key term - Electrolytic cell

Definition

An electrolytic cell is a type of electrochemical cell that uses an external electrical current to drive a non-spontaneous chemical reaction. This process involves the conversion of electrical energy into chemical energy, allowing for reactions such as electrolysis, where compounds are broken down into their elements. The key features include the presence of electrodes immersed in an electrolyte solution, where oxidation occurs at the anode and reduction takes place at the cathode.

5 Must Know Facts For Your Next Test

1. In an electrolytic cell, an external power source, like a battery, is required to provide the energy needed to drive the non-spontaneous reaction.
2. The overall reaction in an electrolytic cell can be represented by combining half-reactions for oxidation and reduction occurring at the anode and cathode, respectively.
3. Electrolytic cells are used in various applications, including electroplating, purification of metals, and production of chemical compounds like chlorine and hydrogen gas.
4. During electrolysis, the electrolyte can be a liquid or gel that conducts electricity through the movement of ions, which is crucial for completing the circuit.
5. Faraday's laws of electrolysis quantify the relationship between the amount of substance produced or consumed during electrolysis and the amount of electric charge passed through the cell.

Review Questions

• How does the role of external power differ in electrolytic cells compared to galvanic cells?
  • In electrolytic cells, an external power source is necessary to provide energy for driving non-spontaneous reactions, whereas galvanic cells generate electrical energy from spontaneous chemical reactions. This fundamental difference means that electrolytic cells require voltage to operate and perform processes like electrolysis. In contrast, galvanic cells can produce electricity autonomously from their chemical reactions.
• Discuss how the configuration of electrodes in an electrolytic cell influences the efficiency of electrolysis.
  • The configuration of electrodes plays a critical role in determining the efficiency of electrolysis in an electrolytic cell. Proper placement and materials for the anode and cathode can enhance ionic conduction and reduce resistance within the electrolyte solution. Additionally, factors such as surface area, material conductivity, and separation distance between electrodes affect current distribution and ultimately impact how effectively the cell performs the desired chemical transformation during electrolysis.
• Evaluate the implications of Faraday's laws of electrolysis on industrial processes that utilize electrolytic cells.
  • Faraday's laws of electrolysis have significant implications for industrial processes that use electrolytic cells, as they provide a quantitative basis for predicting product yield based on electric charge. Understanding these laws allows industries to optimize conditions for processes like electroplating and metal refining by controlling current and charge duration to achieve desired outcomes efficiently. This knowledge helps ensure consistent product quality while minimizing resource waste and costs associated with electricity consumption.

Related terms

Electrolysis: The process of using electrical energy to drive a chemical reaction, often used to decompose compounds into their constituent elements.

Anode:

The electrode in an electrolytic cell where oxidation occurs, typically attracting anions from the electrolyte.

Cathode:

The electrode in an electrolytic cell where reduction takes place, typically attracting cations from the electrolyte.