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Ch01-N52160.fm Page 40 Wednesday, December 27, 2006 12:36 PMCh01-N52160.fm Page 40 Wednesday, December 27,2006 12:36 PM
40 G. Pistoia
electrolyte onto a current collector or loading the material into a honeycombmatrix [48]. Graphite may be included and, sometimes, CoS2 and NiS2 are alsoadded.
The bipolar cell configuration is preferable over the monopolar one. Anexploded view is shown in Figure 1.31(a). The electrodes are of high surfacearea and the cell design is compact, also thanks to the use of starved electrolyteand MgO separator, this resulting in a higher power output. The presence of thetwo-phase alloy at the negative electrode ensures tolerance to overcharge, sothat the state of charge of all cells can be equalized. Indeed, the alloy (LiAl+Li5Al5Fe2) has a sufficiently high Li activity towards the end of charge to causesolubilization of Li metal in the molten-salt electrolyte; Li can be reoxidized atthe positive, thus giving rise to a shuttle mechanism [48].
The design criteria to be met for an efficient bipolar stack are [48]:1. Provision for an equalized state of charge of the cells in series, as mentioned
above.2. The use of a starved-electrolyte regime and a MgO separator. This is made
possible by using the Li-rich LiCl-LiBr-KBr electrolyte that has aconductivity, in the starved configuration, equivalent to that of the LiCl-LiBr eutectic in the flooded configuration. Furthermore, in these conditionsthe corrosion is limited.
3. The use of effective seals. Bipolar cells are more difficult to seal thanmonopolar cells. This problem was solved by introducing the chalcogenideseal mentioned above. For cells with FeS2 cathodes, a steel-ceramic-molibdenum seal was found adequate.
Several prototypes of bipolar Li-Al/FeS* batteries were manufactured inthe early 1990s. Such cells (diameter: 130 mm, weight: 250 g) could deliver 25Ah at the C/5 rate, as shown in Figure 1.31(b). The specific energy and powervalues of cells (not batteries) are presented in Table 1.7 [49]. In terms of energy,both cells meet the mid-term USABC's target (80-100 Wh/kg) and the Li/FeS2
cell approaches the long-term target (200 Wh/kg). However, it has to be notedthat the above targets refer to fully engineered batteries. The specific power ofthe Li/FeS2 cell is very interesting. Indeed, the mid- and long-term values set bythe USABC are 150-200 W/kg and 400 W/kg, respectively. Other positive
Table 1.7. Performance characteristics of bipolar Li-Al/FeS* cells. The data do not includethermal enclosure. {From Ref. 49)
Cell Type
Li-Al/FeS2
Li-Al/FeS
Specific Energy(Wh/kg)
180 at 30 W/kg130 at 25 W/kg
Specific Power at 80%DOD (W/kg)
400240
Previous Page
Ch01-N52160.fm Page 41 Wednesday, December 27, 2006 12:36 PMCh01-N52160.fm Page 41 Wednesday, December 27,2006 12:36 PM
Nonaqueous Batteries Used in Industrial Applications 41
features of this system are: good cyclability (in excess of 1000 cycles),tolerance to overcharge and overdischarge and to freeze-thaw cycles.
Sealed modules with a nominal voltage of 25 V and a capacity of 60 Ahhave been fabricated from prismatic bipolar cells [49]. They have a specificenergy of 75 Wh/kg and an energy density of over 200 Wh/L, and can be cycledfor many hundreds of deep discharge cycles. It is noteworthy that failure ofthese modules occurs via short circuits when they reach the end of life.However, series stacks remain operational after the loss of one or more cells:the loss of energy, in this case, is limited to the energy content of the failedcell(s) [50].
