Electrolytic Cell

Definition

An electrolytic cell is an electrochemical cell that drives a non-spontaneous chemical reaction through the application of an external voltage. This type of cell converts electrical energy into chemical energy by using electricity to induce a chemical change, often seen in processes like electroplating and the production of substances such as chlorine gas. Understanding electrolytic cells is crucial because they showcase the principles of electrochemistry, particularly how electrical energy can facilitate chemical transformations that wouldn't occur naturally.

5 Must Know Facts For Your Next Test

1. Electrolytic cells require a power source to operate, which provides the necessary voltage to drive the non-spontaneous reactions.
2. The process of electrolysis can be used in various applications, including metal extraction, purification, and the production of chemical substances.
3. During operation, the anode is positively charged and attracts negatively charged ions (anions), while the cathode is negatively charged and attracts positively charged ions (cations).
4. The efficiency of an electrolytic cell can be influenced by factors such as temperature, concentration of electrolytes, and current density.
5. Faraday's laws of electrolysis relate the amount of substance produced at each electrode to the quantity of electricity passed through the cell.

Review Questions

• How does an electrolytic cell differ from a galvanic cell in terms of energy conversion?
  • An electrolytic cell converts electrical energy into chemical energy, facilitating a non-spontaneous reaction through an external voltage. In contrast, a galvanic cell generates electrical energy from spontaneous chemical reactions. The key difference lies in their operation: electrolytic cells require power input to drive reactions, while galvanic cells produce power from reactions occurring naturally.
• Discuss the roles of the anode and cathode in an electrolytic cell and how they contribute to the overall process.
  • In an electrolytic cell, the anode serves as the site for oxidation reactions, where electrons are lost, making it positively charged. Conversely, the cathode is where reduction occurs, attracting cations and gaining electrons, giving it a negative charge. This setup is crucial for maintaining electron flow through the circuit and facilitating the required chemical transformations during electrolysis.
• Evaluate the significance of Faraday's laws of electrolysis in understanding the efficiency and practicality of electrolytic cells.
  • Faraday's laws of electrolysis are essential for predicting and calculating how much product will be generated during the electrolysis process based on the current passed through the cell. The first law states that the mass of a substance altered at an electrode during electrolysis is proportional to the quantity of electric charge passed through it. The second law relates this mass to the equivalent weight of the substance. By applying these laws, one can assess the efficiency and optimize operational parameters in industrial applications involving electrolytic cells, making them vital for processes like metal plating and purification.

Related terms

Electrolysis:

A chemical process that uses electricity to break down compounds into their elements or simpler compounds.

Anode:

The electrode where oxidation occurs in an electrolytic cell, attracting negative ions.

Cathode: The electrode where reduction occurs in an electrolytic cell, attracting positive ions.