Next Article in Journal
Next Article in Special Issue
Previous Article in Journal

Membranes 2012, 2(2), 216-227; doi:10.3390/membranes2020216

Review
Oxygen Selective Membranes for Li-Air (O2) Batteries
Owen Crowther * and Mark Salomon *
MaxPower, Inc., 141 Christopher Lane, Harleysville, PA 19438, USA
*
Author to whom correspondence should be addressed; Email: Owen.Crowther@MaxPowerInc.com (O.C.); Mark.Salomon@MaxPowerInc.com (M.S.); Tel.: +1-215-256-4575; Fax: +1-215-256-1674.
Received: 17 April 2012 / Accepted: 7 May 2012 / Published: 11 May 2012

Abstract

: Lithium-air (Li-air) batteries have a much higher theoretical energy density than conventional lithium batteries and other metal air batteries, so they are being developed for applications that require long life. Water vapor from air must be prevented from corroding the lithium (Li) metal negative electrode during discharge under ambient conditions, i.e., in humid air. One method of protecting the Li metal from corrosion is to use an oxygen selective membrane (OSM) that allows oxygen into the cell while stopping or slowing the ingress of water vapor. The desired properties and some potential materials for OSMs for Li-air batteries are discussed and the literature is reviewed.
Keywords:
lithium-air battery; oxygen selective membrane; oxygen permeability; ambient discharge

1. Introduction

While metal-air batteries based on zinc, magnesium and aluminum anodes are well developed technologies [1], the development of lithium-air (Li-air) batteries had remained elusive until the breakthrough study by Abraham and Jiang [2]. The attractiveness of Li-air batteries compared to other common battery systems is due to the promise of greatly improved energies and capacities for Li-air batteries. Theoretical energies and capacities for selected electrochemical systems were calculated [3,4,5] from critically evaluated Gibbs energies of formation data from [6], and the results are given in Table 1. The increasing number of publications on Li-air batteries is indicative of the importance of these batteries for future applications to electric vehicles (EVs) and hybrid electric vehicles (HEVs), portable electronics, unattended remote sensors and other applications that have recently been reviewed by Christensen et al. [7] and by Crowther and Salomon [8]. For the present review, we focus on new approaches under development at MaxPower and others relating to oxygen selective membranes (OSMs) for the air electrode of a primary nonaqueous, Li-air battery. Figure 1 shows two Li-air designs presently under development at MaxPower.

Table Table 1. Theoretical specific energy and capacity comparisons for selected battery systems.

Click here to display table

Table 1. Theoretical specific energy and capacity comparisons for selected battery systems.
Metal-air systemOCV (V)Specific energy (Wh/kg)Specific capacity (mAh/g)
2Li + ½O2→ Li2O (aprotic organic sln)2.91311,248 *3,862
Li + ½O2 ⇌ ½Li2O2 (aprotic organic sln)2.95911,425 *3,862
2Li + ½O2 + H2SO4 ⇌ Li2SO4 + H2O4.2742,046 *479
2Li + ½O2 + H2O ⇌ 2LiOH3.4465,789 *1,681
2Li + H2O (seawater) → 2LiOH + ½H22.5129,701 **3,862
Al + 0.75O2 + 1.5H2O ⇌ Al(OH)32.7014,021 *1,489
Mg + ½O2 + H2O ⇌ Mg(OH)22.7563,491 *1,267
Zn + ½O2 ⇌ ZnO1.6501,353 *820
x6C + LiCoO ⇌ xLiC6 + Li1-xCoO2 (organic)~4.2420 ***139 ***

* The molecular mass of O2 is not included in these calculations because O2 is freely available from the atmosphere and therefore does not have to be stored in the battery or cell; ** The molecular mass of H2O is not included since it is freely available from seawater (pH 8.2) and does not have to be stored in the battery. *** Based on x = 0.5 in Li1−xCoO2.

Membranes 02 00216 g001 1024
Figure 1. Designs for Li-air batteries. In the protected anode approach shown at the left, the lithium anode is protected by a glass-ceramic disc (membrane) which is hermetically sealed to the anode. This solid-state glass-ceramic is a Li+ conductor impervious to water. In the protected cathode design shown at the right, the glass-ceramic solid-state membrane is removed and instead a flexible OSM is attached to the surface of the air electrode facing the atmosphere.

