Otis Singleton
An electric cell is a single-unit device that converts chemical energy into electrical energy. It consists of two terminals, a positive and a negative side, referred to as electrodes, dipped in an electrolyte. The positive terminal is called the cathode, and the negative terminal is called the anode. The electrolyte is a liquid or gel that contains ions. When the cell is connected to an external circuit, chemical reactions occur within the electrolyte, generating positive ions and electrons. The electrons flow towards the positive electrode, and the positive ions move into the electrolyte, completing the circuit and powering the device. The specific voltage of an electric cell depends on its design and chemical composition.
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What You'll Learn
Electrochemical cells
An electric cell is a device that converts chemical energy into electrical energy. It was invented by Alessandro Volta in 1799. An electrochemical cell is a type of electric cell that generates electrical energy from chemical reactions. It can also be used to cause chemical reactions to occur by applying electricity.
An electrochemical cell consists of two half-cells, which are compartments that facilitate separate oxidation and reduction reactions. Each half-cell has a characteristic voltage, depending on the metal and its reduction potential. The half-cell performing oxidation will have a higher potential if the equilibrium lies closer to the ion/atom with a more positive oxidation state. Similarly, the reduction reaction will have a higher potential if the equilibrium lies closer to the ion/atom with a more negative oxidation state.
The two modes in which an electrochemical cell operates are the spontaneous redox reaction and the electrolytic mode. In the former, the cell can be used to provide energy to do work, such as powering flashlights and electrical devices. In the latter, an external energy source is required to drive the reaction.
A salt bridge can be used to connect the two half-cells with different electrolytes, preventing the solutions from mixing and avoiding unwanted side reactions. An alternative to a salt bridge is to allow direct contact between the two half-cells, as seen in the simple electrolysis of water.
A fuel cell is a type of electrochemical cell that reacts hydrogen fuel with oxygen or another oxidizing agent to convert chemical energy to electricity. Fuel cells differ from batteries as they require a continuous supply of fuel and oxygen to sustain the reaction.
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Oxidation-reduction reactions
An electric cell is a device that converts chemical energy to electrical energy. It consists of some chemicals called electrolytes and has two terminals referred to as electrodes. In a cell chemical reaction, an oxidation-reduction (redox) reaction happens between the electrodes. An oxidation-reduction reaction is a type of chemical reaction that involves the transfer of electrons between two species.
An oxidation-reduction reaction is any chemical reaction in which the oxidation number of a molecule, atom, or ion changes by gaining or losing an electron. The two parts of a redox reaction are a reduced half and an oxidized half, which always occur together. The reduced half gains electrons, and the oxidation number decreases, while the oxidized half loses electrons, and the oxidation number increases. The two species that exchange electrons in a redox reaction are given special names: the ion or molecule that accepts electrons is called the oxidizing agent, and the ion or molecule that donates electrons is called the reducing agent.
Redox reactions are common and vital to some of the basic functions of life, including photosynthesis, respiration, combustion, and corrosion or rusting. They are also accompanied by energy changes in the form of heat, light, and electricity. For example, when magnesium reacts with oxygen, magnesium gets oxidized by losing two electrons to oxygen, which gets reduced by accepting two electrons from magnesium.
The oxidation and reduction half-reactions can be balanced using the half-reaction method. First, write the oxidation number of each atom in the skeleton equation, and then find the species involved in the oxidation and reduction half-reactions. As the oxidation number increases by 1, add one electron on the product side to balance the change in oxidation number.
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Primary cells
An electric cell is a device that generates electrical energy from chemical reactions. It is a single-unit device that converts chemical energy into electrical energy. It was invented by Alessandro Volta in 1799.
A major factor reducing the lifetime of primary cells is that they become polarized during use. This means that hydrogen accumulates at the cathode, reducing the effectiveness of the cell. To counter this, chemical depolarization can be used, where an oxidizing agent is added to the cell to oxidize the hydrogen to water.
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Electrolytes
In the context of electricity, an electrolyte is a substance that conducts electricity through the movement of ions, but not through the movement of electrons. Electrolytes are essential components of electric cells, which are devices that convert chemical energy to electrical energy.
An electric cell consists of an electrolyte and two electrodes (two terminals, one positive and one negative, made of metal). The electrolyte can be a liquid or gel that contains ions, or a dry powder. When the cell is connected to an external circuit, chemical reactions occur within the electrolyte, generating positive ions and electrons near the negative electrode. The electrons flow towards the positive electrode from the external circuit, while the positive ions move into the electrolyte. The electrons then recombine with the positive ions at the positive electrode, completing the circuit and allowing electricity to flow.
The chemical reaction that occurs in the electric cell is called an oxidation-reduction reaction. In this process, there is an exchange of electrons between the electrodes and the electrolyte, resulting in a potential difference between them. This potential difference allows electricity to flow when the cell is connected to an external circuit.
In the human body, electrolytes are essential minerals that carry an electrical charge when dissolved in water. They are vital for the nervous system, muscle function, and maintaining fluid balance. Electrolytes such as sodium, potassium, calcium, and magnesium are obtained through diet and are necessary for optimal body function.
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Cell potential
An electric cell is a device that generates electrical energy from chemical reactions. It was invented by Alessandro Volta in 1799. Each cell has two ends called terminals, with one end being the positive terminal and the other being the negative terminal.
An electric cell is composed of two electrodes and an electrolyte. The electrodes are made of materials that can participate in chemical reactions with the electrolyte. In a cell chemical reaction, oxidation-reduction occurs between the electrodes and the electrolyte, causing an exchange of electrons that creates a potential difference between the electrodes. This potential difference allows electricity to flow when the cell is connected to an outer circuit.
The potential difference created by the exchange of electrons is known as the cell potential or voltage. The cell potential can be predicted through the use of electrode potentials, which are the voltages of each half-cell. Each half-cell has a characteristic voltage that depends on the metal and its reduction potential. The cell potential can be calculated by adding the potentials of the two half-cells.
The standard cell potential is the potential of the cell under standard state conditions, which are typically defined as a concentration of 1 mole per liter, a pressure of 1 atmosphere, and a temperature of 25°C. The standard cell potential can be determined by looking up the reduction potential for the reduction half-reaction and the oxidation potential for the oxidation half-reaction, and then adding these potentials together.
The cell potential can also be affected by the identity of the reacting substances, the concentrations of the reacting species, and the temperature of the system. By manipulating these variables, the direction and magnitude of an electrochemical reaction can be predicted.
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Frequently asked questions
A cell is a single unit device that converts chemical energy into electrical energy. It consists of some chemicals called electrolytes and has two terminals referred to as electrodes.
In a cell, a chemical reaction called oxidation-reduction happens between the electrodes and the electrolyte, freeing more electrons in one electrode than the other. This exchange of electrons creates a potential difference between the electrodes that allows electricity to flow when the cell is connected to an external circuit.
A battery is a group of cells that can be either a primary or secondary battery. A primary cell or battery cannot be recharged after use and is usually discarded. A secondary cell can be electrically recharged after use by passing a current through the circuit in the opposite direction to the current during discharge.
The capacity of a cell is measured in ampere-hours (Ah). The higher the discharge current, the lower the effective capacity of the battery.
