Wiktor Wise
An electric cell, also known as an electrolytic cell, is a device that converts energy from one form to another. It is used to generate the electric force required to move electrons through internal and external circuit components. It consists of a container in which a chemical reaction involving electrodes takes place. For example, a simple voltaic cell consists of a zinc and copper base soaked in sulphuric acid. Electric cells are used in batteries and in the generation of solar power.
| Characteristics | Values |
|---|---|
| Definition | A device that is capable of changing some form of energy, such as chemical or radiant energy, into electricity |
| Example | A battery |
| Other Names | Electrical cell, electrolytic cell, voltaic cell |
| Function | Used to generate the electric force required to move electrons through the internal and external circuit components |
| Chemical Reaction | A chemical reaction involving electrodes and electrolysis |
| Chemical Substances | Two pieces of metal, water, and a little electrolyte (e.g., hydrochloric acid, sulfuric acid, sodium bicarbonate, or sodium hydroxide) |
| Electrode Composition | Zinc, copper, silver |
| Electromotive Force (EMF) | 1.1V for Daniel cell, 1.5V for Leclanche cell |
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What You'll Learn
- Electric cells are devices that convert energy into electricity.
- Photoelectric or photovoltaic cells convert light energy into electrical energy
- Electrolytic cells are used for chemical reactions that require high energy
- The Voltaic cell was named after Alexander Volta
- Primary cells are non-rechargeable and have non-reversible chemical reactions
Electric cells are devices that convert energy into electricity.
An electric cell consists of a container in which a chemical reaction involving electrodes takes place. Chemical substances are exposed to electrical power, and an electrolysis reaction occurs inside the cell. For example, two pieces of metal are placed in water with a small amount of an electrolyte such as hydrochloric acid, and an electric current is applied. A gas is released from each electrode.
The Voltaic cell, named after Alexander Volta, is an early example of an electric cell. It consists of a silver and zinc base soaked in brine. However, due to the weight of silver and zinc, smaller cells were later constructed using zinc and copper strips in dilute sulphuric acid. These smaller cells are known as simple cells, and a pile of them forms a battery.
Other examples of electric cells include the Daniel cell and the Leclanche cell. The Daniel cell consists of a copper vessel containing a copper sulfide solution and a porous pot with a zinc rod inside, serving as the positive electrode. The Leclanche cell comes in dry and wet types.
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Photoelectric or photovoltaic cells convert light energy into electrical energy
An electric cell is a device, such as a battery, that can convert some form of energy into electricity. Photoelectric or photovoltaic cells are electric cells that convert light energy into electrical energy.
Photovoltaic cells are composed of two oppositely charged semiconductors separated by a neutral junction. The negative layer (N-semiconductor) is generated by modifying a silicon crystal structure to achieve an excess of electrons, while the positive layer (P-semiconductor) lacks an electron to be stable, so it behaves as a positive charge within the crystal lattice. When the N-area is exposed to sunlight, it releases electrons by increasing the potential difference between the N and P areas. This difference in a closed circuit gives rise to an electric current, which is the electricity available to the user.
Photovoltaic cells convert light energy, usually from the sun, into electrical energy through a process called the photovoltaic effect. This process occurs in materials known as semiconductors, and solar cells are made from semiconducting materials such as silicon, the second most abundant material in the world after oxygen. When photons from the sun strike the surface of the silicon semiconductor material, they can be absorbed, reflected, or pass through the cell. Only the photons that are absorbed provide energy to generate electricity.
The first practical PV cell was developed in 1954 by Bell Telephone researchers. Since then, technological advances, lower costs, and government policies have encouraged the use of PV systems. PV cells are now used to power lighting systems and other electrical appliances in the home, for heating water, and for heating swimming pools, among other uses. PV cells are also used in off-grid locations that do not have electric power lines and in space satellites.
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Electrolytic cells are used for chemical reactions that require high energy
An electric cell is a device that can convert some form of energy, such as chemical or radiant energy, into electricity. An example of an electric cell is a battery.
An electrolytic cell is a type of electric cell used for chemical reactions that require high energy. These reactions are typically carried out in a container with electrodes and involve the conversion of chemical substances by oxidation and reduction. Electrolytic cells are similar to galvanic cells in that they both require a salt bridge, have a cathode and an anode side, and have a consistent flow of electrons from the anode to the cathode. However, electrolytic cells differ from galvanic cells in that they use electrical work as a source of energy to drive the reaction in the opposite direction.
