lead storage battery

• 鉛蓄電池

関

lead accumulator

WordNet

1. tend to or result in; "This remark lead to further arguments among the guests"
2. a soft heavy toxic malleable metallic element; bluish white when freshly cut but tarnishes readily to dull grey; "the children were playing with lead soldiers" (同)Pb, atomic number 82
3. (sports) the score by which a team or individual is winning
4. the angle between the direction a gun is aimed and the position of a moving target (correcting for the flight time of the missile)
5. thin strip of metal used to separate lines of type in printing (同)leading
6. mixture of graphite with clay in different degrees of hardness; the marking substance in a pencil (同)pencil lead
7. a position of leadership (especially in the phrase `take the lead'
8. an advantage held by a competitor in a race; "he took the lead at the last turn"
9. the playing of a card to start a trick in bridge; "the lead was in the dummy"
10. a news story of major importance (同)lead story
11. the introductory section of a story; "it was an amusing lead-in to a very serious matter" (同)lead-in, lede
12. evidence pointing to a possible solution; "the police are following a promising lead"; "the trail led straight to the perpetrator" (同)track, trail
13. (baseball) the position taken by a base runner preparing to advance to the next base; "he took a long lead off first"
14. travel in front of; go in advance of others; "The procession was headed by John" (同)head
15. take somebody somewhere; "We lead him to our chief"; "can you take me to the main entrance?"; "He conducted us to the palace" (同)take, direct, conduct, guide
16. be ahead of others; be the first; "she topped her class every year" (同)top
17. cause to undertake a certain action; "Her greed led her to forge the checks"
18. an assault in which the assailant makes physical contact (同)assault_and_battery
19. a device that produces electricity; may have several primary or secondary cells arranged in parallel or series (同)electric battery
20. a series of stamps operated in one mortar for crushing ores (同)stamp battery
21. a collection of related things intended for use together; "took a battery of achievement tests"
22. a unit composed of the pitcher and catcher
23. group of guns or missile launchers operated together at one place
24. going or proceeding or going in advance; showing the way; "we rode in the leading car"; "the leading edge of technology"
25. greatest in importance or degree or significance or achievement; "our greatest statesmen"; "the countrys leading poet"; "a preeminent archeologist" (同)preeminent
26. indicating the most important performer or role; "the leading man"; "prima ballerina"; "prima donna"; "a star figure skater"; "the starring role"; "a stellar role"; "a stellar performance" (同)prima, star, starring, stellar
27. (baseball) a ballplayer who is batting (同)hitter, slugger, batsman
28. a liquid or semiliquid mixture, as of flour, eggs, and milk, used in cooking
29. (computer science) the process of storing information in a computer memory or on a magnetic tape or disk
30. the act of storing something
31. the commercial enterprise of storing goods and materials

PrepTutorEJDIC

1. 《方向を表す副詞[句]を伴って》…‘を'『導く』,案内する / 〈道・灯火などが〉…‘に'道筋を示す;(…へ)…‘を'導く《+『名』+『to』(『into』)+『名』》 / …‘の'先頭になる,1番である / …‘の'『率いる』,指揮する / 〈ある人生・生活〉‘を'経験する,生きる,送る / 『先頭に立つ』,(競技・成績などで)リードスル / 〈人が〉『案内する』,先導する / (…に)〈道などが〉『通じている』《+『to』+『名』》 / (…の)結果となる《+『to』+『名』(do『ing』)》 / 〈U〉《the~》『先頭』,首位 / 〈C〉《a~》相手を引き離した点(時間,距離) / 〈C〉模範,手本(example) / 〈C〉(問題解決の)手がかり,ヒント(clue) / 〈C〉(劇・映画などの)主役,主演俳優 / 〈C〉(新聞報道記事などの本文の前におく要約した)前文,前書き,リード / 先頭の,主要な
2. 〈U〉『鉛』(化学記号はは『pb』) / 〈C〉鉛のおもり,測鉛 / 〈C〉《複数形で》(ガラスをはめる)鉛の枠(わく);《英》(屋根をふくのに用いる)鉛板 / 〈U〉〈C〉黒鉛,鉛筆のしん / 〈U〉《集合的に》(鉛の)弾丸 / …‘に'鉛をかぶせる,鉛を詰める,鉛のおもりを付ける
3. 〈C〉砲兵中隊;砲列,砲台;(軍艦の)備砲 / 〈C〉『電池』,バッてり‐ / 〈C〉一組みの器具;(関連するものの)一群,一連《+『of』+『名』》 / 〈C〉(野球で)バッテリー(投手と捕手) / 〈U〉(法律用語で)殴打,暴行
4. 『先導する』,先頭の / 『主要な』,一流の / 指導する / 指導
5. (野球・クリケットの)『バッター』,『打者』
6. …'を'乱打する,打ち壊す,たたきつぶす / (ひどい扱いで)…'を'壊す,だめにする / 乱打する,打つける
7. 練り粉(牛乳・鶏卵・バター・メリケン粉などをこね混ぜたもの)
8. (倉庫などに)貯蔵すること,保管 / 貯蔵所,倉庫 / 保管料

Wikipedia preview

出典(authority):フリー百科事典『ウィキペディア（Wikipedia）』「2018/03/09 10:57:02」(JST)

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Lead–acid battery

Lead–acid car battery
Specific energy	33–42 Wh/kg
Energy density	60–110 Wh/L
Specific power	180 W/kg
Charge/discharge efficiency	50–95%
Energy/consumer-price	7 (sld) to 18 (fld) Wh/US$
Self-discharge rate	3–20%/month
Cycle durability	<350 cycles
Nominal cell voltage	2.1 V
Charge temperature interval	Min. −35 °C, max. 45 °C

The lead–acid battery was invented in 1859 by French physicist Gaston Planté and is the oldest type of rechargeable battery. Despite having a very low energy-to-weight ratio and a low energy-to-volume ratio, its ability to supply high surge currents means that the cells have a relatively large power-to-weight ratio. These features, along with their low cost, make them attractive for use in motor vehicles to provide the high current required by automobile starter motors.