The advantages of the Li-Al/FeS* system can be summarized as:• Simple modular design and construction• High energy - at least twice that of lead-acid batteries• High power• Long cycle life• Heat management not requiring auxiliary heating or cooling during use• Safe, even under severe abuses
The Li-Al/FeS* system shows an improved safety over sodium/sulfur(see Sub-section 1.3.3.1), while with respect to sodium/nickel chloride (seeSub-section 1.3.3.2) it has a higher specific power (but less safety). On the otherhand, a couple of disadvantages are evident: a) as any other thermal battery,stored energy is consumed to keep the cell warm during standby periods, and b)the bipolar design is likely to have manufacturing problems and high costs.
The remarkable advancements made with this systems suggested to theUSABC to select it as the long-term battery to be developed for electric vehicles.However, in the mid-1990s the R&D efforts were discontinued also in view ofthe new technologies based on Li-ion and Li-polymer batteries. Indeed, thesetechnologies have power and energy outputs similar to that the Li-Al/FeS2battery, but can operate at much lower temperatures. This system remains aviable candidate for stationary energy storage [50].
Development of the Li/iron sulfide system is continuing, but moltensalts electrolytes have been replaced by polymeric electrolytes. An example,with a composite electrolyte based on PEO, has already been mentioned (seeRfifs. [37,38]).
1.3.3. Batteries with a Sodium Electrode
High-temperature batteries based on sodium as a negative electrode,sulfur or NiCl2 as a positive, and /?"-Al2O3 as a Na+-conducting solidelectrolyte are now used for energy storage applications and are receiving
Ch01-N52160.fm Page 42 Wednesday, December 27, 2006 12:36 PMCh01-N52160.fm Page 42 Wednesday, December 27,2006 12:36 PM
42 G. Pistoia
attention for EV and space applications. The theoretical specific energies of theNa/S system (760 Wh/kg) and Na/NiCl2 system (796 Wh/kg) are much higherthan those of the aqueous systems (Pb/Acid and Ni/Cd) thus far used forenergy storage.
1.3.3.1. Sodium/Sulfur Batteries
Investigations on this battery date back to the early 1970s and wereoriented for several years to motive applications. However, technical andeconomic issues have suggested switching to large battery packs for stationaryapplications. Indeed, the Na/S battery has distinct advantages over othertechnologies, such as high energy and good power density, high cycle life, highenergy efficiency, independence from external temperature, and moderate cost.
The operating temperature of this system is between 310 and 35O°C. Inthis temperature range, both Na and S are liquid, while the solid electrolyte hasa high Na+ conductivity, thus ensuring good kinetics.
During discharge, Na+ migrates from Na to S and forms polysulfides, asindicated in Figure 1.32. The first plateau corresponds to the coexistence oftwo immiscible liquids, S and Na2S5; in the single-phase sloping section, thesulfur content of the polysulfide decreases down to Na2S2.7; the secondplateau corresponds to the formation of Na2S2 [51], but is never reached inpractical cells. Indeed, formation of Na2S3, at 1.78 V, is taken as the dischargelimit. Complete discharge would cause corrosion and local overdischarge due tonon-uniformities in temperature and DOD. At the C/3 rate, the average voltageis 1.9 V.
o 1,8
1,6
1,4
2 ,076 V
1,74 V
Na2S5
20 40 60 80 100 120
State of discharge ( % w.r.t. Na2 S3
140
Figure 1.32. OCV of aNa/S cell at 350°C. (From Ref. 51)
Electrons
SealsLoad
+ –
Celldischarging
Insulator
Sodiumelectrode
Current-collector
Safety can
Beta-aluminaelectrolyte
Metering hole
Sodium ions
Sulfur electrode
Outer case
Ch01-N52160.fm Page 43 Wednesday, December 27, 2006 12:36 PMCh01-N52160.fm Page 43 Wednesday, December 27,2006 12:36 PM
Nonaqueous Batteries Used in Industrial Applications 43
During charge, the reactions described above are reversed and in thefinal stages there is a marked resistance increase due to the insulating characterof sulfur. Therefore, the charge has to be stopped before complete Na recovery,and subsequent discharges provide 85-90% of the theoretical capacity [52].
