

• A galvanic cell, also known as a voltaic cell, is an electrochemical cell that derives electrical energy from spontaneous redox reactions taking place within the cell. It essentially converts chemical energy into electrical energy. The key difference between a galvanic cell and electroplating lies in the direction of electron flow and the nature of the reactions involved.
• In a galvanic cell, two different metals are connected by a salt bridge or a porous disk between the individual half-cells. Each metal is immersed in an electrolyte solution. The metal that is more reactive (anode) undergoes oxidation, losing electrons, while the less reactive metal (cathode) undergoes reduction, gaining electrons. This flow of electrons through an external circuit generates electrical energy.
• In contrast, electroplating is an electrolytic process that requires an external power source to drive the non-spontaneous chemical reactions. In electroplating, the object to be plated is the cathode, and the metal to be deposited is the anode. When current is applied, metal cations from the electrolyte are reduced at the cathode, forming a coating.
• Thus, while electroplating involves the deposition of metal ions onto a surface using an external power source, a galvanic cell generates electrical energy through spontaneous redox reactions. This fundamental difference makes galvanic cells the opposite of the electroplating process.