WO2010016641A1 - Procédé de fabrication d'hydrogène à partir d'eau par des cycles thermochimiques à l'aide d'oxyde de germanium - Google Patents

Procédé de fabrication d'hydrogène à partir d'eau par des cycles thermochimiques à l'aide d'oxyde de germanium Download PDF

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Publication number
WO2010016641A1
WO2010016641A1 PCT/KR2008/006407 KR2008006407W WO2010016641A1 WO 2010016641 A1 WO2010016641 A1 WO 2010016641A1 KR 2008006407 W KR2008006407 W KR 2008006407W WO 2010016641 A1 WO2010016641 A1 WO 2010016641A1
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WIPO (PCT)
Prior art keywords
geo
water
hydrogen
reaction formula
thermochemical
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PCT/KR2008/006407
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English (en)
Inventor
Kyoung-Soo Kang
Chu-Sik Park
Chang-Hee Kim
Ki-Kwang Bae
Won-Chul Cho
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Korea Institute Of Energy Research
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Publication date
Priority claimed from KR1020080106287A external-priority patent/KR101001873B1/ko
Application filed by Korea Institute Of Energy Research filed Critical Korea Institute Of Energy Research
Priority to US12/990,726 priority Critical patent/US8470292B2/en
Priority to AU2008360451A priority patent/AU2008360451B2/en
Publication of WO2010016641A1 publication Critical patent/WO2010016641A1/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
    • C01B13/00—Oxygen; Ozone; Oxides or hydroxides in general
    • C01B13/02—Preparation of oxygen
    • C01B13/0203—Preparation of oxygen from inorganic compounds
    • 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
    • C01B3/02—Production of hydrogen or of gaseous mixtures containing a substantial proportion of hydrogen
    • C01B3/06—Production of hydrogen or of gaseous mixtures containing a substantial proportion of hydrogen by reaction of inorganic compounds containing electro-positively bound hydrogen, e.g. water, acids, bases, ammonia, with inorganic reducing agents
    • C01B3/061—Production of hydrogen or of gaseous mixtures containing a substantial proportion of hydrogen by reaction of inorganic compounds containing electro-positively bound hydrogen, e.g. water, acids, bases, ammonia, with inorganic reducing agents by reaction of metal oxides with water
    • C01B3/063—Cyclic methods
    • 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
    • Y02E60/36—Hydrogen production from non-carbon containing sources, e.g. by water electrolysis

