lead-acid battery oor Thai
lead-acid battery
en
a battery with lead electrodes with dilute sulphuric acid as the electrolyte; each cell generates about 2 volts
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Corrosion of the external metal parts of the lead–acid battery results from a chemical reaction of the battery terminals, lugs and connectors.
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In the 1970s, the valve-regulated lead–acid battery (VRLA, or "sealed") was developed, including modern absorbed glass mat types, allowing operation in any position.
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Section::::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.
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In 1999 lead–acid battery sales accounted for 40–45% of the value from batteries sold worldwide (excluding China and Russia), equivalent to a manufacturing market value of about $15 billion.
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We want to talk about storing energy, and unfortunately the best thing we've got going is something that was developed in France a hundred and fifty years ago, the lead acid battery.
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Sulfation prevention remains the best course of action, by periodically fully charging the lead-acid batteries. Section::::Stratification. A typical lead–acid battery contains a mixture with varying concentrations of water and acid.
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The capacity of a lead–acid battery is not a fixed quantity but varies according to how quickly it is discharged. The empirical relationship between discharge rate and capacity is known as Peukert's law.
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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.
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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 the early 1930s were not fully sealed).
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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.
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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, which can easily be damaged by deep discharge.
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Section::::Gelled electrolytes. 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 the early 1930s were not fully sealed).
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They may be referred to as "marine/motorhome" batteries, or "leisure batteries". Section::::Fast and slow charge and discharge. The capacity of a lead–acid battery is not a fixed quantity but varies according to how quickly it is discharged.
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Similarly, internal physical problems such as cracked plates, corroded connectors, or damaged separators cannot be restored chemically. Section::::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.
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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.
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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.
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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.
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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.
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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.
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Overcharging with high charging voltages generates oxygen and hydrogen gas by electrolysis of water, which bubbles out and is lost. The design of some types of lead-acid battery allows the electrolyte level to be inspected and topped up with pure water to replace any that has been lost this way.
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About 60% of the weight of an automotive-type lead–acid battery rated around 60 A·h is lead or internal parts made of lead; the balance is electrolyte, separators, and the case. For example, there are approximately 8.7 kg (19 lb) of lead in a typical 14.5-kg (32 lb) battery. Section::::Separators.
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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.
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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.
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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.
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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.
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57 sinne gevind in 8 ms. Hulle kom uit baie bronne en word nie nagegaan nie.