Batteries
today
Two hundred years after Volta's
invention of the first electrochemical power source, Ron Dell reviews progress
in battery technology
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Battery specifications |
|
High
cell voltage and stable voltage plateau over most of the discharge
High
stored energy content per unit mass (Wh kg1) and per unit
volume (Wh dm3)
Low
cell resistance (milliohms)
High
peak power output per unit mass (W kg1) and per unit volume (W
dm3)
High
sustained power output
Wide
temperature range of operation
Long
inactive shelf-life (years)
Long
operational life
Low
initial cost
Reliable in use
Sealed and leak-proof
Rugged and resistant to abuse
Safe
in use and under accident conditions
Made
of readily available materials that are environmentally benign
Suitable for recycling
Secondary batteries
High
electrical efficiency (Wh output/Wh input)
Capable of many chargedischarge cycles
Ability to accept fast recharge
Will
withstand overcharge and overdischarge
Sealed and maintenance-free |
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The year 2000 is the bicentenary of
Volta's pile, the first source of continuous or current electricity. From small
beginnings, the applications for portable electrical power have mushroomed in
recent years. Sixty years ago domestic uses for batteries were largely confined
to flashlamps, radio sets and starter batteries for cars and motorcycles.
Modern households typically have 40-50, hidden away in all sorts of consumer
products - from clocks and watches to personal CD players and mobile phones.
Away from the home there are many other applications, particularly for large
batteries. Examples include the standby batteries for emergency use in
hospitals, hotels, department stores, telephone exchanges etc; traction
batteries for electric vehicles (tugs, tractors, forklift trucks, wheelchairs,
golf carts); batteries for solar panels or wind generators; defence batteries
in armaments, missiles, submarines, torpedos. Many of these applications demand
a performance that is barely matched by traditional batteries - which explains
the ever-present demand for new and better varieties.
Batteries are of two general types:
primary cells that are discharged once and then discarded and secondary
batteries that are recharged and used again. One of the interesting features of
batteries is the very wide range of sizes in which they are manufactured, from
a stored energy content of ca 0.1 watt-hour (Wh) for a watch or
calculator battery, to 100MWh for a load-levelling battery in the electrical
supply industry (Table 1). Can there be any other industry in which
products are produced in such a size range? Estimating the market for batteries
is notoriously difficult. In 1991 the world battery market was estimated at
US$21,000m, with 40 per cent by value attributable to primary batteries and 60
per cent secondaries. Undoubtedly, the market has grown since then. A more
recent (1999) estimate of the Japanese market is ca US$8000m, of which
25 per cent is due to primary cells and 75 per cent to secondary
batteries.1 Even if these figures are only
approximate, this is clearly a major industry worldwide.
Table 1. Battery sizes and applications |
|
Battery type |
Stored energy/Wh |
Applications |
Miniature/button cells |
0.1-5 |
Watches, calculators, heart pacemakers |
Portable communications |
2-100 |
Mobile phones, laptops |
Domestic uses |
2-100 |
Portable radio and TV, flashlamps, toys, video
cameras, powertools |
Automotive |
102-103 |
Starting batteries for cars, trucks, buses, boats
etc. Traction batteries for lawnmowers, golfcarts, invalid chairs
etc |
Remote area power supply |
103-105 |
Lighting, water pimping, telecommunications
etc |
Traction |
104-106 |
Electric vehicles, forklift trucks, tractors,
torpedoes |
Stationary |
104-106 |
Standby batteries, un-interruptable power supply
(UPS) |
Submarine |
106-107 |
Underwater propulsion |
Load levelling |
107-108 |
Electicity supply industry, load levelling, peak
shaving, spinning reserve |
Battery addicts
Someone once described a battery as
'a livelihood to the manufacturer, an irritation to the user and an addiction
to the researcher'. If the latter attribute is true of primary batteries, how
much more so is it for rechargable batteries where the technical challenge of
developing a battery capable of being charge-discharge cycled hundreds or
thousands of times is formidable. And we must meet this goal within a framework
of producing a product that is economically viable, safe to use and
environmentally friendly.
