Solid oxide fuel cell

Scheme of a solid-oxide fuel cell

A solid oxide fuel cell (or SOFC) is an electrochemical conversion device that produces electricity directly from oxidizing a fuel. Fuel cells are characterized by their electrolyte material; the SOFC has a solid oxide or ceramic electrolyte. Advantages of this class of fuel cells include high efficiency, long-term stability, fuel flexibility, low emissions, and relatively low cost. The largest disadvantage is the high operating temperature which results in longer start-up times and mechanical and chemical compatibility issues.[1]

Introduction

Solid oxide fuel cells are a class of fuel cells characterized by the use of a solid oxide material as the electrolyte. SOFCs use a solid oxide electrolyte to conduct negative oxygen ions from the cathode to the anode. The electrochemical oxidation of the oxygen ions with hydrogen or carbon monoxide thus occurs on the anode side. More recently, proton-conducting SOFCs (PC-SOFC) are being developed which transport protons instead of oxygen ions through the electrolyte with the advantage of being able to be run at lower temperatures than traditional SOFCs.

They operate at very high temperatures, typically between 500 and 1,000 °C. At these temperatures, SOFCs do not require expensive platinum catalyst material, as is currently necessary for lower-temperature fuel cells such as PEMFCs, and are not vulnerable to carbon monoxide catalyst poisoning. However, vulnerability to sulfur poisoning has been widely observed and the sulfur must be removed before entering the cell through the use of adsorbent beds or other means.

Solid oxide fuel cells have a wide variety of applications from use as auxiliary power units in vehicles to stationary power generation with outputs from 100 W to 2 MW. In 2009, Australian company, Ceramic Fuel Cells successfully achieved an efficiency of a SOFC device up to the previously theoretical mark of 60%.[2][3] The higher operating temperature make SOFCs suitable candidates for application with heat engine energy recovery devices or combined heat and power, which further increases overall fuel efficiency.

Because of these high temperatures, light hydrocarbon fuels, such as methane, propane and butane can be internally reformed within the anode. SOFCs can also be fueled by externally reforming heavier hydrocarbons, such as gasoline, diesel, jet fuel (JP-8) or biofuels. Such reformates are mixtures of hydrogen, carbon monoxide, carbon dioxide, steam and methane, formed by reacting the hydrocarbon fuels with air or steam in a device upstream of the SOFC anode. SOFC power systems can increase efficiency by using the heat given off by the exothermic electrochemical oxidation within the fuel cell for endothermic steam reforming process. Additionally, solid fuels such as coal and biomass may be gasified to form syngas which is suitable for fueling SOFCs in integrated gasification fuel cell power cycles.

Thermal expansion demands a uniform and well-regulated heating process at startup. SOFC stacks with planar geometry require in the order of an hour to be heated to light-off temperature. Micro-tubular fuel cell design geometries promise much faster start up times, typically in the order of minutes.

Unlike most other types of fuel cells, SOFCs can have multiple geometries. The planar fuel cell design geometry is the typical sandwich type geometry employed by most types of fuel cells, where the electrolyte is sandwiched in between the electrodes. SOFCs can also be made in tubular geometries where either air or fuel is passed through the inside of the tube and the other gas is passed along the outside of the tube. The tubular design is advantageous because it is much easier to seal air from the fuel. The performance of the planar design is currently better than the performance of the tubular design however, because the planar design has a lower resistance comparatively. Other geometries of SOFCs include modified planar fuel cell designs (MPC or MPSOFC), where a wave-like structure replaces the traditional flat configuration of the planar cell. Such designs are highly promising, because they share the advantages of both planar cells (low resistance) and tubular cells.

Operation

A solid oxide fuel cell is made up of four layers, three of which are ceramics (hence the name). A single cell consisting of these four layers stacked together is typically only a few millimeters thick. Hundreds of these cells are then connected in series to form what most people refer to as an "SOFC stack". The ceramics used in SOFCs do not become electrically and ionically active until they reach very high temperature and as a consequence the stacks have to run at temperatures ranging from 500 to 1,000 °C. Reduction of oxygen into oxygen ions occurs at the cathode. These ions can then diffuse through the solid oxide electrolyte to the anode where they can electrochemically oxidize the fuel. In this reaction, a water byproduct is given off as well as two electrons. These electrons then flow through an external circuit where they can do work. The cycle then repeats as those electrons enter the cathode material again.

