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  1. AAAA battery
  2. AAA battery
  3. AA battery
  4. A battery
  5. Absorbent glass mat
  6. Alessandro Volta
  7. Alkaline battery
  8. Alkaline fuel cell
  9. Aluminium battery
  10. Ampere
  11. Atomic battery
  12. Backup battery
  13. Baghdad Battery
  14. Batteries
  15. Battery charger
  16. B battery
  17. Bernard S. Baker
  18. Beta-alumina solid electrolyte
  19. Betavoltaics
  20. Bio-nano generator
  21. Blue energy
  22. Bunsen cell
  23. Car battery
  24. C battery
  25. Clark cell
  26. Concentration cell
  27. Coulomb
  28. 2CR5
  29. Daniell cell
  30. Direct borohydride fuel cell
  31. Direct-ethanol fuel cell
  32. Direct methanol fuel cell
  33. Dry cell
  34. Dry pile
  35. Duracell
  36. Duracell Bunny
  37. Earth battery
  38. Electric charge
  39. Electric current
  40. Electricity
  41. Electrochemical cell
  42. Electrochemical potential
  43. Electro-galvanic fuel cell
  44. Electrolysis
  45. Electrolyte
  46. Electrolytic cell
  47. Electromagnetism
  48. Electromotive force
  49. Energizer Bunny
  50. Energy
  51. Energy density
  52. Energy storage
  53. Flashlight
  54. Float charging
  55. Flow Battery
  56. Formic acid fuel cell
  57. Fuel cell
  58. Fuel cell bus trial
  59. Galvanic cell
  60. Gel battery
  61. Grove cell
  62. Half cell
  63. History of the battery
  64. Hybrid vehicle
  65. Lead-acid battery
  66. Leclanché cell
  67. Lemon battery
  68. List of battery sizes
  69. List of battery types
  70. List of fuel cell vehicles
  71. Lithium battery
  72. Lithium ion batteries
  73. Lithium iron phosphate battery
  74. Lithium polymer cell
  75. LR44 battery
  76. Luigi Galvani
  77. Manganese dioxide
  78. Memory effect
  79. Mercury battery
  80. Metal hydride fuel cell
  81. Methane reformer
  82. Methanol reformer
  83. Michael Faraday
  84. Microbial fuel cell
  85. Molten carbonate fuel cell
  86. Molten salt battery
  87. Nickel-cadmium battery
  88. Nickel-iron battery
  89. Nickel metal hydride
  90. Nickel-zinc battery
  91. Open-circuit voltage
  92. Optoelectric nuclear battery
  93. Organic radical battery
  94. Oxyride battery
  95. Panasonic EV Energy Co
  96. Peukert's law
  97. Phosphoric acid fuel cell
  98. Photoelectrochemical cell
  99. Polymer-based battery
  100. Power density
  101. Power management
  102. Power outage
  103. PP3 battery
  104. Primary cell
  105. Prius
  106. Proton exchange membrane
  107. Proton exchange membrane fuel cell
  108. Protonic ceramic fuel cell
  109. Radioisotope piezoelectric generator
  110. Ragone chart
  111. RCR-V3
  112. Rechargeable alkaline battery
  113. Reverse charging
  114. Reversible fuel cell
  115. Searchlight
  116. Secondary cell
  117. Short circuit
  118. Silver-oxide battery
  119. Smart Battery Data
  120. Smart battery system
  121. Sodium-sulfur battery
  122. Solid oxide fuel cell
  123. Super iron battery
  124. Thermionic converter
  125. Trickle charging
  126. Vanadium redox battery
  127. Volt
  128. Voltage
  129. Voltaic pile
  130. Watch battery
  131. Water-activated battery
  132. Weston cell
  133. Wet cell
  134. Zinc-air battery
  135. Zinc-bromine flow battery
  136. Zinc-carbon battery

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Battery (electricity)

From Wikipedia, the free encyclopedia

(Redirected from Batteries)
Four double-A (AA) rechargeable batteries
Four double-A (AA) rechargeable batteries

In science and technology, a battery is a device that stores chemical energy and makes it available in an electrical form. Batteries consist of electrochemical devices such as two or more galvanic cells, electrolytic cells, fuel cells, or flow cells.[1] The modern development of batteries started with the Voltaic pile, announced by the Italian physicist Alessandro Volta in 1800.[2] The worldwide battery industry generates US$48 billion in sales annually (2005 estimate).