The Box above sets out in
more detail the specifications sought in a battery. The problem (and the
challenge) of developing new and better batteries lies in the complexity of
this specification. Not only are there some 20 criteria for a secondary
battery, but these are often highly interactive. For example, the available
stored energy and the peak power output both depend on the temperature; the
peak power also depends on the state of charge of the battery; the
charge-discharge cycle life of a secondary battery depends critically on the
depth to which it is discharged in each cycle, and so on. All of these factors
need to be quantified before we can decide whether a battery is likely to be
commercially viable for a particular application. However, key factors are the
stored energy per unit mass and volume and it is here that modern batteries,
such as lithium-based batteries, come into their own.
Smooth operation
How does a battery operate? A
battery is basically a simple electrochemical device to store electrical energy
as chemicals. It has certain essential components. The negative electrode
consists of a current collector and an active component, often a metal such as
finely divided zinc, lead or cadmium, which is capable of being oxidised with
the release of electrons. The positive electrode also consists of a metallic
current collector and an active component, generally a higher valent metallic
oxide (eg MnO2, PbO2, NiOOH, AgO) that is capable of being reduced. The
electrodes are separated by an electrolyte that conducts ions, but which must
be an electronic insulator to avoid internal short-circuits.
|
Fig 1. Discharging an electrochemical cell |
In most conventional batteries the
electrolyte is an aqueous solution such as ZnCl2, KOH or H2SO4, although some
advanced batteries use ion-conducting ceramics, polymers or molten salts.
During discharge, electrons flow from the negative electrode to the positive
via this 'external load', thereby doing electrical work.
The charging of a secondary battery
is the reverse of discharging (Fig 1). Given the apparent simplicity
of this scheme, and the wide range of elements to choose from in the Periodic
Table, at first sight it is a puzzle why developing new batteries has proved to
be so difficult. Indeed, it seems ludicrous when considering the sophistication
of the microchip in a modern laptop computer that the simple battery should be
the largest and heaviest component. It is the complex and demanding user
specification (see above) that poses the challenge. The more the
specification can be relaxed for a particular application, the better the
chance of meeting it.
Primary batteries
By far the most common primary cells
are based on the zinc-manganese dioxide couple, either so-called zinc-carbon
cells (Leclanché cells) or alkaline manganese cells. These both give
1.5V open circuit, but differ in a number of important respects. Zinc-carbon
cells (Fig 2a) have a central carbon current collector immersed in the
positive cathode (a mixture of impure MnO2
and carbon), a container of metallic zinc as the anode, and an electrolyte of
aqueous NH4Cl and/or ZnCl2. These cells are traditional and
inexpensive.
Alkaline manganese cells (Fig
2b), a superior and more expensive product, use finely divided zinc powder
as the anode and this fills the centre of the cell, with a brass pin to make
contact with the base. The electrolyte is concentrated KOH solution and the
cathode material - a mix of chemically or electrochemically prepared
MnO2 and carbon - forms a concentric annulus
around the zinc powder and the separator. Alkaline manganese cells have a long
shelf life and are particularly useful for high drain (power) applications,
where their useful life is several times that of zinc-carbon.
|
Fig 2. (a) Zinc-carbon battery; (b) Alkaline
manganese dioxide battery |
The cheaper zinc-carbon cells are
adequate for low drain applications and for intermittent use (such as in
flashlights) where there is recovery time between uses, to allow diffusion
processes to remove polarisation at the electrodes and restore equilibrium.
Both types of cell are made by most manufacturers in a variety of standard
sizes and shapes. The prismatic 9V cells, as used in smoke detectors, contain
six small cells wired in series.
Several manufacturers are now
offering 3V lithium-MnO2 cells. These employ
a lithium foil negative and an ion-conducting organic electrolyte. They are
available as cylindrical cells, using spiral-wound electrodes ('jelly roll'
configuration), or as button cells. Their advantages include high gravimetric
and volumetric energy densities, high pulse rate capability, long shelf life
and the ability to operate over a wide temperature range (-40°C to
+60°C).
