EP1569868A1 - Procede de production d'hydrogene - Google Patents

Procede de production d'hydrogene

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Publication number
EP1569868A1
EP1569868A1 EP03767339A EP03767339A EP1569868A1 EP 1569868 A1 EP1569868 A1 EP 1569868A1 EP 03767339 A EP03767339 A EP 03767339A EP 03767339 A EP03767339 A EP 03767339A EP 1569868 A1 EP1569868 A1 EP 1569868A1
Authority
EP
European Patent Office
Prior art keywords
aluminum
water
naoh
reaction
vessel
Prior art date
Legal status (The legal status 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 status listed.)
Withdrawn
Application number
EP03767339A
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German (de)
English (en)
Inventor
Erling Reidar Andersen
Erling Jim Andersen
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Individual
Original Assignee
Individual
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Filing date
Publication date
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Publication of EP1569868A1 publication Critical patent/EP1569868A1/fr
Withdrawn legal-status Critical Current

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Classifications

    • C—CHEMISTRY; METALLURGY
    • C01—INORGANIC CHEMISTRY
    • C01F—COMPOUNDS OF THE METALS BERYLLIUM, MAGNESIUM, ALUMINIUM, CALCIUM, STRONTIUM, BARIUM, RADIUM, THORIUM, OR OF THE RARE-EARTH METALS
    • C01F7/00—Compounds of aluminium
    • C01F7/02—Aluminium oxide; Aluminium hydroxide; Aluminates
    • C01F7/42—Preparation of aluminium oxide or hydroxide from metallic aluminium, e.g. by oxidation
    • C01F7/428—Preparation of aluminium oxide or hydroxide from metallic aluminium, e.g. by oxidation by oxidation in an aqueous solution
    • B—PERFORMING OPERATIONS; TRANSPORTING
    • B01—PHYSICAL OR CHEMICAL PROCESSES OR APPARATUS IN GENERAL
    • B01J—CHEMICAL OR PHYSICAL PROCESSES, e.g. CATALYSIS OR COLLOID CHEMISTRY; THEIR RELEVANT APPARATUS
    • B01J7/00—Apparatus for generating gases
    • B01J7/02—Apparatus for generating gases by wet methods
    • B—PERFORMING OPERATIONS; TRANSPORTING
    • B01—PHYSICAL OR CHEMICAL PROCESSES OR APPARATUS IN GENERAL
    • B01J—CHEMICAL OR PHYSICAL PROCESSES, e.g. CATALYSIS OR COLLOID CHEMISTRY; THEIR RELEVANT APPARATUS
    • B01J8/00—Chemical or physical processes in general, conducted in the presence of fluids and solid particles; Apparatus for such processes
    • B01J8/0015—Feeding of the particles in the reactor; Evacuation of the particles out of the reactor
    • B01J8/002—Feeding of the particles in the reactor; Evacuation of the particles out of the reactor with a moving instrument
    • B—PERFORMING OPERATIONS; TRANSPORTING
    • B01—PHYSICAL OR CHEMICAL PROCESSES OR APPARATUS IN GENERAL
    • B01J—CHEMICAL OR PHYSICAL PROCESSES, e.g. CATALYSIS OR COLLOID CHEMISTRY; THEIR RELEVANT APPARATUS
    • B01J8/00—Chemical or physical processes in general, conducted in the presence of fluids and solid particles; Apparatus for such processes
    • B01J8/0015—Feeding of the particles in the reactor; Evacuation of the particles out of the reactor
    • B01J8/003—Feeding of the particles in the reactor; Evacuation of the particles out of the reactor in a downward flow
    • 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
    • C01B3/08—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 with metals
    • 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