As already mentioned, this system has a high cyclability (up to 5000-6000 cycles). This is mainly due to the liquid state of reactants and products: theaging mechanism based on morphological changes of the electrodes is notoperating here.
A scheme of a Na/S cell is shown in Figure 1.33 for the commonconfiguration with the central sodium electrode. An essential pre-requisite forthis electrode is high purity, i.e. other metals and Na compounds are notallowed. Contaminants tend to concentrate at the interface with the electrolyte,reducing the electrode active area or even causing its failure [48].
In order to minimize cell resistance, molten sodium has to properly wetthe electrolyte surface. This requires a smooth surface, a proper temperaturerange (300-350°C) and the absence of impurities. The sodium electrode iscontained in a metal (safety) can that restricts, through the metering hole, theflow of sodium to the electrolyte, thus reducing the amount of Na that maycome into direct contact with S in case of tube failure.
The sulfur electrode is impregnated into a layer of carbon or graphitefelt. The carbon fibers ensure a good electronic conductivity, as sulfur is an
©Celldischarging
rzt-e©Insulator
Sodiumelectrode
Current-collector
- Safety can
Beta-aluminaelectrolyte
Outer case Metering hole
Figure 1.33. Schematic of cross-section of the Na/S cell. (From Ref. 48)
Ch01-N52160.fm Page 44 Wednesday, December 27, 2006 12:36 PMCh01-N52160.fm Page 44 Wednesday, December 27,2006 12:36 PM
44 G. Pistoia
insulator for both electrons and ions. Fortunately, Na polysulfides are goodionic conductors.
The electrolyte is /?"-Al2O3, which has a negligible electronicconductivity and is impermeable to molten Na and S. Its basic structural unity isa spinel-like slab formed by 4 layers of close-packed oxygen ions in a cubicstacking. The slabs are separated from each other by oxygen bridges. Thesodium ions move in the space between these slabs. The idealized compositionof yfl"-Al2O3is Na2O5.33Al203 or Na6Al32[Vac]A1
3+05i, with a vacancy of Al3+
in the spinel block that is balanced by 3 Na+ in the conduction plane. Thisresults in high conductivity. Pure /?"-Al2O3 is not easy to prepare, so it has to bestabilized with Mg or Li ions that substitute for Al ions. Typical compositionscontain 4.0 wt% MgO or 0.7 wt% Li2O.
The conductivity of this electrolyte is -0.5 ohnf'cm"1 at 350°C for thepolycrystalline form. However, /?"-Al2O3 is rather sensitive to moisture, thisfavoring deterioration of its mechanical properties. Therefore, some /?-Al2O3
(idealized formula, Na2OllAl203) is enclosed in the mixture, in spite of itslower conductivity, as it is less hygroscopic. A conductivity of ~0.2 ohm~'cm"1
is regarded as acceptable for practical electrolytes [48].Production of Na/S batteries for stationary applications is particularly
active in Japan. Table 1.8 presents the basic characteristics of some cells.In Figure 1.34, three single cells and the module constructed with the
largest one are shown [53]. Different modules are presented in Table 1.9, forapplications connected with energy networks (see footnote). Very large energy-storage systems can be built with these modules: their storage capacity may beas high as 57.6 MWh (see Figure 1.35) [54]. A comparison of different energystorage systems, including various batteries, pumped hydro storage, compressed
Table 1.8. Characteristics of stationary Na/S cells {From Ref. 52)
Manufacturer
CellDesignationCapacity, AhDiameter, mmLenght, mmWeight, kgEnergyDensity, Wh/LSpecificEnergy, Wh/kgPower Density,W/L