Click here to enlarge figure

Figure 1. Designs for Li-air batteries. In the protected anode approach shown at the left, the lithium anode is protected by a glass-ceramic disc (membrane) which is hermetically sealed to the anode. This solid-state glass-ceramic is a Li+ conductor impervious to water. In the protected cathode design shown at the right, the glass-ceramic solid-state membrane is removed and instead a flexible OSM is attached to the surface of the air electrode facing the atmosphere.
Membranes 02 00216 g001 1024

The design for the protected anode model is dependent upon a lithium ion (Li+) conducting membrane which is impervious to water, and for both aqueous and nonaqueous electrolyte solutions, present research for this membrane is focusing on Li+ conducting glass ceramics such as those developed by O’Hara Corporation [9,10,11] and its use in practical systems as originally proposed by Visco et al. [12]. Li-air cells based on the protected anode are well suited for application to both primary and rechargeable batteries, but technical problems relating to membrane chemical and mechanical stability, high cost and high resistivity are presently key areas of R&D as reviewed recently by Christensen et al. [7] and Crowther and Salomon [8]. In addition, secondary Li-air batteries face the problem of Li dendrite formation during charging that will limit cell cycle life and safety [13]. For the present review, we focus on nonaqueous primary Li-air cells based on the protected cathode design that use OSMs as shown in Figure 1.

2. Properties of Oxygen Selective Membranes

The protected cathode design for a Li-air power source is best suited for primary cells and batteries using nonaqueous electrolyte solutions. An OSM for Li-air cells and batteries should possess the following desired properties that are discussed in greater detail below.

  • High O2 permeability;

  • No water vapor permeability;

  • No electrolyte solvent permeability;

  • No carbon dioxide (CO2) permeability for secondary applications.

2.1. High O2 Permeability

Basic materials for use as OSM must be capable of dissolving large amounts of O2 (oxygen) and possess a high rate at which O2 can diffuse through these membranes. The permeability, Membranes 02 00216 i001, or transmission rate of O2 (OTR) through a barrier is dependent upon the solubility of O2 in the membrane and the rate of diffusion of O2 through the membrane, and is defined by

Membranes 02 00216 i002
where D is the diffusion coefficient [cm2 s−1] and S is the solubility coefficient (not solubility). The solubility coefficient can be determined experimentally or from known values of Henry’s Law constants, KH,cp, defined as
Membranes 02 00216 i003
where c is the concentration [mole L−1] and p is the partial pressure of O2 [mm Hg or Pa]. For most nonaqueous electrolyte solutions used in Li-air cells, KH,cp data for O2 are not available, but for a number pure nonaqueous solvents, KH,cp, values and solubilities have been compiled by Battino [14,15] and Dias et al. [16]. The units for permeability, P, normalized for membrane thickness is, from Equation (1).

P = cm3 (gas) cm cm−2s−1 mm Hg−1
where cm3 (gas) is actually a molar quantity evaluated at standard temperature and pressure that can determined from KH,cp data. The units for P are often given in Barrer which is defined by
1 Barrer = 10−11 cm3 (gas) cm cm−2 mm Hg−1

The oxygen flux, Membranes 02 00216 i004, can be directly related to maximum (limiting) current density, imax, assuming the oxygen reduction reaction (ORR) is mass transfer limited by O2 transport through the OSM. The maximum (limiting) current density due to O2 diffusion for an air cathode protected by an OSM is highly dependent on the magnitude of P, and below we show that membranes where P < 100 Barrer are not practical for a commercial Li-air cell. In view of the limited amount of data required to calculate permeability values from Equations (1–3), values of P can easily be determined experimentally using a barrier testing instrument such as the one available from MOCON, Inc.

Abraham and Jiang [2] originally hypothesized that the oxygen reduction reaction (ORR) in nonaqueous electrolyte solutions proceeds by the following mechanisms during discharge of a Li-air battery.

Membranes 02 00216 i005

Several recent publications, reviewed by Christensen et al. [6], demonstrated that the solvent actually reacts during ORR for electrolytes that use alkyl carbonates as solvents to form products with limited reversibility, namely lithium carbonate and lithium alkyl carbonates, and not the desired lithium peroxide. However, ORR in ether-based electrolyte solutions will proceed predominantly according to Equation (6).

The maximum current density due to diffusion of O2 through the membrane is based on the oxygen flux, Membranes 02 00216 i004, which can be related to permeability by the following equation.