  • TITLE METHOD FOR PRODUCING HYDROGEN
  • This invention relates to the production of hydrogen gas from the reaction of aluminum with water in the presence of sodium hydroxide as catalyst.
  • Hydrogen energy is environment-friendly. Because of the actual human ecology concerns, the exploitation of hydrogen as an universal fuel would be greatly acclaimed. During the last two decades or so, the elaboration of a hydrogen-based economy has made important progress on acco ⁇ nt of numerous research projects such as the hydrogen fuel cell and the hydrogen car. Although these important discoveries constitute milestones toward a pollution-free society, more research is needed to obtain the hydrogen easily and economically.
  • a convenient source of hydrogen is a reaction of aluminum with water to split the water molecules into hydrogen and oxygen.
  • the hydrogen is released as a gas and the oxygen combines with the aluminum to form aluminum oxide compounds.
  • Aluminum is the third most abundant element after oxygen and silicon in the earth's crust, and constitutes approximately 8% by weight of the earth's crust.
  • Aluminum is a safe material and is commonly used in the food, cosmetics and medical fields. Water is also abundant. Therefore, the reaction of these two elements to produce hydrogen represents an interesting proposal to replace fossil fuels.
  • compositions for generating hydrogen comprise any metal which can form an hydroxide when it is brought into contact with a solution of a suitable hydroxide.
  • a suitable hydroxide For example, aluminum is reacted with sodium hydroxide to release hydrogen and to produce sodium aluminate.
  • the preferred magnesium composition comprises magnesium, and one or more metals selected from the group consisting of iron, zinc, chromium, aluminum and manganese.
  • US 4,730,601 issued on Mar. 15, 1988 both to H.D. Hubele et al. These documents disclose the structure of a fuel cell for producing heat energy and hydrogen gas.
  • the device has a reaction chamber containing a fuel composition that is reactive with water.
  • the fuel composition includes a main fuel part of magnesium and aluminum in a molar ratio of 1 :2, and the second part is composed of lithium hydride, magnesium and aluminum in equal molar ratio.
  • US 4,670,018 issued on June 2, 1987.
  • This document discloses a process for producing hydrogen.
  • Aluminum is reacted with water under an inactive gas or a vacuum to produce hydrogen gas.
  • This patent application discloses a hydrogen generation system wherein a coating on reactive pellets is selectively removed to expose the reactive material to water for producing hydrogen gas on demand.
  • aluminum and sodium hydroxide are reacted with water to release hydrogen gas and produce sodium aluminate.
  • the process for producing hydrogen gas according to the present invention consists of reacting aluminum with water in the presence of sodium hydroxide acting as a catalyst.
  • a process for producing hydrogen gas comprising the initial step of: providing an aqueous solution in a vessel.
  • the aqueous solution contains sodium hydroxide in a concentration between 0.26 M and 19 M NaOH.
  • the next step consists of reacting aluminum with water at the surface of the solution thereby generating a region of effervescence at the surface of the solution and a precipitate sinking to the bottom region of the vessel.
  • the process also includes the step of maintaining the region of effervescence separated from the precipitate at the bottom the vessel, to prevent the precipitate from swirling and mixing with the aluminum in the reaction zone at the surface of the solution.
  • This process is advantageous because it proceeds catalytically with the sodium hydroxide acting as the catalyst.
  • the process mentioned above is best carried out with an aqueous solution containing between about 5M and 10 M NaOH.
  • the process is also more efficient when makeup water is added only after an initial amount of aluminum has been consumed, and when the temperature of the aqueous solution has reached a peak or 75°C.
  • a process for initiating and maintaining a catalytic reaction of aluminum with water for producing hydrogen gas comprises the initial step of providing an aqueous solution in a vessel. This aqueous solution contains a portion of NaOH and a portion of water. The next steps consist of introducing a portion of aluminum in the aqueous solution, and reacting that portion of aluminum with the portion of water. The process also includes the steps of maintaining constant the portion of NaOH in the vessel and adding additional portions of water and additional portions of aluminum in the vessel according to the rates of consumption of the aluminum and the water in the reaction.
