Electric battery

An electric battery is a device consisting of one or more electrochemical cells with external connections provided to power electrical devices such as flashlights, smartphones, and electric cars.[1] When a battery is supplying electric power, its positive terminal is the cathode and its negative terminal is the anode.[2] The terminal marked negative is the source of electrons that will flow through an external electric circuit to the positive terminal. When a battery is connected to an external electric load, a redox reaction converts high-energy reactants to lower-energy products, and the free-energy difference is delivered to the external circuit as electrical energy.[3] Historically the term "battery" specifically referred to a device composed of multiple cells, however the usage has evolved to include devices composed of a single cell.[4]

Primary (single-use or "disposable") batteries are used once and discarded; the electrode materials are irreversibly changed during discharge. Common examples are the alkaline battery used for flashlights and a multitude of portable electronic devices. Secondary (rechargeable) batteries can be discharged and recharged multiple times using an applied electric current; the original composition of the electrodes can be restored by reverse current. Examples include the lead-acid batteries used in vehicles and lithium-ion batteries used for portable electronics such as laptops and smartphones.

Batteries come in many shapes and sizes, from miniature cells used to power hearing aids and wristwatches to small, thin cells used in smartphones, to large lead acid batteries or lithium-ion batteries in vehicles, and at the largest extreme, huge battery banks the size of rooms that provide standby or emergency power for telephone exchanges and computer data centers.

According to a 2005 estimate, the worldwide battery industry generates US$48 billion in sales each year,[5] with 6% annual growth.

Batteries have much lower specific energy (energy per unit mass) than common fuels such as gasoline. In automobiles, this is somewhat offset by the higher efficiency of electric motors in converting chemical energy to mechanical work, compared to combustion engines.

Battery
Batteries
Various cells and batteries (top-left to bottom-right): two AA, one D, one handheld ham radio battery, two 9-volt (PP3), two AAA, one C, one camcorder battery, one cordless phone battery
TypePower source
Working principleElectrochemical reactions, Electromotive force
First production1800s
Electronic symbol
Battery symbol2

The symbol for a battery in a circuit diagram. It originated as a schematic drawing of the earliest type of battery, a voltaic pile.

History

Pila di Volta
A voltaic pile, the first battery
Volta-and-napoleon
Italian physicist Alessandro Volta demonstrating his pile to French emperor Napoleon Bonaparte

The usage of "battery" to describe a group of electrical devices dates to Benjamin Franklin, who in 1748 described multiple Leyden jars by analogy to a battery of cannon[6] (Benjamin Franklin borrowed the term "battery" from the military, which refers to weapons functioning together[7]).

Italian physicist Alessandro Volta built and described the first electrochemical battery, the voltaic pile, in 1800.[8] This was a stack of copper and zinc plates, separated by brine-soaked paper disks, that could produce a steady current for a considerable length of time. Volta did not understand that the voltage was due to chemical reactions. He thought that his cells were an inexhaustible source of energy,[9] and that the associated corrosion effects at the electrodes were a mere nuisance, rather than an unavoidable consequence of their operation, as Michael Faraday showed in 1834.[10]

Although early batteries were of great value for experimental purposes, in practice their voltages fluctuated and they could not provide a large current for a sustained period. The Daniell cell, invented in 1836 by British chemist John Frederic Daniell, was the first practical source of electricity, becoming an industry standard and seeing widespread adoption as a power source for electrical telegraph networks.[11] It consisted of a copper pot filled with a copper sulfate solution, in which was immersed an unglazed earthenware container filled with sulfuric acid and a zinc electrode.[12]

These wet cells used liquid electrolytes, which were prone to leakage and spillage if not handled correctly. Many used glass jars to hold their components, which made them fragile and potentially dangerous. These characteristics made wet cells unsuitable for portable appliances. Near the end of the nineteenth century, the invention of dry cell batteries, which replaced the liquid electrolyte with a paste, made portable electrical devices practical.[13]

Principle of operation

ElectrochemCell
A voltaic cell for demonstration purposes. In this example the two half-cells are linked by a salt bridge that permits the transfer of ions.

Batteries convert chemical energy directly to electrical energy. In many cases, the electrical energy released is the difference in the cohesive [14] or bond energies of the metals, oxides, or molecules undergoing the electrochemical reaction.[3] For instance, energy can be stored in Zn or Li, which are high-energy metals because they are not stabilized by d-electron bonding, unlike transition metals. Batteries are designed such that the energetically favorable redox reaction can occur only if electrons move through the external part of the circuit.

A battery consists of some number of voltaic cells. Each cell consists of two half-cells connected in series by a conductive electrolyte containing metal cations. One half-cell includes electrolyte and the negative electrode, the electrode to which anions (negatively charged ions) migrate; the other half-cell includes electrolyte and the positive electrode, to which cations (positively charged ions) migrate. Cations are reduced (electrons are added) at the cathode, while metal atoms are oxidized (electrons are removed) at the anode.[15] Some cells use different electrolytes for each half-cell; then a separator is used to prevent mixing of the electrolytes while allowing ions to flow between half-cells to complete the electrical circuit.

Each half-cell has an electromotive force (emf, measured in volts) relative to a standard. The net emf of the cell is the difference between the emfs of its half-cells.[16] Thus, if the electrodes have emfs and , then the net emf is ; in other words, the net emf is the difference between the reduction potentials of the half-reactions.[17]

The electrical driving force or across the terminals of a cell is known as the terminal voltage (difference) and is measured in volts.[18] The terminal voltage of a cell that is neither charging nor discharging is called the open-circuit voltage and equals the emf of the cell. Because of internal resistance,[19] the terminal voltage of a cell that is discharging is smaller in magnitude than the open-circuit voltage and the terminal voltage of a cell that is charging exceeds the open-circuit voltage.[20] An ideal cell has negligible internal resistance, so it would maintain a constant terminal voltage of until exhausted, then dropping to zero. If such a cell maintained 1.5 volts and produce a charge of one coulomb then on complete discharge it would have performed 1.5 joules of work.[18] In actual cells, the internal resistance increases under discharge[19] and the open-circuit voltage also decreases under discharge. If the voltage and resistance are plotted against time, the resulting graphs typically are a curve; the shape of the curve varies according to the chemistry and internal arrangement employed.

