Battery electric is a device consisting of one or more electrochemical cells with external connections provided for power devices such as flashlights, smart phones and electric cars. When the battery supplies power, the positive terminal is the cathode and the negative terminal is the anode. Terminals marked negative are the source of electrons that when connected to an external circuit will flow and send energy to an external device. When the battery is connected to an external circuit, the electrolyte can move as an inner ion, allowing chemical reactions to be solved on a separate terminal and thus sending energy to an external circuit. It is the movement of ions in the battery that allows the current to flow out of the battery to do the work. Historically, the term "battery" specifically refers to a device consisting of multiple cells, but its use has evolved additionally to include a single-cell device.
Primary batteries (disposable or "disposable") are used once and discarded; the electrode material changes irreversibly during discharge. A common example is alkaline batteries used for flashlights and many portable electronic devices. Secondary (rechargeable) batteries can be removed and recharged several times using the electrical current used; the original composition of the electrode can be recovered by a reverse current. Examples include lead-acid batteries used in vehicles and lithium-ion batteries used for portable electronics such as laptops and smartphones.
Batteries come in a variety of shapes and sizes, from mini cells used to power hearing aids and watches to small and thin cells used in smartphones, to large lead acid batteries used in cars and trucks, and to large battery banks the largest size of a room that provides standby or emergency power for telephone exchange and computer data centers.
According to 2005 estimates, the battery industry worldwide generates US $ 48 billion in sales annually, with annual growth of 6%.
Batteries have a lower specific energy (energy per unit mass) than common fuel such as gasoline. In the car, this is somewhat offset by the higher efficiency of the electric motor in generating mechanical work, compared to the combustion engine.
Video Electric battery
History
The use of "batteries" to describe a group of electrical devices comes from Benjamin Franklin, who in 1748 described some Leyden jars by analogy with battery guns (Benjamin Franklin borrowed the term "battery" from the military, which refers to joint weapon function).
Italian physicist Alessandro Volta built and described the first electrochemical battery, voltaic pile, in 1800. It is a pile of copper and zinc plates, separated by a saline-soaked paper disk, which can produce steady currents for long periods of time. Volta does not understand that the voltage is caused by a chemical reaction. He thought that his cells were an endless source of energy, and that the associated corrosion effects on the electrodes were mere distractions, rather than the unavoidable consequences of their operation, as Michael Faraday pointed out in 1834.
Although the initial batteries are very valuable for experimental purposes, in practice their voltages fluctuate and they can not provide large currents for sustained periods. The Daniell cell, discovered in 1836 by the English chemist John Frederic Daniell, was the first practical source of electricity, becoming an industry standard and seeing widespread adoption as a resource for electrical telegraph networks. It consists of a copper pot filled with a solution of copper sulphate, where it is immersed in an unmasked pottery container filled with sulfuric acid and a zinc electrode.
These wet cells use liquid electrolytes, which are susceptible to leaks and spills if not handled properly. Many glass jars are used to hold their components, which makes it fragile and potentially dangerous. This characteristic makes wet cells unsuitable for portable equipment. Toward the end of the nineteenth century, the discovery of dry cell batteries, which replaced liquid electrolytes with pastes, made portable electric devices practical.
Maps Electric battery
Principle of operation
Batteries convert chemical energy directly into electrical energy. The battery consists of several voltaic cell numbers. Each cell consists of two and a half cells connected in series by a conductive electrolyte containing anions and cations . One and a half cells including the electrolyte and the negative electrode, the electrode in which the anions (negatively charged ions) migrate; the other half cells include electrolytes and positive electrodes in which the cations (positively charged ions) migrate. The redox reaction gives power to the battery. The cation is reduced (electrons added) to the cathode during filling, while the anion is oxidized (electrons are removed) in the anode during charging. During discharge, the process is reversed. Electrodes do not touch each other, but are electrically connected with an electrolyte. Some cells use different electrolytes for each half cell. The separator allows ions to flow between half the cells, but prevents mixing of the electrolyte.
