Hydrogen storage

From Wikipedia, the free encyclopedia

This is an old revision of this page, as edited by Robert1947 (talk | contribs) at 04:39, 6 December 2019 (→‎Liquid hydrogen: minor rewording.). The present address (URL) is a permanent link to this revision, which may differ significantly from the current revision.

Utility scale underground liquid hydrogen storage

Methods of hydrogen storage for subsequent use span many approaches including high pressures, cryogenics, and chemical compounds that reversibly release H2 upon heating. Underground hydrogen storage is useful to provide grid energy storage for intermittent energy sources, like wind power, as well as providing fuel for transportation, particularly for ships and airplanes.

Most research into hydrogen storage is focused on storing hydrogen as a lightweight, compact energy carrier for mobile applications.

Liquid hydrogen or slush hydrogen may be used, as in the Space Shuttle. However liquid hydrogen requires cryogenic storage and boils around 20.268 K (−252.882 °C or −423.188 °F). Hence, its liquefaction imposes a large energy loss (as energy is needed to cool it down to that temperature). The tanks must also be well insulated to prevent boil off but adding insulation increases cost. Liquid hydrogen has less energy density by volume than hydrocarbon fuels such as gasoline by approximately a factor of four. This highlights the density problem for pure hydrogen: there is actually about 64% more hydrogen in a liter of gasoline (116 grams hydrogen) than there is in a liter of pure liquid hydrogen (71 grams hydrogen). The carbon in the gasoline also contributes to the energy of combustion.

Compressed hydrogen, by comparison, is stored quite differently. Hydrogen gas has good energy density by weight, but poor energy density by volume versus hydrocarbons, hence it requires a larger tank to store. A large hydrogen tank will be heavier than the small hydrocarbon tank used to store the same amount of energy, all other factors remaining equal. Increasing gas pressure would improve the energy density by volume, making for smaller, but not lighter container tanks (see hydrogen tank). Compressed hydrogen is estimated to cost about 2.1% of the energy content[1] to power the compressor for a large scale underground facility such as a cavern or aquifer from 1 to 200 bar. Higher compression without energy recovery will mean more energy lost to the compression step. Compressed hydrogen storage can exhibit very low permeation.[2]

Established technologies

Net storage density of hydrogen

Compressed hydrogen

Compressed hydrogen is a storage form where hydrogen gas is kept under pressures to increase the storage density. Compressed hydrogen in hydrogen tanks at 350 bar (5,000 psi) and 700 bar (10,000 psi) is used for hydrogen tank systems in vehicles, based on type IV carbon-composite technology.[3] Car manufacturers have been developing this solution, such as Honda[4] or Nissan.[5]

Liquid hydrogen

BMW has been working on liquid hydrogen tanks for cars, producing for example the BMW Hydrogen 7. Japan has a liquid hydrogen (LH2) storage site in Kobe port. It is anticipated to receive the first shipment of liquid hydrogen via LH2 carrier in 2020.[6] Hydrogen is liquified by reducing its temperature to -253°C, similar to liquified natural gas (LNG) which is stored at -162°C. A potential efficiency loss of 12.79% can be achieved, or 4.26kWh/kg out of 33.3kWh/kg.[7]

Proposals and research

Hydrogen storage technologies can be divided into physical storage, where hydrogen molecules are stored (including pure hydrogen storage via compression and liquefaction), and chemical storage, where hydrides are stored.

Chemical storage

Chemical storage could offer high storage performance due to the strong binding of hydrogen and the high storage densities. However, the regeneration of storage material is still an issue. A large number of chemical storage systems are under investigation, which involve hydrolysis reactions, hydrogenation/dehydrogenation reactions, ammonia borane and other boron hydrides, ammonia, and alane etc.[8] Storage in hydrocarbons may also be successful in overcoming the issue with low density. For example, supercritical hydrogen at 30 °C and 500 bar only has a density of 15.0 mol/L while methanol has a density of 49.5 mol H2/L methanol and saturated dimethyl ether at 30 °C and 7 bar has a density of 42.1 mol H2/L dimethyl ether. These liquids would use much smaller, cheaper, safer storage tanks.[citation needed] The most promising chemical approach is electrochemical hydrogen storage, as the release of hydrogen can be controlled by the applied electricity.[9] Most of the materials listed below can be directly used for electrochemical hydrogen storage.

Metal hydrides

Metal hydride hydrogen storage

Metal hydrides, such as MgH2, NaAlH4, LiAlH4, LiH, LaNi5H6, TiFeH2 and palladium hydride, with varying degrees of efficiency, can be used as a storage medium for hydrogen, often reversibly.[10] Some are easy-to-fuel liquids at ambient temperature and pressure, whereas others are solids which could be turned into pellets. These materials have good energy density, although their specific energy is often worse than the leading hydrocarbon fuels.

Most metal hydrides bind with hydrogen very strongly. As a result, high temperatures around 120 °C (248 °F) – 200 °C (392 °F) are required to release their hydrogen content. This energy cost can be reduced by using alloys which consists of a strong hydride former and a weak one such as in LiNH2, LiBH4 and NaBH4.[11] These are able to form weaker bonds, thereby requiring less input to release stored hydrogen. However, if the interaction is too weak, the pressure needed for rehydriding is high, thereby eliminating any energy savings. The target for onboard hydrogen fuel systems is roughly <100 °C for release and <700 bar for recharge (20–60 kJ/mol H2).[12]

An alternative method for reducing dissociation temperatures is doping with activators. This has been successfully used for aluminium hydride but its complex synthesis makes it undesirable for most applications as it is not easily recharged with hydrogen.[13]

Currently the only hydrides which are capable of achieving the 9 wt% gravimetric goal for 2015 (see chart above) are limited to lithium, boron and aluminium based compounds; at least one of the second-row elements or Al must be added. Research is being done to determine new compounds which can be used to meet these requirements.