As they are inexpensive compared to newer technologies, lead–acid batteries are widely used even when surge current is not important and other designs could provide higher energy densities. Large-format lead–acid designs are widely used for storage in backup power supplies in cell phone towers, high-availability settings like hospitals, and stand-alone power systems. For these roles, modified versions of the standard cell may be used to improve storage times and reduce maintenance requirements. Gel-cells and absorbed glass-mat batteries are common in these roles, collectively known as VRLA (valve-regulated lead–acid) batteries.

In 1999 lead–acid battery sales accounted for 40–45% of the value from batteries sold worldwide excluding China and Russia, and a manufacturing market value of about $15 billion.

History

Main article: History of the battery

The French scientist Nicolas Gautherot observed in 1801 that wires that had been used for electrolysis experiments would themselves provide a small amount of "secondary" current after the main battery had been disconnected. In 1859, Gaston Planté's lead–acid battery was the first battery that could be recharged by passing a reverse current through it. Planté's first model consisted of two lead sheets separated by rubber strips and rolled into a spiral. His batteries were first used to power the lights in train carriages while stopped at a station. In 1881, Camille Alphonse Faure invented an improved version that consisted of a lead grid lattice, into which a lead oxide paste was pressed, forming a plate. This design was easier to mass-produce. An early manufacturer (from 1886) of lead–acid batteries was Henri Tudor.

Using a gel electrolyte instead of a liquid allows the battery to be used in different positions without leakage. Gel electrolyte batteries for any position date from the 1930s, and even in the late 1920s portable suitcase radio sets allowed the cell vertical or horizontal (but not inverted) due to valve design (see third Edition of Wireless Constructor's Encyclopaedia by Frederick James Camm). In the 1970s, the valve-regulated lead–acid battery (often called "sealed") was developed, including modern absorbed glass mat types, allowing operation in any position.

Electrochemistry

Discharge

Fully discharged: two identical lead sulfate plates

In the discharged state both the positive and negative plates become lead(II) sulfate (PbSO
₄), and the electrolyte loses much of its dissolved sulfuric acid and becomes primarily water. The discharge process is driven by the conduction of electrons from the negative plate back into the cell at the positive plate in the external circuit.

Negative plate reaction

Pb(s) + HSO⁻
₄(aq) → PbSO
₄(s) + H⁺
(aq) + 2e⁻ Release of two conducting electrons gives lead electrode a net negative charge

As electrons accumulate they create an electric field which attracts hydrogen ions and repels sulfate ions, leading to a double-layer near the surface. The hydrogen ions screen the charged electrode from the solution which limits further reactions unless charge is allowed to flow out of electrode.

Positive plate reaction

PbO
₂(s) + HSO⁻
₄(aq) + 3H⁺
(aq) + 2e⁻ → PbSO
₄(s) + 2H
₂O(l)

The total reaction can be written as

Pb(s) + PbO
₂(s) + 2H
₂SO
₄(aq) → 2PbSO
₄(s) + 2H
₂O(l)

The sum of the molecular masses of the reactants is 642.6 g/mol, so theoretically a cell can produce two faradays of charge (192,971 coulombs) from 642.6 g of reactants, or 83.4 ampere-hours per kilogram (or 13.9 ampere-hours per kilogram for a 12-volt battery). For a 2 volts cell, this comes to 167 watt-hours per kilogram of reactants, but a lead–acid cell in practice gives only 30–40 watt-hours per kilogram of battery, due to the mass of the water and other constituent parts.

Charging

Fully recharged: Lead anode, Lead oxide cathode and sulfuric acid electrolyte

In the fully charged state, the negative plate consists of lead, and the positive plate lead dioxide, with the electrolyte of concentrated sulfuric acid.

Overcharging with high charging voltages generates oxygen and hydrogen gas by electrolysis of water, which is lost to the cell. The design of some types of lead-acid battery allow the electrolyte level to be inspected and topped up with any water that has been lost.

Due to the freezing-point depression of the electrolyte, as the battery discharges and the concentration of sulfuric acid decreases, the electrolyte is more likely to freeze during winter weather when discharged.

Ion motion

During discharge, H⁺
produced at the negative plates moves into the electrolyte solution and then is consumed into the positive plates, while HSO⁻
₄ is consumed at both plates. The reverse occurs during charge. This motion can be by electrically driven proton flow or Grotthuss mechanism, or by diffusion through the medium, or by flow of a liquid electrolyte medium. Since the density is greater when the sulfuric acid concentration is higher, the liquid will tend to circulate by convection. Therefore, a liquid-medium cell tends to rapidly discharge and rapidly charge more efficiently than an otherwise similar gel cell.

Measuring the charge level

A hydrometer can be used to test the specific gravity of each cell as a measure of its state of charge.