Formally, an electrical "battery" is an interconnected array of similar voltaic cells ("cells"). However, in many contexts it is common to call a single cell used on its own a battery.[3]


Main article: History of the battery
A Voltaic Pile, the first battery.
A Voltaic Pile, the first battery.

The earliest known artifacts that may have served as batteries are the Baghdad Batteries, which existed some time between 250 BC and 640 AD. However, it is not known what electrical function they may have served, and if they were in fact batteries at all. Scientists have developed several theories about its use, including medicine (as a painkiller) and electroplating jewelry.[4]

The story of the modern battery begins in 1786 with the discovery of "animal electricity" by Luigi Galvani. He created an electric circuit consisting of two different metals, with one touching the frog's leg and the other touching both the leg and the first metal, thus closing the circuit. In modern terms, the frog's leg served as both electrolyte and detector, and the metals served as electrodes. He noticed that even though the frog was dead, its legs would twitch when he touched them with the metals.[5]

By 1791, Alessandro Volta realized that the frog could be replaced by cardboard soaked in salt water, and another form of detection could be employed. Having already studied the electrostatic phenomenon of capacitance, Volta was able to quantitatively measure the "voltage", or electromotive force (emf) associated with each electrode-electrolyte interface, finding the emf to always be on the order of a volt. Such a device is called a voltaic cell, or cell for short. In 1799 Volta invented the modern battery. He did this by placing many galvanic cells in series, literally piling them one above the other. This Voltaic Pile gave a greatly enhanced net emf for the combination. (In many parts of Europe, batteries are called piles.) Later researchers placed galvanic cells in parallel. Such banks of cells are called batteries, presumably after the earlier use by Benjamin Franklin to describe Leyden jars (capacitors) in series and in parallel.

Although early batteries were of great value for experimental purposes, their limitations made them impractical for large current drain. Later batteries, starting with the Daniell cell in 1836, provided more reliable currents and were adopted by industry for use in stationary devices, particularly in telegraph networks where, in the days before electrical distribution networks, they were the only practical source of electricity. These wet cells used liquid electrolytes, which were prone to leaks and spillage if not handled correctly. Some, like the gravity cell, could only function in a certain orientation. Many used glass jars to hold their components, which made them fragile. These characteristics made wet cells unsuitable for portable appliances. Near the end of the 19th century, the invention of dry cell batteries, which replaced liquid electrolyte with a paste made portable electrical devices practical.

How batteries work

Main article: Electrochemical cell
Circuit symbol for a battery; simplified electrical model; and more complex but still incomplete model (the series capacitor has an extremely large value and, as it charges, simulates the discharge of the battery).
Circuit symbol for a battery; simplified electrical model; and more complex but still incomplete model (the series capacitor has an extremely large value and, as it charges, simulates the discharge of the battery).

A battery is a device in which chemical energy is directly converted to electrical energy. It consists of one or more voltaic cells, each of which is composed of two half cells connected in series by the conductive electrolyte. In the figure, the battery consists of one or more voltaic cells in series. (The conventional symbol does not necessarily represent the true number of voltaic cells.) Each cell has a positive terminal, shown by a long horizontal line, and a negative terminal, shown by the shorter horizontal line. These do not touch each other but are immersed in a solid or liquid electrolyte. In a practical cell the materials are enclosed in a container, and a separator between the electrodes prevents them from touching.

As discovered by Volta, each half cell can be assigned an emf, with the net emf E being the difference between the emfs E1 and E2 of the half-cells; two identical half-cells annul one another, giving zero net emf.[6] Unfortunately, Volta did not appreciate that the emf was due to chemical reactions. He thought that his cells were an inexhaustible source of energy, and that the associated chemical effects (e.g., corrosion) were a mere nuisance -- rather than, as Michael Faraday showed around 1830, an unavoidable by-product of their operation.

The electrolyte conducts current by allowing the passage of ions between the two electrodes. Such reactions are called faradaic, and are responsible for current flow through the cell. Non-charge-transferring (non-faradaic) reactions also occur at the electrode-electrolyte interfaces. Non-faradaic reactions are one reason that voltaic cells (particularly the lead-acid cell of ordinary batteries) "run down" when sitting unused.

