"A galvanic cell or voltaic cell [...] is an electrochemical cell in which an electric current is generated from spontaneous Oxidation-Reduction reactions."
An electrochemical cell that converts chemical energy into electrical energy.
Redox reactions: These are the fundamental reactions that occur in galvanic cells. An oxidation-reduction reaction or redox reaction is a type of chemical reaction that involves transfers of electrons between two species.
Half-cell reactions: Half-cell reactions describe the oxidation or reduction that takes place in an electrochemical cell. Each half-cell is a separate oxidation or reduction reaction.
Electrodes: Electrodes are materials used to conduct electricity in an electrochemical cell. They are also responsible for the reactions that occur at the surface of the cell.
Anodes and Cathodes: An electrode where oxidation occurs is called an anode, while an electrode where reduction occurs is called a cathode.
Standard Reduction Potentials: The standard reduction potential is a measure of the tendency of a species to be reduced, which can be used to predict the direction of electron flow in a galvanic cell.
Ionic solutions: The electrolyte is the solution that contains the ions that move between the two half-cells in a galvanic cell during the redox reaction.
Nernst equation: The Nernst equation is used to calculate the potential for an electrochemical cell reaction under non-standard conditions.
Galvanic Cells: Also known as voltaic cells, these are electrochemical cells that convert chemical energy into electrical energy. They operate using redox reactions and can be used for batteries, fuel cells, and other applications.
Cell potential: The cell potential is the voltage difference or electromotive force between the two electrodes in an electrochemical cell.
Faraday's law of electrolysis: This law describes the relationship between the amount of material produced or consumed, the charge that passes through the cell, and the number of electrons transferred.
Corrosion: Corrosion is an electrochemical process that leads to the deterioration of materials due to chemical reactions with the environment.
Batteries: Batteries are devices that generate electrical energy by converting chemical energy using one or more electrochemical cells.
Fuel cells: Fuel cells are similar to batteries but use a continuous flow of reactants to produce electricity.
Electroplating: Electroplating is the process of depositing thin layers of metal onto a surface using an electrochemical cell.
Applications of electrochemistry: Electrochemistry has many practical applications, including in energy storage, electronics, and medicine.
Voltaic or Galvanic Cells: These are electrochemical cells that convert chemical energy into electrical energy when spontaneous redox reactions occur.
Electrolytic Cells: These are electrochemical cells that convert electrical energy into chemical energy when non-spontaneous redox reactions occur.
Daniell Cell: A type of galvanic cell consisting of a Cu electrode immersed in a CuSO4 solution and a Zn electrode in a ZnSO4 solution. The two electrolytes are separated by a porous ceramic partition.
Dry Cell: A type of galvanic cell that uses a paste electrolyte instead of a liquid electrolyte, making it more portable.
Lead-Acid Cell: A type of storage battery where a lead anode and a lead oxide cathode are immersed in a sulfuric acid electrolyte to convert chemical energy into electrical energy.
Fuel Cells: Electrochemical cells that are based on the conversion of hydrogen and oxygen into electricity and water.
Lithium-Ion Cell: Rechargeable electrochemical cells that use lithium ions as the charge carrier.
Nickel-Cadmium Cell: Another type of rechargeable battery that uses nickel oxide hydroxide and metallic cadmium as electrodes to convert chemical energy into electrical energy.
Mercury Cell: Formerly used in battery manufacturing, these cells are now banned in most countries due to the toxic waste products produced by their disposal.
Alkaline Cell: Similar to dry cell batteries but use a concentrated alkaline electrolyte and a zinc anode surrounded by a graphite cathode. These are commonly used in household devices like flashlights and clocks.
"A galvanic cell or voltaic cell, named after the scientists Luigi Galvani and Alessandro Volta, respectively..."
"A common apparatus generally consists of two different metals, each immersed in separate beakers containing their respective metal ions in solution that are connected by a salt bridge or separated by a porous membrane."
"...each immersed in separate beakers containing their respective metal ions in solution that are connected by a salt bridge or separated by a porous membrane."
"...connected by a salt bridge or separated by a porous membrane."
"Volta was the inventor of the voltaic pile, the first electrical battery."
"...a battery properly consists of multiple cells."
"[...] an electric current is generated from spontaneous Oxidation-Reduction reactions."
"[...] connected by a salt bridge [...]"
"A galvanic cell or voltaic cell [...] generated from spontaneous Oxidation-Reduction reactions."
"A galvanic cell or voltaic cell, named after the scientists Luigi Galvani and Alessandro Volta, respectively..."
"A common apparatus generally consists of two different metals..."
"[...] named after the scientists Luigi Galvani and Alessandro Volta, respectively..."
"...each immersed in separate beakers..."
"...separated by a porous membrane."
"...an electric current is generated..."
"...containing their respective metal ions in solution..."
"...connected by a salt bridge or separated by a porous membrane."
"...metal ions in solution that are connected by a salt bridge..."
"...respective metal ions in solution that are connected by a salt bridge or separated by a porous membrane." Note: Due to the limitations of the model, the selected quotes are directly from the given paragraph but may not match the exact wording.