NGK
T4.1
160623752
285
160
36
NGK
T4.2
248683902.4
340
202
43
NGK
T5
632915155.4
370
226
46
Yuasa
17664
4302.7
240
120
60
Hitachi
28075
4004
300
133
Electric HeaterDry Sand
Fuse
Heat Insulated Container(Lower)Cell
Main Pole
Heat Insulated Container (Upper)
T4.2T4.1
T5
518
390
375
6891
62
Ch01-N52160.fm Page 45 Wednesday, December 27, 2006 12:36 PMCh01-N52160.fm Page 45 Wednesday, December 27,2006 12:36 PM
Nonaqueous Batteries Used in Industrial Applications 45
Dry Sand Heat InsulatedElectric Heater Fuse Container (Upper)
Main PoleHeat Insulated Container
C e l l (Lower)
Figure 1.34. Na/S cells (left) and module (right). The module is built with 384 T5 cells and has anenergy of 421 kWh (energy density, 170 Wh/L) and a power of 52.6 kW. (From Ref. 53)
Table 1.9. Na/S modules for stationary applications. (From Ref. 52)
Manufacturer
BatteryDesignationPrimeApplication*Number ofCellsCapacity, AhEnergy, kWhVoltage, VVolume, LWeight, kgSpecificEnergy, Wh/kgEnergyDensity, Wh/L
NGK
12.5 kW
LL;PS;PQ
336
2280105489411400
75
112
NGK
25 kW
LL;PS;PQ
480
227221196
14482000
105
145
NGK
52 kW
LL;PS;PQ
384
3624421128
24813620
116
170
Yuasa
25 kW
LL
320
140810080
10861700
59
92
Hitachi
12.5 kW
Renew
216
290100144
25921900
53
40
' LL: utility-based load leveling; PS: peak shaving; PQ: power quality; Renew: renewable energy hybrid
air storage, and superconducting magnetic storage, has shown that the Na/Sbatteries have the highest energy densities [55]. They can live in this applicationfor up to 15 years providing thousands of cycles. (See also Chapter 8).
All development of Na/S batteries for EV applications was stopped by
Ch01-N52160.fm Page 46 Wednesday, December 27, 2006 12:36 PMCh01-N52160.fm Page 46 Wednesday, December 27,2006 12:36 PM
46 G. Pistoia
Figure 1.35. 57.6 MWh (8 MW) battery installed in Japan for load levelling by NGK. (From Ref.54)
mid-1990s. Two companies (Asea Brown Bovery in Germany and Silent Powerin the U.S.A.) were especially involved in this field. The properties of the cellsdeveloped by these companies are compared in Table 1.10 with those of an
cell developed by the Swiss company MES-DEA.
1.3.3.2. Sodium/Nickel Chloride (Zebra) Batteries
This battery bears some analogies with the Na/S battery. The negativeelectrode and the electrolyte are the same, but a metal chloride is used instead of
Table 1.10. Comparison of cells with Na as a negative electrode for EV applications. (From Ref.52)
Manufacturer
Cell DesignationChemistryCapacity, AhElectrolyte ShapeDiameter, mmLenght, mmWeight, gResistance, ohmSpecific Energy,Wh/kgSpecific Peak Power,W/kg*
Asea Brown Boveri
A04Na/S
38cylindrical
35220410
6
176
390
Silent Power Ltd
PBNa/S10.5
cylindrical444512032
178
250
MES-DEA
ML3Na/NiCl2
32cruciform
36.52327156-20
116
260
• At 2/3 OCV and 80% DOD
Ch01-N52160.fm Page 47 Wednesday, December 27, 2006 12:36 PMCh01-N52160.fm Page 47 Wednesday, December 27,2006 12:36 PM
Nonaqueous Batteries Used in Industrial Applications 47
sulfur as a positive electrode. As the initial research was carried out in SouthAfrica for EV applications, the acronym Zebra (Zero Emission BatteryResearch Activity) is often used [52].
Preferred material for the positive electrode is NiCU, but FeCl2 has alsobeen studied. During normal discharge, Ni and NaCl are formed, as shown bythe scheme of Figure 1.36. The voltage, 2.58 V, is higher than that of Na/S,2.06-1.78 V (see Figure 1.32). Other differences will be remarked in thefollowing description.