Proposed hydrides for use in a hydrogen economy include simple hydrides of magnesium[14] or transition metals and complex metal hydrides, typically containing sodium, lithium, or calcium and aluminium or boron. Hydrides chosen for storage applications provide low reactivity (high safety) and high hydrogen storage densities. Leading candidates are lithium hydride, sodium borohydride, lithium aluminium hydride and ammonia borane. A French company McPhy Energy is developing the first industrial product, based on magnesium hydride, already sold to some major clients such as Iwatani and ENEL.

New Scientist reported that Arizona State University is investigating using a borohydride solution to store hydrogen, which is released when the solution flows over a catalyst made of ruthenium.[15] Researchers at University of Pittsburgh and Georgia Tech performed extensive benchmarking simulations on mixtures of several light metal hydrides to predict possible reaction thermodynamics for hydrogen storage.[16][17][18]

Nanostructured metal hydrides

Metal hydrides have proven to be a good alternative for hydrogen storage systems because of their favorable properties such as high volumetric and gravimetric density. However, more research is necessary to satisfy the United States Department of Energy’s requirements for storage capacity, kinetics, cyclability, cost, and release temperature. Nano-metal hydrides possess a number of properties that make them even better candidates for future hydrogen storage systems compared to their bulk equivalents. At the nanoscale, structural and chemical properties (such as particle size and sorption site density) show a significant improvement in properties such as sorption kinetics, hydrogen diffusion or hydrogen release temperature. However, the downsides of nanoscale materials include poor heat transfer and total sorption capacity. The Key Laboratory of Advanced Materials Technology of Liaoning, China, studied the difference in the reaction kinetics between bulk MgH2 and nanoparticles of this compound.[19] They observed that the amount of hydrogen released by the 30 nm particle was 5wt%, 10 times greater than the bulk material (0.5wt%) over the same period of time (1 hour) and at the same temperature (300ºC). However, a 5 wt% capacity is still not sufficient for large scale applications. Palladium (Pd) proved to be an effective alternative with favorable kinetics, but its high cost suggests favorability in using more affordable metals such as vanadium (V). A MgH2-5 wt% V showed fast adsorption kinetics in much larger quantities than Pd. A mixture of titanium and iron was also successfully used, despite these two metals being ineffective if used separately.[19] The addition of LiBH4 has also been studied for the enhancement of sorption kinetics.[20]

Thermodynamics of nanometal hydrides

As shown before, nanomaterials have proven to be superior for hydrogen storage systems. Nanomaterials offer an alternative that overcomes the two major barriers of bulk materials, rate of sorption and release temperature.

The rate of hydrogen sorption improves at the nanoscale due to the short diffusion distance in comparison to bulk materials. This, combined with the notably greater surface-area-to-volume ratio of nanoparticles, accounts for the significant advantage over bulk metals used for hydrogen storage. The release temperature of a material is defined as the temperature at which the desorption process begins. It is paramount to achieve the lowest release temperature possible to reduce the cost of the heating process required to liberate the gas. To describe the improvement over bulk materials regarding this parameter, researchers base their studies on a modified van ’t Hoff equation, shown below, that relates temperature and partial pressure of hydrogen during the desorption process. The modifications to the standard equation are related to size effects at the nanoscale

Where pH2 is the partial pressure of hydrogen, ΔH is the enthalpy of the sorption process (exothermic), ΔS is the change in entropy, R is the ideal gas constant, T is the temperature in Kelvin, Vm is the molar volume of the metal, r is the radius of the nanoparticle and γ is the surface free energy of the particle.

From the above relation we see that the enthalpy and entropy change of desorption processes depend on the radius of the nanoparticle. Moreover, a new term is included that takes into account the specific surface area of the particle and it can be mathematically proven that a decrease in particle radius leads to a decrease in the release temperature for a given partial pressure.[21]

Non-metal hydrides

The Italian catalyst manufacturer Acta has proposed using hydrazine as an alternative to hydrogen in fuel cells. As the hydrazine fuel is liquid at room temperature, it can be handled and stored more easily than hydrogen. By storing it in a tank full of a double-bonded carbon-oxygen carbonyl, it reacts and forms a safe solid called hydrazone. By then flushing the tank with warm water, the liquid hydrazine hydrate is released. Hydrazine breaks down in the cell to form nitrogen and hydrogen which bonds with oxygen, releasing water.[22] Silicon hydrides and germanium hydrides are also candidates of hydrogen storage materials, as they can subject to energetically favored reaction to form covalently bonded dimers with loss of a hydrogen molecule.[23] [24]

Carbohydrates

Carbohydrates (polymeric C6H10O5) releases H2 in a bioreformer mediated by the enzyme cocktail—cell-free synthetic pathway biotransformation. Carbohydrate provides high hydrogen storage densities as a liquid with mild pressurization and cryogenic constraints: It can also be stored as a solid powder. Carbohydrate is the most abundant renewable bioresource in the world.

In May 2007 biochemical engineers from the Virginia Polytechnic Institute and State University and biologists and chemists from the Oak Ridge National Laboratory announced a method of producing high-yield pure hydrogen from starch and water.[25] In 2009, they demonstrated to produce nearly 12 moles of hydrogen per glucose unit from cellulosic materials and water.[26] Thanks to complete conversion and modest reaction conditions, they propose to use carbohydrate as a high energy density hydrogen carrier with a density of 14.8 wt%.[27]

Synthesized hydrocarbons

An alternative to hydrides is to use regular hydrocarbon fuels as the hydrogen carrier. Then a small hydrogen reformer would extract the hydrogen as needed by the fuel cell. However, these reformers are slow to react to changes in demand and add a large incremental cost to the vehicle powertrain.