Membranes 02 00216 i006
where Membranes 02 00216 i007 is the partial pressure gradient of O2 across the membrane and t is the membrane thickness. The partial pressure of O2 in air is ~160 mm Hg and will be 0 in the air electrode assuming O2 is the limiting reactant so Membranes 02 00216 i007= 160 mm Hg. The flux of O2 through the membrane can also be improved by decreasing the thickness of the membrane. However, membrane fabrication techniques typically limit the thickness to 10–25 µm before pinhole defects are present. Also, decreasing the thickness of the membrane will also increase the permeation of water vapor and electrolyte solvent. The maximum current density is given by
Membranes 02 00216 i008
where n is the equivalents of electrons reacted per mole of oxygen and F is Faraday’s constant Membranes 02 00216 i009. From Equations (5) and (6), n is equal to 4 for Li2O formation and 2 for Li2O2 formation. McCloskey et al. [17] experimentally determined n = 2.6 for the ORR in alkyl carbonates due to the reaction of the electrolyte solvent with Li+ and O2 to form lithium carbonate and lithium alkyl carbonates. Figure 2 shows the effect of O2 permeability in Barrer on maximum current density for a 1 µm thick membrane. The data were derived using the Equations (3, 4, 7, 8). This assumes the air window and air electrode have equal geometric areas. The maximum current density for a Li-air battery limited by O2 transport through an OSM of any thickness can be determined by dividing the imax for a given permeability obtained from Figure 2 by the actual thickness in microns of the OSM. For example, a membrane that is 1 µm thick with a permeability of 500 Barrer would have a limiting current density of approximately 68 mA cm−2 based on Li2O2 formation. The limiting current density is 1.4 mA cm−2 for the same membrane if it is 50 µm thick.

Membranes 02 00216 g002 1024
Figure 2. Effect of O2 permeability on maximum current density, imax, for a 1 µm thick OSM. Black circle points correspond to n = 2, red triangle points correspond to n = 2.6, green square points correspond to n = 4 equivalent e per mole of O2.

Click here to enlarge figure

Figure 2. Effect of O2 permeability on maximum current density, imax, for a 1 µm thick OSM. Black circle points correspond to n = 2, red triangle points correspond to n = 2.6, green square points correspond to n = 4 equivalent e per mole of O2.
Membranes 02 00216 g002 1024

2.2. No Water Vapor Permeability

The three important gases in dry air are N2 (78 o/v), O2 (21 o/v) and CO2 (0.4 o/v), water being variable at ~1–4 o/v depending upon relative humidity. Materials considered for membranes will vary in ability to dissolve and transmit these gases. A solid, gel or immobilized liquid is required to maximize O2 transmission and retard water vapor. Since the molecular diameter of water is smaller than that of oxygen, porous membranes that separate gases based on Knudsen diffusion will not work for this application. In fact it is extremely difficult to prevent water transmission through membranes optimized for high O2 permeabilities. Figure 3 shows the Li metal negative electrode from cells discharged in wet air (23 °C, 20% RH) using a Teflon coated fiberglass cloth (TCFC) OSM (left) and without OSM [18]. The Li is relatively pristine for the cell that used the OSM and completely consumed to form lithium hydroxide in the cell with no OSM.

Practically, it is not necessary for an OSM to be a perfect water vapor barrier for primary applications. However, small amounts of water will react with Li to form a resistive surface film. Even water concentrations of 200 ppm will increase the Li resistivity, most likely due to thickening of the film on the Li. This exact increase in resistivity is highly dependent on electrolyte salt, electrolyte solvent, and the amount of water in the electrolyte [19]. MaxPower has found that selectivities of 2.5 to 5 mol O2 per mol H2O will allow for normal discharge of a primary Li-air cell for at least one week.

Membranes 02 00216 g003 1024
Figure 3. Pictures of Li metal negative electrode after cell discharge in humid air for cells using an OSM (left) and with no membrane (right).

Click here to enlarge figure

Figure 3. Pictures of Li metal negative electrode after cell discharge in humid air for cells using an OSM (left) and with no membrane (right).
Membranes 02 00216 g003 1024