A schematic of this cell (Figure 1.37) shows that liquid Na is placed inthe outer part, while in practical Na/S cells it is in the central part. Furthermore,Na is not initially included in the cell assembly, but produced in situ duringcharge, as the cell is assembled in the discharged state. The positive electrode issolid and this would pose problems, as the solid-solid interface with theelectrolyte would not allow high currents. Therefore, a second electrolyte,NaAlCl4, which is liquid at the operating temperatures, is added. Inside the /?"-A12O3 tube, a compact mix of Ni metal and NaCl is inserted, and moltenNaAlCU is then poured to form a narrow annulus between the positive electrodeand the electrolyte. The presence of the second electrolyte lowers the specificenergy of the ZEBRA battery by -10% [56].
The tolerance to over-charge and over-discharge is outstanding byvirtue of the reversible reactions occurring in these segments (see Figure 1.36).On over-charge, NaAlCLt further chlorinates the Ni matrix, while on over-discharge excess Na reacts with the liquid electrolyte. This feature has apractical implication: it is possible to connect in series several cells, withoutparallel connections, as cell imbalances are leveled out by the above reactions.
3.05
w 2 .58-o>B"5
1.58-
2Na + 2AICI3 + NiCI2<=* N» + 2NaAlCI4
Overcharge| 2Na + NiClj <=> Ni • 2NaC!
Norma!operation
<=* 4NaCJ + Al
Overdischarge
100 0State-of-charge / %
Figure 1.36. Equilibrium voltage vs. state of charge of Na/NiCl2 cell at 250°C. (From Ref. •
Ch01-N52160.fm Page 48 Wednesday, December 27, 2006 12:36 PMCh01-N52160.fm Page 48 Wednesday, December 27,2006 12:36 PM
48 G. Pistoia
NaAICI4
. fi-alumina tube
Porous M, MCI2 electrode
Liquid sodium
Cell case
Figure 1.37. Schematic of sodium/nickel chloride cell. (From Ref. 48)
Another advantage of this battery, with respect to the Na/S system, isrepresented by its enhanced safety. If the electrolyte tube cracks, molten Nareacts first with NaAlCU, according to the reaction of Figure 1.36. The resultingAl metal shorts the cell, while NaCl tends to plug the crack. Therefore, in abattery with a series of cells, the shorted cell does not cause failure of the all
Figure 1.38. Cross-section of a conventional ZEBRA cell (left) and a high-power cell (right).(From Ref. 48)
Ch01-N52160.fm Page 49 Wednesday, December 27, 2006 12:36 PMCh01-N52160.fm Page 49 Wednesday, December 27,2006 12:36 PM
Nonaqueous Batteries Used in Industrial Applications 49
battery [56].As a further advantage, the Zebra cell can work in a wider temperature
range, i.e. 220-450°C, although the practical range has to be restricted to 270-350°C.
To improve the battery capacity and energy, cells with a square sectionmay be constructed, as this greatly reduces the dead space typical of batteriesassembled from cylindrical cells. Specific energies of 120-130 Wh/kg arepossible.
A limitation of the conventional design is the increasing resistance withDOD, this lowering the power capability. A convenient way to overcome thislimitation is designing the ceramic electrolyte with the cruciform shape ofFigure 1.38. The tube so obtained, termed a "monolith", allows the constructionof thinner and less resistive positive electrodes. To further decrease theresistance, Fe-doped NiCl2 is used. As a result, the cell's specific power mayreach 260 W/Kg at 80% DOD (Table 1.10), and batteries with a specific powerof 150 W/kg (the USABC's mid-term target for EV) have recently been built.
The Zebra system is specifically intended for EV applications. Asshown in Table 1.10, it has lower specific energies (but the gap is reduced on avolumetric basis) and powers than Na/S cells. However, it is preferred for EVapplications thanks to such factors as safety, easiness of construction,cyclability (more than 1000 cycles), low corrosion, etc.
