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Electrochemical Cell - Definition, Examples, Types, Uses, FAQs

Electrochemical Cell - Definition, Examples, Types, Uses, FAQs

Edited By Team Careers360 | Updated on Jul 02, 2025 04:30 PM IST

What is an Electrochemical Cell?

An energy cell is a machine that can generate electricity from the chemical reactions that occur in it, or use the electrical energy given to it to make chemical reactions in it. The given devices are capable of converting a chemical energy into an electrical energy, or even vice versa. A common example of an electrochemical cell is a standard 1.5-volt cell used to power many electronic devices such as TV remote and clocks. Such cells are capable of producing energy from the chemical reactions that occur in them and maintain the so-called Galvanic cells or Voltaic cells. In other words, the cells that cause the chemical reaction to take place when they pass through electrical energy are called electrical cells.

This Story also Contains
  1. What is an Electrochemical Cell?
  2. Electrochemical Cell Example
  3. Cell Representation
  4. Electrochemical Cell Diagram
  5. Half-Cells and Cell Strength
  6. Lower and Second Cells
  7. Types of Electric Cells
  8. Electrolytic Cell Function
  9. Simple Electric Cells
  10. Simple Electric Cell Parts:
  11. How Do Simple Electric Cells Work?
  12. Simple Cell Uses

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Electrochemical Cell Example

A typical example of an electrochemical cell is a standard 1.5 volt cell intended for consumer use. A battery consists of one or more cells, usually connected in parallel, series or even series pattern and parallel. We interact with electrical cells in all aspects of our daily lives from disposable AA batteries in our remote controls and lithium-ion batteries on our iPhones to the nerve cells scattered throughout our bodies. There are basically two types of electrical cells namely galvanic cells, also called Voltaic cells and electrolytic cells. Important examples of electrolysis are the decomposition of water into hydrogen and oxygen, and bauxite into aluminum and other chemicals. Electroplating (e.g., copper, silver, nickel or chromium) is performed using an electrolytic cell. Electrolysis is a process that uses direct electric current (DC).

Cell Representation

Keep in mind that normal cell power can be calculated from the E0cell probability in both the connection and the reduction response. The positive energy of the cell indicates that the reaction continues spontaneously in the direction in which the response is recorded. On the other hand, a malignant cell reaction is found automatically on the reverse side. Cell recognition is a brief description of voltaic or galvanic (automatic) cells. Response conditions (pressure, temperature, concentration, etc.), anode, cathode, and electrode components are all described in this unique shortcut. Remember that oxidation occurs in the anode and reduction occurs in the cathode.

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When the anode and cathode are connected by wire, electrons flow from the anode to the cathode. Normal galvanic cell A typical arrangement of half cells connected to form a galvanic cell. Using genetic engineering, let's assemble a cell. One beaker contains 0.15 M Cd (NO3) 2 and Cd metal electrodes. The other beaker even contains 0.20 M AgNO3 and usually the Ag metal electrode. In response, the silver ion is reduced by receiving an electron, and the solid Ag is the cathode. Cadmium is connected by loss of electrons, and a strong Cd is anode.

Electrochemical Cell Diagram

Electrochemical Cell Diagram

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Half-Cells and Cell Strength

Electrochemical cells are made up of two and a half cells, each containing an electrode embedded in the electrolyte. The same electrolyte can also be used for both the half cells.

These half cells are connected by a salt bridge that provides an ionic communication platform between them without allowing them to combine. An example of a salt bridge is filter paper coated with potassium nitrate or sodium chloride solution.

One half part of an electrochemical cell loses electrons due to oxidation and the other gains electrons in the degradation process. It can be known that the equilibrium reaction occurs in both half cells, and when equilibrium is reached, the network voltage becomes 0 and the cell stops producing electricity.

The tendency of the electrode to contact the electrolyte for the loss or acquisition of electrons is explained by its electrode strength. The values of this energy can be used to predict the overall strength of a cell. Typically, the electrode strength is measured with the help of a standard hydrogen electrode as a reference electrode (known electrode).