Button and coin cells are used
widely in watches and pocket calculators. They may be either alkaline manganese
cells (1.5V), zinc-silver oxide cells (1.5V), or 3V lithium cells with several
possible cathodes (usually MnO2 or
CFX). There are also zinc-air button cells,
employing a fuel-cell type air cathode, which find their main application in
hearing aids. Altogether there are over 40 different sizes and chemistries of
button and coin cells.
Secondary batteries
Lead-acid
batteries
The lead-acid battery, invented by
Planté in 1859 and further improved by Fauré in 1881, is the most
widely used secondary battery. The electrode reactions of the cell are unusual
because the electrolyte, sulphuric acid, is one of the reactants, as seen in
the following equations for discharge:
anode:
Pb + H2SO4
« PbSO4 +
2e- + 2H+ |
E0 = 0.356V |
cathode:
PbO2 + H2SO4 + 2H+ + 2e-
« PbSO4 +
2H2O |
E0 = 1.685V |
overall:
Pb +
PbO2 + 2H2SO4
« 2PbSO4 +
2H2O |
E0 = 2.041V |
On discharge, sulphuric acid is
consumed and water is formed, with the converse on charging. We can therefore
determine the state of charge of the battery by measuring the relative density
of the electrolyte (1.28-1.30 for a fully charged cell).
Energy storage options
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Degradation modes
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Fossil fuels Ever since the start of the industrial revolution,
fossil fuels have provided the principal source of the world's energy.
Initially, solid fuels (coal) were employed exclusively, then in the late 19th
and early 20th centuries liquid fuels (petroleum) progressively took over an
increasing share of the market, particularly for transport, and finally in the
latter half of the 20th century gaseous fuels (natural gas) assumed increasing
importance. Fossil fuels are versatile in that they may be combusted to provide
heat, burnt in an internal combustion engine to provide mechanical energy/power
(eg for transport) or used to generate electricity in a power station.
An important feature of fossil fuels is that they are not only concentrated
sources of energy, but are also readily transportable energy stores.
Nuclear fuels Nuclear fuels (uranium, plutonium, thorium) are of
use only for the central generation of electricity in a nuclear reactor.
Although nuclear fuels themselves may be stored, the electricity produced from
them cannot be stored directly.
Renewable energy sources Renewable energy sources (wind energy,
solar PV energy, wave energy, biomass, tidal energy, geothermal energy) are
also best exploited via electricity generation, although in a dispersed mode
and on a smaller scale than nuclear electricity. Again, electricity from these
sources is not readily stored.
Electricity storage As concern grows over fossil fuel usage, in
terms of global warming and resource depletion, there will be a progressive
swing to renewable energy. This will necessitate the development of improved
methods of storing electricity, from periods when it is available (eg sunny or
windy days) to when it is needed (night-time or periods of calm weather).
Because electricity cannot be stored directly (except on a very small scale in
capacitors), it must first be converted to some other energy form for storage.
There are four options:
Potential energy: Pumped-hydro schemes, as currently operated by
electricity utilities in mountainous regions; compressed air
storage.
Kinetic energy: Storage in high-speed flywheels of advanced design,
and made from fibre-reinforced composites.
Thermal energy: Night storage heaters of high thermal capacity, as
commonly used in the UK for space heating.
Chemical energy: Conversion to fuels such as hydrogen or methanol, or
storage as chemicals in batteries. In the 21st century, the requirement for
electricity storage will grow and it is likely that batteries will play a key
role. |
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If a
battery is to be charged-discharged for hundreds, or even thousands, of cycles,
it is essential that the chemical reactions that take place at the electrodes
are quantitatively reversible. Even if as little as 0.1 per cent
irreversibility (or side reaction) occurs, this will soon add cumulatively to a
major loss in capacity. Many, if not most, electrode reactions involve a
reconstructive phase change in the crystal chemistry of the active materials. A
typical positive electrode reaction would be:
Solid (A) + Anion
« Solid (B) + e- (charged)
(eg Ni(OH)2 + OH- « NiOOH + H2O + e-)
This
involves ionic diffusion processes in the crystal structure of the solids,
leading to phase change and recrystallisation. From the viewpoint of the solid
state chemist, the requirement to reverse this reaction quantitatively during
each cycle is exceedingly demanding. The severity of the specification is
apparent when one considers the many possible processes or side reactions
leading to battery deterioration and failure. These include:
densification and swelling of the electroactive material with loss of
porosity;
progressive formation of inactive phases, isolating active
material;
growth of metallic needles (dendrites) at the negative electrode,
causing internal short circuits;
mechanical shedding of active material from electrode
plates;
separator dry-out through over-heating;
corrosion of current collectors, resulting in increased internal
resistance; and
gassing of electrode plates on overcharge.