  • a process for simultaneously producing hydrogen gas and alumina (A1 2 0 3 ).
  • This process firstly comprises the step of providing an aqueous solution in a vessel.
  • the aqueous solution contains sodium hydroxide in a concentration between 0.26 M and 19 M NaOH.
  • the next step consists of reacting aluminum with water at a surface of the aqueous solution and generating hydrogen gas and alumina.
  • the process also includes the step of recovering hydrogen gas from the surface of the aqueous solution and alumina from a bottom region of the vessel.
  • FIG. 1 is graph illustrating a first reaction of aluminum with water to produce hydrogen gas, in a 5.0 M sodium hydroxide solution, carried out over a period of about 130 minutes;
  • FIG.2 is a graph illustrating a second reaction of aluminum with water to produce hydrogen gas, in a 4.95 M sodium hydroxide solution, carried out over a period of about 100 minutes;
  • FIG . 3 is a graph illustrating a third reaction of aluminum with water in a 4.5 M sodium hydroxide solution, while keeping the temperature relatively low
  • FIG. 4 is a graph illustrating a fourth reaction of aluminum with water in a 4.5 M sodium hydroxide solution, while keeping the temperature relatively low;
  • FIG. 5 is a graph illustrating a reaction of aluminum with water in a 1.2 M NaOH solution
  • FIG. 6 is a graph illustrating a reaction of aluminum with water in a 2.5 M NaOH solution
  • FIG. 7 is a graph illustrating a reaction of aluminum with water in a 3.9 M NaOH solution
  • FIG. 8 is a graph illustrating a reaction of aluminum with water in a 4.8 M NaOH solution
  • FIG. 9 is a graph illustrating a reaction of aluminum with water in a 5.5 M NaOH solution
  • FIG. 10 is a graph illustrating a reaction of aluminum with water in a 6 M NaOH solution
  • FIG. 11 is a graph illustrating a reaction of aluminum with water in a 6.03 M NaOH solution
  • FIG. 12 is a graph illustrating a reaction of aluminum with water in a 6.1 M NaOH solution
  • FIG. 13 is a graph illustrating a reaction of aluminum with water in a 6 M NaOH solution, wherein the water was added continuously;
  • FIG. 14 is a graph illustrating a reaction of aluminum with water in a 6 M NaOH solution, wherein the aluminum was added quickly;
  • FIG. 15 is a graph illustrating a reaction of aluminum with water in a 6.7 M NaOH solution
  • FIG. 16 is a graph illustrating a reaction of aluminum with water in a 11.3 M NaOH solution
  • FIG. 17 is a graph illustrating a reaction of aluminum with water in a saturated 19 M NaOH solution
  • FIG. 18 is graph illustrating maximum reaction temperatures obtained with aqueous solutions of various concentrations, and the responsiveness of the reaction for solutions of various concentrations ;
  • FIG. 19 is a graph showing the effects of adding water to the reaction as opposed to adding a fixed-molar NaOH solution to the reaction,
  • FIG. 20 is a partial cross-section view of an apparatus to produce hydrogen gas, embodying some of the preferred conditions to carry out the process according to the present invention. DETAILED DESCRIPTION OF THE PREFERRED EMBODIMENT
  • Stockburger and Belitskus teach that aluminum reacts with an alkaline solution of NaOH and that NaOH is subsequently regenerated by the precipitation of Al(OH) 3 as described by the formulas (5) and (6) respectively.
  • a first series of eight experiments was carried out to measure the volume of hydrogen gas produced in a typical reaction.
  • aluminum foil from Reynolds Aluminum Company of Canada was loosely crumpled and placed in a one litre plastic bottle containing 500 ml of catalytic solution of about 4.5M NaOH.
  • the bottle was quickly capped with a cover fitted with a tube which led to an inverted volumetric cylinder filled with water.
  • the bottle was immersed in a water bath to prevent overheating.
  • the volume of water displaced by the gas produced was measured and corrected to a gas volume at standard temperature and pressure (STP). Atmospheric pressure on that day was obtained from a local weather office. The corrected volume of gas produced was compared to the theoretical quantity of hydrogen gas, which would be obtained according to the equation,
  • the water used was tap water in all cases, in which dissolved air may have been present. If any of this air had been released in the presence of the warm hydrogen gas, this would have increased the volume of gas measured. This would have affected the results by less than 1%. Since the results are within the measurement error, and quantification of these two sources of error would not significantly affect the results, no further experiment was carried out in this area.
