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WO2006005892A1 - Materiaux d'accumulation d'hydrogene - Google Patents

Materiaux d'accumulation d'hydrogene Download PDF

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Publication number
WO2006005892A1
WO2006005892A1 PCT/GB2004/005130 GB2004005130W WO2006005892A1 WO 2006005892 A1 WO2006005892 A1 WO 2006005892A1 GB 2004005130 W GB2004005130 W GB 2004005130W WO 2006005892 A1 WO2006005892 A1 WO 2006005892A1
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WO
WIPO (PCT)
Prior art keywords
hydrogen
metal
hydrogen storage
storage material
less
Prior art date
Application number
PCT/GB2004/005130
Other languages
English (en)
Inventor
Paul Alexander Anderson
Simon Richard Johnson
Peter Philip Edwards
Original Assignee
The University Of Birmingham
Priority date (The priority date is an assumption and is not a legal conclusion. Google has not performed a legal analysis and makes no representation as to the accuracy of the date listed.)
Filing date
Publication date
Application filed by The University Of Birmingham filed Critical The University Of Birmingham
Publication of WO2006005892A1 publication Critical patent/WO2006005892A1/fr

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Classifications

    • C—CHEMISTRY; METALLURGY
    • C01—INORGANIC CHEMISTRY
    • C01B—NON-METALLIC ELEMENTS; COMPOUNDS THEREOF; METALLOIDS OR COMPOUNDS THEREOF NOT COVERED BY SUBCLASS C01C
    • C01B3/00—Hydrogen; Gaseous mixtures containing hydrogen; Separation of hydrogen from mixtures containing it; Purification of hydrogen
    • C01B3/0005—Reversible uptake of hydrogen by an appropriate medium, i.e. based on physical or chemical sorption phenomena or on reversible chemical reactions, e.g. for hydrogen storage purposes ; Reversible gettering of hydrogen; Reversible uptake of hydrogen by electrodes
    • C01B3/001—Reversible uptake of hydrogen by an appropriate medium, i.e. based on physical or chemical sorption phenomena or on reversible chemical reactions, e.g. for hydrogen storage purposes ; Reversible gettering of hydrogen; Reversible uptake of hydrogen by electrodes characterised by the uptaking medium; Treatment thereof
    • C01B3/0031—Intermetallic compounds; Metal alloys; Treatment thereof
    • C—CHEMISTRY; METALLURGY
    • C01—INORGANIC CHEMISTRY
    • C01B—NON-METALLIC ELEMENTS; COMPOUNDS THEREOF; METALLOIDS OR COMPOUNDS THEREOF NOT COVERED BY SUBCLASS C01C
    • C01B3/00—Hydrogen; Gaseous mixtures containing hydrogen; Separation of hydrogen from mixtures containing it; Purification of hydrogen
    • C01B3/0005—Reversible uptake of hydrogen by an appropriate medium, i.e. based on physical or chemical sorption phenomena or on reversible chemical reactions, e.g. for hydrogen storage purposes ; Reversible gettering of hydrogen; Reversible uptake of hydrogen by electrodes
    • C01B3/001—Reversible uptake of hydrogen by an appropriate medium, i.e. based on physical or chemical sorption phenomena or on reversible chemical reactions, e.g. for hydrogen storage purposes ; Reversible gettering of hydrogen; Reversible uptake of hydrogen by electrodes characterised by the uptaking medium; Treatment thereof
    • C01B3/0078—Composite solid storage mediums, i.e. coherent or loose mixtures of different solid constituents, chemically or structurally heterogeneous solid masses, coated solids or solids having a chemically modified surface region
    • Y—GENERAL TAGGING OF NEW TECHNOLOGICAL DEVELOPMENTS; GENERAL TAGGING OF CROSS-SECTIONAL TECHNOLOGIES SPANNING OVER SEVERAL SECTIONS OF THE IPC; TECHNICAL SUBJECTS COVERED BY FORMER USPC CROSS-REFERENCE ART COLLECTIONS [XRACs] AND DIGESTS
    • Y02—TECHNOLOGIES OR APPLICATIONS FOR MITIGATION OR ADAPTATION AGAINST CLIMATE CHANGE
    • Y02E—REDUCTION OF GREENHOUSE GAS [GHG] EMISSIONS, RELATED TO ENERGY GENERATION, TRANSMISSION OR DISTRIBUTION
    • Y02E60/00—Enabling technologies; Technologies with a potential or indirect contribution to GHG emissions mitigation
    • Y02E60/30—Hydrogen technology
    • Y02E60/32—Hydrogen storage