Some specific applications have recently been proposed: in photovoltaicsystems, for instrumentation packs in oil exploration, and in hybrid cars alsocontaining a PEM fuel cells. In this latter application, two 40-kW Na/NiCl2batteries are coupled to a 6-kW fuel cell. Using this hybrid architecture allowsdoubling the EV range from 120 km to 240 km [57].
1.3.4. Basic Parameters of Secondary Nonaqueous Batteries
In Table 1.11, relevant data of the secondary batteries dealt with in thischapter are summarized. Due to the continuous evolution of these batteries,especially Li-ion and Li-polymer, the data have to be considered with somecaution. Caution is also necessary in view of differences in batterysize/configuration and test conditions.
Ch01-N
52160.fm Page 50 W
ednesday, Decem
ber 27, 2006 12:36 PM
Table 1.11. Characteristics of non-aqueous secondary batteries.
8I*
System
Li-ion
b, stationary(L
iNi07C
o03O
2)L
i-ion", EV
(LiN
i i .x_vC
oxM
nvO
2)L
i-ionb, stationary
(Li1+xM
n2O
4)L
i-ionb,E
V(L
iCrxM
n2.xO
4)
Li m
etal-polymer b
Li/FeS
c
Li/FeS
2 c
Na/S
c
Na/N
iCl2 c
Voltage
Range(V
)
4.0-2.8
4.0-2.8
4.0-3.0
4.0-3.0
3.0-2.0
1.7-1.02.0-1.5
2.0-1.8
2.1-1.7
Operating
Tem
perature(°C
)
-20-^60
-20-50
-20^60
-20-50
40-60"60-80
3
375-500375-450
300-350
250-300
Cycle
Life
(cycles)
9001
570
12001
580
80010001000
6000
2500
SpecificE
nergy(W
h/kg)
128
150
122
155
140'120
3
130180155'175
3
115
Energy
Density
(Wh/L
)
197
252
255
244
174'160
3
220350300'350
3
190
SpecificP
ower
(W/kg) a
490
440
260240400
2503
260
Ref.
23,58
23,58
23,58
23,58
39,4241,46
2,50,582,50,58
2,522,522,58
a. pulse discharge, b. battery; c. cell1. single cells; 2. stationary applications; 3. E
V
I
Ch01-N52160.fm Page 51 Wednesday, December 27, 2006 12:36 PMCh01-N52160.fm Page 51 Wednesday, December 27,2006 12:36 PM
Nonaqueous Batteries Used in Industrial Applications 51
References
1. K.M. Abraham, J. Power Sources 34 (1991) 81.2. D. Linden and T.B. Reddy, in "Handbook of Batteries" (Chapter 14), D. Linden and T.B.
Reddy, Eds., McGraw-Hill, New York, 2002.3. T.B. Reddy, in "Modern Battery Technology", C.D.S. Tuck Ed., Ellis Horwood, Chichester
(U.K), 1991.4. www.powertech.co.nz/tadspecs5. P.G. Russel and F. Goebel, J. Power Sources 54 (1995) 180.6. H. Ikeda, T. Saito and H. Tamura, in "7s' International Symposium on Manganese Dioxide",
Cleveland, Ohio, 1975, p. 384.7. H. Ikeda, M. Hara and S. Narukawa, U.S. Patent 4,133,856 (1979).8. M.M. Thackeray, in "Handbook of Battery Materials", J.O. Besenhard, Ed., Wiley-VCH,
Weinstein, 1999.9. G. Pistoia, J. Electrochem. Soc, 129 (1982) 1861.10. Ultralife Batteries - Products, www.ulbi.com11. Duracell: Technical OEM, Lithium/Manganese Dioxide, www.duracell.com12. M. Winter, K.-C. Moeller and J.O. Besenhard, in "Lithium Batteries - Science and
Technology", G. A. Nazri and G. Pistoia, Eds., Kluwer Academic Pub., Boston, 2004.13. (a) L.F. Nazar and O. Crosnier, (b) G.G. Amatucci and N. Pereira, in "Lithium Batteries -
Science and Technology", G. A. Nazri and G. Pistoia, Eds., Kluwer Academic Pub., Boston,2004.