Balance of plant

Most of the downtime of a SOFC stems from the mechanical balance of plant, the air preheater, prereformer, afterburner, water heat exchanger, anode tail gas oxidizer, and electrical balance of plant, power electronics, hydrogen sulfide sensor and fans. Internal reforming leads to a large decrease in the balance of plant costs in designing a full system.[3]

Anode

The ceramic anode layer must be very porous to allow the fuel to flow towards the electrolyte. Consequently, granular matter is often selected for anode fabrication procedures.[4] Like the cathode, it must conduct electrons, with ionic conductivity a definite asset. The most common material used is a cermet made up of nickel mixed with the ceramic material that is used for the electrolyte in that particular cell, typically YSZ (yttria stabilized zirconia) nanomaterial-based catalysts, this YSZ part helps stop the grain growth of nickel. The anode is commonly the thickest and strongest layer in each individual cell, because it has the smallest polarization losses, and is often the layer that provides the mechanical support. Electrochemically speaking, the anode’s job is to use the oxygen ions that diffuse through the electrolyte to oxidize the hydrogen fuel. The oxidation reaction between the oxygen ions and the hydrogen produces heat as well as water and electricity. If the fuel is a light hydrocarbon, for example methane, another function of the anode is to act as a catalyst for steam reforming the fuel into hydrogen. This provides another operational benefit to the fuel cell stack because the reforming reaction is endothermic, which cools the stack internally.

Electrolyte

The electrolyte is a dense layer of ceramic that conducts oxygen ions. Its electronic conductivity must be kept as low as possible to prevent losses from leakage currents. The high operating temperatures of SOFCs allow the kinetics of oxygen ion transport to be sufficient for good performance. However, as the operating temperature approaches the lower limit for SOFCs at around 600 °C, the electrolyte begins to have large ionic transport resistances and affect the performance. Popular electrolyte materials include yttria-stabilized zirconia (YSZ) (often the 8% form Y8SZ), scandia stabilized zirconia (ScSZ) (usually 9 mol%Sc2O3 – 9ScSZ) and gadolinium doped ceria (GDC).[5] The electrolyte material has crucial influence on the cell performances.[6] Detrimental reactions between YSZ electrolytes and modern cathodes such as lanthanum strontium cobalt ferrite (LSCF) have been found, and can be prevented by thin (<100 nm) ceria diffusion barriers.[7]

If the conductivity for oxygen ions in SOFC can remain high even at lower temperature (current target in research ~500 °C), material choice for SOFC will broaden and many existing problems can potentially be solved. Certain processing technique such as thin film deposition[8] can help solve this problem with existing material by:

– reducing the traveling distance of oxygen ions and electrolyte resistance as resistance is inversely proportional to conductor length;

– producing grain structures that are less resistive such as columnar grain structure;

– controlling the micro-structural nano-crystalline fine grains to achieve "fine-tuning" of electrical properties;

– building composite with large interfacial areas as interfaces have shown to have extraordinary electrical properties.

Cathode

The cathode, or air electrode, is a thin porous layer on the electrolyte where oxygen reduction takes place. The overall reaction is written in Kröger-Vink Notation as follows:

\frac{1}{2}\mathrm{O_2(g)} + 2\mathrm{e'} + {V}^{\bullet\bullet}_o \longrightarrow {O}^{\times}_o

Cathode materials must be, at minimum, electronically conductive. Currently, lanthanum strontium manganite (LSM) is the cathode material of choice for commercial use because of its compatibility with doped zirconia electrolytes. Mechanically, it has similar coefficient of thermal expansion to YSZ and thus limits stresses buildup because of CTE mismatch. Also, LSM has low levels of chemical reactivity with YSZ which extends the lifetime of the material. Unfortunately, LSM is a poor ionic conductor, and so the electrochemically active reaction is limited to the triple phase boundary (TPB) where the electrolyte, air and electrode meet. LSM works well as a cathode at high temperatures, but its performance quickly falls as the operating temperature is lowered below 800 °C. In order to increase the reaction zone beyond the TPB, a potential cathode material must be able to conduct both electrons and oxygen ions. Composite cathodes consisting of LSM YSZ have been used to increase this triple phase boundary length. Mixed ionic/electronic conducting (MIEC) ceramics, such as the perovskite LSCF, are also being researched for use in intermediate temperature SOFCs as they are more active and can makeup for the increase in the activation energy of reaction.