Definitions

  • This invention relates to novel hydride materials, a method of producing such materials and to a method of storing hydrogen using such, materials.
  • Hydrogen is widely regarded as the most promising alternative to carbon-based fuels: it can be produced from a variety of renewable resources through electrolysis of water (available xa virtually limitless amounts), and, when coupled with fuel cells, offers near-zero emission of pollutants and greenhouse gases.
  • electrolysis of water available xa virtually limitless amounts
  • fuel cells offers near-zero emission of pollutants and greenhouse gases.
  • hydrogen as a major energy carrier will require solutions to many scientific and technological challenges, including hydrogen storage methods. This has lead to a rapid increase in research spending in this field.
  • solid-state storage employs metal hydrides (e.g. LaNi 5 ) that have excellent volumetric storage densities — higher than for both compressed gas cylinders and liquid hydrogen — but which have poor gravimetric storage densities ( ⁇ ca 2.5 weight%; 1.37 wt % for LaNi 5 ), thereby precluding their use for mobile storage applications (e.g. in hydrogen fuel-cell vehicles), for which a capacity of 5-6 wt % is regarded as a minimum requirement.
  • metal hydrides e.g. LaNi 5
  • LiNi 5 metal hydrides
  • Magnesium reacts reversibly with hydrogen at around 300 0 C to produce magnesium hydride, MgH 2 .
  • Magnesium is a prime candidate for a solid state storage medium, with a theoretical reversible hydrogen uptake value of 7.6 wt %, a value that exceeds the US Department of Energy target of 6 wt % for use as a complete onboard storage system.
  • the absorption and desorption kinetics need to be accelerated, before Mg or Mg-based materials can be used to form the basis of a practical hydrogen storage system.
  • HVBM High Velocity Ball Milling
  • An object of the present invention is to provide an improved method of making a hydrogen storage material; in particular a method that avoids high velocity ball milling.
  • a further object of the invention is to provide a method of storing hydrogen.
  • a yet further object is to provide a new hydride material suitable for cyclic hydrogen storage.
  • the present invention derives from the discovery of a means of producing, through simple heat treatment, activated hydride materials that have similar hydrogen absorption/desorption kinetics to those prepared by grinding Mg-based powder using HVBM.
  • a method of making a hydrogen storage material comprising the steps of: (a) providing a metal M or first hydride of formula MH a , where metal M is selected from the group Li, Mg, Zn or Al and where a is greater than 0 and less than or equal to 3; (b) providing a second hydride of formula M 1 XbH 0 comprising metal M' selected from the group Li, Na, K, Mg, Ca, Zn, Al; element X selected from the group B, N, Al wherein element X is different from the metal M', where b is less than or equal to 3, c is greater than 0 but less than or equal to 12, and where M and M 1 are different metals if b is 0; (c) mixing said metal M or first hydride with said second hydride and heating in a substantially oxygen-free atmosphere.
  • Step (c) may comprise heating to a temperature in the range 50 to 600 °C, preferably to a temperature in the range 150 to 450 °C, more preferably to a temperature in the range 250 to 400 0 C, and most preferably to a temperature in the range 270 to 330 °C.
  • Step (c) may comprise heating for a period of between 0.1 and 72 hours; preferably for a period between 1 and 24 hours, and more preferably between 6 and 12 hours.
  • the method comprises a further step (d) wherein the material produced by step (c) is cyclically dehydrogenating and hydrogenating several times in order to maximise the degree of adsorption obtained during the cyclic step.
  • the metal M' is Li.
  • the second hydride is a borohydride.
  • step (c) is conducted in an atmosphere comprising hydrogen and/or nitrogen.
  • the atomic ratio M'/M is greater than 0 and less than 0.5; more preferably the atomic ratio M'/M is greater than 0 and less than 0.25.
  • the composition of the present invention is particularly well suited for cyclic storage of hydrogen, in use the composition cycling between a hydrogenated state and a dehydrogenated state.
  • the dehydrogenated state is produced when hydrogen is liberated from the hydrogen storage composition in its hydrogenated form.
  • dehydrogenated does not necessarily imply complete removal of hydrogen, but rather may correspond to partial removal.
  • hydrogenation refers to addition of hydrogen to the dehydrogenated composition, by the formation of hydrides and the like.
  • a hydrogen storage material having a hydrogenated state from which hydrogen may be desorbed and a dehydrogenated state wherein hydrogen may be absorbed to produce said hydrogenated state, said hydrogenated state and dehydrogenated state being cyclically reversible; wherein said hydrogenated state comprises: a non-mechanically alloyed composition with: (a) a first metal M selected from the group Li, Mg, Zn or Al; (b) a second metal M' selected from the group Li, Na, K, Mg, Ca 5 Zn or Al; element X selected from the group B, N, Al; wherein the formula of the composition is M M' e X f Hg ; where the first metal and the second metal are different metals, the element X and metal M' are different elements; e is less than 1 ; e is greater than 0 if f is 0; f is less than 3; and g is greater than 0 but less than 12.