The electrical potential across the terminals of a battery is known as its terminal voltage, measured in volts. The terminal voltage of a battery that is neither charging nor discharging (the open-circuit voltage) equals its emf. The terminal voltage of a battery that is discharging is less than the emf, and that of a battery that is charging is greater than the emf.

The voltage produced by a cell depends on the chemicals used in it, which have different electrochemical potentials. For example, alkaline and carbon-zinc cells both have emfs of about 1.5 volts, due to the energy release of the associated chemical reactions. Because of the high electrochemical potentials of lithium compounds, Li cells can provide as much as 3 or more volts.

Classification of batteries

Batteries are usually divided into two broad classes:

  • Primary batteries irreversibly transform chemical energy to electrical energy. Once the initial supply of reactants is exhausted, energy cannot be readily restored to the battery by electrical means.
  • Secondary batteries can have the chemical reactions reversed by supplying electrical energy to the cell, restoring their original composition. [7]

Historically, some types of primary batteries used, for example, for telegraph circuits, were restored to operation by replacing the components of the battery consumed by the chemical reaction. Secondary batteries are not indefinitely rechargeable due to dissipation of the active materials, loss of electrolyte, and internal corrosion.

Main battery features

  • Life span
  • Charge rate.
  • Temperature range.
  • Charge and discharge temperature range.
  • Charge and discharge C rate.
  • Cycle life (charge and discharge cycles).
  • Annual maintenance
  • Calendar life
  • Safety
  • Environmental.

Battery capacity and discharging

The more electrolyte and electrode material in the cell, the greater the capacity of the cell. Thus a tiny cell has much less capacity than a much larger cell, even if both rely on the same chemical reactions (e.g.alkaline cells), which produce the same terminal voltage.

Because of the chemical reactions within the cells, the capacity of a battery depends on the discharge conditions such as the magnitude of the current, the duration of the current, the allowable terminal voltage of the battery, temperature, and other factors.

The available capacity of a battery depends upon the rate at which it is discharged. If a battery is discharged at a relatively high rate, the available capacity will be lower than expected. Therefore, a battery rated at 100 A·h will deliver 20 A over a 5 hour period, but if it is instead discharged at 50 A, it will run out of charge before the theoretically expected 2 hours. For this reason, a battery capacity rating is always related to an expected discharge duration, such as 15 minutes, 8 hours, 20 hours or others.

The relationship between current, discharge time, and capacity for a lead acid battery is expressed by Peukert's law. The efficiency of a battery is different at different discharge rates. When discharging at low rate, the battery's energy is delivered more efficiently than at higher discharge rates.

Battery manufacturers use a standard method to rate their batteries. The battery is discharged at a constant rate of current over a fixed period of time, such as 10 hours or 20 hours, down to a set terminal voltage per cell. So a 100 ampere-hour battery is rated to provide 5 A for 20 hours at room temperature.

In general, the higher the ampere-hour rating, the longer the battery will last for a certain load. Installing batteries with different A·h ratings will not affect the operation of a device rated for a specific voltage.

Conversion to energy

The A·h rating of a battery is related to the amount of energy it stores when fully charged. If two batteries have the same nominal voltage, then the one with the higher A·h rating stores more energy. It would also typically take longer to recharge.

The energy E available from a battery is approximately given by:

E= QV\,


  • Q is the charge, and
  • V is the nominal voltage.

This yields:

number of joules = number of ampere-hours × number of volts × 3600 seconds per hour, or
number of watt-hours = number of ampere-hours × number of volts.

In the previous example of a 2.3 A.h, 3 V battery, the energy is E = 2.3*3600*3 = 24,840 J.

This is only an approximation, because the voltage during discharge is not constant.

Secondary batteries always yield less energy than was used to charge them, since (among other reasons) the terminal voltage during charging is higher than during discharging.

Battery lifetime

Even if never taken out of the original package, disposable (or "primary") batteries can lose two to twenty-five percent of their original charge every year. This is known as the "self discharge" rate and is due to non-current-producing "side" chemical reactions, which occur within the cell even if no load is applied to it. The rate of the side reactions is reduced if the batteries are stored at low temperature, although some batteries can be damaged by freezing. High or low temperatures will reduce battery performance.

Rechargeable batteries self-discharge more rapidly than disposable alkaline batteries; up to three percent a day (depending on temperature). Due to their poor shelf life, they should not be stored and then relied upon to power flashlights or radios in an emergency. For this reason, it is a good idea to keep alkaline batteries on hand. Ni-Cd Batteries are almost always "dead" when purchased, and must be charged before first use.