Definitions

  • the present invention relates to a hydrogen production method from water by using germanium oxide, more precisely a hydrogen production method from water by thermochemical cycles using germanium oxide.
  • Hydrogen energy is the most promising candidate for alternative energy because it uses water as a raw material which is most abundant on earth, it does not produce any pollutant during hydrogen combustion, suggesting that hydrogen energy is very clean energy, and it is also functioning as a storage medium for energy.
  • the representative methods for producing hydrogen from water are biological method, photochemical method, electrolysis, direct thermolysis and thermochemical degradation. Electrolysis, one of the conventional techniques, is in practical use, but others are still under study. To decompose water directly to produce hydrogen, high temperature of at least 4000 K is required. So, direct decomposition of water is in fact very difficult. Therefore, water decomposition is tried stepwise, precisely a method is designed to contain chemical reactions induced stepwise at comparatively low temperatures to decompose water, which is a close cycle. That is the hydrogen production method by using thermochemical cycle.
  • Thermochemical cycle absorbs heat to convert it into hydrogen and oxygen chemically. This method produces hydrogen from water by multi-step reactions including oxidation and reduction of a metal oxide using heat.
  • Themochemical cycle can be classified into pure thermochemical cycle and combined thermochemical cycle.
  • the combined thermochemical cycle is developed to supplement and improve the pure thermochemical cycle, for which electrolysis or photochemical method is introduced.
  • thermochemical cycle is classified as 2 step cycle, 3 step cycle, 4 step cycle, etc, and up to 8 step cycle has been notified so far.
  • thermochemical cycles including 2 step thermochemical cycle using a metal oxide such as Fe, Mn, Zn, Co, Sn and WO 3 , ZnO/Zn, Fe 3 O 4 ZFeO, CeO 2 /Ce 2 O 3 , and SnO 2 ZSn as a material for thermochemical process.
  • a metal oxide such as Fe, Mn, Zn, Co, Sn and WO 3 , ZnO/Zn, Fe 3 O 4 ZFeO, CeO 2 /Ce 2 O 3 , and SnO 2 ZSn
  • a transition metal such as Ni and Co or a refractory such as alumina can be mixed or alloyed, particularly in those cycles of ZnO/Zn thermochemical cycle, Fe 3 O 4 /FeO thermochemical cycle, CeO 2 ZCe 2 O 3 thermochemical cycle and SnO 2 ZSn thermochemical cycle.
  • thermochemical cycle accompanies non- stoichiometric reaction that is the reduction of some of oxygen in M (Co or Ni, or Ni and Mn) -ferrite, resulting in low hydrogen production with the yield of up to 20 cc/g.
  • thermochemical cycle that facilitates reduction at a low temperature to mass-produce hydrogen from water is required.
  • the present invention is characterized by producing hydrogen from water by thermochemical reaction using germanium oxide .
  • the hydrogen production method of the present invention is characterized by producing hydrogen by multi-step thermochemical cycle using germanium oxide as a redox pair.
  • thermochemical cycle of the hydrogen production method of the present invention characteristically produces hydrogen by GeO 2 ZGeO redox pair, Ge ⁇ 2 /Ge redox pair generated by spontaneous decomposition (disproportion) of GeO
  • GeO generated from the decomposition of GeO 2 is apt to be decomposed spontaneously into 1/2Ge and 1/2GeO 2 again during cooling process as shown in the following reaction formula 3 because of chemical instability. At this time, water is decomposed by the following reaction formula 4 to produce hydrogen.
  • Reduction of GeO 2 is performed at 1000 - 1700 °C in the presence of inert gas under the pressure of 1 atm - 0.001 atm.
  • the reduced GeO according to reaction formula 1, decomposes water (vapor) provided in the step of reaction formula 2 to produce hydrogen and GeO itself is oxidized into GeO 2 .
  • the reaction of reaction formula 2 is performed at 200 - 800°C .
  • GeO obtained in the step of reaction formula 1 is a very unstable material, which is easily decomposed into thermodynamically stable Ge and GeO 2 .
  • reaction of reaction formula 1 when the reaction of reaction formula 1 is completed, GeO is cooled down, during which GeO is decomposed spontaneously into Ge and Ge ⁇ 2 , leading not to the cycle of reaction formula 2 but to the cycles of reaction formulas 3 and 4 to produce hydrogen.