  • the element M' is Li.
  • e is greater than 0 and up to 0.25.
  • f is greater than 0 and up to 3 and more preferably f is greater than 0 and up to 0.75.
  • the hydrogen storage material of the invention may be prepared by mixing substantially dehydrogenated first and second hydrides and heating in a vacuum. Consequently, metal M may normally be used in place of first hydride MH a in step (a) of the method. It follows that the values of a, b, c in Claim 1 and e, f and g in Claim 10 can be non-integers.
  • a method of storing hydrogen using a hydrogen storage material according to the invention wherein hydrogen is absorbed when the hydrogen storage material is in a fully or partly dehydrogenated state and wherein hydrogen is subsequently desorbed by lowering the pressure and/or raising the temperature of the hydrogen storage material.
  • the hydrogen storage material is cyclically hydrogenated and dehydrogenated.
  • Figure 1 illustrates the apparatus described in Example 1 where the reactants are heated under vacuum
  • Figure 2 illustrates the apparatus described in Example 2 where the reactants are heated in a gas atmosphere
  • Figure 3 shows morphological SEM (Secondary) images OfMgH 2 and MgH 2 / LiBH 4 both before cycling of the material on an Intelligent Gravimetric Analyser (IGA) and after 6 cycles of hydrogen desorption / absorption
  • Figure 4 is an X-ray diffraction pattern for MgH 2 (not milled), MgH 2 milled for 10 hours and activated material prepared by heating under vacuum according to the invention in all cases after 6 cycles of hydrogen desorption / absorption
  • Figure 5 is an X-ray diffraction pattern for MgH 2 (not milled), MgH 2 milled for 10 hours and activated material prepared by heating in an Argon atmosphere according to the invention in all cases after 6 cycles of hydrogen desorption / absorption;
  • Figure 6 is an X-ray diffraction pattern for MgH 2 (not milled), MgH 2 milled for 10 hours and activated material prepared by heating in a hydrogen/nitrogen atmosphere in all cases after 6 cycles of hydrogen desorption / absorption ;
  • Figure 7 shows 11 B MAS NMR spectra of for LiBH 4 , MgH 2 and activated material prepared by heating under vacuum according to the invention before and after 6 cycles of hydrogen desorption / absorption;
  • Figure 8 shows hydrogen absorption kinetics data for MgH 2 (not milled), MgH 2 milled for 10 hours and activated material prepared by heating under vacuum according to the invention in all cases after 6 cycles of hydrogen desorption / absorption;
  • Figure 9 shows hydrogen absorption kinetics data for MgH 2 (not milled), material activated prepared by heating under vacuum according to the invention; and material activated by heating in an argon atmosphere in all cases after 6 cycles of hydrogen desorption / absorption
  • Figure 10 shows hydrogen absorption kinetics data for MgH 2 (not milled), activated material prepared by heating under vacuum according to the invention; and material activated by heating in a nitrogen/hydrogen atmosphere in all cases after 6 cycles of hydrogen desorption / absorption
  • Figure 11 shows hydrogen adsorption kinetics data measured at 300 °C and 10 mbar for material prepared by heating in a nitrogen/hydrogem atmosphere according to the invention
  • Figure 12 shows hydrogen absorption as a function of temperature measured at 10 mbar for material prepared by heating in a nitrogen/hydrogen atmosphere according to the invention
  • Figure 13 shows hydrogen desorption kinetic data measured at 300 °C and 10 mbar hydrogen pressure for a range of Mg-based materials after 6 cycles of hydrogen desorption / absorption; and Figure 14 shows hydrogen desorption kinetic data measured at 300 °C and 1 bar after 6 cycles of hydrogen desorption / absorption; and
  • Figure 15 shows hydrogen desorption kinetic data measured at 300 0 C and 1 bar for material prepared by heating MgH 2 with Mg B 2 .
  • MgH 2 (0.3 g) and LiBH 4 (0.025g) were weighed out in an argon atmosphere glove box (O 2 content: 6 pip) and transferred to a quartz tube 10.
  • a Young's tap 12 was attached to the quartz tube via a Cajon flexible fitting 14 and the whole assembly was removed from the glove box.
  • the assembly was attached to a vacuum line, consisting of a rotary pump 16 and turbo pump 18, and the Young's tap was opened allowing the assembly to be evacuated.
  • the assembly was evacuated to a pressure of 10 "9 bar.
  • the Young's tap was then closed and the quartz tube was sealed via a gas torch.
  • the sealed tube, containing the MgH 2 and LiBH 4 was then placed in a furnace and heated to 300 °C for 12 hours, after which the ensemble was taken into the glove box. While this Example used a very low pressure of 10 ⁇ 9 bar to prepare the material under vacuum, this merely corresponds to the performance of available laboratory machines and much lower degrees of vacuum may be used.