2.3. No Electrolyte Solvent Permeability

Read et al. [20] demonstrated increasing the O2 solubilities of a Li-air electrolyte results in increased capacity. However, electrolyte solvents with high O2 solubilities tend to have low viscosities and boiling points and will evaporate quickly [20,21]. Electrolyte evaporation will lead to premature cell failure since Li+ in the electrolyte will not be able to reach all of the active carbon reaction sites. Figure 4 shows the evaporation rate for a typical lab cell with and without an OSM [16]. The electrolyte solution used in this study was 1 mol dm−3 LiBF4 in a 1:1:1 (o/v) solvent mixture of propylene carbonate (PC), dimethyl carbonate (DMC) and methoxybenzene (MOB). The use of a TCFC OSM reduces the evaporation from approximately 40% to 2% over the course of a month, a very acceptable number for continuous operation for primary applications. MaxPower has observed materials with high water vapor permeabilities also have high electrolyte solvent permeabilities. One measure of electrolyte compatibility is to soak the OSM in a given electrolyte for a period of time. Ideally, there would be no mass gain and no swelling of the OSM after removal from the solvent. The actual solvent permeation rate can also be measured according to ASTM F739.

Membranes 02 00216 g004 1024
Figure 4. Evaporation rates of a typical electrolyte from a pouch cell with and without an OSM [18].

Click here to enlarge figure

Figure 4. Evaporation rates of a typical electrolyte from a pouch cell with and without an OSM [18].
Membranes 02 00216 g004 1024

2.4. No CO2 Permeability for Secondary Applications

Carbon dioxide transmission through most OSM materials is often comparable to oxygen where, for example, ratios of P(O2)/P(CO2) are often less than unity. Carbon dioxide will react with the Li2O2 (or even Li2O) discharge product to form lithium carbonate (Li2CO3). Li2O2 can reversibly evolve O2 during cell charging while Li2CO3 cannot [22]. McCloskey et al. [23] recently highlighted additional problems with Li2CO3 formation. Therefore, the OSM, if being used for a rechargeable Li-air battery, must also be an effective CO2 barrier for acceptable cycle life. This is a challenge since materials with high O2 permeabilities tend to also have high CO2 permeabilities [14,15,16]. However, the actual discharge product does not matter in primary Li-air cells so there is no requirement that the OSM is a CO2 barrier for primary applications [18].

Nitrogen being inert will also have little or no effect on the performance of Li-air cells. It is interesting to note the for materials which exhibit high O2 solubility, P(O2)/P(N2) ratios are generally >1 thus slightly enriching the relative O2 content over N2.

3. Basic Materials for Oxygen Selective Membranes

Oxygen selective membranes can be fabricated or synthesized, or commercially obtained as polymeric films. Two specific (preferred) groups of materials of interest for fabrication of O2-selective membranes in various configurations (gels, polymers, liquids immobilized in a porous inert substrate) include the following.

1. Fluorinated hydrocarbons, polyethers (e.g., Krytox 1506), polyperfloroalkyl oxides, (polyperfloroalkyl amines) have been used membranes based on liquids immobilized in inert substrates [24,25,26], gels [26,27], and chemically and UV cured polypefloroalkyl oxides [25]. Typical values for P(O2) for these membranes approach 1000 Barrer with P(O2)/P(H2O) ~3–4 [25].

2. Polysiloxanes, silicone oils, fluorinated polysiloxanes, and fluorinated polysiloxane copolymer with alkyl methacrylates. Polysiloxanes are thermally stable, exhibit high O2 solubilities, can be used as a liquid immobilized in an inert polymer [25] and thermally or UV cured (vulcanized) to produce a silicon rubber [4,25,26,27] Typical values for the permeability of O2 in dimethylsilicone rubbers are above 600 Barrer [28,29], and around 100–250 Barrer in methacryloxypropyl terminated polydimethyl contact lenses [30].

Other materials that have been tested as an OSM for Li-air batteries are Melinex 301H (ML) [31,32,33], high density polyethylene (HDPE) [31], silicalite zeolite or PTFE on nickel foam support [34], silicone oil immobilized in Teflon (PTFE) or nickel/ytrria stabilized zirconia (YSZ)/silicate layered membranes [35], and TCFC with [36] and without [18,36] a silicone adhesive layer. These materials will all be discussed further in below.

4. Review of Oxygen Selective Membrane Literature

The two most active groups of researchers developing OSMs are those from MaxPower Inc. and the Pacific Northwest National Laboratory (PNNL). Both groups report different experimental approaches, and a concise summary of these approaches is presented here.