Interconnect

The interconnect can be either a metallic or ceramic layer that sits between each individual cell. Its purpose is to connect each cell in series, so that the electricity each cell generates can be combined. Because the interconnect is exposed to both the oxidizing and reducing side of the cell at high temperatures, it must be extremely stable. For this reason, ceramics have been more successful in the long term than metals as interconnect materials. However, these ceramic interconnect materials are very expensive as compared to metals. Nickel- and steel-based alloys are becoming more promising as lower temperature (600–800 °C) SOFCs are developed. The material of choice for an interconnect in contact with Y8SZ is a metallic 95Cr-5Fe alloy. Ceramic-metal composites called 'cermet' are also under consideration, as they have demonstrated thermal stability at high temperatures and excellent electrical conductivity.

Polarizations

Polarizations, or overpotentials, are losses in voltage due to imperfections in materials, microstructure, and design of the fuel cell. Polarizations result from ohmic resistance of oxygen ions conducting through the electrolyte (iRΩ), electrochemical activation barriers at the anode and cathode, and finally concentration polarizations due to inability of gases to diffuse at high rates through the porous anode and cathode (shown as ηA for the anode and ηC for cathode). The cell voltage can be calculated using the following equation:

{V} = {E}_0 - {iR}_\omega - {\eta}_{cathode} - {\eta}_{anode}

where {E}_0 is the Nernst potential of the reactants and R represents the Thévenin equivalent resistance value of the electrically conducting portions of the cell. {\eta}_{cathode} and {\eta}_{anode} account for the remaining difference between the actual cell voltage and the Nernst potential. In SOFCs, it is often important to focus on the ohmic and concentration polarizations since high operating temperatures experience little activation polarization. However, as the lower limit of SOFC operating temperature is approached (~600 °C), these polarizations do become important.[9]

Above mentioned equation is used for determining the SOFC voltage (in fact for fuel cell voltage in general). This approach results in good agreement with particular experimental data (for which adequate factors were obtained) and poor agreement for other than original experimental working parameters. Moreover, most of the equations used require the addition of numerous factors which are difficult or impossible to determine. It makes very difficult any optimizing process of the SOFC working parameters as well as design architecture configuration selection. Because of those circumstances a few other equations were proposed:[10]

E_{SOFC} = \frac{E_{max}-i_{max}\cdot\eta_f\cdot r_1}{\frac{r_1}{r_2}\cdot\left( 1-\eta_f \right) + 1}

where: E_{SOFC} – cell voltage, E_{max} – maximum voltage given by the Nernst equation, i_{max} – maximum current density (for given fuel flow), \eta_f – fuel utilization factor,[10][11] r_1 – ionic specific resistance of the electrolyte, and r_2 – electric specific resistance of the electrolyte.

This method was validated and found to be suitable for optimization and sensitivity studies in plant-level modelling of various systems with solid oxide fuel cells.[12] With this mathematical description it is possible to account for different properties of the SOFC. There are many parameters which impact cell working conditions, e.g. electrolyte material, electrolyte thickness, cell temperature, inlet and outlet gas compositions at anode and cathode, and electrode porosity, just to name some. The flow in these systems is often calculated using the Navier-stokes equation.

Ohmic polarization

Ohmic losses in an SOFC result from ionic conductivity through the electrolyte. This is inherently a materials property of the crystal structure and atoms involved. However, to maximize the ionic conductivity, several methods can be done. Firstly, operating at higher temperatures can significantly decrease these ohmic losses. Substitutional doping methods to further refine the crystal structure and control defect concentrations can also play a significant role in increasing the conductivity. Another way to decrease ohmic resistance is to decrease the thickness of the electrolyte layer.

Ionic conductivity

An ionic specific resistance of the electrolyte as a function of temperature can be described by the following relationship:[10]

r_1 = \frac{\delta}{\sigma}

where: \delta – electrolyte thickness, and \sigma – ionic conductivity.

The ionic conductivity of the solid oxide is defined as follows:[10]

\sigma = \sigma_0\cdot e^\frac{-E}{R\cdot T}

where: \sigma_0 and E – factors depended on electrolyte materials, T – electrolyte temperature, and R – ideal gas constant.