The voltage developed across a cell's terminals depends on the energy release of the chemical reactions of its electrodes and electrolyte. Alkaline and zinc–carbon cells have different chemistries, but approximately the same emf of 1.5 volts; likewise NiCd and NiMH cells have different chemistries, but approximately the same emf of 1.2 volts.[21] The high electrochemical potential changes in the reactions of lithium compounds give lithium cells emfs of 3 volts or more.[22]

Categories and types of batteries

Batteries comparison 4,5 D C AA AAA AAAA A23 9V CR2032 LR44 matchstick-vertical.jpeg
From top to bottom: a large 4.5-volt (3R12) battery, a D Cell, a C cell, an AA cell, an AAA cell, an AAAA cell, an A23 battery, a 9-volt PP3 battery, and a pair of button cells (CR2032 and LR44)

Batteries are classified into primary and secondary forms:

  • Primary batteries are designed to be used until exhausted of energy then discarded. Their chemical reactions are generally not reversible, so they cannot be recharged. When the supply of reactants in the battery is exhausted, the battery stops producing current and is useless.[23]
  • Secondary batteries can be recharged; that is, they can have their chemical reactions reversed by applying electric current to the cell. This regenerates the original chemical reactants, so they can be used, recharged, and used again multiple times.[24]

Some types of primary batteries used, for example, for telegraph circuits, were restored to operation by replacing the electrodes.[25] Secondary batteries are not indefinitely rechargeable due to dissipation of the active materials, loss of electrolyte and internal corrosion.

Primary

Primary batteries, or primary cells, can produce current immediately on assembly. These are most commonly used in portable devices that have low current drain, are used only intermittently, or are used well away from an alternative power source, such as in alarm and communication circuits where other electric power is only intermittently available. Disposable 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.[26] In general, these have higher energy densities than rechargeable batteries,[27] but disposable batteries do not fare well under high-drain applications with loads under 75 ohms (75 Ω). Common types of disposable batteries include zinc–carbon batteries and alkaline batteries.

Secondary

Secondary batteries, also known as secondary cells, or rechargeable batteries, must be charged before first use; they are usually assembled with active materials in the discharged state. Rechargeable batteries are (re)charged by applying electric current, which reverses the chemical reactions that occur during discharge/use. Devices to supply the appropriate current are called chargers.

The oldest form of rechargeable battery is the lead–acid battery, which are widely used in automotive and boating applications. This technology contains liquid electrolyte 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 it produces during overcharging. The lead–acid battery is relatively heavy for the amount of electrical energy it can supply. Its low manufacturing cost and its high surge current levels make it common where its capacity (over approximately 10 Ah) is more important than weight and handling issues. A common application is the modern car battery, which can, in general, deliver a peak current of 450 amperes.

The sealed valve regulated lead–acid battery (VRLA battery) is popular in the automotive industry as a replacement for the lead–acid wet cell. The VRLA battery uses an immobilized sulfuric acid electrolyte, reducing the chance of leakage and extending shelf life.[28] VRLA batteries immobilize the electrolyte. The two types are:

Other portable rechargeable batteries include several sealed "dry cell" types, that are useful in applications such as mobile phones and laptop computers. Cells of this type (in order of increasing power density and cost) include nickel–cadmium (NiCd), nickel–zinc (NiZn), nickel metal hydride (NiMH), and lithium-ion (Li-ion) cells. Li-ion has by far the highest share of the dry cell rechargeable market. NiMH has replaced NiCd in most applications due to its higher capacity, but NiCd remains in use in power tools, two-way radios, and medical equipment.

In the 2000s, developments include batteries with embedded electronics such as USBCELL, which allows charging an AA battery through a USB connector,[29] nanoball batteries that allow for a discharge rate about 100x greater than current batteries, and smart battery packs with state-of-charge monitors and battery protection circuits that prevent damage on over-discharge. Low self-discharge (LSD) allows secondary cells to be charged prior to shipping.

Cell types

Many types of electrochemical cells have been produced, with varying chemical processes and designs, including galvanic cells, electrolytic cells, fuel cells, flow cells and voltaic piles.[30]

Wet cell

A wet cell battery has a liquid electrolyte. Other names are flooded cell, since the liquid covers all internal parts, or vented cell, since gases produced during operation can escape to the air. Wet cells were a precursor to dry cells and are commonly used as a learning tool for electrochemistry. They can be built with common laboratory supplies, such as beakers, for demonstrations of how electrochemical cells work. A particular type of wet cell known as a concentration cell is important in understanding corrosion. Wet cells may be primary cells (non-rechargeable) or secondary cells (rechargeable). Originally, all practical primary batteries such as the Daniell cell were built as open-top glass jar wet cells. Other primary wet cells are the Leclanche cell, Grove cell, Bunsen cell, Chromic acid cell, Clark cell, and Weston cell. The Leclanche cell chemistry was adapted to the first dry cells. Wet cells are still used in automobile batteries and in industry for standby power for switchgear, telecommunication or large uninterruptible power supplies, but in many places batteries with gel cells have been used instead. These applications commonly use lead–acid or nickel–cadmium cells.

Dry cell

Dry cell (PSF)
Line art drawing of a dry cell:
1. brass cap, 2. plastic seal, 3. expansion space, 4. porous cardboard, 5. zinc can, 6. carbon rod, 7. chemical mixture

A dry cell uses a paste electrolyte, with only enough moisture to allow current to flow. Unlike a wet cell, a dry cell can operate in any orientation without spilling, as it contains no free liquid, making it suitable for portable equipment. By comparison, the first wet cells were typically fragile glass containers with lead rods hanging from the open top and needed careful handling to avoid spillage. Lead–acid batteries did not achieve the safety and portability of the dry cell until the development of the gel battery.

A common dry cell is the zinc–carbon battery, sometimes called the dry Leclanché cell, with a nominal voltage of 1.5 volts, the same as the alkaline battery (since both use the same zincmanganese dioxide combination). A standard dry cell comprises a zinc anode, usually in the form of a cylindrical pot, with a carbon cathode in the form of a central rod. The electrolyte is ammonium chloride in the form of a paste next to the zinc anode. The remaining space between the electrolyte and carbon cathode is taken up by a second paste consisting of ammonium chloride and manganese dioxide, the latter acting as a depolariser. In some designs, the ammonium chloride is replaced by zinc chloride.

Molten salt

Molten salt batteries are primary or secondary batteries that use a molten salt as electrolyte. They operate at high temperatures and must be well insulated to retain heat.

Reserve

A reserve battery can be stored unassembled (unactivated and supplying no power) for a long period (perhaps years). When the battery is needed, then it is assembled (e.g., by adding electrolyte); once assembled, the battery is charged and ready to work. For example, a battery for an electronic artillery fuze might be activated by the impact of firing a gun. The acceleration breaks a capsule of electrolyte that activates the battery and powers the fuze's circuits. Reserve batteries are usually designed for a short service life (seconds or minutes) after long storage (years). A water-activated battery for oceanographic instruments or military applications becomes activated on immersion in water.

