An electrochemical cell is a device capable of either generating electrical energy from chemical reactions or facilitating chemical reactions through the introduction of electrical energy.
However, not all electrochemical cells are electrolytic cells.
Electrochemical cells that generate an electric current are called voltaic or galvanic cells, while those that generate chemical reactions via electrolysis are called electrolytic cells.
Therefore, an electrochemical cell is a broader term that includes both galvanic and electrolytic cells.
5 Key Differences Between Electrochemical and Electrolytic Cells
1. Definition of Electrochemical Cell
An electrochemical cell is a device that can either generate electrical energy from chemical reactions or facilitate chemical reactions by introducing electrical energy.
It includes both galvanic (voltaic) cells and electrolytic cells.
2. Galvanic (Voltaic) Cells
These cells generate electrical energy from spontaneous redox reactions.
They are named after Luigi Galvani and Alessandro Volta.
Galvanic cells consist of two half-cells with separate oxidation and reduction reactions.
When connected in series or parallel, galvanic cells form a battery.
3. Electrolytic Cells
These cells utilize external electrical energy to force a chemical reaction that would otherwise not occur spontaneously.
The external energy source is a voltage applied between the cell's two electrodes (anode and cathode) immersed in an electrolyte solution.
The net reaction in an electrolytic cell is the reverse of a spontaneous reaction, making the Gibbs free energy positive.
4. Key Differences
Energy Generation vs. Utilization
Galvanic cells generate electrical energy from spontaneous chemical reactions.
Electrolytic cells use electrical energy to drive non-spontaneous chemical reactions.
Spontaneity of Reactions
Reactions in galvanic cells are spontaneous (Gibbs free energy is negative).
Reactions in electrolytic cells are non-spontaneous (Gibbs free energy is positive).
Electrode Charges
In galvanic cells, the anode is negative and the cathode is positive.
In electrolytic cells, the anode is positive and the cathode is negative.
5. Applications
Galvanic Cells
Used in batteries, including primary (single-use) and secondary (rechargeable) batteries.
Electrolytic Cells
Used in electrolysis processes for refining metals, plating, and producing chemicals like caustic soda.
Example: Electrolysis of sodium chloride to form sodium metal and chlorine gas.
In summary, while both electrochemical and electrolytic cells involve the interaction between electrical energy and chemical reactions, they serve different purposes and operate under different principles.
Electrochemical cells encompass a broader range of devices, including both galvanic and electrolytic cells, each with distinct functionalities and applications.
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