  • Table 2 shows that the purity of the hydrogen collected in the second sample was 98%. This is close to what was theoretically expected. The lower 92% concentration observed in the first sample was probably due to the fact the system was not completely purged with hydrogen before the sample was taken. By the time the second sample was taken, most of the air had been purged from the tube and the reaction bottle.
  • reaction bottle was placed in a water bath before the aluminum was added to the water, and the hydrogen produced was bubbled through the bath water.
  • the temperature of the bath and the catalytic solution were measured before and after the reaction, and at about four minutes after the reaction was completed.
  • the water equivalent of the plastic containers for absorbing heat and their specific heat were determined experimentally by adding a known quantity of hot water to the reaction system at room temperature and then calculating the heat transfer based on the final temperature.
  • the reaction has a net maximum heat production during hydrogen generation of 195.6 kCal/mole. A further 204.9 kCal/mole will be released if the hydrogen is burned with oxygen. Stated another way, 51% of the reaction energy is used to form hydrogen gas and 49% goes into the production of heat.
  • Sodium hydroxide (NaOH) pellets 40.63 g) from Wiler Fine Chemicals were placed in a two litre Erlenmeyer flask. Tap water (200 ml) was added to the flask. The mixture was swirled and allowed to stand on the lab bench. The lab temperature was 25°C. After about an hour, aluminum (Al) foil (30.72 g) was added in two portions . The first addition of aluminum is referred to as time zero, the start of the reaction. The temperature of the vapour coming from the top of the flask was measured using a thermometer and was found to be 93°C four minutes after the first half of the Al had been added. The flask was open to the atmosphere. The reaction was carried out for a period of 130 minutes. Additional quantities of Al and water were added at regular intervals, and the temperature was observed and recorded. The flask was swirled periodically to ensure the solution was in contact with the Al. No further NaOH was added.
  • NaOH sodium hydroxide
  • thermocouples were inserted through the suction inlet on the flask. The flask was open to the atmosphere. Thermocouple 1 (TCI) was placed in the NaOH solution about one centimetre from the bottom of the flask. The junction of thermocouple 2 (TC2) was placed in the flask neck at the same level as the suction inlet. The thermocouples were read by a Scimetric System 200 data recorder which stored the temperature readings at five second intervals.
  • TCI and TC2 After about half an hour TCI and TC2 read 31°C and 21°C respectively. After 53 minutes, TCI and TC2 read 26°C and 22°C, respectively, and heavy duty Al foil (4.90 g) from Alcan Aluminum Limited was added to the solution. There was vigorous reaction. This is referred to as time zero, the start of the reaction.
  • FIG.2 illustrates the response of this reaction in Experiment 2-2.
  • NaOH sodium hydroxide
  • Sodium hydroxide (NaOH) pellets 39.92 g) from Wiler Fine Chemicals, Lot # 14449, were placed in a two litre Erlenmeyer flask. Tap water (182ml) was added to the flask. The mixture was swirled and allowed to stand on the lab bench over night. Then it was swirled again to dissolve the remaining NaOH and mix the solution. The solution was then transferred to a 400 ml beaker.
  • the Al foil was added in portions over a 59 minute period.
  • gas bubbles were observed to form after about 45 seconds. It was noted that when gas bubbles formed on the surface of the Al, the piece of Al floated at or near the top of the reaction mixture. A small amount of fine black material was observed to float in the reaction mixture after all the Al has been dissolved. By the 44 th minute, the reaction mixture was observed to be very viscous because of the formation of a solid material.
  • tap water (30ml) was added to the reaction mixture. This Experiment 2-3 is explained graphically in FIG. 3.
  • reaction mixture was allowed to stand in the fume hood for about two hours after the addition of the last portion of Al, by which time the mixture had stopped bubbling. Part of the mixture was then filtered through a fine plastic mesh to ensure no un-reacted Al could contaminate the sample to be analysed. The mixture which passed through the mesh was then filtered by suction using qualitative filter paper. A sample of this grey precipitate was taken without washing and labelled P4-1. The remainder of the precipitate was removed from the filter paper and swirled with tap water in a flask, then it was re-filtered and washed with tap water.