Setiap setengah sel memiliki gaya gerak listrik ( emf ), ditentukan oleh kemampuannya untuk mendorong arus listrik dari interior ke luar sel. Ggl net dari sel adalah perbedaan antara emfs dari setengah selnya. Jadi, jika elektroda memiliki emfs dan , maka emf net adalah ; dengan kata lain, net emf adalah perbedaan antara potensi reduksi dari setengah reaksi.
Gaya penggerak listrik atau di terminal sel dikenal sebagai tegangan terminal (perbedaan) dan diukur dalam volt. Tegangan terminal dari sel yang tidak mengisi atau pengosongan disebut tegangan sirkuit terbuka dan sama dengan emf sel. Karena resistansi internal, tegangan terminal dari sel yang mengeluarkan lebih kecil dalam besarnya daripada tegangan sirkuit terbuka dan tegangan terminal sel yang pengisian melebihi tegangan sirkuit terbuka. Sel ideal to remember ketahanan internal yang dapat diabaikan, sehingga akan mempertahankan tegangan terminal konstan hingga habis, lalu turun ke nol. Jika sel tersebut mempertahankan 1,5 volt dan menyimpan muatan satu coulomb maka pada pelepasan penuh itu akan melakukan 1,5 joule kerja. Dalam sel yang sebenarnya, resistansi internal meningkat di bawah debit dan tegangan sirkit terbuka juga menurun di bawah debit. Jika tegangan dan hambatan diplot terhadap waktu, grafik yang dihasilkan biasanya berupa kurva; Bentuk kurva bervariasi sesuai dengan kimia dan pengaturan internal yang digunakan.
The voltage developed across the cell terminals depends on the release of energy from the chemical reaction of the electrode and its electrolyte. Alkaline cells and zinc cells have different chemicals, but about the same as 1.5 volts; also NiCd and NiMH cells have different chemical content, but approximately equal to 1.2 volts. The high electrochemical potential is changed in the lithium compound reaction to produce 3 or more lithium emfs cells.
Categories and types of batteries
Batteries are classified into primary and secondary forms: Battery
- Main is designed to be used until it runs out of energy and then discarded. Their chemical reactions are generally not reversible, so they can not be recharged. When the supply of reactants in the battery runs out, the battery stops generating current and is useless. Battery
- Secondary can be reloaded; that is, they can have their chemical reaction upside down by applying an electric current to the cell. It regenerates the original chemical reactants, so they can be used, refilled, and reused several times.
Some types of primary batteries used, for example, for telegraph circuits, are restored to operation by replacing the electrodes. Secondary batteries can not be recharged indefinitely due to active material dissipation, electrolyte losses and internal corrosion.
Primary
The primary battery, or primary cell, can produce immediate current on the assembly. It is most commonly used in portable devices that have low current flow, used only intermittently, or used away from alternative power sources, such as in alarms and communication circuits where other electrical power is available only intermittently. Disposable primary cells can not be recharged reliably, because the chemical reaction is not easily reversed and the active ingredient may not return to its original form. Battery manufacturers recommend not trying to refill primary cells. In general, it has a higher energy density than a rechargeable battery, but disposable batteries do not run well under high flow applications with loads below 75 ohm (75?). Common types of disposable batteries include zinc-carbon batteries and alkaline batteries.
Secondary
Secondary batteries, also known as secondary cells , or rechargeable batteries , are required before first use; they are usually assembled with active ingredients in a state of discharged. The rechargeable battery is recharged by applying an electric current, which reverses the chemical reaction that occurs during discharge/use. The device to supply the appropriate current is called a charger.
The oldest rechargeable battery form is the lead-acid battery, which is widely used in automotive and boating applications. This technology contains liquid electrolyte in an unopened container, which requires the battery to remain upright and the area is well ventilated to ensure the safe dispersion of hydrogen gas produced during overfilling. The lead-acid battery is relatively heavy for the amount of electrical energy that can be supplied. Low manufacturing costs and high current surge rates make it common where capacity (over 10 Ahs) is more important than weight and handling problems. A common application is modern car batteries, which can, in general, provide a peak current of 450 amperes.