These
and other degradation processes may result in precipitous battery failure,
through an internal short circuit, or may lead to progressive loss in capacity
and performance. Generally the degradation steps are interactive and
accumulative, so that when the performance starts to deteriorate it soon
accelerates and the battery becomes unusable. Despite this gloomy prognosis,
some remarkable success has been achieved in designing batteries of long cycle
life (ca 1000 cycles) for several different chemistries. The nickel-hydrogen
battery has been demonstrated to last for >20000 cycles and is the preferred
type in low Earth orbit satellites, as used for meteorology and Earth
surveillance. For this application the batteries are required to undergo 16
charge-discharge cycles per day (5840 cycles per year, with no loss in capacity
and no opportunity to exchange failed batteries!). Modern weather forecasts and
military defences are dependent on the performance of the batteries in these
satellites. |
Lead-acid batteries find wide
application in vehicles. Originally known as 'starting, lighting and ignition
batteries', they are now more commonly referred to as 'automotive batteries'
because of the range of other duties they must perform in the modern car. Other
engine starting applications are in aircraft, boats and stationary engines for
local electricity generation. These batteries are recharged by the engine's
alternator and in normal use are not subjected to 'deep' discharge (see
Glossary). They are of the 'pasted plate' (Fauré) design, in which
the positive active material is pasted on to a lead grid current collector.
This design is cheap to construct and gives a high power output, but the life
of the battery is considerably shortened by repeated deep discharge. A modified
version of the pasted plate battery is the so-called 'leisure battery' used in
caravans, boats and so on for supplying the 'house electrics'. This is
essentially an improved pasted plate battery which, at higher cost, will give a
reasonable life when subjected to deep discharge duties.
Finally, there is the traction
battery as used to propel electric vehicles (milk floats, tractors, fork-lift
trucks etc). This is a more expensive battery type in which the
positive active material (PbO2) is contained
in a row of polyester or braided glass fibre tubes. Co-axially, in the centres
of the tubes, are vertical lead alloy spines that act as the current
collectors. Figure 3 shows the two principal lead-acid
types.
|
Fig 3. Lead-acid batteries with (a) flat plates and
(b) tubular plates |
Over the years, many improvements
have been made to the lead-acid battery. Although the essential
electrochemistry remains unchanged, the modern battery bears little resemblance
to that of 50 years ago. Major advances have been made in the lead alloys used,
in the materials and design of the separators, in the packaging (polypropylene
containers rather than glass or hard rubber/pitch), and in the methods of
construction. All these changes have led to batteries of improved performance,
lower mass and lower cost. In recent years sealed lead-acid batteries have been
developed that require no maintenance and may be used in any
orientation.
Alkaline electrolytes
Rechargeable alkaline electrolyte
batteries were invented at the end of the 19th century by Jungner in Sweden and
Edison in the US. These were based on nickel oxide cathodes and either iron or
cadmium anodes, and are popularly known as the nickel-iron and nickel-cadmium
batteries, respectively. The electrolyte is concentrated KOH solution. The
overall chemistry of each cell is analogous:
Fe + 2NiOOH +
4H2O «
Fe(OH)2 + 2Ni(OH)2.H2O |
E0 = 1.37V |
Cd + 2NiOOH +
4H2O «
Cd(OH)2 + 2Ni(OH)2.H2O |
E0 = 1.30V |
Both batteries were commercialised
early in the 20th century, though the nickel-cadmium battery has proved more
successful. This is because the iron electrode is more susceptible to corrosion
and to self-discharge on standing. Also, the electrical efficiency is poor and
a low over-potential for hydrogen evolution leads to excessive gassing during
recharge.