Because the electrolyte takes part in the charge-discharge reaction, this battery has one major advantage over other chemistries. It is relatively simple to determine the state of charge by merely measuring the specific gravity of the electrolyte; the specific gravity falls as the battery discharges. Some battery designs include a simple hydrometer using colored floating balls of differing density. When used in diesel-electric submarines, the specific gravity was regularly measured and written on a blackboard in the control room to indicate how much longer the boat could remain submerged.

The battery's open-circuit voltage can also be used to gauge the state of charge. If the connections to the individual cells are accessible, then the state of charge of each cell can be determined which can provide a guide as to the state of health of the battery as a whole, otherwise the overall battery voltage may be assessed.

Note that neither technique gives any indication of charge capacity, only charge level. Charge capacity of any rechargeable battery will decline with age and usage, meaning that it may no longer be fit for purpose even when nominally fully charged. Other tests, usually involving current drain, are used to determine the residual charge capacity of a battery.

Voltages for common usage

IUoU battery charging is a three-stage charging procedure for lead-acid batteries. A lead-acid battery's theoretical voltage is 2 V for one cell. For a single cell, the voltage can range from 1.8 V loaded at full discharge, to 2.10 V in an open circuit at full charge. Float voltage varies depending on battery type, i.e. flooded cells, gelled electrolyte, absorbed glass mat (AGM), and ranges from 1.8 V to 2.27 V. Equalization voltage, and charging voltage for sulfated cells, can range from 2.67 V to almost 3 V. (only until a charge current is flowing) Specific values for a given battery depend on the design and manufacturer recommendations, and are usually given at a baseline temperature of 20 °C (68 °F), requiring adjustment for ambient conditions.

Construction

Plates

Internal view of a small lead-acid battery from an electric-start equipped motorcycle

The lead–acid cell can be demonstrated using sheet lead plates for the two electrodes. However, such a construction produces only around one ampere for roughly postcard-sized plates, and for only a few minutes.

Gaston Planté found a way to provide a much larger effective surface area. In Planté's design, the positive and negative plates were formed of two spirals of lead foil, separated with a sheet of cloth and coiled up. The cells initially had low capacity, so a slow process of "forming" was required to corrode the lead foils, creating lead dioxide on the plates and roughening them to increase surface area. Initially this process used electricity from primary batteries; when generators became available after 1870, the cost of production of batteries greatly declined. Planté plates are still used in some stationary applications, where the plates are mechanically grooved to increase their surface area.

In 1880, Camille Alphonse Faure patented a method of coating a lead grid (which serves as the current conductor) with a paste of lead oxides, sulfuric acid and water, followed by curing phase in which the plates were exposed to gentle heat in a high humidity environment. The curing process caused the paste to change to a mixture of lead sulfates which adhered to the lead plate. Then, during the battery's initial charge (called "formation") the cured paste on the plates was converted into electrochemically active material (the "active mass"). Faure's process significantly reduced the time and cost to manufacture lead–acid batteries, and gave a substantial increase in capacity compared with Planté's battery. Faure's method is still in use today, with only incremental improvements to paste composition, curing (which is still done with steam, but is now a very tightly controlled process), and structure and composition of the grid to which the paste is applied.

The grid developed by Faure was of pure lead with connecting rods of lead at right angles. In contrast, present-day grids are structured for improved mechanical strength and improved current flow. In addition to different grid patterns (ideally, all points on the plate are equidistant from the power conductor), modern-day processes also apply one or two thin fibre-glass mats over the grid to distribute the weight more evenly. And while Faure had used pure lead for his grids, within a year (1881) these had been superseded by lead-antimony (8–12%) alloys to give the structures additional rigidity. However, high-antimony grids have higher hydrogen evolution (which also accelerates as the battery ages), and thus greater outgassing and higher maintenance costs. These issues were identified by U. B. Thomas and W. E. Haring at Bell Labs in the 1930s and eventually led to the development of lead-calcium grid alloys in 1935 for standby power batteries on the U.S. telephone network. Related research led to the development of lead-selenium grid alloys in Europe a few years later. Both lead-calcium and lead-selenium grid alloys still add antimony, albeit in much smaller quantities than the older high-antimony grids: lead-calcium grids have 4–6% antimony while lead-selenium grids have 1–2%. These metallurgical improvements give the grid more strength, which allows it carry more weight, i.e. more active material, and so the plates can be thicker, which in turn contributes to battery lifespan since there is more material available to shed before the battery becomes unusable. High-antimony alloy grids are still used in batteries intended for frequent cycling, e.g. in motor-starting applications where frequent expansion/contraction of the plates needs to be compensated for, but where outgassing is not significant since charge currents remain low. Since the 1950s, batteries designed for infrequent cycling applications (e.g., standby power batteries) increasingly have lead-calcium or lead-selenium alloy grids since these have less hydrogen evolution and thus lower maintenance overhead. Lead-calcium alloy grids are cheaper to manufacture (the cells thus have lower up-front costs), and have a lower self-discharge rate, and lower watering requirements, but have slightly poorer conductivity, are mechanically weaker (and thus require more antimony to compensate), and are strongly subject to corrosion (and thus a shorter lifespan) than cells with lead-selenium alloy grids.

The open circuit effect is also known as the antimony free effect.