Cell performance

A battery's characteristics may vary over load cycle, over charge cycle, and over lifetime due to many factors including internal chemistry, current drain, and temperature. At low temperatures, a battery cannot deliver as much power. As such, in cold climates, some car owners install battery warmers, which are small electric heating pads that keep the car battery warm.

Capacity and discharge

Battery checker
A device to check battery voltage

A battery's capacity is the amount of electric charge it can deliver at the rated voltage. The more electrode material contained in the cell the greater its capacity. A small cell has less capacity than a larger cell with the same chemistry, although they develop the same open-circuit voltage.[31] Capacity is measured in units such as amp-hour (A·h). The rated capacity of a battery is usually expressed as the product of 20 hours multiplied by the current that a new battery can consistently supply for 20 hours at 68 °F (20 °C), while remaining above a specified terminal voltage per cell. For example, a battery rated at 100 A·h can deliver 5 A over a 20-hour period at room temperature. The fraction of the stored charge that a battery can deliver depends on multiple factors, including battery chemistry, the rate at which the charge is delivered (current), the required terminal voltage, the storage period, ambient temperature and other factors.[31]

The higher the discharge rate, the lower the capacity.[32] The relationship between current, discharge time and capacity for a lead acid battery is approximated (over a typical range of current values) by Peukert's law:

where

is the capacity when discharged at a rate of 1 amp.
is the current drawn from battery (A).
is the amount of time (in hours) that a battery can sustain.
is a constant around 1.3.

Batteries that are stored for a long period or that are discharged at a small fraction of the capacity lose capacity due to the presence of generally irreversible side reactions that consume charge carriers without producing current. This phenomenon is known as internal self-discharge. Further, when batteries are recharged, additional side reactions can occur, reducing capacity for subsequent discharges. After enough recharges, in essence all capacity is lost and the battery stops producing power.

Internal energy losses and limitations on the rate that ions pass through the electrolyte cause battery efficiency to vary. Above a minimum threshold, discharging at a low rate delivers more of the battery's capacity than at a higher rate. Installing batteries with varying A·h ratings does not affect device operation (although it may affect the operation interval) rated for a specific voltage unless load limits are exceeded. High-drain loads such as digital cameras can reduce total capacity, as happens with alkaline batteries. For example, a battery rated at 2 A·h for a 10- or 20-hour discharge would not sustain a current of 1 A for a full two hours as its stated capacity implies.

C rate

The C-rate is a measure of the rate at which a battery is being charged or discharged. It is defined as the current through the battery divided by the theoretical current draw under which the battery would deliver its nominal rated capacity in one hour.[33] A 1C discharge rate would deliver the battery's rated capacity in 1 hour. A 2C discharge rate means it will discharge twice as fast (30 minutes). A 1C discharge rate on a 1.6 Ah battery means a discharge current of 1.6 A. A 2C rate would mean a discharge current of 3.2 A. Standards for rechargeable batteries generally rate the capacity over a 4-hour, 8 hour or longer discharge time. Because of internal resistance loss and the chemical processes inside the cells, a battery rarely delivers nameplate rated capacity in only one hour. Types intended for special purposes, such as in a computer uninterruptible power supply, may be rated by manufacturers for discharge periods much less than one hour.

The C-rate presents a dimensional error: C is in ampere-hours and not amperes, and one can not express a current in ampere-hours. For this reason the concept It was introduced by the international standard IEC61434,[34] It being equal to the capacity C divided by one hour, hence allowing a mathematically correct method of current designation. The figures used for expressing the discharge rate remain the same: one can speak of "2 It rate" instead of the dimensionally incorrect "2 C rate".

Fast-charging, large and light batteries

As of 2012, lithium iron phosphate (LiFePO
4
) battery technology
was the fastest-charging/discharging, fully discharging in 10–20 seconds.[35]

As of 2017, the world's largest battery was built in South Australia by Tesla. It can store 129 MWh.[36] A battery in Hebei Province, China which can store 36 MWh of electricity was built in 2013 at a cost of $500 million.[37] Another large battery, composed of Ni–Cd cells, was in Fairbanks, Alaska. It covered 2,000 square metres (22,000 sq ft)—bigger than a football pitch—and weighed 1,300 tonnes. It was manufactured by ABB to provide backup power in the event of a blackout. The battery can provide 40 MW of power for up to seven minutes.[38] Sodium–sulfur batteries have been used to store wind power.[39] A 4.4 MWh battery system that can deliver 11 MW for 25 minutes stabilizes the output of the Auwahi wind farm in Hawaii.[40]

Lithium–sulfur batteries were used on the longest and highest solar-powered flight.[41]

Lifetime

Battery life (and its synonym battery lifetime) has two meanings for rechargeable batteries but only one for non-chargeables. For rechargeables, it can mean either the length of time a device can run on a fully charged battery or the number of charge/discharge cycles possible before the cells fail to operate satisfactorily. For a non-rechargeable these two lives are equal since the cells last for only one cycle by definition. (The term shelf life is used to describe how long a battery will retain its performance between manufacture and use.) Available capacity of all batteries drops with decreasing temperature. In contrast to most of today's batteries, the Zamboni pile, invented in 1812, offers a very long service life without refurbishment or recharge, although it supplies current only in the nanoamp range. The Oxford Electric Bell has been ringing almost continuously since 1840 on its original pair of batteries, thought to be Zamboni piles.

Self-discharge

Disposable batteries typically lose 8 to 20 percent of their original charge per year when stored at room temperature (20–30 °C).[42] This is known as the "self-discharge" rate, and is due to non-current-producing "side" chemical reactions that occur within the cell even when no load is applied. The rate of side reactions is reduced for batteries stored at lower temperatures, although some can be damaged by freezing.

Old rechargeable batteries self-discharge more rapidly than disposable alkaline batteries, especially nickel-based batteries; a freshly charged nickel cadmium (NiCd) battery loses 10% of its charge in the first 24 hours, and thereafter discharges at a rate of about 10% a month. However, newer low self-discharge nickel metal hydride (NiMH) batteries and modern lithium designs display a lower self-discharge rate (but still higher than for primary batteries).

Corrosion

Internal parts may corrode and fail, or the active materials may be slowly converted to inactive forms.