Direct methanol fuel cells do not require a reformer, but provide a lower energy density compared to conventional fuel cells, although this could be counterbalanced with the much better energy densities of ethanol and methanol over hydrogen. Alcohol fuel is a renewable resource.

Solid-oxide fuel cells can operate on light hydrocarbons such as propane and methane without a reformer, or can run on higher hydrocarbons with only partial reforming, but the high temperature and slow startup time of these fuel cells are problematic for automotive applications.

Aluminum
Main article: Aluminum

Aluminum has been proposed as an energy storage method by a number of researchers. Hydrogen can be extracted from aluminum by reacting it with water.[28] To react with water, however, aluminum must be stripped of its natural oxide layer, a process which requires pulverization,[29] chemical reactions with caustic substances, or alloys.[30] The byproduct of the reaction to create hydrogen is aluminum oxide, which can be recycled back into aluminum with the Hall–Héroult process, making the reaction theoretically renewable.

Liquid organic hydrogen carriers (LOHC)

Reversible hydrogenation of N-ethylcarbazole

Unsaturated organic compounds can store huge amounts of hydrogen. These Liquid Organic Hydrogen Carriers (LOHC) are hydrogenated for storage and dehydrogenated again when the energy/hydrogen is needed. Research on LOHC was concentrated on cycloalkanes at an early stage, with its relatively high hydrogen capacity (6-8 wt %) and production of COx-free hydrogen.[31] Heterocyclic aromatic compounds (or N-Heterocycles) are also appropriate for this task. A compound featuring in LOHC research is N-Ethylcarbazole (NEC)[32] but many others do exist.[33] Dibenzyltoluene, which is already used as a heat transfer fluid in industry, was identified as potential LOHC. With a wide liquid range between -39 °C (melting point) and 390 °C (boiling point) and a hydrogen storage density of 6.2 wt% dibenzyltoluene is ideally suited as LOHC material.[34] Formic acid has been suggested as a promising hydrogen storage material with a 4.4wt% hydrogen capacity.[35]

Using LOHCs relatively high gravimetric storage densities can be reached (about 6 wt-%) and the overall energy efficiency is higher than for other chemical storage options such as producing methane from the hydrogen.[36]

Cycloalkanes

Cycloalkanes reported as LOHC include cyclohexane, methyl-cyclohexane and decalin. The dehydrogenation of cycloalkanes is highly endothermic (63-69 kJ/mol H2), which means this process requires high temperature.[31] Dehydrogenation of decalin is the most thermodynamically favored among the three cycloalkanes, and methyl-cyclohexane is second because of the presence of the methyl group.[37] Research on catalyst development for dehydrogenation of cycloalkanes has been carried out for decades. Nickel (Ni), Molybdenum (Mo) and Platinum (Pt) based catalysts are highly investigated for dehydrogenation. However, coking is still a big challenge for catalyst's long-term stability.[38][39]

N-Heterocycles

Both hydrogenation and dehydrogenation of LOHCs requires catalysts.[31] It was demonstrated that replacing hydrocarbons by hetero-atoms, like N, O etc. improves reversible de/hydrogenation properties. The temperature required for hydrogenation and dehydrogenation drops significantly with increasing numbers of heteroatoms.[40] Among all the N-heterocycles, the saturated-unsaturated pair of dodecahydro-N-ethylcarbazole (12H-NEC) and NEC has been considered as a promising candidate for hydrogen storage with a fairly large hydrogen content (5.8wt%).[41] The figure on the top right shows dehydrogenation and hydrogenation of the 12H-NEC and NEC pair. The standard catalyst for NEC to 12H-NEC is Ru and Rh based. The selectivity of hydrogenation can reach 97% at 7 MPa and 130 °C-150 °C.[31] Although N-Heterocyles can optimize the unfavorable thermodynamic properties of cycloalkanes, a lot of issues remain unsolved, such as high cost, high toxicity and kinetic barriers etc.[31]

Formic acid

In 2006, Swiss researchers at EPFL reported the use of formic acid as a hydrogen storage material.[42] Carbon monoxide free hydrogen has been generated in a very wide pressure range (1–600 bar). A homogeneous catalytic system based on water-soluble ruthenium catalysts selectively decompose HCOOH into H2 and CO2 in aqueous solution.[43] This catalytic system overcomes the limitations of other catalysts (e.g. poor stability, limited catalytic lifetimes, formation of CO) for the decomposition of formic acid making it a viable hydrogen storage material.[44] And the co-product of this decomposition, carbon dioxide, can be used as hydrogen vector by hydrogenating it back to formic acid in a second step. The catalytic hydrogenation of CO2 has long been studied and efficient procedures have been developed.[45][46] Formic acid contains 53 g L−1 hydrogen at room temperature and atmospheric pressure. By weight, pure formic acid stores 4.3 wt% hydrogen. Pure formic acid is a liquid with a flash point 69 °C (cf. gasoline −40 °C, ethanol 13 °C). 85% formic acid is not flammable.

Ammonia

Further information: Ammonia production

Ammonia (NH3) releases H2 in an appropriate catalytic reformer. Ammonia provides high hydrogen storage densities as a liquid with mild pressurization and cryogenic constraints: It can also be stored as a liquid at room temperature and pressure when mixed with water. Ammonia is the second most commonly produced chemical in the world and a large infrastructure for making, transporting, and distributing ammonia exists. Ammonia can be reformed to produce hydrogen with no harmful waste, or can mix with existing fuels and under the right conditions burn efficiently. Since there is no carbon in ammonia, no carbon by-products are produced; thereby making this possibility a "carbon neutral" option for the future. Pure ammonia burns poorly at the atmospheric pressures found in natural gas fired water heaters and stoves. Under compression in an automobile engine it is a suitable fuel for slightly modified gasoline engines. Ammonia is the suitable alternative fuel because it has 18.6 MJ/kg energy density at NTP and carbon-free combustion byproducts.[47] However, ammonia is a toxic gas at normal temperature and pressure and has a potent odor.[48]