Modern-day paste contains carbon black, blanc fixe (barium sulfate) and lignosulfonate. The blanc fixe acts as a seed crystal for the lead–to–lead sulfate reaction. The blanc fixe must be fully dispersed in the paste in order for it to be effective. The lignosulfonate prevents the negative plate from forming a solid mass during the discharge cycle, instead enabling the formation of long needle–like dendrites. The long crystals have more surface area and are easily converted back to the original state on charging. Carbon black counteracts the effect of inhibiting formation caused by the lignosulfonates. Sulfonated naphthalene condensate dispersant is a more effective expander than lignosulfonate and speeds up formation. This dispersant improves dispersion of barium sulfate in the paste, reduces hydroset time, produces a more breakage-resistant plate, reduces fine lead particles and thereby improves handling and pasting characteristics. It extends battery life by increasing end-of-charge voltage. Sulfonated naphthalene requires about one-third to one-half the amount of lignosulfonate and is stable to higher temperatures.

Once dry, the plates are stacked with suitable separators and inserted in a cell container. The alternate plates then constitute alternating positive and negative electrodes, and within the cell are later connected to one another (negative to negative, positive to positive) in parallel. The separators inhibit the plates from touching each other, which would otherwise constitute a short circuit. In flooded and gel cells, the separators are insulating rails or studs, formerly of glass or ceramic, and now of plastic. In AGM cells, the separator is the glass mat itself, and the rack of plates with separators are squeezed together before insertion into the cell; once in the cell, the glass mats expand slightly, effectively locking the plates in place. In multi-cell batteries, the cells are then connected to one another in series, either through connectors through the cell walls, or by a bridge over the cell walls. All intra-cell and inter-cell connections are of the same lead alloy as that used in the grids. This is necessary to prevent galvanic corrosion.

So-called "deep cycle" batteries employ a different geometry for their positive electrodes. In this geometry, the positive electrode is not a flat plate but a row of lead-oxide cylinders or tubes strung side by side (hence the term "tubular" or "cylindrical" batteries for this geometry). The advantage of this geometry is an increased surface area in contact with the electrolyte, which in turn allows higher discharge/charge currents than a flat-plate cell of the same volume and depth-of-charge. Tubular-electrode cells thus exhibit a higher power density than flat-plate cells. This makes tubular/cylindrical geometry plates especially suitable for high-current applications with storage weight/space limitations, such as for forklifts or for starting marine diesel engines. However, because tubes/cylinders have less active material in the same volume, they also have a lower energy density than flat-plate cells. And, less active material at the electrode also means they have less material available to shed before the cell becomes unusable. Tubular/cylindrical electrodes are also more complicated to manufacture uniformly, which tends to make them more expensive than flat-plate cells. These trade-offs limit the range of applications in which tubular/cylindrical batteries are meaningful to situations where there is insufficient space to install higher capacity (and thus larger) flat-plate units.

About 60% of the weight of an automotive-type lead–acid battery rated around 60 A·h (8.7 kg of a 14.5 kg battery) is lead or internal parts made of lead; the balance is electrolyte, separators, and the case.

Separators

Separators between the positive and negative plates prevent short-circuit through physical contact, mostly through dendrites ("treeing"), but also through shedding of the active material. Separators obstruct the flow of ions between the plates and increase the internal resistance of the cell. Wood, rubber, glass fiber mat, cellulose, and PVC or polyethylene plastic have been used to make separators. Wood was the original choice, but deteriorated in the acid electrolyte. Rubber separators are stable in battery acid and provide valuable electrochemical advantages that other materials cannot.

An effective separator must possess a number of mechanical properties; such as permeability, porosity, pore size distribution, specific surface area, mechanical design and strength, electrical resistance, ionic conductivity, and chemical compatibility with the electrolyte. In service, the separator must have good resistance to acid and oxidation. The area of the separator must be a little larger than the area of the plates to prevent material shorting between the plates. The separators must remain stable over the battery's operating temperature range.

Absorbed glass mat (AGM)

In the absorbed glass mat design, or AGM for short, the spaces between the cells is replaced by a glass fibre mat soaked in electrolyte. There is only enough electrolyte in the mat to keep it wet, and if the battery is punctured the electrolyte will not flow out of the mats. Likewise, the mat greatly reduces evaporation, to the point that the batteries do not require periodic refilling of the water. This combination of features allows the battery to be completely sealed, which makes them useful in portable devices and similar roles.

To reduce the water loss rate calcium is alloyed with the plates, however gas build-up remains a problem when the battery is deeply or rapidly charged or discharged. To prevent over-pressurization of the battery casing, AGM batteries include a one-way blow-off valve, and are often known as "valve regulated lead–acid", or VRLA, designs.

Another advantage to the AGM design is that the electrolyte becomes the separator material, and mechanically strong. This allows the plate stack to be compressed together in the battery shell, slightly increasing energy density compared to liquid or gel versions. AGM batteries often show a characteristic "bulging" in their shells when built in common rectangular shapes.

The mat also prevents the vertical motion of the electrolyte within the battery. When a normal wet cell is stored in a discharged state, the heavier acid molecules tend to settle to the bottom of the battery, causing the electrolyte to stratify. When the battery is then used, the majority of the current flows only in this area, and the bottom of the plates tend to wear out rapidly. This is one of the reasons a conventional car battery can be ruined by leaving it stored for a long period and then used and recharged. The mat significantly prevents this stratification, eliminating the need to periodically shake the batteries, boil them, or run an "equalization charge" through them to mix the electrolyte. Stratification also causes the upper layers of the battery to become almost completely water, which can freeze in cold weather, AGMs are significantly less susceptible to damage due to low-temperature use.