The conditions under which an electrolytic cell operates are crucial. The substance with the highest standard cell potential value will undergo oxidation, while the strongest oxidizing agent will be reduced. For example, the electrolysis of a dissolved chloride sample can be used to determine the amount of chloride content in the sample. The amount of substance consumed or produced at one of the electrodes in an electrolytic cell is directly proportional to the amount of electricity that passes through the cell, as described by Faraday's law of electrolysis.
Inert electrodes are often used in electrolytic cells to collect the gases given off during the reaction. These electrodes are sealed in opposite ends of a container and connected to a battery or another source of electric current. An electrolyte is added to the water to provide ions that can complete the electric circuit.
Electrolytic cells are useful for chemical reactions that require high energy, such as the breakdown of water into hydrogen and oxygen. By carefully controlling the potential at which the cell operates, we can ensure that only the desired products are produced. For example, in the electrolysis of aqueous sodium chloride, we can produce hydrogen and chlorine gas, which are both commercially valuable.
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The Voltaic cell was named after Alexander Volta
An electric cell is a device that can convert energy from one form to another, such as chemical energy to electricity. An example of an electric cell is a battery.
The Voltaic cell, also known as the galvanic cell, was named after Italian chemist and physicist Alessandro Giuseppe Antonio Anastasio Volta. Volta was a pioneer in the field of electricity and power and is credited with inventing the electric battery and discovering methane.
In 1799, Volta invented the voltaic pile, which is a stack of galvanic cells, each consisting of a metal disk, an electrolyte layer, and a disk of a different metal. He built this entirely out of non-biological materials to challenge the prevalent theory at the time, proposed by Galvani, that electricity was generated solely by living beings. Volta's invention proved that electricity could be generated chemically.
Volta determined that the most effective pair of dissimilar metals to produce electricity was zinc and copper. The battery he created is considered one of the first electrochemical cells. It consists of two electrodes: one made of zinc and the other of copper. The electrolyte in the battery is either sulfuric acid mixed with water or a form of saltwater brine.
The voltaic cell was a significant development in the understanding of electricity and led to further experiments in the field, eventually resulting in the development of electrochemistry.
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Primary cells are non-rechargeable and have non-reversible chemical reactions
An electric cell, or electrolytic cell, is a device that can convert one form of energy into another. For example, a battery is an electric cell that can convert chemical energy into electricity.
Primary cells are a type of non-rechargeable battery that undergo irreversible chemical changes during use. This is in contrast to rechargeable batteries, which must be able to efficiently reverse the chemical changes that occur during an electrical discharge. In other words, primary cells can only be used once, whereas rechargeable batteries can be reused multiple times.
The ability to recharge a battery depends on the reversibility of the chemical reactions occurring within the cell. When a battery is discharged, an electrochemical oxidation reaction occurs at the negative electrode, and an electrochemical reduction reaction occurs at the positive electrode. To recharge the battery, the direction of the electric current flow is reversed, and the opposite reactions should take place. In rechargeable batteries, the electrochemical oxidation-reduction reactions are fully reversible. However, in non-rechargeable primary cells, at least one of these reactions is not reversible.
For example, in a nickel-cadmium (NiCad) battery, the chemical changes that occur during discharge can be easily reversed when the cell is recharged. The Cd(OH)2 and Ni(OH)2 formed during discharge are converted back into the original electrode materials of Cd and NiOOH. On the other hand, carbon-fluoride-lithium primary batteries undergo irreversible chemical changes. When attempting to recharge these batteries, the starting material at the cathode is not reformed, and instead, the cell electrolyte decomposes, leading to the formation of fluorine gas.
The distinction between rechargeable and non-rechargeable batteries is important, as it determines the usability and lifespan of the battery. While primary cells can provide energy for a single use, rechargeable batteries offer the advantage of multiple recharging cycles, making them more cost-effective and environmentally friendly.
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Frequently asked questions
An electric cell is a device that generates an electric force to move electrons through internal and external circuit components.
Electric cells are used to convert energy, such as chemical or radiant energy, into electricity. They are also used to facilitate chemical reactions that require high energy.
A simple example of an electric cell is the voltaic cell, which was named after Alexander Volta. It consists of strips of zinc and copper placed into dilute sulphuric acid.
Other examples of electric cells include the Daniel cell and the Leclanche cell. The Daniel cell consists of a copper vessel containing copper sulphide solution, while the Leclanche cell comes in dry and wet types.