  • Solutions of NaOH were typically cooled before starting the reactions. The starting temperature for each reaction was often in the range of 4- 10°C. The reactions were carried out in glass vessels ranging in size from 25 ml to 500 ml. Solutions of NaOH were prepared by dissolving NaOH pellets from BDH Inc., Toronto, Ontario, Canada, M8Z 1K5, Lot #128142-125228, in tap water at room temperature. The heat of solvation was allowed to dissipate and the portion of the solution to be used in the experiment was cooled in an ice bath in the reaction vessel.
  • thermocouple junction was placed in the solution about one centimetre below the surface.
  • the thermocouple reading was monitored continually and recorded on a computer file every 15 seconds.
  • Aluminum foil (Reynolds Wrap from Canadian Reynolds Metals Company Ltd., Montreal, Toronto, Calgary, Canada) was crumpled or folded and added in portions ranging from 0.2 g to 1.1 g. Each portion of Al foil was initially submerged in the solution using a glass stirring rod. Then it was allowed to float to the top of the solution. The start time for every experiment was the time when the first aluminum was added. Aluminum was added in amounts to keep the temperature above 60°C.
  • catalytic ratio in the above table is calculated by dividing the amount of Al that actually reacted by the amount that would have reacted if the reaction were stoichiometric with respect to NaOH as in equation (3), (4) or (5).
  • Table 8 also shows the results of the analyses of the precipitates filtered from twelve of the experiments. In every case the concentration of the Al species is larger than 96%. Sodium was detectable in only three of the samples, and then at a maximum concentration of only 1.14% or less. Thus, aluminum is present in the precipitate at levels that are two orders of magnitude above sodium.
  • reaction according to the present invention is catalytic in aqueous solutions from 0.26 M NaOH to 19 M NaOH. It should be noted that although the 0.26 M and 0.60 M solutions showed a catalytic reaction, the reaction temperature did not rise above 30°C during those experiments. However, FIG.5 shows that the temperature of the 1.2 M solution rose above 45°C even though the Al was added very slowly and only after the previous portion had dissolved.
  • FIGS. 5-17 show that the reaction can and does occur over a temperature range from 4°C to 165°C.
  • a temperature of 170°C was observed.
  • the molal boiling point elevation constant will result in a higher boiling point for the more concentrated solutions, ensuring that water does not boil off until the higher boiling point is reached.
  • the boiling point elevation would have contributed to the high boiling point of the solution.
  • NaOH did not precipitate from the solution even at the higher concentration, probably because of the known higher solubility of NaOH in hot aqueous solutions.
  • the present process to produce hydrogen is reproducible with aqueous solutions from 1.2 M NaOH to 19 M NaOH and over a temperature range from 4°C to greater than 170°C. Furthermore, the reaction is catalytic over the same temperature range and over a NaOH concentration range of 0.26 M to above 19 M.
  • the reaction's by-product comprises high-purity alumina (A1 2 0 3 ).
  • FIG. 18 shows a first curve 30 showing the maximum temperatures obtained with different NaOH concentrations.
  • This best-fit curve was plotted from the data shown in FIGS. 5-17, and is presented herein for illustrating the effect of NaOH concentration on the maximum temperature of the reaction.
  • FIG. 18 shows another curve 32 which represents the responsiveness of the reaction to aluminum and water additions. This curve has been prepared by plotting the time required to reach the initial maximum temperature of the reactions, against the different NaOH concentrations studied.
  • the resulting best-fit curve is a complex inverted hyperbolic curve centred on a concentration of about 8 M NaOH.
  • the first curve 34 represents the effect of adding plain water to the catalytic reaction of equation (1) or (2). As the reaction proceeds, the water is consumed, and therefore, the concentration of NaOH increases, as shown by the segment 36, from its initial concentration 38. When water is added, as indicated by segment 40, the concentration drops back to or below the initial concentration 38. If water is added in portions to maintain a certain level in a reaction vessel for example, the solution concentration fluctuates up and down from the initial concentration 38, as generally represented by the curve 34.
  • the arrows 50, 52 and the corresponding theory explain the facts that in some experiments, a water addition has caused the reaction to slow down, according to the arrow 50, and in other experiments, the addition of water caused an immediate response, as in 52.