Nickel-cadmium batteries are best
known as small (AA size) rechargeable cells for use in childrens' toys. Much
larger 6V batteries (5 cells in series) are available for engine-starting, for
stationary battery applications, and for electric traction. These have several
advantages over lead-acid: stable discharge voltage, long operational life
(ca 1000 cycles), low maintenance, faster discharge rate, better
low-temperature performance and excellent reliability. However, they are
considerably more expensive and there are environmental concerns over the
disposal of batteries containing toxic cadmium. This disposal problem may be
easier to solve for the larger batteries used by industry, which can easily be
recycled, than for domestic AA size cells that tend to be discarded with the
domestic refuse.
For this reason, at least, two
recent developments in rechargeable alkaline batteries are welcome.
Traditionally, alkaline Zn-MnO2 cells have
always been seen as primary cells, but rechargeable cells of this type are now
being marketed. This has come about as a result of advances in separator
materials, which prevent the formation of elongated zinc needles or dendrites,
which lead to internal short-circuiting. Changes in cell design prevent
discharge from occurring beyond the first electron removal step (Mn4+ ® Mn3+). In addition it is necessary to use special chargers
that taper-charge the cell to a maximum of 1.7V per cell, to prevent
over-charge and gassing. Such cells are capable of relatively few
charge-discharge cycles, but have several times the capacity of comparably
sized Ni-Cd cells and are cheaper. They may be seen as intermediate between
primary alkaline manganese cells and rechargeable Ni-Cd cells.
The second major advance in
rechargeable alkaline batteries was the development of the nickel-metal hydride
battery. This retains the nickel oxide positive electrode and the KOH
electrolyte, but uses a metallic hydride rather than cadmium. Effectively, the
negative electrode is hydrogen (as in a fuel cell), immobilised in the form of
a metallic hydride. The hydride is a complex alloy of rare-earth elements and
other metals that may be decomposed and reformed reversibly. The operating
voltage of a Ni-MH cell is almost the same as that of Ni-Cd (1.2-1.3V), making
for ready interchangeability. The specific energy of Ni- MH batteries (60-70
Whkg-1) is up to double that of Ni-Cd and
their specific power may be as high as 250Wkg-1. These batteries are resilient to overcharge and
overdischarge and operate from -30 to +45°C. Cells of both cylindrical and
prismatic design are now manufactured in a range of sizes; small cells are used
in portable electronic devices (eg mobile phones), while prismatic
cells of 100Ah capacity are available for assembly into 12-14V modules (eg for
use as traction batteries). The new material technology involved in developing
Ni- MH batteries is almost entirely associated with the hydride negative
electrode.
Lithium batteries
Lithium, with an atomic mass of
6.94, is the lightest of all the metals and is therefore an obvious candidate
for battery use. It has a high specific capacity (3.86Ahg-1) and a much higher electrochemical reduction
potential (-3.045V) than zinc (-0.76V). The problems in developing lithium
batteries stem from the high reactivity of lithium metal. It is necessary to
use a non-aqueous electrolyte, which may be either an organic liquid or a solid
polymer - each with a dissolved lithium salt to make it ionically conducting -
or a fused lithium salt.
|
Some key manufacturers |
|
Zinc-carbon and alkaline manganese primary batteries
Duracell, Ever Ready (Energizer), Panasonic, UCAR, Vidor, Varta, Kodak,
Rayovac
Lithium primary cells Duracell, Ultralife, Energizer,
Sanyo
Button and coin cells Duracell, Varta,
Hitachi
Rechargeable alkaline manganese Rayovac
Lead-acid Hawker (Tungstone), CMP, Johnson Controls,
Varta, Tudor, CEAC
Rechargeable nickel-cadmium batteries SAFT, Varta,
Eagle-Picher
Nickel-metal hydride batteries SAFT, GM-Ovonics, Varta,
Panasonic, Matsushita
Lithium ion AEA Technology, Sony, Sanyo,
Varta |
|
|
Primary lithium batteries using a
lithium foil negative electrode, an organic liquid electrolyte and any one of
several positive electrode materials are commercially available from several
suppliers. The difficulties arise when one tries to develop a rechargeable
lithium battery of this type. Much work has been done in this field with oniy
limited success. In general, lithium is not electrodeposited as a smooth layer
on the metal current collector, but as a mossy deposit.