  • MgH 2 (0.3g) and LiBH 4 (0.025g) were weighed out in an argon atmosphere glove box (O 2 content: 6 ppmv) and transferred to a quartz tube 10.
  • a Young's tap modified to enable gas flow 12 was attached to the quartz tube via a Cajon fitting 14 and the whole assembly was removed from the glove box.
  • the assembly was attached to a vacuum line, consisting of a rotary pump 16 and turbo pump 18, and a gas cylinder was attached at inlet 20 of the gas flow enabled Young's tap.
  • the assembly was first evacuated to a pressure of 10 "9 bar, after which the Young's tap was closed and the gas taps opened, allowing the argon to flow through the assembly at a pressure of 1 bar.
  • the tube containing the MgH 2 and LiBH 4 was then placed in a furnace and heated to 300 °C for 12 hrs; after which the assembly was taken into the glove box.
  • the gas flow enabled Young's tap was then swapped with a 'normal' Young's tap and the whole assembly was removed from the glove box.
  • the assembly was reattached to the vacuum line and evacuated to a pressure of 10 "9 bar before being sealed via a gas torch. This final step is required in order to protect it from degradation.
  • TMs example followed the method of Example 2, except that after the assembly was first evacuated to a pressure of 10 '9 bar, the Young's tap was closed and the gas taps opened, Nitrogen was then allowed to flow through the assembly at a pressure of 1 bar.
  • Example 2 followed the method of Example 1 except that 0.026g OfMgB 2 was used instead of 0.026g Of LiBH 4 .
  • Example 4 followed the method of Example 4 except that 0.026g OfLiNH 2 was used instead of 0.025g OfLiBH 4 , a gas mixture of 90% nitrogen and 10% hydrogen was used instead of nitrogen, and the material was heated to 375 °C instead of 300 0 C.
  • Figure 7 shows 11 B MAS NMR spectra of an increased surface area material
  • Figure 3 shows morphological SEM (Secondary) images Of MgH 2 and MgH 2 / LiBH 4 both before cycling of the material on an Intelligent Gravimetric Analyser (IGA) and after 6 cycles of hydrogen desorption / absorption.
  • IGA Intelligent Gravimetric Analyser
  • each grain was a solid particulate OfMgH 2 with a relatively smooth surface. After treatment with LiBH 4 followed by cycling, the particles are all characterised by a porous.
  • a powder X — Ray diffraction (XRD) trace of an increased surface area material (Synthesised in a static vacuum, cycled six times on the IGA), together with corresponding traces for MgH 2 and ball milled MgH 2 is shown in Figure 4.
  • XRD X — Ray diffraction
  • the increased surface area does not result in any significant broadening of the powder XRD pattern for MgH 2 vacuum treated witfi LiBH 4 , but each of the diffraction lines exhibited a shoulder at low angle, indicating the presence of at least two isostructural compounds.
  • a powder XRD trace of an increased surface area material (synthesised in an argon atmosphere, cycled six times on the IGA), together with corresponding traces for MgH 2 and ball milled MgH 2 is shown in Figure 5.
  • the extra peaks present in the pattern of the increased surface area material are due to the presence of Mg metal.
  • the increased surface area structure formed by the reaction Of LiBH 4 with MgH 2 does not result in significant broadening of the powder XRD pattern, and in this case no shoulder on the diffraction lines was observed.
  • a powder XRD trace of the increased surface area material (Synthesised in a H 2 / N 2 , 10 % / 90 % atmosphere, cycled 6 times on the IGA), together with corresponding traces for MgH2 and ball milled MgH 2 is shown in Figure 6.
  • the increased surface area structure formed by the reaction of LiBH 4 with MgH 2 does not result in any significant broadening of the powder XRD pattern. Again no shoulder on the diffraction lines was observed.
  • Figure 8 shows that the absorption of hydrogen in MgH 2 is very slow; at 300 °C and 10 bar of H 2 it takes two hours to reach maximum absorption. In contrast, the absorption Of MgH 2 / LiBH 4 (heated in a static vacuum) at the same temperature and pressure occurs within 20 minutes to a value of 6 wt %. This is very similar to the hydrogen uptake data of ball milled MgH 2 .
  • Figure 9 shows that MgH 2 / LiBH 4 (heated in an argon atmosphere) at the same temperature and pressure reaches maximum absorption of hydrogen within 40 minutes. However it has higher uptake value, 6.6 wt %.
  • Figure 10 shows that MgH 2 / LiBH 4 (heated in a H 2 / N 2 atmosphere) at the same temperature and pressure reaches maximum hydrogen absorption within 20 minutes to a value of 6 wt %.
  • Figure 11 shows that MgH 2 / LiNH 2 (heated in a H 2 / N 2 atmosphere) absorbs hydrogen at 300 °C at the very low pressure of 10 mbar.
  • Figure 12 shows that MgH 2 / LiNH 2 (heated in a H 2 /N 2 atmosphere) absorbs hydrogen at 10 mbar, at temperatures as low as 100 °C.
  • the method of the invention is expected to result in considerable cost savings over the alternative of using a HVBM-based method.
  • the option of preparing the active material using metal powder promises to further reduce preparation costs.
  • metal powder for example; magnesium powder
  • the process may also be applied to Mg-Ni based alloys suitable for electrochemical hydrogen storage in rechargeable batteries.