Sealed valves regulate lead-acid batteries (VRLA batteries) are very popular in the automotive industry in lieu of acid-lead wet cells. The VRLA batteries use an immobilized sulfuric acid electrolyte, reducing the possibility of leakage and prolonging shelf life. VRLA battery disables electrolyte. The two types are:
- Gel battery (or "gel cell") using semi-solid electrolyte.
- Glass Absorbed Mat (AGM) batteries absorb electrolytes in special fiberglass woven.
Other portable rechargeable batteries include some sealed "dry cell" types, which are useful in applications such as cell phones and laptop computers. These types of cells (in order to increase power and charge density) include nickel-cadmium (NiCd), nickel-zinc (NiZn), nickel metal hydride (NiMH), and lithium-ion (Li-ion) cells. Li-ion so far has the highest share of the dry cell refill market. NiMH has replaced NiCd in most applications due to its higher capacity, but NiCd is still used in power tools, two-way radios, and medical equipment.
In the 2000s, developments include batteries with embedded electronics such as USBCELL, which allows charging AA batteries via USB connectors, nanoball batteries that allow for discharge rates about 100x larger than current batteries, and smart battery packs with state-of- charge monitor and battery protection circuitry that prevents damage to over discharge. Low self discharge (LSD) allows secondary cells to be charged before shipping.
Cell type
Many types of electrochemical cells have been produced, with various processes and chemical designs, including galvanic cells, electrolytic cells, fuel cells, flow cells and voltaic piles.
Wet cell
Battery wet cell has an electrolyte solution. Another name is flood cells , because the liquid covers all the internal parts, or the released cells , because the gas produced during the operation can escape into the air. Wet cells are precursors of dry cells and are generally used as a learning tool for electrochemistry. They can be built with general laboratory supplies, such as glasses of chemistry, for demonstrations of how electrochemical cells work. Certain types of wet cells known as concentration cells are important in understanding corrosion. Wet cells may be primary (non-rechargeable) or secondary (rechargeable) cells. Initially, all practical primary batteries such as Daniell cells are built as open top glass jar cells. Other primary wet cells are Leclanche cells, Grove cells, Bunsen cells, Chromic acid cells, Clark cells, and Weston cells. Leclanche cell chemistry was adapted to the first dry cells. Wet cells are still used in car batteries and in the industry for standby power for switchgear, telecommunications or large uninterruptible power supplies, but in many places batteries with gel cells have been used instead. This application typically uses acid-lead or nickel-cadmium cells.
Dry cell
A dry cell uses a paste electrolyte, with enough moisture to allow the current to flow. Unlike wet cells, a dry cell can operate in any orientation without spill, as it contains no free liquids, making it suitable for portable equipment. In comparison, the first wet cell is usually a fragile glass container with tin rods hanging from the top open and requires careful handling to avoid spills. The lead-acid battery does not achieve the safety and portability of the dry cell until the development of the gel battery.
The common dry cell is a zinc-carbon battery, sometimes called dry Leclanchà © cell, with a nominal voltage of 1.5 volts, the same as an alkaline battery (since both use the same combination of zinc-manganese dioxide). The standard dry cell consists of a zinc anode, usually in the form of a cylindrical pot, with a carbon cathode in the central rod shape. The electrolyte is ammonium chloride in the paste form next to the zinc anode. The remaining space between the electrolyte and the carbon cathode is taken up by a second paste comprising ammonium chloride and manganese dioxide, the latter acting as a depolariser. In some designs, ammonium chloride is replaced with zinc chloride.
Liquid Salt
The battery of a molten salt is a primary or secondary battery that uses a molten salt as an electrolyte. They operate at high temperatures and must be well insulated to maintain heat.