In 2018, researchers at CSIRO in Australia powered a Toyota Mirai and Hyundai Nexo with hydrogen separated from ammonia using a membrane technology. [49]

In September 2005 chemists from the Technical University of Denmark announced a method of storing hydrogen in the form of ammonia saturated into a salt tablet. They claim it will be an inexpensive and safe storage method.[50]

Amine borane complexes

Main article: Amine borane complex

Prior to 1980, several compounds were investigated for hydrogen storage including complex borohydrides, or aluminohydrides, and ammonium salts. These hydrides have an upper theoretical hydrogen yield limited to about 8.5% by weight. Amongst the compounds that contain only B, N, and H (both positive and negative ions), representative examples include: amine boranes, boron hydride ammoniates, hydrazine-borane complexes, and ammonium octahydrotriborates or tetrahydroborates. Of these, amine boranes (and especially ammonia borane) have been extensively investigated as hydrogen carriers. During the 1970s and 1980s, the U.S. Army and Navy funded efforts aimed at developing hydrogen/deuterium gas-generating compounds for use in the HF/DF and HCl chemical lasers, and gas dynamic lasers. Earlier hydrogen gas-generating formulations used amine boranes and their derivatives. Ignition of the amine borane(s) forms boron nitride (BN) and hydrogen gas. In addition to ammonia borane (H3BNH3), other gas-generators include diborane diammoniate, H2B(NH3)2BH4.

Nano borohydrides and nanocatalyst doping

Enhancement of sorption kinetics and storage capacity can be improved through nanomaterial-based catalyst doping, as shown in the work of the Clean Energy Research Center in the University of South Florida.[20] This research group studied LiBH4 doped with nickel nanoparticles and analyzed the weight loss and release temperature of the different species. They observed that an increasing amount of nanocatalyst lowers the release temperature by approximately 20ºC and increases the weight loss of the material by 2-3%. The optimum amount of Ni particles was found to be 3 mol%, for which the temperature was within the limits established (around 100ºC) and the weight loss was notably greater than the undoped species.

Imidazolium ionic liquids

In 2007, Dupont and others reported hydrogen-storage materials based on imidazolium ionic liquids. Simple alkyl(aryl)-3-methylimidazolium N-bis(trifluoromethanesulfonyl)imidate salts that possess very low vapour pressure, high density, and thermal stability and are nonflammable can add reversibly 6–12 hydrogen atoms in the presence of classical Pd/C or Ir0 nanoparticle catalysts and can be used as alternative materials for on-board hydrogen-storage devices. These salts can hold up to 30 g L−1 of hydrogen at atmospheric pressure.[51]

Phosphonium borate

In 2006 researchers of University of Windsor reported on reversible hydrogen storage in a non-metal phosphonium borate frustrated Lewis pair:[52][53][54]

Phosphino borane hydrogenstorage
Phosphino borane hydrogenstorage

The phosphino-borane on the left accepts one equivalent of hydrogen at one atmosphere and 25 °C and expels it again by heating to 100 °C. The storage capacity is 0.25 wt% still rather below the 6 to 9 wt% required for practical use.

Carbonite substances

Research has proven that graphene can store hydrogen efficiently. After taking up hydrogen, the substance becomes graphane. After tests, conducted by dr André Geim at the University of Manchester, it was shown that not only can graphene store hydrogen easily, it can also release the hydrogen again, after heating to 450 °C.[55][56]

Metal-organic frameworks

Metal-organic frameworks represent another class of synthetic porous materials that store hydrogen and energy at the molecular level. MOFs are highly crystalline inorganic-organic hybrid structures that contain metal clusters or ions (secondary building units) as nodes and organic ligands as linkers. When guest molecules (solvent) occupying the pores are removed during solvent exchange and heating under vacuum, porous structure of MOFs can be achieved without destabilizing the frame and hydrogen molecules will be adsorbed onto the surface of the pores by physisorption. Compared to traditional zeolites and porous carbon materials, MOFs have very high number of pores and surface area which allow higher hydrogen uptake in a given volume. Thus, research interests on hydrogen storage in MOFs have been growing since 2003 when the first MOF-based hydrogen storage was introduced. Since there are infinite geometric and chemical variations of MOFs based on different combinations of SBUs and linkers, many researches explore what combination will provide the maximum hydrogen uptake by varying materials of metal ions and linkers.

In 2006, chemists at UCLA and the University of Michigan have achieved hydrogen storage concentrations of up to 7.5 wt% in MOF-74 at a low temperature of 77 K.[57][58] In 2009, researchers at University of Nottingham reached 10 wt% at 77 bar (1,117 psi) and 77 K with MOF NOTT-112.[59] Most articles about hydrogen storage in MOFs report hydrogen uptake capacity at a temperature of 77K and a pressure of 1 bar because these conditions are commonly available and the binding energy between hydrogen and the MOF at this temperature is large compared to the thermal vibration energy. Varying several factors such as surface area, pore size, catenation, ligand structure, and sample purity can result in different amounts of hydrogen uptake in MOFs.

Encapsulation

Cella Energy technology is based around the encapsulation of hydrogen gas and nano-structuring of chemical hydrides in small plastic balls, at room temperature and pressure.[60]

Physical storage

In this case hydrogen remains in physical forms, i.e., as gas, supercritical fluid, adsorbate, or molecular inclusions. Theoretical limitations and experimental results are considered [61] concerning the volumetric and gravimetric capacity of glass microvessels, microporous, and nanoporous media, as well as safety and refilling-time demands.