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  • Chemical & Material Sciences (AREA)
  • Organic Chemistry (AREA)
  • Chemical Kinetics & Catalysis (AREA)
  • Engineering & Computer Science (AREA)
  • Combustion & Propulsion (AREA)
  • Inorganic Chemistry (AREA)
  • Hydrogen, Water And Hydrids (AREA)

Abstract

Procédé servant à fabriquer un matériau d'accumulation d'hydrogène et consistant à: mettre en application un métal M ou un premier hydrure de M, ce métal M étant sélectionné dans le groupe Li, Mg, Zn ou Al et un deuxième hydrure comprenant un métal M' sélectionné dans le groupe Li, Na, K, Mg, Ca, Zn, Al; un élément X sélectionné dans le groupe B, N, Al, cet élément X étant différent du métal M', et mélanger ledit métal M ou le premier hydrure avec ledit deuxième hydrure et les réchauffer dans une atmosphère pratiquement exempte d'oxygène.
PCT/GB2004/005130 2004-07-12 2004-12-07 Materiaux d'accumulation d'hydrogene WO2006005892A1 (fr)

Applications Claiming Priority (2)

Application Number Priority Date Filing Date Title
GB0415561.0 2004-07-12
GBGB0415561.0A GB0415561D0 (en) 2004-07-12 2004-07-12 Hydrogen storage system

Publications (1)

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WO2006005892A1 true WO2006005892A1 (fr) 2006-01-19

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Cited By (8)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
WO2008007068A1 (fr) * 2006-07-10 2008-01-17 The Science And Technology Facilities Council Procédé de production de (nh2(r2)) et/ou d'hydrogène
EP2055669A2 (fr) 2007-11-01 2009-05-06 Honeywell International Inc. Combustible produisant de l'hydrogène pour générateur électrique
WO2009067312A3 (fr) * 2007-11-20 2009-07-16 Gm Global Tech Operations Inc Préparation de matériaux de stockage d'hydrogène
US7736805B2 (en) * 2007-05-16 2010-06-15 Gm Global Technology Operations, Inc. Lithium hydride negative electrode for rechargeable lithium batteries
US8187348B2 (en) 2008-04-07 2012-05-29 Honeywell International Inc. Hydrogen generator
US8551663B2 (en) 2007-04-25 2013-10-08 Honeywell International Inc. Power generator with additional hydrogen storage
US8993135B2 (en) 2007-11-01 2015-03-31 Honeywell International Inc. Fuel cell stack for hydrogen fuel power generator
US9029038B2 (en) 2007-11-01 2015-05-12 Honeywell International Inc. Method of forming a fuel cell stack