Concentration polarization

The concentration polarization is the result of practical limitations on mass transport within the cell, and represents the voltage loss due to spatial variations in reactant concentration at the chemically active sites. This situation can be caused when the reactants are consumed by the electrochemical reaction faster than they can diffuse into the porous electrode, and can also be caused by variation in bulk flow composition. The latter is due to the fact that the consumption of reacting species in the reactant flows causes a drop in reactant concentration as it travels along the cell, which causes a drop in the local potential near the tail end of the cell.

The concentration polarization occurs in both the anode and cathode. The anode can be particularly problematic, as the oxidation of the hydrogen produces steam, which further dilutes the fuel stream as it travels along the length of the cell. This polarization can be mitigated by reducing the reactant utilization fraction or increasing the electrode porosity, but these approaches each have significant design trade-offs.

Activation polarization

The activation polarization is the result of the kinetics involved with the electrochemical reactions. Each reaction has a certain activation barrier that must be overcome in order to proceed and this barrier leads to the polarization. The activation barrier is the result of many complex electrochemical reaction steps where typically the rate limiting step is responsible for the polarization. The polarization equation shown below is found by solving the Butler–Volmer equation in the high current density regime (where the cell typically operates), and can be used to estimate the activation polarization:

{\eta}_{act} = \frac {RT} {{\beta}zF} \times ln \left(\frac {i} {{i}_0} \right)

where:

The polarization can be modified by microstructural optimization. The Triple Phase Boundary (TPB) length, which is the length where porous, ionic and electronically conducting pathways all meet, directly relates to the electrochemically active length in the cell. The larger the length, the more reactions can occur and thus the less the activation polarization. Optimization of TPB length can be done by processing conditions to affect microstructure or by materials selection to use a mixed ionic/electronic conductor to further increase TPB length.

Target

DOE target requirements are 40,000 hours of service for stationary fuel cell applications and greater than 5,000 hours for transportation systems (fuel cell vehicles) at a factory cost of $40/kW for a 10 kW coal-based system[13] without additional requirements. Lifetime effects (phase stability, thermal expansion compatibility, element migration, conductivity and aging) must be addressed. The Solid State Energy Conversion Alliance 2008 (interim) target for overall degradation per 1,000 hours is 4.0%.[14]

Research

Research is going now in the direction of lower-temperature SOFC (600 °C) in order to decrease the materials cost, which will enable the use of metallic materials with better mechanical properties and thermal conductivity.

Research is currently under way to improve the fuel flexibility of SOFCs. While stable operation has been achieved on a variety of hydrocarbon fuels, these cells typically rely on external fuel processing. For the case of natural gas, the fuel is either externally or internally reformed and the sulfur compounds are removed. These processes add to the cost and complexity of SOFC systems. Work is under way at a number of institutions to improve the stability of anode materials for hydrocarbon oxidation and, therefore, relax the requirements for fuel processing and decrease SOFC balance of plant costs.

Research is also going on in reducing start-up time to be able to implement SOFCs in mobile applications.[15] Due to their fuel flexibility they may run on partially reformed diesel, and this makes SOFCs interesting as auxiliary power units (APU) in refrigerated trucks.

Specifically, Delphi Automotive Systems are developing an SOFC that will power auxiliary units in automobiles and tractor-trailers, while BMW has recently stopped a similar project. A high-temperature SOFC will generate all of the needed electricity to allow the engine to be smaller and more efficient. The SOFC would run on the same gasoline or diesel as the engine and would keep the air conditioning unit and other necessary electrical systems running while the engine shuts off when not needed (e.g., at a stop light or truck stop).

Rolls-Royce is developing solid-oxide fuel cells produced by screen printing onto inexpensive ceramic materials. Rolls-Royce Fuel Cell Systems Ltd is developing a SOFC gas turbine hybrid system fueled by natural gas for power generation applications in the order of a megawatt (e.g. Futuregen).

Ceres Power Ltd. has developed a low cost and low temperature (500–600 degrees) SOFC stack using cerium gadolinium oxide (CGO) in place of current industry standard ceramic, yttria stabilized zirconia (YSZ), which allows the use of stainless steel to support the ceramic.[16]

Solid Cell Inc. has developed a unique, low cost cell architecture that combines properties of planar and tubular designs, along with a Cr-free cermet interconnect.

