An electrolytic cell is an electrochemical device that uses electrical energy to facilitate a non-spontaneous redox reaction. It is commonly used for the electrolysis of certain compounds, such as water, to form gaseous oxygen and gaseous hydrogen. The three primary components of electrolytic cells are the cathode (negatively charged), the anode (positively charged), and the electrolyte. Electrolytic cells are also used for the extraction of aluminum from bauxite, in electroplating, and in electrowinning processes. Additionally, the industrial production of high-purity copper, high-purity zinc, and high-purity aluminum is almost always done through electrolytic cells.
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electrolytic cell
Multifunctional Electrolytic Electrochemical Cell Water Bath Single Layer Double Layer
Item Number: ELCM
$159.00
H-Type Double-Layer Optical Electrolytic Electrochemical Cell with Water Bath
Item Number: ELCHD
$269.00
PTFE Electrolytic Cell Electrochemical Cell Corrosion-Resistant Sealed and Non-Sealed
Item Number: ELCP
$29.90
We have the best Electrolytic Cell solutions to meet your needs. Our extensive portfolio of electrolytic cells includes standard solutions for common applications, as well as bespoke designs for unique requirements.
Applications of Electrolytic Cell
- Decomposition of chemical compounds, such as water into hydrogen and oxygen, and bauxite into aluminum and other chemicals.
- Electroplating of copper, silver, nickel, or chromium.
- Electrorefining and electrowinning of non-ferrous metals like high-purity aluminum, copper, zinc, and lead.
- Production of caustic soda and other chemicals.
- Refining copper and other metals.
- Determination of electrode potential of different metals.
- Determination of electrochemical series via a Standard Hydrogen Electrode (SHE) system.
Advantages of Electrolytic Cell
- Electrolytic cells are used for the production of hydrogen and oxygen gas from water.
- They are used to extract aluminum from bauxite.
- Electrolytic cells are used in electroplating to create a thin protective layer of a specific metal on the surface of another metal.
- The electrorefining of many non-ferrous metals is done with the help of electrolytic cells.
- Electrolytic cells are used in electrowinning processes.
- Industrial production of high-purity copper, high-purity zinc, and high-purity aluminium is almost always done through electrolytic cells.
Electrolytic cell is an electrochemical cell that drives a non-spontaneous redox reaction with electrical energy. It is widely used to decompose chemical compounds and electroplate various metals. Our extensive product line provides you with a standard solution that fits your needs, and for more unique applications, our custom design service will help us cater to your specific requirements.
FAQ
What Are Electrolytic Cells Used For?
Electrolytic cells are used for the decomposition of chemical compounds through electrolysis. This process involves the use of an external electric current to facilitate a non-spontaneous redox reaction. Electrolytic cells are commonly used to produce oxygen and hydrogen gas from water, extract aluminum from bauxite, and electroplate various metals. Additionally, electrolytic cells are used in the electrorefining and electrowinning of non-ferrous metals such as aluminum, copper, zinc, and lead. Overall, electrolytic cells have numerous industrial applications in the production and refinement of various chemical compounds and metals.
What Is The Difference Between Galvanic Cell And Electrolytic Cell?
The main difference between a galvanic cell and an electrolytic cell is that a galvanic cell generates electrical energy from a spontaneous redox reaction, while an electrolytic cell uses electrical energy to drive a non-spontaneous redox reaction. Another difference is that a galvanic cell has a positive cell potential, while an electrolytic cell has a negative cell potential. Galvanic cells are used in batteries, while electrolytic cells are used in processes such as electroplating and purification of metals.
What Is An Electrolytic Cell And How Does It Work?
An electrolytic cell is an electrochemical cell that uses electrical energy to drive a non-spontaneous redox reaction. It consists of an electrolyte and two electrodes (a cathode and an anode). When an external voltage is supplied to the electrodes, the ions in the electrolyte are attracted to an electrode with the opposite charge, allowing charge-transferring (also known as faradaic or redox) events to occur. The negative electrode is called the cathode and the positive electrode is called the anode. Oxidation occurs at the anode, and reduction occurs at the cathode.
What Are The Two Points Of Difference Between Electrochemical And Electrolytic Cells?
Electrochemical and electrolytic cells both rely on the movement of electrons through the system. However, spontaneous chemical reactions occur in electrochemical cells, whereas nonspontaneous chemical reactions occur in electrolytic cells.
What Is The Example Of Electrolytic Cell?
Important examples of electrolysis are the decomposition of water into hydrogen and oxygen, and bauxite into aluminum and other chemicals. Electroplating (e.g., of copper, silver, nickel, or chromium) is done using an electrolytic cell.
Are Electrolytic Cells Spontaneous?
Galvanic cells derives its energy from spontaneous redox reactions, while electrolytic cells involve non-spontaneous reactions and thus require an external electron source like a DC battery or an AC power source.
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