Most NiMH and NiCd batteries can be charged several hundred times. Also, they both can be completely discharged and then recharged without their capacity being damaged or shortened.

Automotive lead-acid rechargeable batteries have a much harder life. Because of vibration, shock, heat, cold, and sulfation of their lead plates, few automotive batteries last beyond six years of regular use. Automotive starting batteries have many thin plates to provide as many amps as possible in a reasonably small package, and are only drained a small amount before being immediately recharged. Care should be taken to avoid deep discharging a starter battery, since each charge and discharge cycle causes active material to be shed from the plates. When holes form in the plates it results in less surface area for the chemical reaction, which results in less measured voltage. Leaving a lead-acid battery in a deeply discharged state for any length of time allows the sulfate to become more deeply adhered to the plate, making sulfate removal during the charging process difficult. This can result in less available plate surface and the resulting lower voltage, shortening the battery's life. "Deep-Cycle" lead-acid batteries such as those used in electric golf carts have much thicker plates to aid their longevity. The main benefit of lead-acid is its low cost, the main drawbacks are their large size and weight per a given capacity and voltage. Lead-acid batteries should never be discharged to below 20% of their full capacity as internal resistance will cause heat and damage when attempting to recharge them. Deep-cycle lead-acid systems often use a low-charge warning light or a low-charge power cut-off switch to prevent the type of damage that will shorten the battery's life.

Special "reserve" batteries intended for long storage in emergency equipment or munitions keep the electrolyte of the battery separate from the plates until the battery is activated, allowing the cells to be filled with the electrolyte. Shelf times for such batteries can be years or decades. However, their construction is more expensive than more common forms.

Battery life can be extended by storing the batteries at a low temperature, as in a refrigerator or freezer, because the chemical reactions in the batteries are slower. Such storage can extend the life of alkaline batteries by an insignificant 5%; however, the life of rechargeable batteries can be extended dramatically from a few days to several months.[8] In order to reach their full power, batteries must be returned to room temperature; therefore, alkaline battery manufacturers like Duracell do not recommend refrigerating or freezing batteries. [9]

Battery explosion

A battery explosion is caused by the misuse or malfunction of a battery, such as attempting to recharge a primary battery, or short circuiting a battery. With car batteries, explosions are most likely to occur when a short circuit generates very large currents. In addition, car batteries liberate hydrogen when they are overcharged (because of electrolysis of the water in the electrolyte). Normally the amount of overcharging is very small, as is the amount of explosive gas developed, and the gas dissipates quickly. However, when "jumping" a car battery, the high current can cause the rapid release of large volumes of hydrogen, which can be ignited by a nearby spark (for example, when removing the jumper cables).

When a battery is recharged at an excessive rate, an explosive gas mixture of hydrogen and oxygen may be produced faster than it can escape from within the walls of the battery, leading to pressure build-up and the possibility of the battery case bursting. In extreme cases, the battery acid may spray violently from the casing of the battery and cause injury.

Additionally, disposing of a battery in fire may cause an explosion as steam builds up within the sealed case of the battery.

Overcharging -- that is, attempting to charge a battery beyond its electrical capacity -- can also lead to a battery explosion, leakage, or irreversible damage to the battery. It may also cause damage to the charger or device in which the overcharged battery is later used.

Disposable and rechargeable batteries

Various batteries(clockwise from bottom left): two 9-volt, two "AA", one "D", a cordless phone battery, a camcorder battery, a 2-meter handheld ham radio battery, and a button battery, one "C" and two "AAA", plus a U.S. quarter, for scale
Various batteries(clockwise from bottom left): two 9-volt, two "AA", one "D", a cordless phone battery, a camcorder battery, a 2-meter handheld ham radio battery, and a button battery, one "C" and two "AAA", plus a U.S. quarter, for scale
From top to bottom:Two button cells, a 9 volt PP3 battery, a AAA battery, a AA battery, a C battery, a D battery, a large 3R12
From top to bottom:Two button cells, a 9 volt PP3 battery, a AAA battery, a AA battery, a C battery, a D battery, a large 3R12

From a user's viewpoint, at least, batteries can be generally divided into two main types: non-rechargeable (disposable) and rechargeable. Each is in wide usage.