Zhang et al. [31] tested both ML and HDPE in various sized Li-air cells discharged under ambient conditions. ML (Dupont Teijin Films) is a heat sealable polymer that acted both as the packaging and OSM. It consists of a polyethylene terephthalate (PET) layer and a terephthalate/isophthalate copolyester of ethylene glycol thermal bonding layer. Cells using 20 µm ML were able to discharge in 20% RH for 33 days at a current density of 0.05 mA cm−2 with a taper at the 2V cutoff to 0.01 mA cm−2. An optimized pouch cell demonstrated a energy density of 362 Wh kg−1 including package, which is the highest published energy density for a nonaqueous Li-air battery. Cells using 30 µm thick ML could not discharge for more than one day due to O2 starvation. The measured O2 permeability of the ML membrane was ~0.02 Barrer. This value corresponds well with the literature value of PET of 0.01 Barrer [37]. From this permeability value the maximum operating current density for this cell ~0.2 µA cm−2 depending on the discharge product using the Equations (4), (7) and (8). The cell packaging was made of ML, so the assumption in Equation (8) that the OSM and air electrode have equal areas is not true in the case. Applying an assumed correction factor that the OSM has an area of 3 times the electrode, the cell should only be able to support a current density of ~0.6 µA cm−2. This is two orders of magnitude lower than the actual current density of 50 µA cm−2. This discrepancy was attributed to the fact the ML absorbed electrolyte causing the polymer pore size to expand resulting in a higher diffusion coefficient for O2 than in the case of the dry measurement of permeability. Higher O2 diffusion coefficients would result in higher permeabilities via Equation (1). The low current density results in a lower power density of 46 mW g−1 that limits the applications of this battery despite the high energy density [38]. HDPE was also tested in this study but the cells did not run well despite the improved O2 permeability of 2 Barrer (membrane from Mid South Extrusion) and 4 Barrer (membrane from Blueridge Films, Inc.). This is most likely because the permeabilities of moisture was also high, so the cells failed because of corrosion of the Li anode [31].

Other OSM membranes developed at PNNL were supported either YSZ/silicate or PTFE on Ni metal foam substrates [34]. Initial experiments on these membranes proved unsuccessful because the porosity of the membranes allowed water vapor to enter the cell via Knudsen diffusion and corrode the Li anode. The cells performed better when a dense, thin PTFE membrane was spin coated on the substrate. Cells using this membrane were able to discharge for 21 days in air at 20% RH at a current density of 0.05 mA cm−2, corresponding to capacities of 1,022 mAh g−1 C. The control cell for this experiment discharged under the same conditions with no OSM only demonstrated a capacity of ~300 mAh g−1 C. The actual thickness of the PTFE layer was 1–10 µm. The literature value for O2 permeability in Teflon is 4–10 Barrer [39]. Therefore, a 1 µm membrane should be able to support a 0.25–2 mA cm−2 discharge depending on the actual permeability and discharge product. Thicker membranes would demonstrate lower maximum current densities. However, they did not attempt to test these membranes at higher rates, to our knowledge. Hydrophobic liquids with high O2 solubility were also immobilized in porous membranes to fabricate OSMs [35]. Silicone oils were used as the hydrophobic liquid and several substrates were studied. Silicone oils with higher viscosities performed better, which was attributed to lower water vapor permeation rates. Another possibility is the higher viscosity liquids remained immobilized in the substrate pore better. Cells discharged in 20% RH at 0.05 mA cm−2 demonstrated capacities between 600–800 mAh g−1 C using the OSMs and only 250 mAh g−1 with no protection.

MaxPower, Inc. has been developing higher rate OSMs for Li-air batteries with increased power densities. Early work focused on immobilizing hydrophobic liquids with high O2 solubilities like perfluorotributylamine, perfluorodecalin, and Krytox 1506 into microporous membranes [26]. Other OSMs were fabricated from gelled FMS123 liquid and silicon rubber [26]. One method to immobilize liquids under development is hardening silicone based liquids via UV curing [27]. For example, a polysiloxane-methacrylate copolymer (Gelest) was prepare by dipping a nonwoven polyphenylene sulfide (PPS) membrane into a mixture of methacryloxypropyle polydimethylsiolxanes and photo initiator and exposing to a UV source with 210–315 nm wavelength with an average power of 1,400 mJ cm−2 to crosslink the material. Finished OSMs had thicknesses between 330–1,016 µm. Li-air cell laboratory cells (pouch type, 10 cm2) were discharged at a rate of 0.1 mA cm−2 at room temperature and 15% RH. The cells with thinner OSMs demonstrated improved discharged capacities of 947 mAh g−1 C compared to 786 mAh g−1 C for the control cell discharged with no OSM. However, these OSMs were relatively thick limiting O2 flux to the air electrode and thus maximum current density. Thinner OSMs (76–89 µm) were fabricated using a RTV-amine (Semicosil 964, Wacker Silicones) coated directly onto an air electrode. The silicone rubber hardened by being moisture cured overnight. Cells discharged with this OSM were able to demonstrate capacities of almost 600 mAh g−1 C at a high rate of 0.5 mA cm−2. This capacity was three times higher than that demonstrated by the control cell discharged under the same conditions with no OSM.