Backup
Backup batteries can be stored without assemblies (not activated and not supplying power) for long periods (possibly years). When the battery is needed, it is assembled (for example, by adding electrolyte); once assembled, the battery is charged and ready to work. For example, batteries for artillery fuze electronics may be activated by the impact of firing a gun. Acceleration breaks electrolyte capsules that activate the battery and drive the fuze circuit. Backup batteries are typically designed for short life spans (seconds or minutes) after long storage (years). Water-activated batteries for oceanographic instruments or military applications become active when immersed in water.
Cell performance
Battery characteristics may vary over load cycles, charging cycles, and life overload due to many factors including internal chemistry, current flow, and temperature. At low temperatures, the battery can not generate as much power as possible. Thus, in cold climates, some car owners install battery warmers, which are small electric heating pads that keep the car battery warm.
Capacity and debit
Capacity battery is the amount of electrical charge it can generate at rated voltage. The more electrode material contained in the cell the greater the capacity. Smaller cells have a smaller capacity of larger cells with the same chemistry, although they develop the same open-circuit voltage. Capacity is measured in units like amp-hour (AÃ, Â · h). Battery recognition capacity is usually expressed as a 20-hour product multiplied by a current that can consistently supply a new battery for 20 hours at a temperature of 68 ° F (20 ° C), while remaining above the specified terminal voltage per cell. For example, a battery rated at 100 AÃ, can give 5 A for 20 hours at room temperature. A small portion of the stored charge that the battery can provide depends on several factors, including battery chemistry, the rate at which the charge is delivered (current), the required terminal voltage, storage period, ambient temperature, and other factors.
Semakin tinggi tingkat debit, semakin rendah kapasitasnya. Hubungan antara arus, waktu pengosongan dan kapasitas untuk baterai asam timbal diperkirakan (lebih dari kisaran umum nilai saat ini) oleh hukum Peukert:
dimana
- adalah kapasitas ketika habis pada tingkat 1 amp.
- adalah arus yang diambil dari baterai (A).
- adalah jumlah waktu (dalam jam) yang dapat dipertahankan oleh baterai.
- adalah konstanta sekitar 1,3.
Long-term or discharged batteries for a fraction of capacity capacity loss due to the irreversible side reactions that consume unattended carriers. This phenomenon is known as self-discharge internally. Furthermore, when the battery is recharged, additional side reactions may occur, reducing the capacity for subsequent disposal. After enough refilling, at its core all the capacity is lost and the battery stops producing power.
Loss of internal energy and limiting the rate of ions passing through the electrolyte causes the battery efficiency to vary. Above the minimum threshold, low-level usage results in more battery capacity than at a higher level. Installing batteries with various ratings AÃ, Â · h does not affect the operation of the device (although it may affect operating intervals) assessed for a particular voltage unless the limit of charge is exceeded. High channel loads such as digital cameras can reduce total capacity, as is the case with alkaline batteries. For example, batteries rated 2 A A Â · h for 10 or 20 hour discharge will not maintain 1 A current for the full two hours as stated by the stated capacity.
Level C
C-rate is a measure of the rate at which the battery is being discarded. This is defined as the discharge currents divided by the theoretical current withdrawal where the battery will provide its nominal capacity in an hour. The 1C discharge rate will result in battery rated capacity in 1 hour. The discharge rate of 2C means the debit is twice as fast (30 minutes). The discharge rate of 1C on the 1.6 Ah battery means the discharge stream of 1.6 A. The 2C level will mean discharge current 3.2 A. Standards for rechargeable batteries generally assess capacity for 4 hours, 8 hours or longer discharge time. Due to the loss of internal resistance and chemical processes inside the cell, the battery rarely provides nameplate identification capacity in just one hour. Types designated for special purposes, such as in an uninterruptible computer power supply, may be rated by the manufacturer for a less than one hour termination period.
The C-rate presents the dimension error: C in ampere-hour and not ampere, and one can not express the current in ampere-hour. For this reason the concept I t was introduced by the international standard IEC61434, I t equal to the capacity of C divided by one hour, thus allowing the correct mathematical method of the current designation. The numbers used to declare the level of debit remain the same: one can talk about "2 I t rate" instead of "2 C rate" is wrong dimensionally.