Lower and Second Cells

The primary cells actually use and dislodge galvanic cells. The electrochemical reactions which take place in these cells are irreversible. Therefore, reactants are used for the production of electrical energy and the cell stops producing electricity when the reactants are completely depleted. Second cells (also known as rechargeable batteries) are electrical cells in which the cell has a flexible response, i.e. the cell can function as a Galvanic cell and an Electrolytic cell. Most primary batteries (many cells connected to a series, similarities, or combinations of the two) are considered to be harmful and environmentally damaging devices. This is because they require about 50 percent of the energy they contain in their production process. They also contain a lot of toxic metals and are considered hazardous waste.

Types of Electric Cells

There are two main types of electrochemical cells that are:

1. Galvanic cells (that are also called as Voltaic cells)

2. Electrical cells

The three main components of electrolytic cells are:

Cathode (negatively charged by electrolytic cells)

Anode (charged well with electrolytic cells)

Electrolyte

The electrolyte provides the electron exchange between the cathode and the anode. The most widely used electrolytes in electrolytic cells include water (containing dissolved ions) and molten sodium chloride.

Electrolytic Cell Function

Melted sodium chloride (NaCl) can be subjected to electrolysis. Here, two inert electrodes are placed in molten sodium chloride (containing Na + cations separated from Cl- anions). When electrical energy is transferred to a region, the cathode becomes rich in electrons and has a negative charge. The well-charged sodium cation is now attracted to the badly charged cathode. This causes the formation of metallic sodium in the cathode. At the same time, chlorine atoms are attracted to a well-charged cathode. This causes the formation of chlorine gas (Cl2) in the anode (corresponding to the release of two electrons, terminating the circuit). The corresponding chemical estimates and overall cell response are given below.

Cathode reaction: [Na+ + e → Na] x 2

Anode reaction: 2Cl- → Cl2 + 2e

Cell Response: 2NaCl → 2Na + Cl2

Therefore, the molten sodium chloride can be subjected to electrolysis in an electrolytic cell to produce metallic sodium and chlorine gas as products.

Electrolytic Cell Applications

The primary use of electrolytic cells is to produce oxygen gas and hydrogen gas in water. They are used to extract aluminum from bauxite. Another notable use of electrolytic cells is electroplating, which is the process of forming a thin protective layer of a particular metal on the surface of another metal. Electrorefining of most non-ferrous metals is performed with the help of electrolytic cells. Such electrical cells are also used in electrowinning processes. It can be noted that the industrial production of very pure copper, pure zinc, and high-grade aluminum is regularly performed by electrolytic cells.

Simple Electric Cells

In Simple Electric Cells, the electricity is used to produce chemical changes. Similarly, we say that electrical energy is converted into chemical energy. Reversal occurs in Simple Cells (also known as Electric Cells) where chemical changes are used to generate electricity which means that chemical energy is converted into electrical energy.

Simple Electric Cell Parts:

A simple cell consists of two solid electrodes embedded in an electrolyte connected together by a cable-like conductor.

The two electrodes should be two separate metals.

The electrolyte can be an acid solution, an alkaline solution, a salt solution or a fruit like orange or lemon.

The electrical power generated depends on the positions of the two metals in the reactivity series.

"The farther the metal is in the regenerative series, the greater will be the electric current".

For example, a magnesium/ electrode pair will provide greater strength than a zinc/ copper electrode pair.

NCERT Chemistry Notes :

How Do Simple Electric Cells Work?

Let's use a simple cell example to discuss further.

Metal electrode 1: Zinc

Steel electrode 2: Copper

Electrolyte: Reduce NaCl

The highest metal in the recycled steel chain will be selected and oxidized. It will easily remove electrons and a non-electrode (known as Anode). In the example above, zinc is more effective than copper, so the zinc electrode will be a non-electrode. Electrons leave the zinc electrode passing through the connecting wires to the copper electrode.

The lower metal at the bottom of the reconstituted metal chain will be a fine electrode (known as Cathode). Thus, the copper will be a fine electrode. The electrolyte contains good ions (sodium cations) and hydrogen ions. Hydrogen ions have a greater release rate than sodium ions and will be specially released (reduced) by receiving electrons from a non-wireless electrode. This is a redox reaction where oxidation and decomposition occur simultaneously. Here, electrons are transferred from zinc atoms to hydrogen ions.