Activated carbons

Activated carbons are highly porous amorphous carbon materials with high apparent surface area. Hydrogen physisorption can be increased in these materials by increasing the apparent surface area and optimizing pore diameter to around 7 Å.[62] These materials are of particular interest due to the fact that they can be made from waste materials, such as cigarette butts which have shown great potential as precursor materials for high-capacity hydrogen storage materials.[63][64]

Cryo-compressed

Cryo-compressed storage of hydrogen is the only technology that meets 2015 DOE targets for volumetric and gravimetric efficiency (see "CcH2" on slide 6 in [65]).

Furthermore, another study has shown that cryo-compressed exhibits interesting cost advantages: ownership cost (price per mile) and storage system cost (price per vehicle) are actually the lowest when compared to any other technology (see third row in slide 13 of [66]). For example, a cryo-compressed hydrogen system would cost $0.12 per mile (including cost of fuel and every associated other cost), while conventional gasoline vehicles cost between $0.05 and $0.07 per mile.

Like liquid storage, cryo-compressed uses cold hydrogen (20.3 K and slightly above) in order to reach a high energy density. However, the main difference is that, when the hydrogen would warm-up due to heat transfer with the environment ("boil off"), the tank is allowed to go to pressures much higher (up to 350 bars versus a couple of bars for liquid storage). As a consequence, it takes more time before the hydrogen has to vent, and in most driving situations, enough hydrogen is used by the car to keep the pressure well below the venting limit.

Consequently, it has been demonstrated that a high driving range could be achieved with a cryo-compressed tank : more than 650 miles (1,050 km) were driven with a full tank mounted on an hydrogen-fueled engine of Toyota Prius.[67] Research is still underway to study and demonstrate the full potential of the technology.[68]

As of 2010, the BMW Group has started a thorough component and system level validation of cryo-compressed vehicle storage on its way to a commercial product.[69]

Carbon nanotubes

Carbon nanotubes

Hydrogen carriers based on nanostructured carbon (such as carbon buckyballs and nanotubes) have been proposed. However, since Hydrogen usually amounts up to ~3.0-7.0 wt% at 77K which is far from the value set by US department of Energy (6 wt% at nearly ambient conditions), it makes carbon materials poor candidates for hydrogen storage.

To realize carbon materials as effective hydrogen storage technologies, the Clean Energy Research Center has doped carbon nanotubes (CNTs) with MgH2.[20] The metal hydride has proven to have a theoretical storage capacity (7.6 wt%) that fulfills the United States Department of Energy requirement of 6 wt%, but has limited practical applications due to its high release temperature. The proposed mechanism involves the creation of fast diffusion channels by CNTs within the MgH2 lattice. Fullerene is other carbonaceous nanomaterials that has been tested for hydrogen storage in this center. Fullerene molecules are composed of a C60 close-caged structure, that allows for hydrogenation of the double bonded carbons leading to a theoretical C60H60 isomer with a hydrogen content of 7.7 wt%. However, the release temperature in these systems is too high (600oC) for practical applications.

Clathrate hydrates

H2 caged in a clathrate hydrate was first reported in 2002, but requires very high pressures to be stable. In 2004, researchers from Delft University of Technology and Colorado School of Mines showed solid H2-containing hydrates could be formed at ambient temperature and 10s of bar by adding small amounts of promoting substances such as THF.[70] These clathrates have a theoretical maximum hydrogen densities of around 5 wt% and 40 kg/m3.

Glass capillary arrays

A team of Russian, Israeli and German scientists have collaboratively developed an innovative technology based on glass capillary arrays for the safe infusion, storage and controlled release of hydrogen in mobile applications.[71][72] The C.En technology has achieved the United States Department of Energy (DOE) 2010 targets for on-board hydrogen storage systems.[73] DOE 2015 targets can be achieved using flexible glass capillaries and cryo-compressed method of hydrogen storage.[74]

Glass microspheres

Hollow glass microspheres (HGM) can be utilized for controlled storage and release of hydrogen.[75][76]

Stationary hydrogen storage

Unlike mobile applications, hydrogen density is not a huge problem for stationary applications. As for mobile applications, stationary applications can use established technology:

Underground hydrogen storage

'Available storage technologies, their capacity and discharge time.'[78]: 12 

Underground hydrogen storage is the practice of hydrogen storage in caverns, salt domes and depleted oil and gas fields. Large quantities of gaseous hydrogen have been stored in caverns by ICI for many years without any difficulties.[79] The storage of large quantities of liquid hydrogen underground can function as grid energy storage. The round-trip efficiency is approximately 40% (vs. 75-80% for pumped-hydro (PHES)), and the cost is slightly higher than pumped hydro, if only a limited number of hours of storage is required.[80] Another study referenced by a European staff working paper found that for large scale storage, the cheapest option is hydrogen at €140/MWh for 2,000 hours of storage using an electrolyser, salt cavern storage and combined-cycle power plant.[78]: 15  The European project Hyunder[81] indicated in 2013 that for the storage of wind and solar energy an additional 85 caverns are required as it cannot be covered by PHES and CAES systems.[82] A German case study on storage of hydrogen in salt caverns found that if the German power surplus (7% of total variable renewable generation by 2025 and 20% by 2050) would be converted to hydrogen and stored underground, these quantities would require some 15 caverns of 500,000 cubic metres each by 2025 and some 60 caverns by 2050 – corresponding to approximately one third of the number of gas caverns currently operated in Germany.[83] In the US, Sandia Labs are conducting research into the storage of hydrogen in depleted oil and gas fields, which could easily absorb large amounts of renewably produced hydrogen as there are some 2.7 million depleted wells in existence.[84]

Power to gas

Power to gas is a technology which converts electrical power to a gas fuel. There are two methods: the first is to use the electricity for water splitting and inject the resulting hydrogen into the natural gas grid; the second, less efficient method is used to convert carbon dioxide and hydrogen to methane, (see natural gas) using electrolysis and the Sabatier reaction. A third option is to combine the hydrogen via electrolysis with a source of carbon (either carbon dioxide or carbon monoxide from biogas, from industrial processes or via direct air-captured carbon dioxide) via biomethanation,[85][86] where biomethanogens (archaea) consume carbon dioxide and hydrogen and produce methane within an anaerobic environment. This process is highly efficient, as the archaea are self-replicating and only require low-grade (60°C) heat to perform the reaction.