Fast, large and light weight charging battery
In 2012, lithium iron phosphate ( LiFePO
4 ) battery technology is the fastest-charging/discharging, fully usable in 10-20 seconds.
By 2017, the world's largest battery built in South Australia by Tesla. It can store 129 MWh. Batteries in Hebei Province, China that can store 36 MWh of electricity built in 2013 at a cost of $ 500 million. Other large batteries, composed of Ni-Cd cells, are in Fairbanks, Alaska. It covers 2,000 square meters (22,000 sq ft) - larger than a football pitch - and weighs 1,300 tonnes. It is manufactured by ABB to provide backup power in case of a power outage. The battery can provide 40 MW of power up to seven minutes. Sodium-sulfur batteries have been used to store wind power. A 4.4 MWh battery system that can deliver 11 MW for 25 minutes stabilizes the output of the Hawaiian wind farms in Hawaii.
Lithium-sulfur batteries are used on the longest and highest solar power flights.
Lifetime
Battery life (and its synonymous battery life) has two meanings for rechargeable batteries but only one for unencumbered batteries. For recharge, it could mean either the length of time the device can run on a fully charged battery or the number of charge/discharge cycles possible before the cell fails to operate satisfactorily. For non-rechargeable, these two lives are the same because the cells survive only one cycle by definition. (The term shelf life is used to describe how long the battery will maintain its performance between manufacturing and usage.) The available capacity of all batteries drops with a decrease in temperature. In contrast to most current batteries, the Zamboni pile, discovered in 1812, offers very long service life without repairs or recharges, although it only supplies currents within the nanoamp range. The Oxford Electric Bell has been ringing almost continuously since 1840 on the original pair of batteries, considered a Zamboni pile.
Self-discharge
Disposable batteries typically lose 8 to 20 percent of their original charge per year when stored at room temperature (20-30 ° C). This is known as the "self-discharge" level, and because of the "side" chemical reaction that produces no current going inside the cell even when no load is applied. The side reaction rate is reduced for batteries stored at lower temperatures, although some may be damaged by freezing.
Long self-discharge rechargeable batteries are faster than disposable alkaline batteries, especially nickel-based batteries; the newly charged nickel cadmium (NiCd) battery loses 10% of its charge within the first 24 hours, and then releases it at a rate of about 10% per month. However, the new low nickel metal hydride (NiMH) batteries and modern lithium designs show a lower level of self-discharge (but still higher than the primary battery).
Corrosion
The internal part can corrode and fail, or the active ingredient can be slowly converted into an inactive form.
Changes to physical components
The active ingredient on the battery plate changes the chemical composition at each charge and discharge cycle; the active ingredient may be lost due to physical changes in volume, further limiting the number of times the battery can be recharged. Most nickel-based batteries will be partially discharged when purchased, and must be charged before first use. The newer NiMH batteries are ready for use when purchased, and only have a 15% discharge in a year.
Some damage occurs in each charge-charging cycle. Degradation usually occurs because the electrolyte migrates away from the electrode or because the active material releases from the electrode. Low-capacity NiMH batteries (1,700-2,000 mA Â · h) can be charged about 1,000 times, while high-capacity NiMH batteries (above 2,500 mA Â · h) last about 500 cycles. NiCd batteries tend to be rated for 1,000 cycles before their internal resilience increases permanently beyond usable values.
Speed ​​/speed debit
Fast charging increases component changes, shortening battery life.
Overcharging
If the charger can not detect when the battery is fully charged then overcharging may, damaging it.
Memory effect
NiCd cells, if used in certain repetitive ways, may indicate a decrease in capacity called "memory effect". The effect can be avoided by simple practice. The NiMH cells, though similar in chemistry, suffer less from memory effects.
Environmental conditions
Automotive lead-acid rechargeable batteries must bear the stress due to vibration, shock, and temperature range. Due to the pressure and sulfidation of these lead plates, some automotive batteries last more than six years of regular use. Starting automotive (SLI: Start, Lighting, Ignition ) The battery has many thin plates to maximize the flow. In general, the thicker the plates the longer the age. They usually only run out a little before recharging.