Physical component changes

The active material on the battery plates changes chemical composition on each charge and discharge cycle; active material may be lost due to physical changes of volume, further limiting the number of times the battery can be recharged. Most nickel-based batteries are partially discharged when purchased, and must be charged before first use.[43] Newer NiMH batteries are ready to be used when purchased, and have only 15% discharge in a year.[44]

Some deterioration occurs on each charge–discharge cycle. Degradation usually occurs because electrolyte migrates away from the electrodes or because active material detaches from the electrodes. Low-capacity NiMH batteries (1,700–2,000 mA·h) can be charged some 1,000 times, whereas high-capacity NiMH batteries (above 2,500 mA·h) last about 500 cycles.[45] NiCd batteries tend to be rated for 1,000 cycles before their internal resistance permanently increases beyond usable values.

Charge/discharge speed

Fast charging increases component changes, shortening battery lifespan.[45]

Overcharging

If a charger cannot detect when the battery is fully charged then overcharging is likely, damaging it.[46]

Memory effect

NiCd cells, if used in a particular repetitive manner, may show a decrease in capacity called "memory effect".[47] The effect can be avoided with simple practices. NiMH cells, although similar in chemistry, suffer less from memory effect.[48]

2011-04-04 18-35-26 267
An analog camcorder [lithium ion] battery

Environmental conditions

Automotive lead–acid rechargeable batteries must endure stress due to vibration, shock, and temperature range. Because of these stresses and sulfation of their lead plates, few automotive batteries last beyond six years of regular use.[49] Automotive starting (SLI: Starting, Lighting, Ignition) batteries have many thin plates to maximize current. In general, the thicker the plates the longer the life. They are typically discharged only slightly before recharge.

"Deep-cycle" lead–acid batteries such as those used in electric golf carts have much thicker plates to extend longevity.[50] The main benefit of the lead–acid battery is its low cost; its main drawbacks are large size and weight for a given capacity and voltage. Lead–acid batteries should never be discharged to below 20% of their capacity,[51] because internal resistance will cause heat and damage when they are recharged. 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.[52]

Storage

Battery life can be extended by storing the batteries at a low temperature, as in a refrigerator or freezer, which slows the side reactions. Such storage can extend the life of alkaline batteries by about 5%; rechargeable batteries can hold their charge much longer, depending upon type.[53] To reach their maximum voltage, batteries must be returned to room temperature; discharging an alkaline battery at 250 mA at 0 °C is only half as efficient as at 20 °C.[27] Alkaline battery manufacturers such as Duracell do not recommend refrigerating batteries.[26]

Battery sizes

Primary batteries readily available to consumers range from tiny button cells used for electric watches, to the No. 6 cell used for signal circuits or other long duration applications. Secondary cells are made in very large sizes; very large batteries can power a submarine or stabilize an electrical grid and help level out peak loads.

Hazards

Explosion

A battery explosion is generally caused by misuse or malfunction, such as attempting to recharge a primary (non-rechargeable) battery, or a short circuit.

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 battery (e.g. through a built-in vent), leading to pressure build-up and eventual bursting of the battery case. In extreme cases, battery chemicals may spray violently from the casing and cause injury. Overcharging – that is, attempting to charge a battery beyond its electrical capacity – can also lead to a battery explosion, in addition to leakage or irreversible damage. It may also cause damage to the charger or device in which the overcharged battery is later used.

Car batteries are most likely to explode when a short-circuit generates very large currents. Such batteries produce hydrogen, which is very explosive, when they are overcharged (because of electrolysis of the water in the electrolyte). During normal use, the amount of overcharging is usually very small and generates little hydrogen, which dissipates quickly. However, when "jump starting" a car, the high current can cause the rapid release of large volumes of hydrogen, which can be ignited explosively by a nearby spark, e.g. when disconnecting a jumper cable.

Disposing of a battery via incineration may cause an explosion as steam builds up within the sealed case.

Recalls of devices using Lithium-ion batteries have become more common in recent years. This is in response to reported accidents and failures, occasionally ignition or explosion.[54][55] An expert summary of the problem indicates that this type uses "liquid electrolytes to transport lithium ions between the anode and the cathode. If a battery cell is charged too quickly, it can cause a short circuit, leading to explosions and fires".[56][57]

Leakage

LeakedBattery 2701a
Leak-damaged alkaline battery

Many battery chemicals are corrosive, poisonous or both. If leakage occurs, either spontaneously or through accident, the chemicals released may be dangerous. For example, disposable batteries often use a zinc "can" both as a reactant and as the container to hold the other reagents. If this kind of battery is over-discharged, the reagents can emerge through the cardboard and plastic that form the remainder of the container. The active chemical leakage can then damage or disable the equipment that the batteries power. For this reason, many electronic device manufacturers recommend removing the batteries from devices that will not be used for extended periods of time.

Toxic materials

Many types of batteries employ toxic materials such as lead, mercury, and cadmium as an electrode or electrolyte. When each battery reaches end of life it must be disposed of to prevent environmental damage.[58] Batteries are one form of electronic waste (e-waste). E-waste recycling services recover toxic substances, which can then be used for new batteries.[59] Of the nearly three billion batteries purchased annually in the United States, about 179,000 tons end up in landfills across the country.[60] In the United States, the Mercury-Containing and Rechargeable Battery Management Act of 1996 banned the sale of mercury-containing batteries, enacted uniform labeling requirements for rechargeable batteries and required that rechargeable batteries be easily removable.[61] California and New York City prohibit the disposal of rechargeable batteries in solid waste, and along with Maine require recycling of cell phones.[62] The rechargeable battery industry operates nationwide recycling programs in the United States and Canada, with dropoff points at local retailers.[62]

The Battery Directive of the European Union has similar requirements, in addition to requiring increased recycling of batteries and promoting research on improved battery recycling methods.[63] In accordance with this directive all batteries to be sold within the EU must be marked with the "collection symbol" (a crossed-out wheeled bin). This must cover at least 3% of the surface of prismatic batteries and 1.5% of the surface of cylindrical batteries. All packaging must be marked likewise.[64]

Ingestion

Batteries may be harmful or fatal if swallowed.[65] Small button cells can be swallowed, in particular by young children. While in the digestive tract, the battery's electrical discharge may lead to tissue damage;[66] such damage is occasionally serious and can lead to death. Ingested disk batteries do not usually cause problems unless they become lodged in the gastrointestinal tract. The most common place for disk batteries to become lodged is the esophagus, resulting in clinical sequelae. Batteries that successfully traverse the esophagus are unlikely to lodge elsewhere. The likelihood that a disk battery will lodge in the esophagus is a function of the patient's age and battery size. Disk batteries of 16 mm have become lodged in the esophagi of 2 children younger than 1 year. Older children do not have problems with batteries smaller than 21–23 mm. Liquefaction necrosis may occur because sodium hydroxide is generated by the current produced by the battery (usually at the anode). Perforation has occurred as rapidly as 6 hours after ingestion.[67]

Chemistry

Many important cell properties, such as voltage, energy density, flammability, available cell constructions, operating temperature range and shelf life, are dictated by battery chemistry.