Disposable batteries, also called primary cells, are intended to be used once and discarded. These are most commonly used in portable devices with either low current drain, only used intermittently, or used well away from an alternative power source. Primary cells were also commonly used for alarm and communication circuits where other electric power was only intermittently available. Primary cells cannot be reliably recharged, since the chemical reactions are not easily reversible and active materials may not return to their original forms. Battery manufacturers recommend against attempting to recharge primary cells, although some electronics enthusiasts claim it is possible to do so using a special type of charger. [10]

By contrast, rechargeable batteries or secondary cells can be re-charged by applying electrical current, which reverses the chemical reactions that occur in use. Devices to supply the appropriate current are called chargers or rechargers.

The oldest form of rechargeable battery still in modern usage is the "wet cell" lead-acid battery. This battery is notable in that it contains a liquid in an unsealed container, requiring that the battery be kept upright and the area be well-ventilated to ensure safe dispersal of the hydrogen gas which is vented by these batteries during overcharging. The lead-acid battery is also very heavy for the amount of electrical energy it can supply. Despite this, its low manufacturing cost and its high surge current levels make its use common where a large capacity (over approximately 10Ah) is required or where the weight and ease of handling are not concerns.

A common form of lead-acid battery is the modern wet-cell car battery. This can deliver about 10,000 watts of power for a short period, and has a peak current output that varies from 450 to 1100 amperes. An improved type of lead-acid battery called a gel battery (or "gel cell") has become popular in automotive industry as a replacement for the lead-acid wet cell. The gel battery contains a semi-solid electrolyte to prevent spillage, electrolyte evaporation, and out-gassing, as well as greatly improving its resistance to damage from vibration and heat. Another type of battery, the Absorbed Glass Mat (AGM) suspends the electrolyte in a special fibreglass matting to achieve similar results. More portable rechargeable batteries include several "dry cell" types, which are sealed units and are therefore useful in appliances like mobile phones and laptops. Cells of this type (in order of increasing power density and cost) include nickel-cadmium (NiCd), nickel metal hydride (NiMH), and lithium-ion (Li-Ion) cells.


Not designed to be rechargeable - sometimes called "primary cells".

  • Zinc-carbon battery - mid cost - used in light drain applications
  • Zinc-chloride battery - similar to zinc carbon but slightly longer life
  • Alkaline battery - alkaline/manganese "long life" batteries widely used in both light drain and heavy drain applications
  • Silver-oxide battery - commonly used in hearing aids
  • Lithium battery - commonly used in digital cameras. Sometimes used in watches and computer clocks. Very long life (up to ten years in wristwatches) and capable of delivering high currents but expensive
  • Mercury battery - formerly used in digital watches, radio communications, and portable electronic instruments, no longer manufactured due to toxicity
  • Zinc-air battery - commonly used in hearing aids
  • Thermal battery - high temperature reserve. Almost exclusively military applications.
  • Water-activated battery - used for radiosondes and emergency applications


main article: Rechargeable battery.
A rechargeable lithium polymer Nokia mobile phone battery.
A rechargeable lithium polymer Nokia mobile phone battery.

Also known as secondary batteries or accumulators.

  • Lead-acid battery - used in vehicles, alarm systems and uninterruptible power supplies. The major advantage of this chemistry is its low cost - a large lead-acid battery (e.g. 70Ah) is relatively inexpensive compared to batteries based on other chemistries. However, this historically important battery type has a lower energy/mass than other battery types now available (see below).
    • Absorbed glass mat
    • Gel battery
  • Lithium ion battery - used in laptops (notebook PCs), modern camera phones, some rechargeable MP3 players and most other portable rechargeable digital equipment. This relatively modern battery type has a very high energy/mass (i.e. a light battery will store a lot of energy) and shows no "memory effect".
  • Lithium ion polymer battery - similar characteristics to lithium-ion, but with slightly less energy/mass. This battery type can be shaped according to need, as in ultra-thin (1 mm thick) cells for PDAs.
  • NaS battery
  • Nickel-iron battery
  • Nickel metal hydride battery
  • Nickel-cadmium battery - used in many domestic applications but being superseded by Li-Ion and Ni-MH types. This chemistry gives the longest cycle life (over 1500 cycles), but has low energy/mass compared to Li-Ion and Ni-MH. Ni-Cd cells using older technology suffer from memory effect; this has been reduced drastically in modern batteries.
  • Nickel-zinc battery
  • Molten salt battery