The "deep-cycle" lead-acid batteries such as those used in electric golf carts have thicker plates to extend long life. The main benefit of lead-acid batteries is its low cost; The main drawback is the large size and weight for the given capacity and voltage. Lead-acid batteries should not be disposed of below 20% of their capacity, because internal resistance will cause heat and damage when they are recharged. Lead-acid systems in cycles often use low-charge warning lights or low cost power disconnect switches to prevent the type of damage that will shorten battery life.
Storage
The battery life can be extended by storing the battery at low temperatures, such as in refrigerators or freezers, which slows down side reactions. Such storage may extend the life of the alkaline battery by about 5%; The rechargeable battery can hold its charge longer, depending on its type. To achieve maximum voltage, the battery must be restored to room temperature; the use of alkaline batteries at 250 mA at 0 Â ° C is only half as efficient as at 20 Â ° C. Alkaline battery manufacturers such as Duracell do not recommend cooling batteries.
Battery size
Primary batteries are available to consumers ranging from small button cells used for electric watches, to cell No. 6 which is used for signal circuits or other long-duration applications. Secondary cells are made in a very large size; a very large battery can drive a submarine or stabilize the power grid and help raise the peak load.
Dangers
Explosion
Battery explosions are generally caused by abuse or malfunctions, such as attempting to recharge a primary (non-rechargeable) battery, or short circuit.
When the battery is recharged at an excessive level, a mixture of explosive gases of hydrogen and oxygen can be produced much faster than can be discharged from the battery (eg via internal ventilation), leading to pressure buildup and finally bursting of battery casing. In extreme cases, the battery chemicals may spray violently from the casing and cause injury. Overcharging - that is, trying to charge the battery over its electrical capacity - can also cause battery explosions, in addition to leaks or permanent damage. It may also cause damage to the charger or device where excessive battery will be used.
The car battery will most likely explode when the short current generates a very large current. Such batteries produce hydrogen, which is very explosive, when they are overcharged (due to electrolysis of water in the electrolyte). During normal use, excessive amounts of filling are usually very small and produce little hydrogen, which disappears quickly. However, when a car's "jump start", high currents can cause rapid release of large volumes of hydrogen, which can be explosively ignited by nearby splashes, for example when removing jumper cables.
Removing the battery through incineration can cause an explosion as the vapor builds up in a sealed container.
Withdrawal of devices using Lithium-ion batteries has become more common in recent years. This is a response to reported accidents and failures, occasional ignition or explosion. The expert summary of the problem indicates that this type uses "liquid electrolyte to transport lithium ions between the anode and cathode." If the battery cell is charged too fast, it can cause a short circuit, causing an explosion and a fire. "
Leakage
Many battery chemicals are corrosive, toxic or both. If a leak occurs, either spontaneously or by accident, the chemicals released may be harmful. For example, disposable batteries often use zinc "can" both as a reactant and as a container to withstand other reagents. If this type of battery is overloaded, the reagent can appear through cardboard and plastic forming the rest of the container. An active chemical leak can then damage or disable equipment that is battery powered. For this reason, many electronic device manufacturers recommend removing batteries from devices that will not be used for a long time.
Toxic substances
Many types of batteries use toxic materials such as lead, mercury, and cadmium as electrodes or electrolytes. When every battery reaches the end of life it must be removed to prevent environmental damage. Battery is one form of electronic waste (e-waste). The electronic waste recycling service recovers toxic substances, which can then be used for new batteries. Of the nearly three billion batteries purchased annually in the United States, about 179,000 tonnes end up in landfills across the country. In the United States, the 1996 Compliant and Refillable Battery Management Act prohibits the sale of mercury-containing batteries, imposes uniform labeling requirements for rechargeable batteries and requires that rechargeable batteries be easily removed. California and New York City prohibit the disposal of rechargeable batteries in solid waste, and along with Maine requires mobile recycling. The rechargeable battery industry operates a nationwide recycling program in the United States and Canada, with dropoff points at local retailers.