Difficulties reproducibly fabricating thin, pinhole free OSMs led to the investigation of commercially produced membranes. TCFC, mentioned above, was found to work successfully [18,36]. The membrane is 70 µm thick and has an O2 permeability of 240 Barrer. The selectivity at room temperature from air is 2.5–5 mole of O2 per mole water vapor depending on the relative humidity. Cells were demonstrated to discharge at rates as high as 0.2 mA cm−2, though they failed at rates of 0.5 mA cm−2. 100 cm2 fixtured cells with dramatically reduced electrolyte quantities discharged for more than 2000 mAh g−1 C at a rate of 0.1 mA cm−2 in air at 40–50% RH. This was evidence in addition to figure 4 that electrolyte evaporation was slowed to acceptable rates. Pouch type laboratory cells (10 cm2) discharged for over 6,000 mAh g−1 C in air at 20% RH at a rate of 0.1 mA cm−2.

Sigmund et al. [40,41] has reported on superhydrophobic membranes potentially for Li-air cells based on electrospun Teflon AF2400 though it has not been tested in an operating Li-air cell to our knowledge. Teflon AF2400 is an interesting potential OSM material because of its high O2 permeability of 990 Barrer and excellent solvent resistance [42]. However, these electrospun membranes may not work well in an actual cell due to the highly porous nature of electrospun mats, leading to problems associated with Knudsen diffusion of water vapor described above.

5. Conclusions

OSMs have been demonstrated to successfully allow for ambient operation of Li-air batteries in literature. The desired properties of an OSM are high oxygen permeability, no water vapor permeability, no electrolyte solvent permeability, and no carbon dioxide permeability for secondary applications. In practice, no materials exist with no water vapor permeability, however, materials with higher O2 permeation rates (compared to water vapor) can successfully protect the lithium metal anode in a primary Li-air battery. All materials demonstrated as OSMs in the available literature suffer from relatively low O2 permeabilities, thus limiting the maximum discharge current density. Therefore novel membranes based on materials with higher O2 permeabilities (> 100 Barrer at least) must be developed to increase the power density of Li-air batteries.

Acknowledgments

We would like to acknowledge the US Army for funding MaxPower Inc.’s primary Li-air program under contract W15P7T-10-C-H602.