Primary batteries and their characteristics

Chemistry Anode (−) Cathode (+) Max. voltage, theoretical (V) Nominal voltage, practical (V) Specific energy (MJ/kg) Elaboration Shelf life at 25 °C, 80% capacity (months)
Zinc–carbon Zn MnO2 1.6 1.2 0.13 Inexpensive. 18
Zinc–chloride 1.5 Also known as "heavy-duty", inexpensive.
Alkaline
(zinc–manganese dioxide)
Zn MnO2 1.5 1.15 0.4–0.59 Moderate energy density.
Good for high- and low-drain uses.
30
Nickel oxyhydroxide
(zinc–manganese dioxide/nickel oxyhydroxide)
1.7 Moderate energy density.
Good for high drain uses.
Lithium
(lithium–copper oxide)
Li–CuO
Li CuO 1.7 No longer manufactured.
Replaced by silver oxide (IEC-type "SR") batteries.
Lithium
(lithium–iron disulfide)
LiFeS2
Li FeS2 1.8 1.5 1.07 Expensive.
Used in 'plus' or 'extra' batteries.
337[68]
Lithium
(lithium–manganese dioxide)
LiMnO2
Li MnO2 3.0 0.83–1.01 Expensive.
Used only in high-drain devices or for long shelf-life due to very low rate of self-discharge.
'Lithium' alone usually refers to this type of chemistry.
Lithium
(lithium–carbon fluoride)
Li–(CF)n
Li (CF)n 3.6 3.0 120
Lithium
(lithium–chromium oxide)
Li–CrO2
Li CrO2 3.8 3.0 108
Lithium

(lithium-silicon)

Li22Si5
Mercury oxide Zn HgO 1.34 1.2 High-drain and constant voltage.
Banned in most countries because of health concerns.
36
Zinc–air Zn O2 1.6 1.1 1.59[69] Used mostly in hearing aids.
Zamboni pile Zn Ag or Au 0.8 Very long life
Very low (nanoamp, nA) current
>2,000
Silver-oxide (silver–zinc) Zn Ag2O 1.85 1.5 0.47 Very expensive.
Used only commercially in 'button' cells.
30
Magnesium Mg MnO2 2.0 1.5 40

Secondary (rechargeable) batteries and their characteristics

Chemistry Cell
voltage
Specific
energy

(kJ/kg)
Energy
density

(kJ/liter)
Comments
NiCd 1.2 140 Nickel–cadmium chemistry.
Inexpensive.
High-/low-drain, moderate energy density.
Can withstand very high discharge rates with virtually no loss of capacity.
Moderate rate of self-discharge.
Environmental hazard due to Cadmium – use now virtually prohibited in Europe.
Lead–acid 2.1 140 Moderately expensive.
Moderate energy density.
Moderate rate of self-discharge.
Higher discharge rates result in considerable loss of capacity.
Environmental hazard due to Lead.
Common use – Automobile batteries
NiMH 1.2 360 Nickel–metal hydride chemistry.
Inexpensive.
Performs better than alkaline batteries in higher drain devices.
Traditional chemistry has high energy density, but also a high rate of self-discharge.
Newer chemistry has low self-discharge rate, but also a ~25% lower energy density.
Used in some cars.
NiZn 1.6 360 Nickel-zinc chemistry.
Moderately inexpensive.
High drain device suitable.
Low self-discharge rate.
Voltage closer to alkaline primary cells than other secondary cells.
No toxic components.
Newly introduced to the market (2009). Has not yet established a track record.
Limited size availability.
AgZn 1.86
1.5
460 Silver-zinc chemistry.
Smaller volume than equivalent Li-ion.
Extremely expensive due to silver.
Very high energy density.
Very high drain capable.
For many years considered obsolete due to high silver prices.
Cell suffers from oxidation if unused.
Reactions are not fully understood.
Terminal voltage very stable but suddenly drops to 1.5 volts at 70–80% charge (believed to be
due to presence of both argentous and argentic oxide in positive plate – one is consumed first).
Has been used in lieu of primary battery (moon buggy).
Is being developed once again as a replacement for Li-ion.
LiFePO4 3.3
3.0
360 790 Lithium-Iron-Phosphate chemistry.
Lithium ion 3.6 460 Various lithium chemistries.
Very expensive.
Very high energy density.
Not usually available in "common" battery sizes.
Lithium polymer battery is common in laptop computers, digital cameras, camcorders, and cellphones.
Very low rate of self-discharge.

Terminal voltage varies from 4.2 to 3.0 volts during discharge.
Volatile: Chance of explosion if short-circuited, allowed to overheat, or not manufactured with rigorous quality standards.

Solid state batteries

On 28 February 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 Lithium-ion (Li-Ion) inventor John Goodenough, "that could lead to safer, faster-charging, longer-lasting rechargeable batteries for handheld mobile devices, electric cars and stationary energy storage".[70] More specifics about the new technology were published in the peer-reviewed scientific journal Energy & Environmental Science.

Independent reviews of the technology discuss the risk of fire and explosion from Lithium-ion batteries under certain conditions because they use liquid electrolytes. The newly developed battery should be safer since it uses glass electrolytes, that should eliminate short circuits. The solid-state battery is also said to have "three times the energy density" increasing its useful life in electric vehicles, for example. It should also be more ecologically sound since the technology uses less expensive, earth-friendly materials such as sodium extracted from seawater. They also have much longer life; ("the cells have demonstrated more than 1,200 cycles with low cell resistance"). The research and prototypes are not expected to lead to a commercially viable product in the near future, if ever, according to Chris Robinson of LUX Research. "This will have no tangible effect on electric vehicle adoption in the next 15 years, if it does at all. A key hurdle that many solid-state electrolytes face is lack of a scalable and cost-effective manufacturing process," he told The American Energy News in an e-mail.[71]

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,[72] potato,[73] etc. and generate small amounts of electricity. "Two-potato clocks" are also widely available in hobby and toy stores; they consist of a pair of cells, each consisting of a potato (lemon, et cetera) with two electrodes inserted into it, wired in series to form a battery with enough voltage to power a digital clock.[74] Homemade cells of this kind are of no practical use.