While AGM cells do not permit watering (typically it is impossible to add water without drilling a hole in the battery), their recombination process is fundamentally limited by the usual chemical processes. Hydrogen gas will even diffuse right through the plastic case itself. Some have found that it is profitable to add water to an AGM battery, but this must be done slowly to allow for the water to mix via diffusion throughout the battery. When a lead-acid battery loses water, its acid concentration increases, increasing the corrosion rate of the plates significantly. AGM cells already have a high acid content in an attempt to lower the water loss rate and increase standby voltage, and this brings about short life. If the open circuit voltage of AGM cells is significantly higher than 2.093 volts, or 12.56 V for a 12 V battery, then they have a higher acid content than a flooded cell; while this is normal for an AGM battery, it is not desirable for long life.

AGM cells intentionally or accidentally overcharged will show a higher open circuit voltage according to the water lost (and acid concentration increased). One amp-hour of overcharge will liberate 0.335 grams of water; some of this liberated hydrogen and oxygen will recombine, but not all of it.

Gelled electrolytes

Main article: VRLA battery § Gel_battery

During the 1970s, researchers developed the sealed version or "gel battery", which mixes a silica gelling agent into the electrolyte (silica-gel based lead-acid batteries used in portable radios from early 1930s were not fully sealed). This converts the formerly liquid interior of the cells into a semi-stiff paste, providing many of the same advantages of the AGM. Such designs are even less susceptible to evaporation and are often used in situations where little or no periodic maintenance is possible. Gel cells also have lower freezing and higher boiling points than the liquid electrolytes used in conventional wet cells and AGMs, which makes them suitable for use in extreme conditions.

The only downside to the gel design is that the gel prevents rapid motion of the ions in the electrolyte, which reduces carrier mobility and thus surge current capability. For this reason, gel cells are most commonly found in energy storage applications like off-grid systems.

"Maintenance free", "sealed" and "VRLA"

Both gel and AGM designs are sealed, do not require watering, can be used in any orientation, and use a valve for gas blowoff. For this reason, both designs can be called maintenance free, sealed and VRLA. However, it is quite common to find resources stating that these terms refer to one or another of these designs, specifically.

Applications

Most of the world's lead-acid batteries are automobile starting, lighting and ignition (SLI) batteries, with an estimated 320 million units shipped in 1999. In 1992 about 3 million tons of lead were used in the manufacture of batteries.

Wet cell stand-by (stationary) batteries designed for deep discharge are commonly used in large backup power supplies for telephone and computer centres, grid energy storage, and off-grid household electric power systems. Lead–acid batteries are used in emergency lighting and to power sump pumps in case of power failure.

Traction (propulsion) batteries are used in golf carts and other battery electric vehicles. Large lead-acid batteries are also used to power the electric motors in diesel-electric (conventional) submarines when submerged, and are used as emergency power on nuclear submarines as well. Valve-regulated lead acid batteries cannot spill their electrolyte. They are used in back-up power supplies for alarm and smaller computer systems (particularly in uninterruptible power supplies; UPS) and for electric scooters, electric wheelchairs, electrified bicycles, marine applications, battery electric vehicles or micro hybrid vehicles, and motorcycles.

Lead-acid batteries were used to supply the filament (heater) voltage, with 2 V common in early vacuum tube (valve) radio receivers.

Portable batteries for miners' cap lamps headlamps typically have two or three cells.

Cycles

Starting batteries

Main article: Automotive battery

Lead–acid batteries designed for starting automotive engines are not designed for deep discharge. They have a large number of thin plates designed for maximum surface area, and therefore maximum current output, but which can easily be damaged by deep discharge. Repeated deep discharges will result in capacity loss and ultimately in premature failure, as the electrodes disintegrate due to mechanical stresses that arise from cycling. Starting batteries kept on continuous float charge will have corrosion in the electrodes which will result in premature failure. Starting batteries should be kept open circuit but charged regularly (at least once every two weeks) to prevent sulfation.

Starting batteries are lighter weight than deep cycle batteries of the same battery dimensions, because the cell plates do not extend all the way to the bottom of the battery case. This allows loose disintegrated lead to fall off the plates and collect under the cells, to prolong the service life of the battery. If this loose debris rises high enough it can touch the plates and lead to failure of a cell, resulting in loss of battery voltage and capacity.

Deep-cycle batteries

Main article: Deep-cycle battery

Specially designed deep-cycle cells are much less susceptible to degradation due to cycling, and are required for applications where the batteries are regularly discharged, such as photovoltaic systems, electric vehicles (forklift, golf cart, electric cars and other) and uninterruptible power supplies. These batteries have thicker plates that can deliver less peak current, but can withstand frequent discharging.

Some batteries are designed as a compromise between starter (high-current) and deep cycle batteries. They are able to be discharged to a greater degree than automotive batteries, but less so than deep cycle batteries. They may be referred to as "marine/motorhome" batteries, or "leisure batteries".

Fast and slow charge and discharge

Charge current needs to match the ability of the battery to absorb the energy. Using too large a charge current on a small battery can lead to boiling and venting of the electrolyte. In this image a VRLA battery case has ballooned due to the high gas pressure developed during overcharge.

The capacity of a lead–acid battery is not a fixed quantity but varies according to how quickly it is discharged. An empirical relationship between discharge rate and capacity is known as Peukert's law.

When a battery is charged or discharged, only the reacting chemicals, which are at the interface between the electrodes and the electrolyte, are initially affected. With time, the charge stored in the chemicals at the interface, often called "interface charge" or "surface charge", spreads by diffusion of these chemicals throughout the volume of the active material.