Simple Cell Uses

Light cells are also commonly referred to as batteries that provide a portable form of electrical energy. They supply electricity to watches, lights, etc. that do not need to be connected to a large power supply.

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Frequently Asked Questions (FAQs)

1. 1.Write any one main difference between electrolytic cells and Galvanic cells?

The cellular response of electrolytic cells does not occur spontaneously and the reaction of Galvanic cells is spontaneous. Galvanic cells produce electrical energy from chemical reactions and electrolytic cells produce spontaneous redox reactions from electrical input.

2. 2.What are the three main components of electrolytic cells?

The three main components which are available in electrolytic cells are the cathode, anode, and electrolyte. In electrolytic cells (as is the case with most electrochemical cells), oxidation occurs at the anode and decomposition occurs at the cathode.

3. 3.What types of cases are held by electrolytic cell electrodes?

In electrolytic cells, the cathode is poorly charged and the anode is well charged. Well-charged ions flow to the cathode and poorly charged ions flow to the anode.

4. 4.What is the use of electrolytic cells?

Electrolytic cells can be used to produce oxygen gas and hydrogen gas in water by moving it into electrolysis. These devices can also be used to obtain chlorine gas and metallic sodium from strong solutions of sodium chloride (common salt). Another important use of electrolytic cells is electroplating.

5. 5.How do electrical cells work?

When external electrical energy flows into the cathode of an electrolytic cell, the negatively charge attracts the separated ions present in the electrolyte. This results in the insertion of well-charged ions into the cathode. At the same time, negatively charged ions flow into the anode, charged well.