Another process has also been achieved by SoCalGas to convert the carbon dioxide in raw biogas to methane in a single electrochemical step, representing a simpler method of converting excess renewable electricity into storable natural gas.[87]

The UK has completed surveys and is preparing to start injecting hydrogen into the gas grid as the grid previously carried 'town gas' which is a 50% hydrogen-methane gas formed from coal. Auditors KPMG found that converting the UK to hydrogen gas could be £150bn to £200bn cheaper than rewiring British homes to use electric heating powered by lower-carbon sources.[88]

Excess power or off peak power generated by wind generators or solar arrays can then be used for load balancing in the energy grid. Using the existing natural gas system for hydrogen, Fuel cell maker Hydrogenics and natural gas distributor Enbridge have teamed up to develop such a power to gas system in Canada.[89]

Pipeline storage of hydrogen where a natural gas network is used for the storage of hydrogen. Before switching to natural gas, the German gas networks were operated using towngas, which for the most part (60-65%) consisted of hydrogen. The storage capacity of the German natural gas network is more than 200,000 GW·h which is enough for several months of energy requirement. By comparison, the capacity of all German pumped storage power plants amounts to only about 40 GW·h. The transport of energy through a gas network is done with much less loss (<0.1%) than in a power network (8%). The use of the existing natural gas pipelines for hydrogen was studied by NaturalHy[90]

Automotive Onboard hydrogen storage

Targets for on-board hydrogen storage assuming storage of 5 kg of hydrogen.[91]

Targets were set by the FreedomCAR Partnership in January 2002 between the United States Council for Automotive Research (USCAR) and U.S. DOE (Targets assume a 5-kg H2 storage system). The 2005 targets were not reached in 2005.[92] The targets were revised in 2009 to reflect new data on system efficiencies obtained from fleets of test cars.[93] The ultimate goal for volumetric storage is still above the theoretical density of liquid hydrogen.[94][clarification needed][failed verification]

It is important to note that these targets are for the hydrogen storage system, not the hydrogen storage material. System densities are often around half those of the working material, thus while a material may store 6 wt% H2, a working system using that material may only achieve 3 wt% when the weight of tanks, temperature and pressure control equipment, etc., is considered.

In 2010, only two storage technologies were identified as having the potential to meet DOE targets: MOF-177 exceeds 2010 target for volumetric capacity, while cryo-compressed H2 exceeds more restrictive 2015 targets for both gravimetric and volumetric capacity (see slide 6 in [65]).

The existing options for hydrogen storage require large storage volumes which makes them impractical for stationary and portable applications. Portability is one of the biggest challenges in the automotive industry, where high density storage systems are problematic due to safety concerns.

Fuel cell powered vehicles are required to provide a driving range over 300 miles—this cannot be achieved with traditional storage methods. A long term goal set by the Fuel Cell Technology Office involves the usage of nanomaterials to improve maximum range.[95]

U.S. Department of Energy's requirements

The Department of Energy has set the targets for onboard hydrogen storage for light vehicles. The list of requirements include parameters related to gravimetric and volumetric capacity, operability, durability and cost. These targets have been set as the goal for a multiyear research plan expected to offer an alternative to fossil fuels.[96]

Fuel cells and storage

Due to its clean-burning characteristics, hydrogen is one of the most promising fuel alternatives in the automotive industry. Hydrogen based fuel could significantly reduce the emissions of greenhouse gases such as CO2, SO2 and NOx. The three limiting factor for the use of hydrogen fuel cells (HFC) include efficiency, size, and safe onboard storage of the gas. Other major disadvantages of this emerging technology involve cost, operability and durability issues, that are still to be improved from the existing systems. To address these challenges, the use of nanomaterials has been proposed as an alternative option to the traditional hydrogen storage systems. The use of nanomaterials could provide a higher density system that is expected to increase the driving range limit set by the DOE at 300 miles. Carbonaceous materials such as CNTs and metal hydrides are the main focus of researchers. Carbonaceous materials are currently being considered for onboard storage systems due to their versatility, multifunctionality, mechanical properties and low cost with respect to other alternatives.[97]

Other advantages of nanomaterials in fuel cells

The introduction of nanomaterials in onboard hydrogen storage systems can be a major turning point in the automotive industry. However, storing is not the only practical aspect of the fuel cell to which nanomaterials may contribute. Different studies have shown that the transport and catalytic properties of Nafion membranes used in HFCs can be enhanced with TiO2/SnO2 nanoparticles.[97] The increased performance is caused by an improvement in hydrogen splitting kinetics due to catalytic activity of the nanoparticles. Furthermore, this system exhibits faster transport of protons across the cell which makes HFCs with nanoparticle composite membranes a promising alternative.

Another application of nanomaterials in water splitting has been introduced by a research group at Manchester Metropolitan University in the UK using screen-printed electrodes consisting of a graphene-like material.[98] Similar systems have been developed using photoelectrochemical techniques.