A voltaic pile can be made from two coins (such as a nickel and a penny) and a piece of paper towel dipped in salt water. Such a pile generates a very low voltage but, when many are stacked in series, they can replace normal batteries for a short time.[75]

Sony has developed a biological battery that generates electricity from sugar in a way that is similar to the processes observed in living organisms. The battery generates electricity through the use of enzymes that break down carbohydrates.[76]

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 in which 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, increasing the surface area, increasing the current the cell can deliver.[77]

Daniell cells are easy to make at home. Aluminium–air batteries can be produced with high-purity aluminium. Aluminium foil batteries will produce some electricity, but are not efficient, in part because a significant amount of (combustible) hydrogen gas is produced.

See also

References

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Further reading

  • Dingrando, Laurel; et al. (2007). Chemistry: Matter and Change. New York: Glencoe/McGraw-Hill. ISBN 978-0-07-877237-5. Ch. 21 (pp. 662–695) is on electrochemistry.
  • Fink, Donald G.; H. Wayne Beaty (1978). Standard Handbook for Electrical Engineers, Eleventh Edition. New York: McGraw-Hill. ISBN 978-0-07-020974-9.
  • Knight, Randall D. (2004). Physics for Scientists and Engineers: A Strategic Approach. San Francisco: Pearson Education. ISBN 978-0-8053-8960-9. Chs. 28–31 (pp. 879–995) contain information on electric potential.
  • Linden, David; Thomas B. Reddy (2001). Handbook of Batteries. New York: McGraw-Hill. ISBN 978-0-07-135978-8.
  • Saslow, Wayne M. (2002). Electricity, Magnetism, and Light. Toronto: Thomson Learning. ISBN 978-0-12-619455-5. Chs. 8–9 (pp. 336–418) have more information on batteries.

External links

Alessandro Volta

Alessandro Giuseppe Antonio Anastasio Volta (Italian: [alesˈsandro ˈvɔlta]; 18 February 1745 – 5 March 1827) was an Italian physicist, chemist, and a pioneer of electricity and power, who is credited as the inventor of the electric battery and the discoverer of methane. He invented the Voltaic pile in 1799, and reported the results of his experiments in 1800 in a two-part letter to the President of the Royal Society. With this invention Volta proved that electricity could be generated chemically and debunked the prevalent theory that electricity was generated solely by living beings. Volta's invention sparked a great amount of scientific excitement and led others to conduct similar experiments which eventually led to the development of the field of electrochemistry.Alessandro Volta also drew admiration from Napoleon Bonaparte for his invention, and was invited to the Institute of France to demonstrate his invention to the members of the Institute. Volta enjoyed a certain amount of closeness with the Emperor throughout his life and he was conferred numerous honours by him. Alessandro Volta held the chair of experimental physics at the University of Pavia for nearly 40 years and was widely idolised by his students.Despite his professional success, Volta tended to be a person inclined towards domestic life and this was more apparent in his later years. At this time he tended to live secluded from public life and more for the sake of his family until his eventual death in 1827 from a series of illnesses which began in 1823. The SI unit of electric potential is named in his honour as the volt.

All-electric range

All-electric range (AER) is the driving range of a vehicle using only power from its electric battery pack to traverse a given driving cycle. In the case of a battery electric vehicle, it means the total range per charge. For a plug-in hybrid (PHEV), it means the range of the vehicle in charge-depleting mode. PHEVs can travel considerably further in charge-sustaining mode which uses both on-board fuel and the battery pack.

Calculating AER is made more complicated because of variations in PHEV design. A vehicle like the Fisker Karma that uses a serial hybrid design has a clear AER. Similarly a vehicle like the Chevrolet Volt which disengages the internal combustion engine (ICE) from the drive train while in electric mode has a clear AER, however blended mode PHEVs which use the ICE and electric motor in conjunction do not have a clear AER because they use gasoline and grid provided electricity at the same time. Equivalent AER is the AER of vehicles following this architecture. One example of this calculation can be found in Argonne National Labs report titled "TEST PROCEDURES AND BENCHMARKING Blended-Type and EV-Capable Plug-In Hybrid Electric Vehicles."

This procedure uses the formula below to calculate an equivalent AER for vehicles that operate in blended mode:

Where GPMCD designates efficiency in charge-depleting mode, and GPMCS charge-sustaining mode as designated and dCD is distance in charge depleting mode.

A plug-in hybrid's all-electric range is designated by PHEV-(miles) or PHEV(kilometers)km representing the distance the vehicle can travel on battery power alone. For example, a PHEV-20 can travel 20 miles without using its internal combustion engine, or about 32 kilometers, so it may also be designated as PHEV32km.

Battery Energy Drink

Battery is a Finnish energy drink. Its stimulating effects are based on coffee and guarana extracts, as well as taurine. The drink is yellow, sparkly and sweetish.

Battery’s owner and manufacturer is Oy Sinebrychoff Ab, which is part of the international brewery group Carlsberg Breweries A/S. It was launched in 1997 and is currently being sold in over 35 countries.The basic idea of the brand is the energy-containing battery. The package is designed to imitate the appearance of an electric battery. “Keeps you going” is the brand's slogan.

Battery electric vehicle

A battery electric vehicle (BEV), pure electric vehicle, only-electric vehicle or all-electric vehicle is a type of electric vehicle (EV) that uses chemical energy stored in rechargeable battery packs. BEVs use electric motors and motor controllers instead of internal combustion engines (ICEs) for propulsion. They derive all power from battery packs and thus have no internal combustion engine, fuel cell, or fuel tank. BEVs include - but are not limited to - motorcycles, bicycles, scooters, skateboards, rail cars, watercraft, forklifts, buses, trucks, and cars.

In 2016 there were 210 million electric bikes worldwide used daily. Cumulative global sales of highway-capable light-duty pure electric car vehicles passed the one million unit milestone in September 2016. As of April 2018, the world's top selling highway legal all-electric car in history is the Nissan Leaf with global sales of over 300,000 units, followed by the Tesla Model S with more than 200,000 units delivered worldwide.

Cobalt oxide nanoparticle

In materials and electric battery research, cobalt oxide nanoparticles usually refers to particles of cobalt(II,III) oxide Co3O4 of nanometer size, with various shapes and crystal structures.

Cobalt oxide nanoparticles have potential applications in lithium-ion batteries and electronic gas sensors.