See also

  • List of battery sizes

Homemade cells

Almost any liquid or moist object that has enough ions to be electrically conductive can serve as the electrolyte for a cell. As a novelty or science demonstration, it is possible to insert two electrodes made of different metals into a lemon, potato, glass of soft drink, etc. and generate small amounts of electricity. As of 2005, "two-potato clocks" are widely available in hobby and toy stores; they consist of a pair of cells, each consisting of a potato (lemon, etc.) with two electrodes inserted into it, wired in series to form a battery with enough voltage to power a digital clock. Homemade cells of this kind are of no real practical use, because they produce far less current—and cost far more per unit of energy generated—than commercial cells, due to the need for frequent replacement of the fruit or vegetable. In addition, in the two-book series "Sneaky Uses for Everyday Things", there are instructions to make a battery from a nickel, a penny, and a piece of paper towel dipped in salt water. Each of these can make up to 0.3 volts and when many of them are used, they can replace normal batteries for a short amount of time.

Lead acid cells can easily be manufactured at home, but a tedious charge/discharge cycle is needed to 'form' the plates. This is a process whereby lead sulfate forms on the plates, and during charge is converted to lead dioxide (positive plate) and pure lead (negative plate). Repeating this process results in a microscopically rough surface, with far greater surface area being exposed. This increases the current the cell can deliver. For an example, see [2].

Traction batteries

Traction batteries are high power batteries designed to provide propulsion to move a vehicle, such as an electric car or tow motor. A major design consideration is power to weight ratio since the vehicle must carry the battery. While conventional lead acid batteries with liquid electrolyte have been used, gelled electrolyte and (AGM-type) can also be used, especially in smaller sizes. The largest installations of batteries for propulsion of vehicles are found in submarines, although the toxic gas produced by seawater contact with acide electrolyte is a considerable hazard.

Battery types commercially used in electric vehicles include:

  • lead-acid battery
    • flooded type with liquid electrolyte.
    • AGM-type (Absorbed Glass Mat)
  • Zebra Na/NiCl2 battery operating at 270 °C requiring cooling in case of temperature excursions
  • NiZn battery (higher cell voltage 1.6 V and thus 25% increased specific energy, very short lifespan)

Lithium-ion batteries are now pushing out NiMh-technology [3].

See also: Battery pack, battery electric vehicles and hydrogen vehicle.

Flow batteries

Flow batteries are a special class of battery where additional quantities of electrolyte are stored outside the main power cell of the battery, and circulated through it by pumps or by movement. Flow batteries can have extremely large capacities and are used in marine applications and are gaining popularity in grid energy storage applications.

Zinc-bromine and vanadium redox batteries are typical examples of commercially-available flow batteries.

Environmental considerations

Since their development over 250 years ago, batteries have remained among the most expensive energy sources, and their manufacture consumes many valuable resources and often involves hazardous chemicals. For this reason many areas now have battery recycling services available to recover some of the more toxic (and sometimes valuable) materials from used batteries. Batteries may be harmful or fatal if swallowed.

This changes with the nanotechnology batteries.

Cells in series or in parallel

The cells in a battery can be connected in parallel, series, or in both. A parallel combination of cells has the same voltage as a single cell, but can supply a higher current (the sum of the currents from all the cells). A series combination has the same current rating as a single cell but its voltage is the sum of the voltages of all the cells. Most practical electrochemical batteries, such as 9 volt flashlight (torch) batteries and 12 V automobile (car) batteries, have several cells connected in series inside the casing. Parallel arrangements suffer from the problem that, if one cell discharges faster than its neighbour, current will flow from the full cell to the empty cell, wasting power and possibly causing overheating. Even worse, if one cell becomes short-circuited due to an internal fault, its neighbour will be forced to discharge its maximum current into the faulty cell, leading to overheating and possibly explosion. Cells in parallel are therefore usually fitted with an electronic circuit to protect them against these problems. In both series and parallel types, the energy stored in the battery is equal to the sum of the energies stored in all the cells.

