Learn More on Electrochemical Cell

Electrochemical cells may be found in various places in our daily lives, from throwaway

AA batteries in remote controls to lithium-ion batteries in iPhones to nerve cells

scattered throughout our bodies. Galvanic (also known as Voltaic) and electrolytic cells

are the two kinds of electrochemical cells. A DC battery or an AC power source provides an external supply of electrons while electrolytic cells use non-spontaneous reactions. Read till the end to know what electrochemical cells, and some of their applications.

What Is an Electrochemical Cell?

An electrochemical cell is a type of apparatus capable of producing electric current from chemical change caused due to chemical reactions and further releasing this energy by a spontaneous redox reaction. Electric current is the transfer of free electrons from one species to the other. An electrochemical cell consists of two half-cells. Each half-cell has one electrode and one electrolyte; it can be of the same element or different as well. The components of an electrochemical cell are:

Electrodes – Electrodes are cylindrical-shaped conducting solids that are made up of metals. They are of two types:

1. The Anode – In an electrochemical cell, oxidation takes place at the anode. 
2. The Cathode – In electrochemical cells, reduction takes place at the cathode.

Electrolyte – An electrolyte is a solution made up of compounds mixed with polar solvents like water that can produce free ions responsible for producing electricity.

Salt Bridge – A salt bridge is responsible for completing the electrochemical circuit because it acts as a bridge by connecting the reduction half of the cell to the corresponding oxidation half. A salt bridge consists of saturated salt solution such as potassium chloride (KCl).

Electrochemical Cell Types

Galvanic Cell

Galvanic cells have typically been employed as DC power sources. A basic galvanic cell

may have one electrolyte separated by a semipermeable membrane or a more

a complicated version may have two half-cells linked by a salt bridge. 

The salt bridge comprises an inert electrolyte, such as potassium sulphate, whose ions flow into the individual half-cells to balance the charges that are building up at the electrodes. 

The mnemonic “Red Cat An Ox” states that oxidation occurs at the anode, and reduction

occurs at the cathode. The anode holds the status of carrying the name as the negative terminal of the galvanic cell because the reaction at the anode provides the source of electrons for the current.

Electrolytic Cell

An electrolytic cell is a transformed version of the electrochemical cell only. When a potential difference higher than the potential difference of an electrochemical cell is applied, the electrochemical cell starts to act like an electrolytic cell.  This potential difference causes the electric current direction opposite to the original direction. 

Electrolytic cells are encountered during the charging process of every rechargeable battery, from lead-acid vehicle batteries to smartphone lithium-ion batteries. The electrodes of an electrolytic cell may be positioned in a single compartment holding the molten or aqueous electrolyte, unlike the galvanic cell.

The electrodes will also match the positive and negative terminals of the battery since the external battery supply is what propels the electrons through the circuit. The anode remains the oxidation site, but it now serves as the positive terminal, whereas the cathode serves as the negative terminal.

An electrolytic cell may also decompose substances into simpler chemicals, such as water and sodium

chloride. This is used to synthesise chlorine and sodium

hydroxide in industrial operations. Because electrolytic cells may be run in either molten

or aqueous electrolytes, depending on the cation and anion, the products produced by

molten electrolysis may vary from those produced by aqueous electrolysis.

Electrochemical Cell Applications

1. Metallurgy: – Electrochemical cells are utilised in the electric ore refining process for extracting highly pure metals such as copper, aluminium, lead, and zinc.
2. Hearing Aids: – Sodium oxide produced from electrochemical cells is very beneficial for developing hearing aids devices.
3. Batteries & Cells: – Electrochemical cells are nothing but a core structure and model of what a battery is.

Electrochemical cells, like primary cells, are non-rechargeable batteries; they have used torches and TV remotes. 

Electrochemical cells, like secondary cells, are rechargeable because they can work both as galvanic or electrolytic cells. The lithium-ion battery, the most popular battery in the 21st century, is a type of secondary cell utilised in electronic gadgets and automobiles.

Conclusion

An electrochemical cell is capable of generating electrical energy from chemical reactions inside it or using electrical energy supplied to aid chemical reactions. These devices can turn chemical energy into electrical energy and vice versa. An electrochemical cell is a standard 1.5-volt cell used to operate various electrical goods such as remotes and watches. These electrochemical cells are used in batteries in several applications, some of the common applications include computers,  smartphones, remote controls, laptops, smartphones, and other electronic gadgets like watches, clocks, etc. We saw what an electrochemical cell is, and the types of electrochemical cells that are used globally.