What is the Difference Between Electrochemical Cell and Electrolytic Cell?

The main difference between an electrochemical cell and an electrolytic cell lies in the purpose and energy conversion process. Here are the key distinctions between the two:

• Electrochemical Cell: These cells convert chemical energy into electrical energy. They are also known as galvanic or voltaic cells. In an electrochemical cell, a spontaneous redox reaction generates electrical energy. Examples of electrochemical cells include batteries and fuel cells.
• Electrolytic Cell: These cells require an external power source to drive non-spontaneous chemical reactions. They convert electrical energy into chemical energy. In an electrolytic cell, an external power source creates an electric field, causing positive ions (cations) to move towards the cathode, where reduction occurs, and negative ions (anions) to move towards the anode, where oxidation occurs. Examples of electrolytic cells include electroplating and the electrolysis of water to produce hydrogen and oxygen.

In summary:

• Electrochemical cells generate electrical energy from spontaneous redox reactions.
• Electrolytic cells require an external power source to drive non-spontaneous reactions, converting electrical energy into chemical energy.

Comparative Table: Electrochemical Cell vs Electrolytic Cell

Here is a table summarizing the differences between electrochemical cells and electrolytic cells:

In summary, electrochemical cells convert chemical energy into electrical energy through spontaneous redox reactions, while electrolytic cells require an external source of electrical energy to drive non-spontaneous redox reactions and convert electrical energy into chemical energy.