Consider a battery that has been completely discharged (such as occurs when leaving the car lights on overnight, a current draw of about 6 amps). If it then is given a fast charge for only a few minutes, the battery plates charge only near the interface between the plates and the electrolyte. In this case the battery voltage might rise to a value near that of the charger voltage; this causes the charging current to decrease significantly. After a few hours this interface charge will spread to the volume of the electrode and electrolyte; this leads to an interface charge so low that it may be insufficient to start the car. As long as the charging voltage stays below the gassing voltage (about 14.4 volts in a normal lead–acid battery), battery damage is unlikely, and in time the battery should return to a nominally charged state.

Valve regulated (VRLA)

In a valve regulated lead acid battery (VRLA) the hydrogen and oxygen produced in the cells largely recombine into water. Leakage is minimal, although some electrolyte still escapes if the recombination cannot keep up with gas evolution. Since VRLA batteries do not require (and make impossible) regular checking of the electrolyte level, they have been called maintenance free batteries. However, this is somewhat of a misnomer. VRLA cells do require maintenance. As electrolyte is lost, VRLA cells "dry-out" and lose capacity. This can be detected by taking regular internal resistance, conductance or impedance measurements. Regular testing reveals whether more involved testing and maintenance is required. Recent maintenance procedures have been developed allowing "rehydration", often restoring significant amounts of lost capacity.

VRLA types became popular on motorcycles around 1983, because the acid electrolyte is absorbed into the separator, so it cannot spill. The separator also helps them better withstand vibration. They are also popular in stationary applications such as telecommunications sites, due to their small footprint and installation flexibility.

The electrical characteristics of VRLA batteries differ somewhat from wet-cell lead–acid batteries, requiring caution in charging and discharging.

Sulfation and desulfation

Sulfated plates from 12 V 5 Ah battery

Lead–acid batteries lose the ability to accept a charge when discharged for too long due to sulfation, the crystallization of lead sulfate. They generate electricity through a double sulfate chemical reaction. Lead and lead dioxide, the active materials on the battery's plates, react with sulfuric acid in the electrolyte to form lead sulfate. The lead sulfate first forms in a finely divided, amorphous state, and easily reverts to lead, lead dioxide and sulfuric acid when the battery recharges. As batteries cycle through numerous discharges and charges, some lead sulfate is not recombined into electrolyte and slowly converts to a stable crystalline form that no longer dissolves on recharging. Thus, not all the lead is returned to the battery plates, and the amount of usable active material necessary for electricity generation declines over time.

Sulfation occurs in lead–acid batteries when they are subjected to insufficient charging during normal operation. It impedes recharging; sulfate deposits ultimately expand, cracking the plates and destroying the battery. Eventually so much of the battery plate area is unable to supply current that the battery capacity is greatly reduced. In addition, the sulfate portion (of the lead sulfate) is not returned to the electrolyte as sulfuric acid. It is believed that large crystals physically block the electrolyte from entering the pores of the plates. Sulfation can be avoided if the battery is fully recharged immediately after a discharge cycle. A white coating on the plates may be visible (in batteries with clear cases, or after dismantling the battery). Batteries that are sulfated show a high internal resistance and can deliver only a small fraction of normal discharge current. Sulfation also affects the charging cycle, resulting in longer charging times, less efficient and incomplete charging, and higher battery temperatures.

SLI batteries (starting, lighting, ignition; i.e., car batteries) suffer most deterioration because vehicles normally stand unused for relatively long periods of time. Deep cycle and motive power batteries are subjected to regular controlled overcharging, eventually failing due to corrosion of the positive plate grids rather than sulfation.

There are no known, independently verified ways to reverse sulfation. There are commercial products claiming to achieve desulfation through various techniques (such as pulse charging), but there are no peer-reviewed publications verifying their claims. Sulfation prevention remains the best course of action, by periodically fully charging the lead-acid batteries.

Stratification

A typical lead–acid battery contains a mixture with varying concentrations of water and acid. Sulfuric acid has a higher density than water, which causes the acid formed at the plates during charging to flow downward and collect at the bottom of the battery. Eventually the mixture will again reach uniform composition by diffusion, but this is a very slow process. Repeated cycles of partial charging and discharging will increase stratification of the electrolyte, reducing the capacity and performance of the battery because the lack of acid on top limits plate activation. The stratification also promotes corrosion on the upper half of the plates and sulfation at the bottom.

Periodic overcharging creates gaseous reaction products at the plate, causing convection currents which mix the electrolyte and resolve the stratification. Mechanical stirring of the electrolyte would have the same effect. Batteries in moving vehicles are also subject to sloshing and splashing in the cells, as the vehicle accelerates, brakes, and turns.

Risk of explosion

Car lead-acid battery after explosion showing brittle cracking in casing ends

Excessive charging causes electrolysis, emitting hydrogen and oxygen. This process is known as "gassing". Wet cells have open vents to release any gas produced, and VRLA batteries rely on valves fitted to each cell. Catalytic caps are available for flooded cells to recombine hydrogen and oxygen. A VRLA cell normally recombines any hydrogen and oxygen produced inside the cell, but malfunction or overheating may cause gas to build up. If this happens (for example, on overcharging) the valve vents the gas and normalizes the pressure, producing a characteristic acid smell. However, valves can fail, such as if dirt and debris accumulate, allowing pressure to build up.