References

  1. Atwater, T.G.; Dobley, A. Metal/air batteries. In Linden’s Handbook of Batteries, 4th; Reddy, T.B., Ed.; McGraw-Hill Professional: New York, NY, USA, 2010. [Google Scholar]
  2. Abraham, K.M.; Jiang, Z. A polymer electrolyte-based rechargeable lithium/oxygen battery. J. Electrochem. Soc. 1996, 143, 1–5. [Google Scholar]
  3. Kowalczk, I.; Read, J.; Salomon, M. Li-air batteries: A classic example of limitations owing to solubilities. Pure Appl. Chem 2007, 79, 851–860. [Google Scholar]
  4. Crowther, O.; Meyer, B.; Morgan, M.; Salomon, M. Primary Li-air cell development. J. Power Sources 2011, 196, 1498–1502. [Google Scholar]
  5. Crowther, O.; Meyer, B.; Morgan, M.; Salomon, M. Erratum to “primary Li-air cell development”. J. Power Sources 2011, 196, 1498–1502. [Google Scholar]
  6. Bard, A.J.; Parsons, R.; Jordan, J. Standard Potentials in Aqueous Solution; Marcel Dekker: New York, NY, USA, 1995. [Google Scholar]
  7. Christensen, J.; Albertus, P.; Sanchez-Carrera, R.S.; Lohmann, T.; Kozinsky, B.; Liedtke, R.; Ahmed, J. A critical review of Li/air batteries. J. Electrochem. Soc. 2012, 159, R1–R30. [Google Scholar]
  8. Crowther, O.; Salomon, M. Aqueous Li-air (O2) systems. In Advanced Lithium Batteries; Scrosati, B., Abraham, K.M., van Shalkwijk, W., Eds.; John Wiley: Hoboken, NJ, USA, 2012. in press.. [Google Scholar]
  9. Fu, J. Superionic conductivity of glass-ceramics in the system Li2O-Al2O3-TiO2-P2O5. Solid State Ionics 1997, 96, 195–200. [Google Scholar]
  10. Fu, J. Fast Li+ ion conducting glass-ceramics in the system Li2O-Al2O3-GeO2-P2O5. Solid State Ionics 1997, 104, 191–194. [Google Scholar]
  11. Fu, J. Lithium Ion Conductive Glass-Ceramics and Electric Cells And Gas Sensors Using the Same. U.S. Patent 6,030,909, 24 October 1997. [Google Scholar]
  12. Visco, S.J.; Katz, B.D.; Nimon, Y.S.; de Jonghe, L.C. Protected Active Metal Electrode and Battery Cell Structure with Non-Aqueous Interlayer Architecture. US Patent 7,282,295, 16 October 2007. [Google Scholar]
  13. Scrosati, B.; Garche, J. Lithium batteries: Status, prospects, and future. J. Power Sources 2010, 195, 2419–2430. [Google Scholar] [CrossRef]
  14. Battino, R.; Rettich, T.R.; Tominaga, T. The solubility of oxygen and ozone in liquids. J. Phys. Chem. Ref. Data 1983, 12, 163–179. [Google Scholar]
  15. Battino, R. IUPAC Solubility Data Ser. 1984, 7, 1–519.
  16. Dias, A.M.A.; Freire, M.; Coutinho, J.A.P.; Marrucho, I.M. Solubility of oxygen in liquid perfluorocarbons. Fluid Phase Equilib. 2004, 222–223, 325–330. [Google Scholar] [CrossRef]
  17. McCloskey, B.D.; Bethune, D.S.; Shelby, R.M.; Girishkumar, G.; Luntz, A.C. Solvent’ critical role in nonaqueous lithium-oxygen battery electrochemistry. J. Phys. Chem. Lett. 2011, 2, 1161–1166. [Google Scholar]
  18. Crowther, O.; Keeny, D.; Moureau, D.M.; Meyer, B.; Salomon, M.; Hendrickson, M. Electrolyte optimization for the primary lithium metal air battery using an oxygen selective membrane. J. Power Sources 2012, 202, 347–351. [Google Scholar]
  19. Zaban, A.; Zinigrad, E.; Aurbarch, D. Impedance spectroscopy of li electrodes. 4. A general simple model of the li-solution interphase in polar aprotic systems. J. Phys. Chem. 1996, 100, 3089–3101. [Google Scholar] [CrossRef]
  20. Read, J.; Mutolo, K.; Ervin, M.; Behl, W.; Wolfenstine, J.; Driedger, A.; Foster, D. Oxygen transport properties of organic electrolytes and performance of lithium/oxygen battery. J. Electrochem. Soc. 2003, 150, A1351–A1356. [Google Scholar]
  21. Xu, W.; Xiao, J.; Zhang, J.; Wang, D.; Zhang, J.-G. Optimization of nonaqueous electrolyte for primary lithium/air batteries operated in ambient environments. J. Electrochem. Soc. 2009, 156, A773–A779. [Google Scholar]
  22. Freunberger, S.A.; Chen, Y.; Peng, Z.; Griffin, J.M.; Hardwick, L.J.; Bardé, F.; Novák, P.; Bruce, P.G. Reactions in rechargeable lithium-o2 battery with alkyl carbonate electrolytes. J. Am. Chem. Soc. 2011, 133, 8040–8047. [Google Scholar]