Concept Two

Concept Two, concept ii, CONCEPT 2, or variation, may refer to:

Concept2, a rowing machine manufacturer

Rimac Concept Two, an all-electric battery-powered hypercar

AMC Concept II, a concept car proposed as a replacement for the Gremlin

Deep-submergence vehicle

A deep-submergence vehicle (DSV) is a deep-diving manned submarine that is self-propelled. Several navies operate vehicles that can be accurately described as DSVs. DSVs are commonly divided into two types: research DSVs, which are used for exploration and surveying, and DSRVs (Deep Submergence Rescue Vehicle), which can be used for rescuing the crew of a sunken navy submarine, clandestine (espionage) missions (primarily installing wiretaps on undersea cables), or both. DSRVs are equipped with docking chambers to allow personnel ingress and egress via a manhole.

The real-life feasibility of any DSRV-based rescue attempt is hotly debated, because the few available docking chambers of a stricken submarine may be flooded, trapping the sailors still alive in other dry compartments. The only attempt to rescue a stricken submarine with these so far (the Russian submarine Kursk) ended in failure as the entire crew who survived the explosion had either suffocated or burned to death before the rescuers could get there. Because of these difficulties, the use of integrated crew escape capsules, detachable conning towers, or both have gained favour in military submarine design during the last two decades. DSRVs that remain in use are primarily relegated to clandestine missions and undersea military equipment maintenance. The rapid development of safe, cost-saving ROV technology has also rendered some DSVs obsolete.

Strictly speaking, bathyscaphes are not submarines because they have minimal mobility and are built like a balloon, using a habitable spherical pressure vessel hung under a liquid hydrocarbon filled float drum. In a DSV/DSRV, the passenger compartment and the ballast tank functionality is incorporated into a single structure to afford more habitable space (up to 24 people in the case of a DSRV).

Most DSV/DSRV vehicles are powered by traditional electric battery propulsion and have very limited endurance. Plans have been made to equip DSVs with LOX Stirling engines but none have been realized so far due to cost and maintenance considerations. All DSVs are dependent upon a surface support ship or a mother submarine, that can piggyback or tow them (in case of the NR-1) to the scene of operations. Some DSRV vessels are air transportable in very large military cargo planes to speed up deployment in case of emergency rescue missions.

Dry cell

A dry cell is a type of electric battery, commonly used for portable electrical devices. It was developed in 1886 by the German scientist Carl Gassner, after development of wet zinc-carbon batteries by Georges Leclanché in 1866. The modern version was developed by Japanese Yai Sakizo in 1887.

A dry cell uses a paste electrolyte, with only enough moisture to allow current to flow. Unlike a wet cell, a dry cell can operate in any orientation without spilling, as it contains no free liquid, making it suitable for portable equipment. By comparison, the first wet cells were typically fragile glass containers with lead rods hanging from the open top and needed careful handling to avoid spillage. Lead–acid batteries did not achieve the safety and portability of the dry cell until the development of the gel battery. Wet cells have continued to be used for high-drain applications, such as starting internal combustion engines, because inhibiting the electrolyte flow tends to reduce the current capability.

A common dry cell is the zinc-carbon cell, sometimes called the dry Leclanché cell, with a nominal voltage of 1.5 volts, the same as the alkaline cell (since both use the same zinc–manganese dioxide combination).

A standard dry cell comprises a zinc anode, usually in the form of a cylindrical pot, with a carbon cathode in the form of a central rod. The electrolyte is ammonium chloride in the form of a paste next to the zinc anode. The remaining space between the electrolyte and carbon cathode is taken up by a second paste consisting of ammonium chloride and manganese dioxide, the latter acting as a depolariser. In some designs, often marketed as "heavy duty", the ammonium chloride is replaced with zinc chloride.

Eveready Battery Company

Eveready Battery Company, Inc. is an American manufacturer of electric battery brands Eveready and Energizer, owned by Energizer Holdings. It should not be confused with the almost identically named and defunct UK battery company, Ever Ready. Its headquarters are located in St. Louis, Missouri. The predecessor company began in 1890 in New York and was renamed in 1905. Today the company makes batteries in the United States and China, and production facilities around the world.

Giuseppe Zamboni

Giuseppe Zamboni (June 1, 1776 – July 25, 1846) was an Italian Roman Catholic priest and physicist who invented the Zamboni pile, an early electric battery similar to the voltaic pile.

Glenside Museum

Glenside Museum is situated within the Glenside Campus of the University of the West of England in Fishponds, Bristol, England.

The museum was founded by Dr Donal F. Early; a consultant psychiatrist at Glenside Hospital from the 1950s. He collected items of memorabilia and started a collection on the balcony of the dining hall of Glenside. When the building closed, the collection was re-located to the Glenside Chapel, and the collection slowly was built up to the museum it is today. The chapel was built in 1861 and is a grade II listed building. The museums collection consists of a wide range of paraphernalia and images from the life of Glenside Hospital (previously known as the Bristol Lunatic Asylum, Beaufort War Hospital in World War I, then Bristol Mental Hospital) and of the local Learning disability Hospitals of the Stoke Park Group and the Burden Neurological Institution. The museum has drawings and paintings by the accomplished artist Dennis Reed who painted images of life at Glenside during the 1950s. These painting are located in the chancel. The museum charges no entrance fee, but depends on donations from the public.

Exhibits include several early Electroconvulsive therapy (ECT) machines.

One of the most celebrated workers at the former Bristol Lunatic Asylum was the painter Stanley Spencer (later Sir Stanley Spencer RA CBE) who worked there in 1915–1916 as medical orderly in the Royal Army Medical Corps. During the Great War the asylum was turned over to military use and renamed the Beaufort War Hospital. It had to accommodate some 1,460 wounded soldiers at any one time, usually more. A number of the patients were retained to perform menial duties. As is recounted in Paul Gough's book, Journey to Burghclere Spencer had a difficult time in the hospital, leavened by moments of quiet reverie, as the painter wrote of his second day:

"I had to scrub out the Asylum Church. It was a splendid test of my feelings about this war. And I still feel the necessity of the war, & I have seen some sights, but not what one might expect. The lunatics are good workers & one persists in saluting us & always with the wrong hand. Another one thinks he is an electric battery... "On 14 December 2009, on the 50th anniversary of Spencer's death the University of the West of England — who now own the hospital building — held a celebratory event to unveil a series of artwork and a blue plaque remembering the painter's time in the vast teeming metropolis of the Beaufort.