  • Some of GeO generated in the step of reaction formula 1 proceeds to the step of reaction formula 3, so simultaneously with the water decomposition in the step of reaction formula 2, hydrogen can be produced by the water decomposition in the step of reaction formula 4.
  • the reaction of reaction formula 4 is performed at 200 - 800 ° C.
  • thermochemical water decomposition using an oxide of Fe, Ce, Sn or Zn requires a high reduction temperature, making the construction of composition of a reactor difficult. In addition, efficiency is also very low because of heat loss caused by such high temperature .
  • the hydrogen production method of the present invention produces hydrogen by thermochemical cycle using germanium oxide, in which the thermochemical cycle is a low temperature reaction, no other materials than water is consumed and instead they are only circulated, hydrogen production efficiency is high and physical properties of germanium oxide are not damaged by the thermochemical cycle.
  • Figure 1 is a graph illustrating the reaction Gibbs ' free energy changes of GeO 2 decomposition according to the temperature changes
  • Figure 2 is a graph illustrating the changes of equilibrium composition of 1 kmol of GeO 2 in the presence of 1 kmol of inert gas under the pressure of 1 atm according to the temperature changes
  • Figure 3 is a graph illustrating the changes of equilibrium composition of 1 kmol of GeO 2 in the presence of 1 kmol of inert gas under the pressure of 0.001 atm according to the temperature changes
  • Figure 4 is a graph illustrating the reaction Gibbs 1 free energy changes over temperatures when the reduced GeO and water are reacted
  • Figure 5 is a graph illustrating the weight changes and oxygen generation due to GeO 2 decomposition over temperatures measured by thermogravimetry analyzer-mass spectrometer
  • Figure 6 is a photograph illustrating that the condensed and filtered particles from GeO 2 decomposition at 1460 ° C, examined under electron microscope,
  • Figure 7 is a graph illustrating that X-ray diffraction peaks of the condensed and filtered particles from GeO 2 decomposition at 1460°C,
  • Figure 8 is a graph illustrating the hydrogen production
  • Figure 9 is a graph illustrating the result of X-ray diffraction performed after the reaction of water and the product of GeO 2 obtained by the processes of decomposition at 1460°C, cooling and filtering thereof in a fixed-bed reactor.
  • Metal oxides can be reduced by thermochemical decomposition at a high temperature range where Gibb's free energy is negative value. By this reaction, solar energy can be converted into chemical energy as the reduced form of metal oxides.
  • the reduced metal oxide can be used for decomposition of water to produce hydrogen.
  • the hydrogen production method of the present invention characteristically produces hydrogen by reducing germanium oxide by thermochemical decomposition and by reacting the reduced germanium oxide with water (vapor) .
  • the hydrogen production method of the present invention using multi-step thermochemical cycle produces hydrogen by using GeC> 2 /GeO redox pair, GeO 2 ZGe redox pair or the combination thereof.
  • the step of reaction formula 1 is the reduction step of germanium oxide by thermochemical decomposition.
  • Figure 1 illustrates the reaction Gibbs ' free energy changes of GeO 2 decomposition (reduction) according to the temperature changes .
  • germanium oxide (GeO 2 ) used in this invention demonstrates the reaction Gibbs ' free energy change close to 0 at 1500 "C under normal pressure, indicating that spontaneous thermal decomposition can be induced. Even if the reaction Gibb's free energy change is a positive value close to 0, decomposition can be continued as long as the reaction product is constantly eliminated by inert gas (argon, helium) .
  • inert gas argon, helium
  • high temperature gas furnace, concentrated solar heat, nuclear reactor, and waste heat of blast furnace can be used.
  • Figure 2 is a graph illustrating the changes of equilibrium composition of 1 kmol of GeO 2 in the presence of 1 kmol of inert gas under the pressure of 1 atm according to the temperature changes.
  • Spontaneous decomposition of germanium oxide (GeO 2 ) is induced fast at 1500 ° C and when the temperature reaches 1700°C, all germanium oxides (GeO 2 ) are decomposed into GeO.