Effect of a battery's internal resistance

A battery can be simply modelled as a perfect voltage source (i.e. one with zero internal resistance) in series with a resistor. The voltage source depends mainly on the chemistry of the battery, not on whether it is empty or full. When a battery runs down, its internal resistance increases. When the battery is connected to a load (e.g. a light bulb), which has its own resistance, the resulting voltage across the load depends on the ratio of the battery's internal resistance to the resistance of the load. When the battery is fresh, its internal resistance is low, so the voltage across the load is almost equal to that of the battery's internal voltage source. As the battery runs down and its internal resistance increases, the voltage drop across its internal resistance increases, so the voltage at its terminals decreases, and the battery's ability to deliver power to the load decreases.

The formula for calculating the voltage Vt at the terminals of a battery is:

V_t = V_{oc}-R_i \cdot I


Voc is the open-circuit voltage of the battery
Ri is the battery's internal resistance
I is the current flowing through the battery

This can be rearranged to calculate the internal resistance given the other quantities:

R_i=\frac {V_{oc}-V_t} {I}


Some common Battery-related terms:

  • W Watt, unit of power. One Watt equals approximately 0.00134 horsepower.
  • W/kg, Watts per kilogram, unit of energy per mass.
  • W/l, Watts per liter, unit power per volume.
  • W•h Watt-hour, unit of energy, or work. 1 Watt expended continuously for 1 hour equals 1 Watt-hour.
  • W•h/kg, Watt-hours per kilogram, unit of energy per mass.
  • W•h/l, Watt-hours per litre, unit of energy density.
  • W•h/lb, Watt-hours per pound, unit of energy per mass.

See also

  • Electrochemical cell
  • Galvanic cell
  • Duracell
  • List of battery types
  • Nanotitanate
  • Recharging batteries
  • Replacing batteries
  • Solid Electrolyte Interface (high resistance crust).
  • Thermal runaway



  1. ^ Spotlight on Photovoltaics & Fuel Cells. Accessed 14 March 2007.
  2. ^ Banks, Sir Joseph (1800), "On the Electricity excited by the mere Contact of conducting Substances of different Kinds. In a Letter from Mr. Alexandro Volta, F.R.S., Professor of Natural Philosophy at the University of Pavia, to the Rt. Hon. Sir. Joseph Banks, Bart. K.B. P.R.S. Read June 26, 1800." Philosophical Transactions of the Royal Society of London, 1800, p. 403[1]. The paper was submitted in April 1800 and read before the Royal Society on June 26, 1800: Matthews, Michael R.; Fabio Bevilacqua, Enrico Giannetto (2001). "Science Education and Culture: The Contribution of History and Philosophy of Science". Springer. ISBN 0-7923-6972-6. , p. 261. Some sources identify the year of invention as 1799; e.g. "The voltaic pile... was constructed by Volta in 1799, and became known in England in 1800," Beard, George Miller (1883). A Practical Treatise on the Medical and Surgical Uses of Electricity Including Localized and General Faradization, Localized and Central Galvanization, Franklinization, Electrolysis and Galvano-cautery. Wood. , p. 30 The publication in 1800 "caused a sensation" according to Hankins, Thomas Leroy (1985). Science and the Enlightenment. Cambridge University Press. ISBN. p. 72
  3. ^ "Battery" (def. 6), The Random House Dictionary of the English Language, the Unabridged Edition (2nd edition), 1996 ed.
  4. ^ World Mysteries - Strange Artifacts, Baghdad Battery. Retrieved 16 March 2007.
  5. ^ Luigi Galvani - Corrosion Doctors. Accessed 16 March 2007.
  6. ^
  7. ^ *Donald G. Fink and H. Wayne Beaty, Standard Handbook for Electrical Engineers, Eleventh Edition,McGraw-Hill, New York, 1978, ISBN 0-07020974-X, chapter 11, section "Batteries and Fuel Cells"
  8. ^ Ask Yahoo: Does putting batteries in the freezer make them last longer?. Retrieved 7 March 2007.
  9. ^ Duracell: Battery Care. Retrieved 7 March 2007.
  10. ^ Battery Xtender. Retrieved 7 March 2007.


  1. David Linden and Thomas B. Reddy ed., Handbook Of Batteries. McGraw-Hill (2001). ISBN 0-0713-5978-8. This is rather technical.
  1. Electricity, Magnetism, and Light, by Wayne M. Saslow, Academic (2002). ISBN 0-12-619455-6. pp.302-304 contrasts fast and slow discharge (and charge). pp.304-315 discusses capacity, resistance, battery life, and energy storage.
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