  23. McCloskey, B.D.; Speidel, A.; Scheffler, R.; Miller, D.C.; Viswanathan, V.; Hummelshøj, J.S.; Nørskov, J.K.; Luntz, A.C. Twin problems of interfacial carbonate formation in nonaqueous Li-O2 batteries. J. Phys. Chem. Lett. 2012, 3, 997–1001. [Google Scholar]
  24. Goldstein, J.; Korall, M.; Brokman, A. Electrodes for Metal/Air Batteries and Bipolar Metal/Air Batteries Incorporating the Same. US Patent 5,145,752, 8 September 1992. [Google Scholar]
  25. Reynolds, T.A.; Brose, D.J.; Golovin, M.N. Membrane for Selective Transport of Oxygen Over Water Vapor and Metal-Air Electrochemical Cell Including Said Membrane. US Patent 5,985,475, 16 November 1999. [Google Scholar]
  26. Chua, D.; Driedger, A.; Meyer, B.; Morgan, M.; Salomon, M. Protected Lithium-Air Cells by Oxygen-Selective Permeable Cathode Membranes. US Patent 0,177,400, 21 January 2011. [Google Scholar]
  27. Clarke, R. Fluorosiloxane Optical Cladding. US Patent 4,317,616, 2 March 1982. [Google Scholar]
  28. Blume, I.; Schwering, P.J.F.; Mulder, M.H.V.; Smolders, C.A. Vapor sorption and permeation properties of poly(dimethylsiloxane) films. J. Membr. Sci. 1991, 61, 85–97. [Google Scholar]
  29. Zhang, H.; Cloud, A. The permeability characteristics of silicone rubber. Dallas, TX, USA, November 2006; Pilato, L.A., Kliger, H.S., Beckwith, S.W., Eds.; Destech Pubns Inc.: Lancaster, PA, USA, 2006. [Google Scholar]
  30. Lai, Y.-C.; Lang, W.; Quinn, E.T.; Ruscio, D.V. Hydrogel Copolymers for Biomedical Devices. US Patent 2006/0142525 A1, 29 June 2006. [Google Scholar]
  31. Zhang, J.-G.; Wang, D.; Xu, W.; Xiao, J.; Williford, R.E. Ambient operation of Li/air batteries. J. Power Sources 2010, 195, 4332–4337. [Google Scholar]
  32. Wang, D.; Xiao, J.; Xu, W.; Zhang, J.-G. High capacity pouch-type Li-air batteries. J. Electrochem. Soc. 2010, 157, A760–A764. [Google Scholar]
  33. Xiao, J.; Mei, D.; Li, X.; Xu, W.; Wang, D.; Graff, G.L.; Bennet, W.D.; Ne, Z.; Saraf, L.V.; Aksay, I.A.; Liu, J.; Zhang, J.-Z. Hierarchically porous graphene as lithium-air battery electrode. Nano Lett. 2011, 11, 5071–5078. [Google Scholar]
  34. Zhang, J.; Xu, W.; Li, X.; Liu, W. Air dehydration membranes for nonaqueous lithium-air batteries. J. Electrochem. Soc. 2010, 157, A940–A946. [Google Scholar]
  35. Zhang, J.; Xu, W.; Liu, W. Oxygen-selective immobilized liquid membranes for operation of lithium-air batteries in ambient air. J. Power Sources 2010, 195, 7438–7444. [Google Scholar]
  36. Crowther, O.; Chua, D.; Eppley, W.; Meyer, B.; Salomon, M.; Driedger, A.; Morgan, M. Lithium-air cell protective membranes comprising polytetrafluroethylene coated fiberglass cloth. US Patent 2011/0177401 A1, 21 July 2011. [Google Scholar]
  37. Liu, R.Y.F.; Hu, Y.S.; Schiraldi, D.A.; Hiltner, A.; Baer, E. Crystallinity and oxygen transport properties of PET bottle walls. J. Appl. Polymer Sci. 2004, 94, 671–677. [Google Scholar]
  38. Kraytsberg, A.; Ein-Eli, Y. Review on Li-air batteries-opportunities, limitations, and perspective. J. Power Sources 2011, 196, 886–893. [Google Scholar] [CrossRef]
  39. Aiba, S.; Ohashi, M.; Huang, S.-Y. Rapid determination of oxygen permeability of polymer membranes. Ind. Eng. Chem. Fundamen. 1968, 7, 497–502. [Google Scholar]
  40. Muthiah, P.; Hsu, S.H.; Sigmund, W. Coaxially electrospun PVDF-Teflon AF and Teflon AF-PVDF core-sheath nanofiber mats with superhydrophobic properties. Langmuir 2010, 26, 12483–12487. [Google Scholar]
  41. Scheffler, R.; Bell, N.S.; Sigmund, W. Electrospun Teflon AF fibers for superhydrophobic membranes. J. Mater. Res. 2010, 25, 1595–1600. [Google Scholar]
  42. DuPont™ Teflon® Afamorphous Fluoropolymers; DuPont Fluoroproducts: Wilmington, DE, USA, 2012. Available online: http://www2.dupont.com/Teflon_Industrial/en_US./downloads/h44587.pdf (accessed on 12 April 2012).
Membranes EISSN 2077-0375 Published by MDPI AG, Basel, Switzerland RSS E-Mail Table of Contents Alert