  • GeO is stable even at 1700 "C or higher.
  • Figure 1 and Figure 2 illustrate the changes of equilibrium composition of germanium oxide over the temperatures in the presence of inert gas under the pressure of 1 atm.
  • Figure 3 illustrates the changes of equilibrium composition of 1 kmol of GeO 2 over the temperatures in the presence of 1 kmol of inert gas under the pressure of 0.001 atm.
  • germanium oxide begins to be decomposed spontaneously at 1000 ° C and when the temperature reaches 1200 ° C, all germanium oxides (GeO 2 ) are decomposed into
  • thermochemical reduction (decomposition) of GeO 2 presented in reaction formula 1 is preferably performed in the presence of inert gas, at
  • thermochemical reduction of GeO 2 at 1000 ° C - 1500 "C under the pressure of 0.1 atm - 0.001 atm.
  • the gas phase GeO (g) obtained by thermochemical reduction (decomposition) according to reaction formula 1 is preferably recovered by fast quenching and the recovered GeO (s) is reacted with water to produce hydrogen as shown in reaction formula 2.
  • the mixture of Ge and GeO 2 generated by spontaneous decomposition (disproportion) of GeO can also be recovered along with GeO.
  • the recovered mixture (GeO, Ge, GeO 2 ) is reacted with water to produce hydrogen according to reaction formula 2 and reaction formula 4.
  • reaction formula 4 When all the GeO obtained in the step of reaction formula 1 are decomposed and the mixture of Ge and GeO 2 is recovered by fast quenching, the recovered mixture (Ge, GeO 2 ) is reacted with water to produce hydrogen according to reaction formula 4.
  • Figure 4 illustrates the reaction Gibb's free energy values over the temperatures when the reduced GeO and water are reacted.
  • reaction Gibb's free energy is negative value at the temperature of at lest 200°C, suggesting that the reaction is spontaneous .
  • Reaction of the reduced GeO or Ge generated from GeO and water (vapor) presented in reaction formula 2 or reaction formula 4 is preferably performed at 200 "C - 800 ° C where spontaneous decomposition is induced.
  • reaction speed is so slow that hydrogen production rate is decreased.
  • reaction is induced at higher than 800 ° C, vaporization of GeO is so strong that construction of a production reactor is difficult.
  • Hydrogen can be produced from water by the said multi- step thermochemical cycles. And, satisfactory conversion rate of chemical reaction and production yield of hydrogen can be accomplished by the thermochemical cycles composed of spontaneous reaction at the said conditions (reaction temperature and pressure) .
  • FIG. 6 is a SEM photograph showing the collected product. As shown in Figure 6, the round shaped product (30-60 nm in diameter) was obtained. As shown in Figure 7, the obtained product was confirmed by X-ray diffraction as the mixture of Ge and GeO 2 .
  • Example 3 0.11 g of the collected product on the filter in Example 2 was loaded in a fixed-bed reactor, and then temperature was raised to room temperature to 750°C at the speed of 20 ° C/min.
  • the temperature was maintained at 750 "C for 30 minutes, and then raised again at the speed of 20°C/min to 800 ° C. The temperature was maintained at 800°C for 1 hour.
  • Ar gas was supplied at the flow speed of 18 cc/min until the temperature was raised to 150 "C from room temperature. When the temperature of the reactor reached 150 ° C, Ar gas was saturated with 70 "C water vapor, which was provided into the reactor at the speed of 18 cc/min.
  • the reaction product was cooled down to eliminate moisture, followed by sampling at 2 minutes interval. Hydrogen concentration was measured by gas chromatography (Agilent 7890, TCD) . The amount of generated hydrogen was calculated by hydrogen concentration, gas flow rate and sampling time.
  • the red line in Figure 8 indicates the changes of temperature over the time and the black line indicates hydrogen amount.
  • hydrogen began to be generated from the temperature of 300 ° C . And, when the temperature reached 600 ° C , hydrogen was generated massively. The total amount of hydrogen generated was 28 cc.
  • X-ray diffraction was performed with the sample after water decomposition. As a result, as shown in Figure 9, GeO 2 comprising the two structures of tetragonal and hexagonal was obtained.

