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. It is essential in various applications, such as electroplating and the production of chemicals like chlorine and hydrogen. In these cells, oxidation and reduction reactions occur at the electrodes, where anode reactions involve oxidation and cathode reactions involve reduction.

5 Must Know Facts For Your Next Test

1. Electrolytic cells convert electrical energy into chemical energy, allowing non-spontaneous reactions to occur.
2. These cells consist of two electrodes: an anode where oxidation happens and a cathode where reduction takes place.
3. The overall reaction in an electrolytic cell can be driven by a voltage applied across the electrodes that exceeds the cell's equilibrium potential.
4. Electrolytic cells are widely used in industrial processes, such as the extraction of metals from their ores and electroplating to provide a protective or decorative coating.
5. The efficiency of electrolytic cells can be affected by factors such as temperature, concentration of electrolytes, and the design of the cell itself.

Review Questions

• How does the function of an electrolytic cell differ from that of a galvanic cell?
  • An electrolytic cell functions by using an external electrical current to drive non-spontaneous chemical reactions, while a galvanic cell generates electrical energy from spontaneous reactions. In electrolytic cells, external power sources supply the necessary energy to facilitate reactions at the electrodes, resulting in oxidation at the anode and reduction at the cathode. Conversely, galvanic cells harness energy from spontaneous reactions occurring naturally between reactants without the need for external energy input.
• Discuss the role of electrolysis in an electrolytic cell and its real-world applications.
  • Electrolysis is the key process occurring within an electrolytic cell, where electrical energy is used to induce chemical changes, resulting in reactions such as the decomposition of compounds. Real-world applications include electroplating, where a metal layer is deposited on an object for protection or aesthetic purposes, and the production of gases like hydrogen and chlorine during water electrolysis. These applications demonstrate how electrolytic cells are critical for both industrial processes and advancements in materials science.
• Evaluate how varying conditions such as temperature and electrolyte concentration influence the efficiency of an electrolytic cell.
  • The efficiency of an electrolytic cell can be significantly impacted by changing conditions like temperature and electrolyte concentration. Higher temperatures generally increase reaction rates by providing more kinetic energy to the particles involved, thus enhancing overall efficiency. Likewise, altering electrolyte concentration affects ion availability; higher concentrations facilitate faster ion movement toward electrodes, reducing resistance and improving current flow. These factors must be carefully controlled in industrial settings to maximize yield and minimize energy consumption.

Related terms

Electrolysis:

The process of using electrical energy to cause a chemical change, typically to decompose chemical compounds in an electrolytic cell.

Anode: The electrode at which oxidation occurs in an electrolytic cell, drawing electrons away from the substance being oxidized.

Cathode: The electrode at which reduction takes place in an electrolytic cell, attracting electrons to the substance being reduced.