14. A. Manthiram, in "Lithium Batteries - Science and Technology", G. A. Nazri and G. Pistoia,Eds., Kluwer Academic Pub., Boston, 2004.
15. (a) S. Yang, Y. Song, K. Ngala, P. Y. Zavaliy and M. S. Whittingham, J. Power Sources119-121 (2003) 239; (b) M. S. Whittingham, Chem. Rev. 104 (2004) 4271; (c) M. S.Whittingham, IBA-HBC Meeting, Waikoloa, Hawaii, January 2006.
16. (a) G. Pistoia, in "Lithium Batteries - Science and Technology", G. A. Nazri and G. Pistoia,Eds., Kluwer Academic Pub., Boston, 2004; (b) M.-H. Yang, H.-C. Wu, D.-T. Shieh, C.-Y.Su and Z.Z. Guo, IBA-HBC Meeting, Waikoloa, Hawaii, January 2006.
17. C.-K. Huang, J.S. Sakamoto, J. Wolfenstine and S. Surampudi, J. Electrochem. Soc. 147(2000) 2893.
18. G.E. Blomgren, J. Power Sources 119-121 (2003) 326.19. Sony Global - Press Release, www.sony.net/Sonv Info/News/Press/20. K. Imasaka et al, 12th IMLB Meeting, Abs. 418, Nara, Japan, June 2004.21. M. Broussely, 22nd International Seminar on Primary/Secondary Batteries, Fort Lauderdale
(FL, USA), March 2005.22. M. Broussely, Ph. Blanchard, Ph. Biensan, J.P. Planchat, K. Nechev and R.J. Staniewicz, J.
Power Sources 119-121 (2003) 859.23. K. Takei, K. Ishihara, K. Kumai, T. Iwahori, K. Miyake, T. Nakatsu, N. Terada and N. Arai,
J. Power Sources 119-121 (2003) 887.24. C. Amemiya, J. Kurihara, M. Yonezawa, NEC R§D 42 (2001) 24125. M. Broussely, in "Advances in Lithium-Ion Batteries", W. van Schalkwijk and B. Scrosati,
Eds., Kluwer Academic Pub. Boston 2002.26. M. Broussely, Is' International Symposium on Large Lithium Ion Battery Technology and
Applications, Honolulu, Hawaii, June 2005.27. K. Amine, C.H. Chen, J. Liu, M. Hammond, A. Jansen, D. Dees, I. Bloom, D. Vissers and G.
Henriksen, J. Power Sources 97-98 (2001) 684.28. Y. Nishi, in "Advances in Lithium-Ion Batteries", W. van Schalkwijk and B. Scrosati, Eds.,
Kluwer Academic Pub. Boston 2002.
Ch01-N52160.fm Page 52 Wednesday, December 27, 2006 12:36 PMCh01-N52160.fm Page 52 Wednesday, December 27,2006 12:36 PM
52 G. Pistoia
29. M. Broussely in "Lithium Batteries - Science and Technology", G. A. Nazri and G. Pistoia,Eds., Kluwer Academic Pub., Boston, 2003.
30. B.V. Ratnakumar et al, 12th IMLB Meeting, Abs. 424, Nara, Japan, June 2004.31. T. Horiba et al, 12th IMLB Meeting, Abs. 49, Nara, Japan, June 2004.32. N.H. Clark and D.H. Doughty, 12th IMLB Meeting, Abs. 420, Nara, Japan, June 2004.33. M. Broussely and G. Archdale, J. Power Sources 136 (2004) 386.34. (a) Y.V. Mikhaylik and J.R. Akridge, 12th IMLB Meeting, Abs. 190, Nara, Japan, June 2004;
(b) Y.V. Mikhaylik, IBA-HBC Meeting, Waikoloa, Hawaii, January 2006.35. J.B. Kerr in "Lithium Batteries - Science and Technology", G. A. Nazri and G. Pistoia, Eds.,
Kluwer Academic Pub., Boston, 2004.36. V. Dorval, C. St-Pierre and A. Vallee, "Lithium-Metal-Polymer Batteries: From the
Electrochemical Cell to the Integrated Energy Storage System"(www.avestor.com/rtecontent/document/Battcon), 2004.