Accumulated hydrogen and oxygen sometimes ignite in an internal explosion. The force of the explosion can cause the battery's casing to burst, or cause its top to fly off, spraying acid and casing fragments. An explosion in one cell may ignite any combustible gas mixture in the remaining cells. Similarly, in a poorly ventilated area, connecting or disconnecting a closed circuit (such as a load or a charger) to the battery terminals can also cause sparks and an explosion, if any gas was vented from the cells.

Individual cells within a battery can also short circuit, causing an explosion.

The cells of VRLA batteries typically swell when the internal pressure rises. The deformation varies from cell to cell, and is greater at the ends where the walls are unsupported by other cells. Such over-pressurized batteries should be carefully isolated and discarded. Personnel working near batteries at risk for explosion should protect their eyes and exposed skin from burns due to spraying acid and fire by wearing a face shield, overalls, and gloves. Using goggles instead of a face shield sacrifices safety by leaving the face exposed to possible flying acid, case or battery fragments, and heat from a potential explosion.

Environment

Environmental concerns

According to a 2003 report entitled "Getting the Lead Out", by Environmental Defense and the Ecology Center of Ann Arbor, Michigan, the batteries of vehicles on the road contained an estimated 2,600,000 metric tons (2,600,000 long tons; 2,900,000 short tons) of lead. Some lead compounds are extremely toxic. Long-term exposure to even tiny amounts of these compounds can cause brain and kidney damage, hearing impairment, and learning problems in children. The auto industry uses over 1,000,000 metric tons (980,000 long tons; 1,100,000 short tons) every year, with 90% going to conventional lead–acid vehicle batteries. While lead recycling is a well-established industry, more than 40,000 metric tons (39,000 long tons; 44,000 short tons) ends up in landfills every year. According to the federal Toxic Release Inventory, another 70,000 metric tons (69,000 long tons; 77,000 short tons) are released in the lead mining and manufacturing process.

Attempts are being made to develop alternatives (particularly for automotive use) because of concerns about the environmental consequences of improper disposal and of lead smelting operations, among other reasons. Alternatives are unlikely to displace them for applications such as engine starting or backup power systems, since the batteries, although heavy, are low-cost.

Recycling

See also: Automotive battery recycling

A worker recycling molten lead in a battery recycling facility.

Lead–acid battery recycling is one of the most successful recycling programs in the world. In the United States 99% of all battery lead was recycled between 2009 and 2013. An effective pollution control system is a necessity to prevent lead emission. Continuous improvement in battery recycling plants and furnace designs is required to keep pace with emission standards for lead smelters.

Additives

Chemical additives have been used ever since the lead–acid battery became a commercial item, to reduce lead sulfate build up on plates and improve battery condition when added to the electrolyte of a vented lead–acid battery. Such treatments are rarely, if ever, effective.

Two compounds used for such purposes are Epsom salts and EDTA. Epsom salts reduces the internal resistance in a weak or damaged battery and may allow a small amount of extended life. EDTA can be used to dissolve the sulfate deposits of heavily discharged plates. However, the dissolved material is then no longer available to participate in the normal charge/discharge cycle, so a battery temporarily revived with EDTA will have a reduced life expectancy. Residual EDTA in the lead–acid cell forms organic acids which will accelerate corrosion of the lead plates and internal connectors.

The active materials change physical form during charge/discharge, resulting in growth and distortion of the electrodes, and shedding of electrode into the electrolyte. Once the active material has fallen out of the plates, it cannot be restored into position by any chemical treatment. Similarly, internal physical problems such as cracked plates, corroded connectors, or damaged separators cannot be restored chemically.

Corrosion problems

Corrosion of the external metal parts of the lead–acid battery results from a chemical reaction of the battery terminals, lugs and connectors.

Corrosion on the positive terminal is caused by electrolysis, due to a mismatch of metal alloys used in the manufacture of the battery terminal and cable connector. White corrosion is usually lead or zinc sulfate crystals. Aluminum connectors corrode to aluminum sulfate. Copper connectors produce blue and white corrosion crystals. Corrosion of a battery's terminals can be reduced by coating the terminals with petroleum jelly or a commercially available product made for the purpose.

If the battery is over-filled with water and electrolyte, thermal expansion can force some of the liquid out of the battery vents onto the top of the battery. This solution can then react with the lead and other metals in the battery connector and cause corrosion.

The electrolyte can seep from the plastic-to-lead seal where the battery terminals penetrate the plastic case.

Acid fumes that vaporize through the vent caps, often caused by overcharging, and insufficient battery box ventilation can allow the sulfuric acid fumes to build up and react with the exposed metals.

Maintenance precautions

Ammonia can neutralize spilled battery acid. Surplus ammonia and water evaporate, leaving an ammonium sulfate residue. Sodium bicarbonate (baking soda) is also commonly used for this purpose.

Sizing nomenclature

With the broad range of possible electrical attributes, a part number nomenclature is used by many battery manufacturers to convey basic information such as voltage, ampere-hour capacity, and terminals. The format follows a pattern such as <mfr><voltage><capacity>.

Part number	Manufacturer	Voltage (V)	Capacity (Ah)
AP12-24	Avon Battery	12	24.0
NB12-18HR	National Battery	12	18.0
TB12100	Tenergy	12	10.0
CBL18-12	Canbat Batteries	12	18.0
SP12-18HR	Sigmas Battery Tek	12	18.0
UB12180	Universal Power Group	12	18.0

Some vendors append a suffix, indicating the terminal types, terminal locations, and battery dimensions. Batteries for passenger motor vehicles usually use BCI sizing nomenclature.