See also

References

  1. ^ Energy technology analysis. International Energy Agency (2005) p. 70
  2. ^ Modeling of dispersion following hydrogen permeation for safety engineering and risk assessment (PDF). II International Conference "Hydrogen Storage Technologies" Moscow, Russia, 28–29 October 2009. Archived from the original (PDF) on 2011-07-23. Retrieved 2012-01-08.
  3. ^ Eberle, Ulrich; Mueller, Bernd; von Helmolt, Rittmar (2012). "Fuel cell electric vehicles and hydrogen infrastructure: status 2012". Energy & Environmental Science. 5 (10): 8780. doi:10.1039/C2EE22596D. Retrieved 2014-12-19.
  4. ^ "FCX Clarity". Honda Worldwide. Retrieved 2012-01-08.
  5. ^ "X-TRAIL FCV '03 model". Nissan-global.com. Archived from the original on 2010-09-17. Retrieved 2012-01-08.
  6. ^ Savvides, Nick (2017-01-11). "Japan plans to use imported liquefied hydrogen to fuel Tokyo 2020 Olympics". Fairplay. IHS Markit Maritime Portal. Retrieved 22 April 2018.
  7. ^ Sadaghiani, Mirhadi S. (2 March 2017). "Introducing and energy analysis of a novel cryogenic hydrogen liquefaction process configuration". International Journal of Hydrogen Energy. 42 (9): 6033–6050. doi:10.1016/j.ijhydene.2017.01.136.
  8. ^ Sunita, Satyapal (2007). "The U.S. Department of Energy's National Hydrogen Storage Project: Progress towards meeting hydrogen-powered vehicle requirements". Catalysis Today. 120 (3–4): 246–256. doi:10.1016/j.cattod.2006.09.022.
  9. ^ Eftekhari, Ali; Baizeng, Fang (2017). "Electrochemical hydrogen storage: Opportunities for fuel storage, batteries, fuel cells, and supercapacitors". International Journal of Hydrogen Energy. 42 (40): 25143–25165. doi:10.1016/j.ijhydene.2017.08.103.
  10. ^ DOE Metal hydrides. eere.energy.gov (2008-12-19). Retrieved on 2012-01-08.
  11. ^ Christian, Meganne; Aguey-Zinsou, Kondo François (2012). "Core–Shell Strategy Leading to High Reversible Hydrogen Storage Capacity for NaBH4". ACS Nano. 6 (9): 7739–7751. doi:10.1021/nn3030018. PMID 22873406.
  12. ^ EU Hydrogen Storage. (PDF) . Retrieved on 2012-01-08.
  13. ^ Graetz, J.; Reilly, J.; Sandrock, G.; Johnson, J.; Zhou, W. M.; Wegrzyn, J. (2006). "Aluminum Hydride, A1H3, As a Hydrogen Storage Compound". doi:10.2172/899889. {{cite journal}}: Cite journal requires |journal= (help)
  14. ^ CNRS Institut Neel H2 Storage. Neel.cnrs.fr. Retrieved on 2012-01-08.
  15. ^ "New type of hydrogen fuel cell powers up". newscientist. Retrieved 2006-09-16.
  16. ^ Ki Chul Kim; Anant D. Kulkarni; J. Karl Johnson; David S. Sholl (2011). "Examining the robustness of first-principles calculations for metal hydride reaction thermodynamics by detection of metastable reaction pathways". Phys. Chem. Chem. Phys. 13 (48): 21520–9. Bibcode:2011PCCP...1321520K. doi:10.1039/C1CP22489A. PMID 22068383.
  17. ^ Ki Chul Kim; Anant D. Kulkarni; J. Karl Johnson; David S. Sholl (2011). "Large-scale screening of promising metal hydrides for hydrogen storage system from first-principles calculations based on equilibrium reaction thermodynamics". Phys. Chem. Chem. Phys. 13 (15): 7218–29. Bibcode:2011PCCP...13.7218K. doi:10.1039/c0cp02950e. PMID 21409194.
  18. ^ Anant D. Kulkarni; Lin-Lin Wang; Duane D. Johnson; David S. Sholl; J. Karl Johnson (2010). "First-Principles Characterization of Amorphous Phases of MB12H12, M = Mg, Ca". J. Phys. Chem. C. 114 (34): 14601–14605. doi:10.1021/jp101326g.
  19. ^ a b Kan, H.M.; Sun, M.; Zhang, N. (2014). "Nanomaterials for Hydrogen Storage". Applied Mechanics and Materials. 587: 216–219.
  20. ^ a b c Niemann, Michael U.; Srinivasan, Sesha S.; Phani, Ayala R.; Kumar, Ashok; Goswami, D. Yogi; Stefanakos, Elias K. (2008). "Nanomaterials for hydrogen storage applications: a review". Journal of Nanomaterials. 2008: 1–9. doi:10.1155/2008/950967.{{cite journal}}: CS1 maint: unflagged free DOI (link)
  21. ^ Sunandana, C.S. (2007). "Nanomaterials for hydrogen storage". Resonance. 12 (5): 31–36. doi:10.1007/s12045-007-0047-9.
  22. ^ "Liquid asset". The Engineer. 2008-01-15. Retrieved 2015-01-09.[permanent dead link]
  23. ^ Zong, J., J. T. Mague, and R. A. Pascal, Jr., Exceptional Steric Congestion in an in,in-Bis(hydrosilane), J. Am. Chem. Soc. 2013, 135, 13235-13237.
  24. ^ Echeverría, Jorge, Gabriel Aullón, and Santiago Alvarez. "Intermolecular interactions in group 14 hydrides: Beyond C H··· H C contacts." International Journal of Quantum Chemistry 117.21 (2017): e25432.
  25. ^ Zhang, Y.-H. Percival; Evans, Barbara R.; Mielenz, Jonathan R.; Hopkins, Robert C.; Adams, Michael W.W. (2007). Melis, Anastasios (ed.). "High-Yield Hydrogen Production from Starch and Water by a Synthetic Enzymatic Pathway". PLoS ONE. 2 (5): e456. Bibcode:2007PLoSO...2..456Z. doi:10.1371/journal.pone.0000456. PMC 1866174. PMID 17520015.{{cite journal}}: CS1 maint: unflagged free DOI (link)
