Electrolytic Cell vs. Galvanic Cell

Attribute	Electrolytic Cell	Galvanic Cell
Energy Source	External electrical energy source	Chemical reactions
Reaction Type	Non-spontaneous	Spontaneous
Anode	Positive electrode	Negative electrode
Cathode	Negative electrode	Positive electrode
Electrolyte	Conducting solution	Conducting solution

Introduction

Electrochemical cells are devices that convert chemical energy into electrical energy through redox reactions. There are two main types of electrochemical cells: electrolytic cells and galvanic cells. While both cells involve redox reactions, they operate in different ways and have distinct attributes that make them suitable for different applications.

Electrolytic Cell

An electrolytic cell is an electrochemical cell that uses electrical energy to drive a non-spontaneous redox reaction. In an electrolytic cell, an external voltage source is connected to the cell, causing a flow of electrons from the anode to the cathode. This flow of electrons drives the non-spontaneous redox reaction, allowing for the production of desired products or the decomposition of compounds.

• Requires an external voltage source
• Non-spontaneous redox reaction
• Electrons flow from anode to cathode
• Used for electrolysis and electroplating
• Produces desired products or decomposes compounds

Galvanic Cell

A galvanic cell, also known as a voltaic cell, is an electrochemical cell that uses spontaneous redox reactions to generate electrical energy. In a galvanic cell, the redox reaction occurs spontaneously, producing a flow of electrons from the anode to the cathode. This flow of electrons can be harnessed to power external devices, making galvanic cells a common choice for batteries and other portable power sources.

• Spontaneous redox reaction
• Electrons flow from anode to cathode
• Generates electrical energy
• Used in batteries and portable power sources
• Does not require an external voltage source

Key Differences

One of the key differences between electrolytic cells and galvanic cells is the source of energy used to drive the redox reaction. In an electrolytic cell, an external voltage source is required to drive the non-spontaneous redox reaction, while a galvanic cell operates spontaneously without the need for an external voltage source. This difference in energy source makes electrolytic cells suitable for electrolysis and electroplating processes, while galvanic cells are commonly used in batteries and portable power sources.

Another important difference between electrolytic cells and galvanic cells is the direction of electron flow. In both types of cells, electrons flow from the anode to the cathode, but the reason for this flow differs. In an electrolytic cell, the external voltage source forces electrons to flow in a specific direction to drive the non-spontaneous redox reaction. In contrast, in a galvanic cell, the spontaneous redox reaction naturally causes electrons to flow from the anode to the cathode, generating electrical energy in the process.

Additionally, the products of the redox reactions in electrolytic cells and galvanic cells differ. In an electrolytic cell, the redox reaction is driven to produce specific desired products or to decompose compounds. This makes electrolytic cells useful for processes such as electrolysis, electroplating, and the production of chemicals. On the other hand, in a galvanic cell, the spontaneous redox reaction generates electrical energy that can be used to power external devices. This makes galvanic cells ideal for applications where a portable power source is needed, such as in batteries for electronic devices.

Conclusion

In conclusion, electrolytic cells and galvanic cells are two types of electrochemical cells that operate in different ways and have distinct attributes. Electrolytic cells require an external voltage source to drive non-spontaneous redox reactions, while galvanic cells operate spontaneously to generate electrical energy. The direction of electron flow, the products of the redox reactions, and the applications of these cells also differ. Understanding the differences between electrolytic cells and galvanic cells is important for choosing the right type of electrochemical cell for a specific application.