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  • Chemical & Material Sciences (AREA)
  • Organic Chemistry (AREA)
  • Inorganic Chemistry (AREA)
  • Health & Medical Sciences (AREA)
  • Chemical Kinetics & Catalysis (AREA)
  • General Health & Medical Sciences (AREA)
  • Engineering & Computer Science (AREA)
  • Combustion & Propulsion (AREA)
  • Fuel Cell (AREA)

Abstract

La présente invention porte sur un procédé de fabrication d'hydrogène à partir d'eau à l'aide d'oxyde de germanium, plus précisément sur un procédé de fabrication d'hydrogène et d'oxygène à partir d'eau par des cycles thermochimiques utilisant l'oxyde de germanium. Le procédé de la présente invention facilite la fabrication d'hydrogène par un cycle thermochimique multi-étapes utilisant l'oxyde de germanium, de telle sorte qu'il est caractérisé par le fait que le cycle thermochimique est une réaction à basse température et seulement de l'eau est consommée et d'autres matières ne sont pas consommées mais recyclées.
PCT/KR2008/006407 2008-08-06 2008-10-30 Procédé de fabrication d'hydrogène à partir d'eau par des cycles thermochimiques à l'aide d'oxyde de germanium WO2010016641A1 (fr)

Priority Applications (2)

Application Number Priority Date Filing Date Title
US12/990,726 US8470292B2 (en) 2008-08-06 2008-10-30 Hydrogen production method from water by thermochemical cycles using germanium oxide
AU2008360451A AU2008360451B2 (en) 2008-08-06 2008-10-30 Hydrogen production method from water by thermochemical cycles using germanium oxide

Applications Claiming Priority (4)

Application Number Priority Date Filing Date Title
KR10-2008-0076880 2008-08-06
KR20080076880 2008-08-06
KR10-2008-0106287 2008-10-29
KR1020080106287A KR101001873B1 (ko) 2008-08-06 2008-10-29 게르마늄 산화물을 이용한 열화학적 물분해 수소 제조방법

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Cited By (3)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
WO2013151973A1 (fr) * 2012-04-06 2013-10-10 California Institute Of Technology Nouveaux procédés et nouvelles matières pour la fabrication thermochimique d'hydrogène à partir de l'eau
US9106209B2 (en) 2012-03-21 2015-08-11 Lg Display Co., Ltd. Gate driving unit having gate signal of reduced off-time and liquid crystal display device having the same
US11634322B2 (en) 2019-04-03 2023-04-25 California Institute Of Technology Integration of thermochemical water splitting with CO2 direct air capture

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US4182748A (en) * 1978-05-04 1980-01-08 Horizon Manufacturing Corporation Material and method for obtaining hydrogen and oxygen by dissociation of water
US4310503A (en) * 1975-03-21 1982-01-12 Erickson Donald C Hydrogen production by multistaged intermediate oxidation-reduction
US6663981B1 (en) * 1997-07-30 2003-12-16 Vacuumschmelze Gmbh Marker for use in a magnetic anti-theft security system and method for marking the marker
US20060213331A1 (en) * 2003-05-09 2006-09-28 Kiyoshi Otsuka Method for reducing metal oxide and method for producing hydrogen

Patent Citations (4)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
US4310503A (en) * 1975-03-21 1982-01-12 Erickson Donald C Hydrogen production by multistaged intermediate oxidation-reduction
US4182748A (en) * 1978-05-04 1980-01-08 Horizon Manufacturing Corporation Material and method for obtaining hydrogen and oxygen by dissociation of water
US6663981B1 (en) * 1997-07-30 2003-12-16 Vacuumschmelze Gmbh Marker for use in a magnetic anti-theft security system and method for marking the marker
US20060213331A1 (en) * 2003-05-09 2006-09-28 Kiyoshi Otsuka Method for reducing metal oxide and method for producing hydrogen

Non-Patent Citations (1)

* Cited by examiner, † Cited by third party
Title
AKIRA MIYAMOTO ET AL., IND. ENG. CHEM. PROD. RES. DEV., vol. 23, 1984, pages 467 - 470 *

Cited By (6)

* Cited by examiner, † Cited by third party
Publication number Priority date Publication date Assignee Title
US9106209B2 (en) 2012-03-21 2015-08-11 Lg Display Co., Ltd. Gate driving unit having gate signal of reduced off-time and liquid crystal display device having the same
TWI497478B (zh) * 2012-03-21 2015-08-21 Lg Display Co Ltd 一種閘極驅動單元及具有此閘極驅動單元的液晶顯示裝置
WO2013151973A1 (fr) * 2012-04-06 2013-10-10 California Institute Of Technology Nouveaux procédés et nouvelles matières pour la fabrication thermochimique d'hydrogène à partir de l'eau
US8940269B2 (en) 2012-04-06 2015-01-27 California Institute Of Technology Methods and materials for the thermochemical production of hydrogen from water
US9206042B2 (en) 2012-04-06 2015-12-08 California Institute Of Technology Methods and materials for the catayltic reduction of carbon dioxide
US11634322B2 (en) 2019-04-03 2023-04-25 California Institute Of Technology Integration of thermochemical water splitting with CO2 direct air capture

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