37. E. Peled, D. Golodnitsky, E. Strauss, J. Lang and Y. Lavi, Electrochim. Ada 43 (1998) 1593.38. E. Strauss, D. Golodnitsky and E. Peled, Electrochim. Ada 45 (2000) 1519.39. www.avestor.com/se48s80.ch240. G. Pistoia, S. Panero, M. Tocci, R.V. Moshtev and V. Manev, Solid State Ionics 13 (1984)
311.41. C. Letourneau, D. Geoffroy, P. St-Germain, A. Belanger and R. Atanasoski, "Progress in
Lithium-Metal-Polymer Battery System for Electric Vehicles",(www.avestor.com/rtecontent/document/evs 15)
42. C. St-Pierre, T. Gauthier, M. Hamel, M. Leclair, M. Parent and M.S. Davis, , "AvestorLithium-Metal-Polymer Batteries Proven Reliability Based on Customer Field Trials",(www.avestor.com/rtecontent/document/AVESTOR WhitePaper Battcon2003")
43. C. Robillard, A. Valle"e and H. Wilkinson, "The Impact of Lithium-Metal-Polymer BatteryCharacteristics on Telecom Power System Design", (www.avestor.com/ rtecontent/document/AVESTOR Intelec paper 20041
44. C. St-Pierre, R. Rouillard, A. Belanger, B. Kapfer, M. Simoneau, -Y. Choquette, L.Gastonguay, R. Heiti and C. Behun, "Lithium-Metal-Polymer Battery for Electric Vehicleand Hybrid Electric Vehicle Applications", (www.avestor.com/rtecontent/document/evs 16)
45. www.greencarcongress.com/2005/03/bolloreacute gr46. www.avestor.com/automotiveev.ch247. G.L. Henriksen and D.R. Vissers, J. Power Sources 51 (1994) 115.48. D.A.J. Rand, R. Woods and R.M. Dell, "Batteries for Electric Vehicles", Research Study
Press, Taunton, U.K., 1998.49. T.D. Kaun, P.A. Nelson, L. Redey, D.R. Vissers and G.L. Hendriksen, Electrochim. Ada 38
(1993) 1269.50. G.L. Henricksen and A.N. Jansen, in "Handbook of Batteries" (Chapter 41), D. Linden and
T.B. Reddy, Eds., McGraw-Hill, New York, 2002.51. H. Bohm, in "Handbook of Battery Materials", J.O. Besenhard, Ed., Wiley-VCH, Weinstein,
1999.52. J.W. Braithwaite and W.L. Auxer, in "Handbook of Batteries" (Chapter 40), D. Linden and
T.B. Reddy, Eds., McGraw-Hill, New York, 2002.53. www.electricitvstorage.org/pubs/2001/IEEE PES Winter2001/wm01nas54. www.electricitvstorage.org/pubs/2004/Newsletter Oct 200455. J. Kondoh, I. Ishii, H. Yamaguchi, A. Murata, K. Otani, K. Sakuta, N. Higuchi, S. Sekine
and M. Kamimoto, Energy Convers. Manag. 41 (2000) 1863.56. R.M. Dell and D.A.J. Rand, "Understanding Batteries", RSC, Cambridge, U.K., 2001.57. www.greencarcongress.com/2005/05/zestful58. P.C. Symons and P.C. Butler, in "Handbook of Batteries" (Chapter 37), D. Linden and T.B.
Reddy, Eds., McGraw-Hill, New York, 2002.