  • the same theory explains why both events can occur in a same experiment, such as when the NaOH concentration is maintained substantially in the median region, between 5 and 10 M NaOH.
  • the curve 44 and arrows 48 on the other hand, explain why prior inventors may have failed to observe a catalytic reaction with the same elements.
  • reaction (1) or (2) is reproducible with aluminum flakes from beverage cans and food packages, aluminum chips, shavings and sawdust found in machine shop waste, and aluminum powder available commercially for different purposes including fireworks, or other small aluminum particles of the like. It is to be expected that the intensity of the reaction depends upon the surface of contact between the aluminum and water. Aluminum foil for example reacts faster than a heavy gauge aluminum wire, and aluminum powder would react almost instantly to produce hydrogen gas.
  • a preferred hydrogen generator 60 is illustrated in FIG.20.
  • the hydrogen generator 60 comprises a reaction vessel 62 made of non-corrosive material, in which the reaction is carried out.
  • a minimum amount of an alkaline solution 64 is maintained in this vessel.
  • aluminum particles reacts with water at the surface 66 of the alkaline solution and defines at and near the surface 66, a region of substantial effervescence. This region is defined as the reaction zone 'F'.
  • the height of the reaction zone *F' vary with the intensity of the reaction, and extends above and below the surface 66 of the alkaline solution 64.
  • aprecipitate 68 accumulates at the bottom of the reaction vessel 62.
  • reaction zone 'F' it is recommended to maintain the reaction zone 'F' at a height 'H' of at least about 1 cm above the precipitate 68, to prevent the precipitate from swirling into the reaction zone and mixing with the aluminum particles.
  • this dimension can be reduced in some installations, a dimension of one centimetre is suggested herein to enable those skilled in the art to readily use the process according to the present invention successfully.
  • a water bottle 70 is affixed to the side of the reaction vessel 62 and has a piping system 72 connected to an array of nozzles 74 in the bottom of the reaction vessel 62. Only one nozzle is shown for clarity.
  • the introduction of water through the bottom of the vessel 62 has the effect of capturing some of the heat in the precipitate 68 to preheat the water entering the reaction vessel.
  • a second purpose for the feeding of water through the bottom of the reaction vessel 62 is to entrain to the reaction zone 'F', any sodium hydroxide which may be present in the precipitate 68.
  • the upper limit should be defined as to maintain the concentration of the alkaline solution over about lMNaOH, and more preferably, a concentration of 5M NaOH.
  • a sight glass 76 on the side of the reaction vessel 62 is provided to monitor the minimum distance 'H' of the reaction zone 'F' above the precipitate 68.
  • Aluminum particles 78 are delivered into the reaction vessel 62 from a hopper 80 mounted on the top of the vessel 62, though an airlockTM rotary feeder 84 and through a drop pipe 86 at the center of the reaction vessel 62.
  • a deflector 88 is mounted at the end of the drop pipe 86 to disperse the aluminum particles 78 over the entire surface of the alkaline solution 64.
  • the hydrogen generated in the reaction vessel exits through the drop pipe 86 and the spout 90.
  • the drop pipe 86 is preferably mounted through a large openable cap 92 on the top of the reaction vessel. This cap 92 preferably covers a substantial portion of the upper end of the reaction vessel 62 and provides access to the reaction vessel for periodically cleaning the vessel.
  • a bung 94 is provided in the bottom surface of the reaction vessel 62 to recover the precipitate 68.
  • the aluminum particles 78 are preferably flakes, sawdust, milling shavings and chips, powder or other similar small particles having a large surface over volume ratio. It has been noticed that aluminum foil fragments for example, have a tendency to float at the surface 66 of the alkaline solution 64. This is preferable and is explained by the buoyancy created by the foam 96 and the bubbling action generate in the reaction zone 'F' . It is believed that the bubbling action and the high temperature in this reaction zone is ideal to prevent or reduce the formation of a protective oxide layer on the surface of the aluminum particles. It is believed that the retention of the aluminum particles in this reaction zone contributes largely to maintaining the catalytic effect.