6. What is the Daniell cell and why is it significant?
The Daniell cell is a type of electrochemical cell consisting of zinc and copper electrodes in solutions of their respective sulfates. It's significant because:
7. What is the principle behind electroplating, and how does it use electrochemical cells?
Electroplating uses an electrolytic cell to deposit a layer of metal on a surface:
8. What is the difference between a galvanic cell and an electrolytic cell?
A galvanic cell (also called a voltaic cell) produces electricity spontaneously from a chemical reaction. An electrolytic cell, on the other hand, uses electrical energy to drive a non-spontaneous chemical reaction. In essence, a galvanic cell converts chemical energy to electrical energy, while an electrolytic cell does the opposite.
9. What is the role of the electrolyte in an electrochemical cell?
The electrolyte in an electrochemical cell serves several crucial functions:
10. What is the difference between a galvanic series and an electrochemical series?
While related, these series have distinct differences:
11. How does electrode surface area affect an electrochemical cell?
Electrode surface area affects the rate of reaction in an electrochemical cell:
12. What is meant by a "half-cell reaction"?
A half-cell reaction is either the oxidation or reduction process occurring at one electrode of an electrochemical cell. The complete cell reaction is the sum of two half-cell reactions. For example, in a zinc-copper cell:
13. What is the function of the salt bridge in an electrochemical cell?
The salt bridge maintains electrical neutrality in the cell by allowing ions to flow between the half-cells. It prevents the buildup of charge in either half-cell, which would stop the flow of electrons. The salt bridge does not participate in the redox reactions directly.
14. How is the voltage of an electrochemical cell determined?
The voltage of an electrochemical cell is determined by the difference in reduction potentials of the two half-reactions occurring at the electrodes. It can be calculated using the Nernst equation, which takes into account standard reduction potentials and the concentrations of reactants and products.
15. How does the concept of electrochemical series relate to electrochemical cells?
The electrochemical series is a ranking of elements based on their standard reduction potentials. In an electrochemical cell:
16. What is the significance of the standard hydrogen electrode (SHE)?
The standard hydrogen electrode (SHE) serves as a reference point for measuring the standard reduction potentials of other half-reactions. Its potential is arbitrarily set to zero, allowing for the creation of a table of standard reduction potentials that can be used to predict the direction of redox reactions and calculate cell potentials.
17. How does electron flow occur in an electrochemical cell?
Electrons flow from the anode (where oxidation occurs) through the external circuit to the cathode (where reduction occurs). This flow of electrons generates an electric current that can be used to power devices or perform work.
18. What is meant by the term "cell potential"?
Cell potential, also known as electromotive force (EMF), is the difference in electrical potential between the two electrodes of an electrochemical cell. It represents the maximum voltage that the cell can produce under ideal conditions and is measured in volts.
19. What is the purpose of a porous barrier in some electrochemical cells?
A porous barrier, like a salt bridge, separates the two half-cells while allowing ion movement to maintain electrical neutrality. It prevents direct mixing of the electrolytes, which could lead to unwanted side reactions, while still permitting the necessary ion flow for the cell to function.
20. How does an electrochemical cell generate electricity?
An electrochemical cell generates electricity through redox reactions:
21. How does concentration affect the voltage of an electrochemical cell?
Concentration affects cell voltage according to the Nernst equation. As the concentration of reactants increases or products decreases, the cell voltage increases. Conversely, as the concentration of reactants decreases or products increases, the cell voltage decreases.
22. What is the significance of the standard cell potential (E°cell)?
The standard cell potential (E°cell):
23. How does a fuel cell differ from a typical electrochemical cell?
A fuel cell is a special type of electrochemical cell that continuously converts chemical energy from a fuel (like hydrogen) into electrical energy. Unlike typical cells:
24. How do electrochemical cells relate to corrosion processes?
Corrosion, particularly of metals, is an electrochemical process:
25. How do electrochemical cells contribute to energy storage technologies?
Electrochemical cells are crucial in energy storage:
26. How do electrochemical cells contribute to analytical chemistry techniques?
Electrochemical cells are used in various analytical techniques:
27. How does temperature affect an electrochemical cell?
Temperature affects an electrochemical cell in several ways:
28. What are the main components of an electrochemical cell?
The main components of an electrochemical cell are:
29. How can you determine which electrode is the anode and which is the cathode?
To determine which electrode is the anode and which is the cathode:
30. What is the role of a separator in battery-type electrochemical cells?
The separator in a battery:
31. What is the importance of the internal resistance in an electrochemical cell?
Internal resistance in an electrochemical cell:
32. What is the role of catalysts in electrochemical cells?
Catalysts play important roles in many electrochemical cells:
33. What is cyclic voltammetry and how does it relate to electrochemical cells?
Cyclic voltammetry is an electrochemical technique:
34. How do electrochemical cells contribute to the development of sustainable energy technologies?
Electrochemical cells are crucial in sustainable energy:
35. How does an electrochemical cell differ from a battery?
While all batteries are electrochemical cells, not all electrochemical cells are batteries. A battery is typically a self-contained unit with a fixed amount of reactants, while an electrochemical cell can be set up with external reactants and may be rechargeable or continuously supplied with new reactants.
36. What is the difference between primary and secondary cells?
Primary cells are non-rechargeable and can only be used once. The chemical reactions are irreversible. Examples include alkaline batteries.
37. How do pH meters work using electrochemical principles?
pH meters use a special type of electrochemical cell:
38. What is the difference between a wet cell and a dry cell?
Wet cells and dry cells differ in their electrolyte state:
39. How do concentration cells work?
Concentration cells generate electricity from the difference in concentration of the same electrolyte at the two electrodes:
40. What is an electrochemical cell?
An electrochemical cell is a device that converts chemical energy into electrical energy or vice versa. It consists of two electrodes (anode and cathode) connected by an electrolyte, allowing for the flow of ions and electrons to generate an electric current.
41. How do electrochemical cells relate to the concept of redox reactions?
Electrochemical cells are practical applications of redox (reduction-oxidation) reactions:
42. What is the principle behind electrochemical sensors?
Electrochemical sensors work on the principle that chemical reactions produce an electrical signal:
43. How do electrochemical gradients relate to electrochemical cells?
Electrochemical gradients are important in many cellular processes and relate to electrochemical cells:
44. How do electrochemical cells relate to the concept of electronegativity?
Electronegativity and electrochemical cells are related:
45. What is overpotential and why is it important in electrochemistry?
Overpotential is the additional potential (beyond the thermodynamically determined potential) required to drive a reaction at a certain rate. It's important because:
46. What is the significance of the Faraday constant in electrochemistry?
The Faraday constant (F) is crucial in electrochemistry:
47. How do electrochemical cells contribute to water treatment technologies?
Electrochemical cells are used in various water treatment processes:
48. How do electrochemical cells contribute to the field of nanotechnology?
Electrochemical cells are important in nanotechnology:

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