See also

• Automotive battery
• Battery room
• Comparison of battery types
• Dry cell
• History of the battery
• List of battery sizes
• List of battery types
• Rechargeable battery
• Silver calcium battery
• UltraBattery
• Wet cell

References

General

• Lead Acid Battery Desulfator (Home Power #77 June/July 2000) [1]
• Battery Plate Sulfation (MagnaLabs)[2]
• Battery Desulfation [3]
• Lead Acid Batteries [4]
• DC Supply! (April 2002) [5]
• Some Technical Details on Lead Acid Batteries [6]

External links

• Battery Council International (BCI), lead–acid battery manufacturers' trade organization.
• Car and Deep Cycle Battery Frequently Asked Questions
• Case Studies in Environmental Medicine – Lead Toxicity
• Lead Acid Battery Desulfator (Home Power #77 June/July 2000)
• Battery Desulfation

UpToDate Contents

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• 1. 成人における鉛中毒 adult lead poisoning
• 2. ボタン型電池および乾電池の誤飲 button and cylindrical battery ingestion
• 3. 鉛腎症および鉛関連腎毒性 lead nephropathy and lead related nephrotoxicity
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English Journal

• In situ solid-state NMR spectroscopy of electrochemical cells: batteries, supercapacitors, and fuel cells.

• Blanc F, Leskes M, Grey CP.SourceDepartment of Chemistry, University of Cambridge , Lensfield Road, Cambridge CB2 1EW, United Kingdom.
• Accounts of chemical research.Acc Chem Res.2013 Sep 17;46(9):1952-63. doi: 10.1021/ar400022u. Epub 2013 Jun 21.
• Electrochemical cells, in the form of batteries (or supercapacitors) and fuel cells, are efficient devices for energy storage and conversion. These devices show considerable promise for use in portable and static devices to power electronics and various modes of transport and to produce and store el
• PMID 24041242

• The relationship between blood lead levels and morbidities among workers employed in a factory manufacturing lead-acid storage battery.

• Kalahasthi RB, Barman T, Rajmohan HR.Sourcea Department of Biochemistry , Regional Occupational Health Centre (Southern) , Bangalore , India.
• International journal of environmental health research.Int J Environ Health Res.2013 Jul 16. [Epub ahead of print]
• The present study was carried out to find the relationship between blood lead levels (BLLs) and morbidities among 391 male workers employed in a factory manufacturing lead-acid storage batteries. A predesigned questionnaire was used to collect information on subjective health complaints and clinical
• PMID 23859360

• [Relationship between XRCC3 gene polymorphism and susceptibility to lead poisoning in male lead-exposed workers].

• Liu XQ, Zhang Z.SourceDepartment of Occupational Health, Fuzhou City Center for Disease Control and Prevention, Fujian China.
• Zhonghua lao dong wei sheng zhi ye bing za zhi = Zhonghua laodong weisheng zhiyebing zazhi = Chinese journal of industrial hygiene and occupational diseases.Zhonghua Lao Dong Wei Sheng Zhi Ye Bing Za Zhi.2013 Jun;31(6):401-4.
• OBJECTIVE: To investigate the relationship between genetic polymorphism of X-ray repair cross-complementing gene3 (XRCC3) and susceptibility to lead poisoning in male lead-exposed workers.METHODS: Peripheral venous blood and morning urine samples were collected from 326 male lead-exposed workers in
• PMID 23803535

Japanese Journal

• 2種類の蓄電デバイス(鉛蓄電池とリチウムイオンキャパシタ)を用いた新開発1.5MWハイブリッド型蓄電システム (保護リレーシステム研究会・電力系統の保護・監視制御・計測解析技術)

• 電気学会研究会資料. PPR 2016(14-28), 65-70, 2016-11-18
• NAID 40021027340

• 電池廃棄処理について : 産業用鉛電池のリサイクル (特集 電気設備における環境対策の現状と動向)

• 電気設備学会誌 = The Journal of the Institute of Electrical Installation Engineers of Japan 36(9), 656-658, 2016-09
• NAID 40020957098

• Development of Design Methodology for 60Hz Wireless Power Transmission System

• IEEJ Journal of Industry Applications 5(6), 429-438, 2016
• NAID 130005277260

Related Links

• lead storage batteryの意味 - 英和辞書 - goo辞書

lead storage batteryとは。意味や和訳。鉛蓄電池，鉛バッテリー. - goo辞書は国語、英和、和英、中国語、百科事典等からまとめて探せる辞書検索サービスです。 lead storage batteryの意味 - 英和辞書 - goo辞書 |

• Lead Storage Battery- Batteries - Boundless

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Related Pictures

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★リンクテーブル★

リンク元	「鉛蓄電池」「lead accumulator」
関連記事	「battery」「storage」「lead」

「鉛蓄電池」

　　[★]

英

lead storage battery、lead accumulator

「lead accumulator」

　　[★]

• 鉛蓄電池

関

lead storage battery

「battery」

　　[★]

• n.

• 電池、バッテリー。
• 一組の装置/器具。(同種の/関連したものの)一群、ひと続き。(ヒトを圧倒するような)勢揃い)。(心理)バッテリー(知能・適正・能力などの総合テスト)
• 何度も打ち叩くこと、乱打。殴打、故意の接触

　 　 　 　 　 　 　

「storage」

　　[★]

• n.

• 貯蔵

関

pool、pooling、preservation、preserve、reserve、store

　 　 　 　

「lead」

　　[★]

• n.

• 鉛