Lithium foil that has been exposed to
air is covered with a thin layer of hydroxide-nitride, which limits its
reactivity. Freshly electrodeposited lithium is finely divided and highly
reactive, and decomposes the electrolyte. Some of the deposit becomes
electrically isolated from the electrode and so capacity is lost rapidly.
Lithium metal may also be plated out as crystalline dendrites that ultimately
penetrate the separator and cause an internal short-circuit of the cell.
Finally, these processes constitute a fire risk and cells have been known to
ignite spontaneously during recharge. For all these reasons, the commercial
prospects for rechargeable cells based on liquid electrolytes and lithium metal
negatives do not seem too bright, although much research is still in progress.
The lithium ion battery, the rising star of the 1990s, circumvents most of
these problems.
The essential feature of the lithium
ion battery is that at no stage in the charge-discharge cycle should there be
any lithium metal present. Rather, lithium ions are intercalated into the
positive electrode in the discharged state and into the negative electrode in
the charged state and move from one to the other across the electrolyte. The
latter is a solution of a lithium salt in an organic solvent. The origin of the
cell voltage is then the difference in free energy between Li+ ions in the crystal structures of the two electrode
materials.
Commercial cells use carbon as the
negative electrode: lithium ions will intercalate readily into graphite up to a
composition approaching C6Li, at a voltage of
zero to 1V with respect to a lithium reference electrode. Using a positive
electrode of LiCoO2 or LiNiO2, the cells are assembled in the discharged state and a
3V lithum ion cell results. After a few initial cycles, approximately half of
the intercalated lithium may be removed reversibly, as shown:
charged |
Li0.55CoO2 +
0.45Li+ + 0.45e- « LiCoO2
(123mAhg-1) |
discharged |
charged |
Li0.35NiO2 +
0.5Li+ + 0.5e- « Li0.85NiO2
(135mAhg-1) |
discharged |
The solid state chemistry of the
LiNiO2 structure is more complex than that of
LiCoO2 and the fully lithiated compound is
not stable during electrochemical cycling. Nevertheless, the practical Ah
capacities are much the same, as are the cell voltages. When cycling
Li+ ion cells it is important to control the
top-of-charge voltage carefully (4.1V for LiNiO2 and 4.2V for LiCoO2). Failure to do so results in decomposition of the
'positives' to give oxygen gas and Co3O4 or LiNi2O4, a
hazardous situation in a sealed cell. For this reason, lithium ion cells must
be recharged using a specially designed charger incorporating both voltage and
temperature control. Over-discharge must also be avoided and it is usual to
have a limiting cut-off voltage on discharge of ca 2.7V. (In this
regard the NiMH battery has the advantage of being much better able to
withstand overcharge and overdischarge.)
The Sony Corporation in Japan first
commercialised lithium ion cells in the early 1990s, and they have since been
marketed by many other battery manufacturers. They are extensively employed in
laptop computers, mobile phones and other portable electronic equipment. In
1997 alone it is estimated2 that 190m cells
were manufactured in Japan with a value exceeding US$2000m. With worldwide
R&D in progress, we may hope for future improvements in performance as well
as price reductions for lithium ion cells.
From this brief survey it is clear
that battery research is a dynamic and challenging field for chemists, working
closely with material scientists and design engineers. The rapid advances of
the past 20 years augur well for new power sources in the 21st
century.
Ronald Dell worked in applied
electrochemistry for 20 years, and may be contacted at 2 Tullis Close, Sutton
Courtenay, Abingdon, Oxfordshire OX14 4BD.