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  • Chemical & Material Sciences (AREA)
  • Organic Chemistry (AREA)
  • Chemical Kinetics & Catalysis (AREA)
  • Inorganic Chemistry (AREA)
  • General Health & Medical Sciences (AREA)
  • Combustion & Propulsion (AREA)
  • Engineering & Computer Science (AREA)
  • Health & Medical Sciences (AREA)
  • Life Sciences & Earth Sciences (AREA)
  • Geology (AREA)
  • Catalysts (AREA)
  • Compounds Of Alkaline-Earth Elements, Aluminum Or Rare-Earth Metals (AREA)
  • Fuel Cell (AREA)

Abstract

L'invention concerne un procédé de production d'hydrogène qui consiste à faire réagir de l'aluminium (78) avec de l'eau (70) en présence d'hydroxyde de sodium en tant que catalyseur. L'invention concerne, selon un aspect, un procédé de production d'hydrogène qui comprend les étapes consistant: à utiliser une solution aqueuse contenant entre 0,26M et 19M de NaOH dans une cuve; à faire réagir de l'aluminium avec de l'eau à la surface de la solution afin de générer une région d'effervescence à la surface de la solution et un précipité s'écoulant depuis la région d'effervescence jusqu'au fond de la cuve; et à maintenir ladite région d'effervescence séparée du précipité au fond de la cuve, afin d'empêcher tout précipité de se mélanger avec l'aluminium au niveau dudit fond de la cuve.
EP03767339A 2002-12-12 2003-12-10 Procede de production d'hydrogene Withdrawn EP1569868A1 (fr)

Applications Claiming Priority (3)

Application Number Priority Date Filing Date Title
CA002414135A CA2414135C (fr) 2002-12-12 2002-12-12 Methode de production d'hydrogene
CA2414135 2002-12-12
PCT/CA2003/001908 WO2004052775A1 (fr) 2002-12-12 2003-12-10 Procede de production d'hydrogene

Publications (1)

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EP1569868A1 true EP1569868A1 (fr) 2005-09-07

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EP (1) EP1569868A1 (fr)
AU (1) AU2003291881B2 (fr)
CA (1) CA2414135C (fr)
WO (1) WO2004052775A1 (fr)

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WO2002006153A1 (fr) * 2000-07-13 2002-01-24 Hydrogen Energy America Llc Procede et dispositif de production commandee d'hydrogene par dissociation de l'eau
WO2006025511A1 (fr) * 2004-08-30 2006-03-09 Nitto Denko Corporation Preparation generatrice d'hydrogene
JP2006335603A (ja) * 2005-06-02 2006-12-14 Nitto Denko Corp 水素発生剤及び水素発生方法
US7803349B1 (en) 2005-06-08 2010-09-28 University Of Central Florida Research Foundation, Inc. Method and apparatus for hydrogen production from water
EP1905735B1 (fr) * 2005-07-20 2011-09-14 Hitachi Maxell Energy, Ltd. Matière générant de l'hydrogène et procédé de production d'une matière générant de l'hydrogène
FR2893355A1 (fr) * 2005-11-16 2007-05-18 Fabien Lecler Moteur a hydrogene produit par reaction chimique de l'hydroxyde de sodium et de poudre d'aluminium avec l'eau
WO2009018468A1 (fr) 2007-07-31 2009-02-05 Purdue Research Foundation Système de commande pour un générateur de gaz à la demande
WO2013009158A1 (fr) * 2011-07-08 2013-01-17 Iturbe Garcia Jose Luis Procédé pour la production de gaz hydrogène, d'alumine et de carbonate de sodium en une seule étape à partir de la réaction entre des particules d'aluminium et une solution aqueuse d'hydroxyde de sodium
WO2013150527A1 (fr) * 2012-04-05 2013-10-10 H Force Ltd Système et procédé pour la production efficace d'hydrogène
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WO2004052775A1 (fr) 2004-06-24

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