The high temperature electrochemistry center (HITEC) at the University of Florida, Gainesville is focused on studying ionic transport, electrocatalytic phenomena and microstructural characterization of ion conducting materials.[17]

SiEnergy Systems, a Harvard spin-off company, has demonstrated the first macro-scale thin-film solid-oxide fuel cell that can operate at 500 degrees.[18]

SOEC

A solid oxide electrolyser cell (SOEC) is a solid oxide fuel cell set in regenerative mode for the electrolysis of water with a solid oxide, or ceramic, electrolyte to produce oxygen and hydrogen gas.[19]

ITSOFC

SOFCs that operate in an intermediate temperature (IT) range, meaning between 600 and 800 °C, are named ITSOFCs. Because of the high degradation rates and materials costs incurred at temperatures in excess of 900 °C, it is economically more favorable to operate SOFCs at lower temperatures. The push for high performance ITSOFCs is currently the topic of much research and development. One area of focus is the cathode material. It is thought that the oxygen reduction reaction is responsible for much of the loss in performance so the catalytic activity of the cathode is being studied and enhanced through various techniques, including catalyst impregnation.

LT-SOFC

Low temperature solid oxide fuel cells (LT-SOFCs), operating lower than 650 °C, are of great interest for future research because the high operating temperature is currently what restricts the development and deployment of SOFCs. A low temperature SOFC is more reliable due to smaller thermal mismatch and easier sealing. Additionally, a lower temperature requires less insulation, and therefore has lower cost. Cost is further lowered due to wider material choices for interconnects and compressive nonglass/ceramic seals. Perhaps most importantly, at a lower temperature, SOFCs can be started more rapidly and with less energy, which lends itself for uses in in portable and transport applications. Interestingly, as temperature decreases, the maximum theoretical fuel cell efficiency increases, in contrast to the Carnot cycle. For example, the maximum theoretical efficiency of an SOFC using CO as a fuel increases from 63% at 900 °C to 81% at 350 °C. [20] This is a materials issue, particularly for the electrolyte in the SOFC. YSZ is the most commonly used electrolyte because of its superior stability, despite not having the highest conductivity. Currently, the thickness of YSZ electrolytes is a minimum of ~10 μm due to deposition methods, and this requires a temperature above 700 °C. Therefore, low-temperature SOFCs are only possible with higher conductivity electrolytes. Various alternatives that could be successful at low temperature include gallium-doped ceria (GDC) and erbia-cation-stabilized bismuth (ERB). They have superior ionic conductivity at lower temperature, but this comes at the expense of lower thermodynamic stability. CeO2 electrolytes become electronically conductive and Bi2O3 electrolytes decompose to metallic Bi under the reducing fuel environment.[21] To combat this, researchers created a functionally graded ceria/bismuth-oxide bilayered electrolyte where the GDC layer on the anode side protects the ESB layer from decomposing while the ESB on the cathode side blocks the leakage current through the GDC layer. This leads to near-theoretical open-circuit potential (OPC) with two highly conductive electrolytes, that by themselves would not have been sufficiently stable for the application. This bilayer proved to be stable for 1400 hours of testing at 500 °C and showed no indication of interfacial phase formation or thermal mismatch. While this makes strides towards lowering the operating temperature of SOFCs, it also opens doors for future research to try and understand this mechanism.[22]

Researchers at the Georgia Institute of Technology dealt with the instability of BaCeO3 differently. They replaced a desired fraction of Ce in BaCeO3 with Zr to form a solid solution that exhibits proton conductivity, but also chemical and thermal stability over the range of conditions relevant to fuel cell operation. A new specific composition, Ba(Zr0.1Ce0.7Y0.2)O3-δ (BZCY7) that displays the highest ionic conductivity of all known electrolyte materials for SOFC applications. This electrolyte was fabricated by dry-pressing powders, which allowed for the production of crack free films thinner than 15 μm. The implementation of this simple and cost-effective fabrication method may enable significant cost reductions in SOFC fabrication.[23] However, this electrolyte operates at higher temperatures than the bilayered electrolyte model, closer to 600 °C rather than 500 °C.

Currently, given the state of the field for LT-SOFCs, progress in the electrolyte would reap the most benefits, but research into potential anode and cathode materials would also lead to useful results, and has started to be discussed more frequently in literature.

SOFC-GT

An SOFC-GT system is one which comprises a solid oxide fuel cell combined with a gas turbine. Such systems have been evaluated by Siemens Westinghouse and Rolls-Royce as a means to achieve higher operating efficiencies by running the SOFC under pressure. SOFC-GT systems typically include anodic and/or cathodic atmosphere recirculation, thus increasing efficiency.