Ground propulsion

Ground propulsion is any mechanism for propelling solid bodies along the ground, usually for the purposes of transportation. The propulsion system often consists of a combination of an engine or motor, a gearbox and wheel and axles (or caterpillar tracks) in standard applications.

The primary and most natural type of propulsion is the use of muscle power. The invention of the wheel allowed for the development of vehicles like Carts and Wagons that make more efficient use of muscle power, allowing larger loads to be transported. Vehicles drawn by humans and domesticated animals are not economically as important as they once were, but they still exist. Examples of human-powered vehicles are rickshaws and cycle rickshaws.

The development of the steam engine and internal combustion engine allowed for the development of rail vehicles and motor vehicles, all of which have some form of a powertrain. The electric motor allowed for quieter vehicles with lower emissions, and frequently higher engine efficiency.

Some less commonly used or experimental engines are:

Turbines

Stirling engines

Fuel cells

Marine propulsion

Marine propulsion is the mechanism or system used to generate thrust to move a ship or boat across water. While paddles and sails are still used on some smaller boats, most modern ships are propelled by mechanical systems consisting of an electric motor or engine turning a propeller, or less frequently, in pump-jets, an impeller. Marine engineering is the discipline concerned with the engineering design process of marine propulsion systems.

Manpower, in the form of paddles, and sail were the first forms of marine propulsion. Rowed galleys, some equipped with sail, also played an important early role. The first advanced mechanical means of marine propulsion was the

marine steam engine, introduced in the early 19th century. During the 20th century it was replaced by two-stroke or four-stroke diesel engines, outboard motors, and gas turbine engines on faster ships. Marine nuclear reactors, which appeared in the 1950s, produce steam to propel warships and icebreakers; commercial application, attempted late that decade, failed to catch on. Electric motors using electric battery storage have been used for propulsion on submarines and electric boats and have been proposed for energy-efficient propulsion.Development in liquefied natural gas (LNG) fueled engines are gaining recognition for their low emissions and cost advantages. Stirling engines, which are more efficient, quieter, smoother running producing less harmful emissions than diesel engines, propel a number of small submarines. Its design has yet to be upscaled for larger surface ships.

Science and technology in Italy

Science and technology in Italy has a long presence, from the Roman era and the Renaissance. Through the centuries, Italy has advanced the scientific community which produced many significant inventions and discoveries in biology, physics, chemistry, mathematics, astronomy and the other sciences.

Skateboard

A skateboard is a type of sports equipment used primarily for the sport of skateboarding. It usually consists of a specially designed maplewood board combined with a polyurethane coating used for making smoother slides and stronger durability. Most skateboards are made with 7 plies of this wood.

A skateboard is moved by pushing with one foot while the other remains on the board, or by pumping one's legs in structures such as a bowl or half pipe. A skateboard can also be used by simply standing on the deck while on a downward slope and allowing gravity to propel the board and rider. If the rider's leading foot is their right foot, they are said to ride "goofy;" if the rider's leading foot is their left foot, they are said to ride "regular." If the rider is normally regular but chooses to ride goofy, they are said to be riding in "switch," and vice versa. A skater is typically more comfortable pushing with their back foot; choosing to push with the front foot is commonly referred to as riding "mongo", and has negative connotations of style and effectiveness in the skateboarding community.

Recently, electric skateboards have also appeared. These no longer require the propelling of the skateboard by means of the feet; rather an electric motor propels the board, fed by an electric battery.

There is no governing body that declares any regulations on what constitutes a skateboard or the parts from which it is assembled. Historically, the skateboard has conformed both to contemporary trends and to the ever-evolving array of stunts performed by riders/users, who require a certain functionality from the board. The board shape depends largely upon its desired function. Longboards are a type of skateboard with a longer wheelbase and larger, softer wheels.

The two main types of skateboards are the longboard and the shortboard. The shape of the board is also important: the skateboard must be concaved to perform tricks. Longboards are usually faster and are mostly used for cruising and racing, while shortboards are mostly used for doing tricks and riding in skateparks.

Stefan Drzewiecki

Stefan Drzewiecki (Russian: Джеве́цкий Степа́н Ка́рлович (Казими́рович); 26 July 1844, Kunka, Podolia, Russian Empire (today Ukraine) – 23 April 1938, Paris) was a Polish and Russian scientist, journalist, engineer, constructor and inventor, working in France and the Russian Empire. He built the first submarine in the world with electric battery-powered propulsion (1884).

Super-iron battery

The Super-iron battery is a moniker for a proposed class of rechargeable electric battery. Such batteries feature cathodes composed of ferrate salts, either potassium ferrate (K2FeO4) or barium ferrate (BaFeO4). One attraction to the proposed device is that the spent cathode would consist of a rust-like material, which is preferable to batteries based on cadmium, manganese and nickel.

Tesla Roadster (2020)

The Tesla Roadster is an upcoming all-electric battery-powered four-seater sports car made by Tesla, Inc. Tesla has said it will be capable of 0 to 60 mph (0 to 97 km/h) in 1.9 seconds and 0 to 100 km/h (0 to 62 mph) in 2.1 seconds, quicker than any street legal production car to date at its announcement in November 2017. The Roadster is the successor to Tesla's first production car, which was the 2008 Roadster.

Tesla indicates that Roadster sales will begin in 2020, although not before the Tesla Model Y goes on sale. Elon Musk has said that higher-performance trim levels will be available beyond the base specifications.

Zamboni pile

The Zamboni pile (also referred to as a Duluc Dry Pile) is an early electric battery, invented by Giuseppe Zamboni in 1812.

A Zamboni pile is an "electrostatic battery" and is constructed from discs of silver foil, zinc foil, and paper. Alternatively, discs of "silver paper" (paper with a thin layer of zinc on one side) gilded on one side or silver paper smeared with manganese oxide and honey might be used. Discs of approximately 20 mm diameter are assembled in stacks, which may be several thousand discs thick, and then either compressed in a glass tube with end caps or stacked between three glass rods with wooden end plates and insulated by dipping in molten sulfur or pitch.Zamboni piles of more modern construction were manufactured as recently as the 1980s for providing the accelerating voltage for image intensifier tubes, particularly in military use. Today such voltages are obtained from transistorised inverter circuits powered by conventional (low-voltage) batteries.

The EMF per element is approximately 0.8 volts; with thousands of stacked elements, Zamboni piles have output potential differences in the kilovolt range, but current output in the nanoampere range. The famous Oxford Electric Bell, which has been ringing continuously since 1840, is thought to be powered by a pair of Zamboni piles.

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