Citations (1)

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WO1999024355A1 (fr) * 1997-11-07 1999-05-20 Mcgill University Composition de stockage d'hydrogene

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Publication number Priority date Publication date Assignee Title
WO1999024355A1 (fr) * 1997-11-07 1999-05-20 Mcgill University Composition de stockage d'hydrogene

Non-Patent Citations (3)

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Title
DAL TOE S ET AL: "Hydrogen desorption from magnesium hydride-graphite nanocomposites produced by ball milling", MATERIALS SCIENCE AND ENGINEERING B, ELSEVIER SEQUOIA, LAUSANNE, CH, vol. 108, no. 1-2, 25 April 2004 (2004-04-25), pages 24 - 27, XP004500892, ISSN: 0921-5107 *
DOUGLASS D L: "The formation and dissociation of magnesium alloy hydrides and their use for fuel storage in the hydrogen car", METALLURGICAL TRANSACTIONS A. PHYSICAL METALLURGY AND MATERIALS SCIENCE, METALLURGICAL SOCIETY OF AIME. NEW YORK, US, vol. 6A, no. 12, December 1975 (1975-12-01), pages 2179 - 2189, XP002088735 *
HUOT J ET AL: "Magnesium-based nanocomposites chemical hydrides", JOURNAL OF ALLOYS AND COMPOUNDS, ELSEVIER SEQUOIA, LAUSANNE, CH, vol. 353, no. 1-2, 7 April 2003 (2003-04-07), pages L12 - L15, XP004416859, ISSN: 0925-8388 *

Cited By (18)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
EP2420471A3 (fr) * 2006-07-10 2012-03-28 The Science and Technology Facilities Council Procédé de production de (NH2(R2)) et/ou d'hydrogène
JP2009542576A (ja) * 2006-07-10 2009-12-03 ザ サイエンス アンド テクノロジー ファシリティーズ カウンシル （ｎｈ２（ｒ２））および／または水素の製造方法
WO2008007068A1 (fr) * 2006-07-10 2008-01-17 The Science And Technology Facilities Council Procédé de production de (nh2(r2)) et/ou d'hydrogène
US8168342B2 (en) 2006-07-10 2012-05-01 The Science And Technology Facilities Council Method of producing (NH2(R2)) and/or hydrogen
US9799899B2 (en) 2007-04-25 2017-10-24 Honeywell International Inc. Power generator with additional hydrogen storage
US8551663B2 (en) 2007-04-25 2013-10-08 Honeywell International Inc. Power generator with additional hydrogen storage
US7736805B2 (en) * 2007-05-16 2010-06-15 Gm Global Technology Operations, Inc. Lithium hydride negative electrode for rechargeable lithium batteries
KR101043423B1 (ko) 2007-05-16 2011-06-22 지엠 글로벌 테크놀러지 오퍼레이션스 엘엘씨 재충전이 가능한 리튬배터리용 리튬 하이드라이드 음극
US8337806B2 (en) 2007-11-01 2012-12-25 Honeywell International Inc. Hydrogen producing fuel for power generator
US7807131B2 (en) 2007-11-01 2010-10-05 Honeywell International Inc. Hydrogen producing fuel for power generator
EP2055669A3 (fr) * 2007-11-01 2010-01-06 Honeywell International Inc. Combustible produisant de l'hydrogène pour générateur électrique
US8993135B2 (en) 2007-11-01 2015-03-31 Honeywell International Inc. Fuel cell stack for hydrogen fuel power generator
US9029038B2 (en) 2007-11-01 2015-05-12 Honeywell International Inc. Method of forming a fuel cell stack
US9225027B2 (en) 2007-11-01 2015-12-29 Honeywell International Inc. Method of forming a fuel cell stack
EP2055669A2 (fr) 2007-11-01 2009-05-06 Honeywell International Inc. Combustible produisant de l'hydrogène pour générateur électrique
US8021533B2 (en) 2007-11-20 2011-09-20 GM Global Technology Operations LLC Preparation of hydrogen storage materials
WO2009067312A3 (fr) * 2007-11-20 2009-07-16 Gm Global Tech Operations Inc Préparation de matériaux de stockage d'hydrogène
US8187348B2 (en) 2008-04-07 2012-05-29 Honeywell International Inc. Hydrogen generator

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