References
- K. Tamura and T. Horiba, J.
Power Sources. 1999, 81-82, 156.
- T. Kodama and H. Sakaebe, J.
Power Sources, 1999, 81-82, 144.
Battery
bibliography |
|
Journals
Batteries International. London: Euromoney
Publications.
Electrochimica Acta. London: Elsevier Science.
Journal of Applied Electrochemistry. The Netherlands: Kluwer
Academic.
Journal of the Electrochemical Society USA. Pennington, NJ:
The Electrochemical Society.
Journal of Power Sources. London: Elsevier
Science.
Proceedings of the ninth international meeting on lithium batteries,
J. Power Sources, vol 81-82, 1999.
Solid State lonics. London: Elsevier Science.
Books
D.
Berndt, Maintenance-free batteries, 2nd edn. Taunton: Research Studies
Press, 1997.
S. U.
Falk and A. J. Salkind, Alkaline storage batteries. Chichester: John
Wiley, 1969.
Lithium batteries, J.-P. Gabano (ed). Maidenhead: Academic
Press, 1983.
Handbook of batteries and fuel cells, 2nd edn, D. Linden
(ed). New York: McGraw-Hill, 1995.
D. A.
J. Rand, R. Woods and R. M. Dell, Batteries for electric vehicles.
Taunton: Research Studies Press, 1998.
P.
Reasbeck and J. G. Smith, Batteries for automotive use. Taunton:
Research Studies Press, 1997.
Solid state batteries, C. A. C. Sequeira and A. Hooper
(eds). NATO ASI series. The Netherlands: Martinus Nijhoff International,
1985.
J. L.
Sudworth and A. R. Tilley, The sodium sulfur battery. London: Chapman
& Hall, 1985.
Modern battery technology, C. D. S. Tuck (ed). Chichester:
Ellis Horwood, 1991.
C. A.
Vincent, Modern batteries, 2nd edn. Maidenhead: Edward Arnold,
1998. |
Useful
websites
AEA Technology
Duracell
Electric Fuel
Energizer
Hawker
Rayovac
SAFT
Ultralife Varta International Power Sources Symposium
Royal Society of Chemistry links
The
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coordinates the interests of a wide range of scientists involved in all aspects
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Also of interest is
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Glossary |
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Active material: The electrode material that takes part in the
electrochemical reactions that store/deliver electrical energy.
Active material utilisation: The fraction of active material
that reacts during discharge before the battery can no longer deliver the
required current at a useful voltage. Anode: The negative
electrode from which electrons flow during discharge. Battery
management: The regulation of charging and discharging conditions (eg
control of temperature, cut-off voltages, current).
Capacity: The amount of charge (measured in ampere-hours, Ah)
that can be withdrawn from a fully charged battery under specified
conditions. Cathode: The positive electrode to which
electrons flow during discharge. Current collector: The
metallic part of an electrode which conducts electrons to and from the active
material. Depth of discharge: The ratio of the
ampere-hours discharged from a battery to the available capacity measured at
the same temperature and discharge rate. Energy density:
The energy output from a battery per unit volume, expressed in Wh
dm3. Energy efficiency: The fraction of
the energy used in charging the battery, expressed in watt-hours, which is
available on discharge. |
Open-circuit voltage: The voltage of a battery when there is
no net current flowing. Over-discharge: The discharge of a
battery beyond the level specified for correct operation.
Passivation: The formation of a surface layer that impedes the
electrochemical reactions at an electrode. Power density:
The power output of a battery per unit volume, usually expressed in W
dm3 and quoted at 80 per cent depth of discharge.
Self-discharge: The loss of capacity of a battery under
open-circuit conditions as a result of internal chemical reactions and/or
short-circuits. Separator: An electronically
non-conducting, but ion-permeable, material that prevents electrodes of
opposite polarity making contact. Shelf-life: The period
over which a battery may be stored and still meet specified performance
criteria. Specific energy: The energy output of a battery
per unit weight, usually expressed as Wh kg1.
Specific power: The power output of a battery per unit weight,
usually expressed as W kg1. |
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