Theoretically, the combination of the SOFC and gas turbine can give result in high overall (electrical and thermal) efficiency.[24] Further combination of the SOFC-GT in a combined cooling, heat and power (or trigeneration) configuration (via HVAC) also has the potential to yield even higher thermal efficiencies in some cases.[25]

DCFC

For the direct use of solid coal fuel without additional gasification and reforming processes, a direct carbon fuel cell (DCFC) has been developed as a promising novel concept of a high-temperature energy conversion system. The underlying progress in the development of a coal-based DCFC has been categorized mainly according to the electrolyte materials used, such as solid oxide, molten carbonate, and molten hydroxide, as well as hybrid systems consisting of solid oxide and molten carbonate binary electrolyte or of liquid anode (Fe, Ag, In, Sn, Sb, Pb, Bi, and its alloying and its metal/metal oxide) solid oxide electrolyte.[26][27][28][29][30]

See also

References

  1. ↑ Badwal, SPS. "Review of Progress in High Temperature Solid Oxide Fuel Cells". Journal of the Australian Ceramics society 50 (1).
  2. ↑ Ceramic fuel cells achieves world-best 60% efficiency for its electricity generator units. Ceramic Fuel Cells Limited. 19 February 2009
  3. 1 2 Electricity from wood through the combination of gasification and solid oxide fuel cells, Ph.D. Thesis by Florian Nagel, Swiss Federal Institute of Technology Zurich, 2008
  4. ↑ Ott, J; Gan, Y; McMeeking, R; Kamlah, M (2013). "A micromechanical model for effective conductivity in granular electrode structures" (PDF). Acta Mechanica Sinica. 29 (5): 682–698.
  5. ↑ Nigel Sammes, Alevtina Smirnova, Oleksandr Vasylyev (2005). "Fuel Cell Technologies: State and Perspectives". NATO Science Series, Mathematics, Physics and Chemistry 202: 19–34. doi:10.1007/1-4020-3498-9_3.
  6. ↑ Steele, B.C.H., Heinzel, A. (2001). "Materials for fuel-cell technologies". Nature 414 (Nov 15): 345–352. doi:10.1038/35104620. PMID 11713541.
  7. ↑ Mohan Menon, Kent Kammer; et al. (2007). "Processing of Ce1-xGdxO2-δ (GDC) thin films from precursors for application in solid oxide fuel cells". Advanced Materials Engineering. 15–17: 293–298. doi:10.4028/www.scientific.net/AMR.15-17.293.
  8. ↑ Charpentier, P (2000). "Preparation of thin film SOFCs working at reduced temperature". Solid State Ionics 135 (1-4): 373–380. doi:10.1016/S0167-2738(00)00472-0. ISSN 0167-2738.
  9. ↑ Hai-Bo Huo, Xin-Jian Zhu, Guang-Yi Cao (2006). "Nonlinear modeling of a SOFC stack based on a least squares support vector machine". Journal of Power Sources 162 (2): 1220–1225. doi:10.1016/j.jpowsour.2006.07.031.
  10. 1 2 3 4 Milewski J, Miller A. (2006). "Influences of The Type and Thickness of Electrolyte on Solid Oxide Fuel Cell Hybrid System Performance". Journal of Fuel Cell Science and Technology 3 (4): 396–402. doi:10.1115/1.2349519.
  11. ↑ M. Santarelli, P. Leone, M. Calì, G. Orsello (2007). "Experimental evaluation of the sensitivity to fuel utilization and air management on a 100 kW SOFC system". Journal of Power Sources 171 (2): 155–168. doi:10.1016/j.jpowsour.2006.12.032.
  12. ↑ Kupecki J., Milewski J., Jewulski J. (2013). "Investigation of SOFC material properties for plant-level modeling". Central European Journal of Chemistry 11 (5): 664–671. doi:10.2478/s11532-013-0211-x.
  13. ↑ SECA-Coal and Power Systems. Netl.doe.gov. Retrieved on 2011-11-27.