EU Battery Directives have similar requirements, in addition to requiring increased battery recycling and promoting research on improved battery recycling methods. In accordance with these instructions, all batteries sold in the EU must be marked with a "collection symbol" (crossed trash cans). This should cover at least 3% of the prismatic battery surface and 1.5% of the cylindrical battery surface. All packages must be marked as well.
Ingestion
Batteries may be dangerous or fatal if swallowed. Small button cells can be swallowed, especially by children. While in the gastrointestinal tract, battery discharge may cause tissue damage; Such damage is sometimes serious and can lead to death. Sucked disc batteries usually do not cause problems unless they get stuck in the digestive tract. The most common place for the disc battery to become caught is the esophagus, resulting in clinical residual symptoms. Batteries that successfully traverse the esophagus are unlikely to be placed elsewhere. The likelihood that the disc battery will be in the esophagus is a function of the patient's age and size of battery. The 16 mm disc battery has been caught in the esophagus of 2 children younger than 1 year. Older children have no problems with batteries smaller than 21-23 mm. Liquefaction necrosis may occur because sodium hydroxide is produced by the current generated by the battery (usually at the anode). Perforation has occurred as fast as 6 hours after consumption.
Chemistry
Many important cell properties, such as voltage, energy density, flammability, available cell construction, operating temperature range and shelf life, are determined by the chemical battery.
Primary battery and its characteristics
Secondary battery (rechargeable) and its characteristics
Solid state battery
On February 28, 2017, The University of Texas at Austin issued a press release about a new type of solid-state battery, developed by a team led by the inventor of Lithium-ion (Li-Ion) John Goodenough, "which can lead to safer, faster and longer lasting reset for handheld grips, electric cars and stationary energy storage. " More specifically about new technologies published in peer-reviewed scientific journals Energy & amp; Environmental Science.
The independent reviews of this technology discuss the risks of fire and explosion of Lithium-ion batteries under certain conditions because they use liquid electrolyte. Newly developed batteries should be safer because they use glass electrolytes, which should eliminate short circuits. Solid-state batteries are also said to have "three times the energy density" increase their useful life in electric vehicles, for example. It should also be more ecological because the technology uses cheaper and environmentally friendly materials such as sodium extracted from seawater. They also have a longer life; ("The cells have shown more than 1,200 cycles with low cell resistance"). Research and prototypes are not expected to lead to commercial products in the near future, if ever, according to Chris Robinson of LUX Research. "This will have no real effect on the adoption of electric vehicles in the next 15 years, if that's the case." The main obstacle facing many solid-state electrolytes is the lack of a measurable and cost-effective production process, "he told The American. Energy News in e-mail.
Homemade cell
Almost all liquid or moist objects that have enough ions to be electrically conductive can function as electrolytes for cells. As a demonstration of novelty or science, it is possible to insert two electrodes made of different metals into lemons, potatoes, etc. And generate a small amount of electricity. "Hours of two potatoes" are also widely available in hobby shops and toys; they consist of a pair of cells, each composed of potato (lemon, et cetera) with two electrodes inserted into it, wires in series to form batteries with sufficient voltage to turn on the digital clock. These homemade cells are not practical to use.
Voltaic piles can be made of two coins (like nickel and one cent) and a paper towel dipped in salt water. Such stacks produce very low voltages but, when many are stacked in series, they can replace normal batteries for a short time.
Sony has developed a biological battery that generates electricity from sugar in a manner similar to the process observed in living organisms. Batteries generate electricity through the use of enzymes that break down carbohydrates.
Lead acid cells can be easily produced at home, but the exhausting filling/discharging cycle is required to 'form' the plates. This is the process by which lead sulfate is formed on the plate, and as long as the charge is converted into lead dioxide (positive plate) and pure lead (negative plate). Repeating this process produces a microscopic rough surface, increasing the surface area, increasing the current that the cell can produce.
Source of the article : Wikipedia
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