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A battery converts chemical energy into electrical energy through redox reactions in electrochemical cells.
An electric battery is a power source made of one or more electrochemical cells with external connections, used to supply electricity to devices. When operating, the battery’s positive terminal acts as the cathode and the negative terminal as the anode; the negative terminal is the source of electrons. Connecting the battery to an external load causes electrons to flow through the circuit, driving a redox reaction inside the cells as ions move, converting chemical energy into electrical energy delivered to the outside circuit. Batteries are built from voltaic (electrochemical) cells, each containing two half-cells and an electrolyte that allows ion movement between electrodes. The cathode and anode undergo reduction and oxidation respectively, producing an electromotive force (emf) measured in volts. The terminal voltage depends on whether the battery is charging or discharging and is affected by internal resistance: during discharge it is lower than the open-circuit voltage (emf), while during charging it can exceed it. Batteries can be single-use (primary) or rechargeable (secondary), with secondary batteries restoring their electrode chemistry when recharged by applying current.
A battery converts chemical energy into electrical energy through redox reactions in electrochemical cells.
Electrons flow from the battery’s negative terminal (anode) through the external circuit to the positive terminal (cathode).
Each cell’s emf is determined by the difference between the half-cell reduction potentials, and terminal voltage varies with internal resistance and operating state.
Primary batteries are not rechargeable because their reactions are generally irreversible, while secondary batteries can be recharged by reversing the reactions with applied current.
A source of electric power consisting of one or more electrochemical cells with external connections for powering electrical devices.
A device that produces electrical energy from chemical reactions, typically consisting of two half-cells connected by an electrolyte that allows ion transport.
The positive electrode where reduction occurs and where cations are attracted during battery operation.
The negative electrode where oxidation occurs and where electrons are released during battery operation.
The voltage a cell produces under open-circuit conditions, equal to the difference between the half-cell emfs (reduction potentials).
The voltage measured across a battery’s terminals during operation, which differs from emf due to internal resistance.
A battery designed for single use, where the chemical reactions are generally not reversible and the battery cannot be reliably recharged.
A rechargeable battery whose chemical reactions can be reversed by applying electric current to restore the original electrode materials.
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