  14. ↑ Fuel Cell Stacks Still Going Strong After 5,000 Hours. Netl.doe.gov (2009-03-24). Retrieved on 2011-11-27. Archived October 8, 2009 at the Wayback Machine
  15. ↑ Spivey, B. (2012). "Dynamic modeling, simulation, and MIMO predictive control of a tubular solid oxide fuel cell". Journal of Process Control. doi:10.1016/j.jprocont.2012.01.015.
  16. ↑ "The Ceres Cell". Company Website. Ceres Power. Retrieved 2009-11-30. Archived December 13, 2013 at the Wayback Machine
  17. ↑ "HITEC". Hitec.mse.ufl.edu. Retrieved 2013-12-08.
  18. ↑ Cooling Down Solid-Oxide Fuel Cells. Technologyreview.com. April 20, 2011. Retrieved on 2011-11-27.
  19. ↑ Anne Hauch, Søren Højgaard Jensen, Sune Dalgaard Ebbesen, Mogens Mogensen (2009). "Durability of solid oxide electrolysis cells for hydrogen production" (PDF). Risoe Reports 1608: 327–338.
  20. ↑ Choi, S.; Yoo, S.; Park, S.; Jun, A.; Sengodan, S.; Kim, J.; Shin, J. Highly efficient and robust cathode materials for low-temperature solid oxide fuel cells: PrBa0.5Sr0.5Co(2-x)Fe(x)O(5+δ). Sci Rep. 2013, 3, 2426-2428.
  21. ↑ Hibini, T.; Hashimoto, A.; Inoue, T.; Tokuno, J.; Yoshida, S.; Sano, M. A Low-Operating-Temperature Solid Oxide Fuel Cell in Hydrocarbon-Air Mixtuers. Science. 2000. 288, 2031-2033.
  22. ↑ Wachsman, E.; Lee, Kang T. Lowering the Temperature of Solid Oxide Fuel Cells. Science. 2011, 334, 935-939.
  23. ↑ Zuo, C.; Zha, S.; Liu, M.; Hatano, M.; Uchiyama, M. Ba(Zr0.1Ce0.7Y0.2)O3-δ as an Electrolyte for Low-Temperature Solid-Oxide Fuel Cells. Advanced Materials. 2006, 18, 3318-3320
  24. ↑ S.H. Chan, H.K. Ho, Y. Tian (2003). "Multi-level modeling of SOFC-gas turbine hybrid system". International Journal of Hydrogen Energy 28 (8): 889–900. doi:10.1016/S0360-3199(02)00160-X.
  25. ↑ L. K. C. Tse, S. Wilkins, N. McGlashan, B. Urban, R. Martinez-Botas (2011). "Solid oxide fuel cell/gas turbine trigeneration system for marine applications". Journal of Power Sources 196 (6): 3149–3162. doi:10.1016/j.jpowsour.2010.11.099.
  26. ↑ Giddey, S; Badwal SPS; Kulkarni A; Munnings C (2012). "A comprehensive review of direct carbon fuel cell technology". Progress in energy and combustion science 38 (3): 360–399. doi:10.1016/j.pecs.2012.01.003.
  27. ↑ HyungKuk Ju, Jiyoung Eom, Jae Kwang Lee, Hokyung Choi, Tak-Hyoung Lim, Rak-Hyun Song, and Jaeyoung Lee, Durable power performance of a direct ash-free coal fuel cell, Electrochimica Acta 115 (2014) 511. doi:10.1016/j.electacta.2013.10.124
  28. ↑ HyungKuk Ju, Sunghyun Uhm, Jin Won Kim, Rak-Hyun Song, Hokyung Choi, Si-Hyun Lee, Jaeyoung Lee, Enhanced anode interface for electrochemical oxidation of solid fuel in direct carbon fuel cells: The role of liquid Sn in mixed state, Journal of Power Sources 198 (2012) 36. doi:10.1016/j.jpowsour.2011.09.082
  29. ↑ HyungKuk Ju and Jaeyoung Lee, High-temperature liquid Sn-air energy storage cell, Journal of Energy Chemistry, 24 (2015) 614. doi:10.1016/j.jechem.2015.08.006
  30. ↑ Hansaem Janga, et al, Ameliorated performance in a direct carbon fuel cell using Snmediator on Ni–YSZ anode surface, Journal of Power Sources, 260 (2016) 158. doi:10.1016/j.cattod.2015.06.013

External links

This article is issued from Wikipedia - version of the Thursday, February 11, 2016. The text is available under the Creative Commons Attribution/Share Alike but additional terms may apply for the media files.