  26. ^ Ye, Xinhao; Wang, Yiran; Hopkins, Robert C.; Adams, Michael W. W.; Evans, Barbara R.; Mielenz, Jonathan R.; Zhang, Y.-H. Percival (2009). "Spontaneous High-Yield Production of Hydrogen from Cellulosic Materials and Water Catalyzed by Enzyme Cocktails". ChemSusChem. 2 (2): 149–52. doi:10.1002/cssc.200900017. PMID 19185036.
  27. ^ Zhang, Y.-H. Percival (2009). "A sweet out-of-the-box solution to the hydrogen economy: is the sugar-powered car science fiction?". Energy & Environmental Science. 2 (3): 272. doi:10.1039/b818694d.
  28. ^ White Paper: A Novel Method For Grid Energy Storage Using Aluminum Fuel Archived 2013-05-31 at the Wayback Machine, Alchemy Research, April 2012.
  29. ^ "Army discovery may offer new energy source | U.S. Army Research Laboratory". www.arl.army.mil.
  30. ^ "New process generates hydrogen from aluminum alloy to run engines, fuel cells". phys.org.
  31. ^ a b c d e He, Teng; Pei, Qijun; Chen, Ping (2015-09-01). "Liquid organic hydrogen carriers". Journal of Energy Chemistry. 24 (5): 587–594. doi:10.1016/j.jechem.2015.08.007.
  32. ^ Teichmann, Daniel; Arlt, Wolfgang; Wasserscheid, Peter; Freymann, Raymond (2011). "A future energy supply based on Liquid Organic Hydrogen Carriers (LOHC)". Energy & Environmental Science. 4 (8): 2767–2773. doi:10.1039/C1EE01454D.
  33. ^ US patent 7351395, "Hydrogen storage by reversible hydrogenation of pi-conjugated substrates" 
  34. ^ Brückner, Nicole (2013). "Evaluation of Industrially Applied Heat-Transfer Fluids as Liquid Organic Hydrogen Carrier Systems". ChemSusChem. 7 (1): 229–235. doi:10.1002/cssc.201300426. PMID 23956191.
  35. ^ Grasemann, Martin; Laurenczy, Gábor (2012-07-18). "Formic acid as a hydrogen source – recent developments and future trends". Energy & Environmental Science. 5 (8): 8171–8181. doi:10.1039/C2EE21928J.
  36. ^ Müller, Benjamin (2011). "Energiespeicherung mittels Methan und energietragenden Stoffen - ein thermodynamischer Vergleich" [Energy Storage by CO2 Methanization and Energy Carrying Compounds: A Thermodynamic Comparison]. Chemie Ingenieur Technik (in German). 83 (11): 2002–2013. doi:10.1002/cite.201100113.
  37. ^ Wang, Bo; Goodman, D. Wayne; Froment, Gilbert F. (2008-01-25). "Kinetic modeling of pure hydrogen production from decalin". Journal of Catalysis. 253 (2): 229–238. doi:10.1016/j.jcat.2007.11.012.
  38. ^ Kariya, Nobuko; Fukuoka, Atsushi; Ichikawa, Masaru (2002-07-10). "Efficient evolution of hydrogen from liquid cycloalkanes over Pt-containing catalysts supported on active carbons under "wet–dry multiphase conditions"". Applied Catalysis A: General. 233 (1–2): 91–102. doi:10.1016/S0926-860X(02)00139-4.
  39. ^ Yolcular, Sevim; Olgun, Özden (2008-11-01). "Ni/Al2O3 catalysts and their activity in dehydrogenation of methylcyclohexane for hydrogen production". Catalysis Today. Selected papers from the EUROPACAT VIII Hydrogen Society Session, Turku, Finland, 26–31 August 2007. 138 (3–4): 198–202. doi:10.1016/j.cattod.2008.07.020.
  40. ^ Clot, Eric; Eisenstein, Odile; Crabtree, Robert H. (2007-05-30). "Computational structure–activity relationships in H2 storage: how placement of N atoms affects release temperatures in organic liquid storage materials". Chemical Communications. 0 (22): 2231–2233. doi:10.1039/B705037B. PMID 17534500.
  41. ^ Eblagon, Katarzyna Morawa; Tam, Kin; Tsang, Shik Chi Edman (2012). "Comparison of catalytic performance of supported ruthenium and rhodium for hydrogenation of 9-ethylcarbazole for hydrogen storage applications". Energy & Environmental Science. 5 (9): 8621. doi:10.1039/C2EE22066K.
  42. ^ G. Laurenczy, C. Fellay, P. J. Dyson, Hydrogen production from formic acid. PCT Int. Appl. (2008), CODEN: PIXXD2 WO 2008047312 A1 20080424 AN 2008:502691
  43. ^ Fellay, C; Dyson, PJ; Laurenczy, G (2008). "A Viable Hydrogen-Storage System Based On Selective Formic Acid Decomposition with a Ruthenium Catalyst". Angewandte Chemie International Edition in English. 47 (21): 3966–8. doi:10.1002/anie.200800320. PMID 18393267.
  44. ^ F. Joó (2008). "Breakthroughs in Hydrogen Storage – Formic Acid as a Sustainable Storage Material for Hydrogen". ChemSusChem. 1 (10): 805–8. doi:10.1002/cssc.200800133. PMID 18781551.
  45. ^ P. G. Jessop, in Handbook of Homogeneous Hydrogenation (Eds.: J. G. de Vries, C. J. Elsevier), Wiley-VCH, Weinheim, Germany, 2007, pp. 489–511.
  46. ^ P. G. Jessop; F. Joó; C.-C. Tai (2004). "Recent advances in the homogeneous hydrogenation of carbon dioxide". Coordination Chemistry Reviews. 248 (21–24): 2425. doi:10.1016/j.ccr.2004.05.019.
  47. ^ AVERY, W (1988). "A role for ammonia in the hydrogen economy". International Journal of Hydrogen Energy. 13 (12): 761–773. doi:10.1016/0360-3199(88)90037-7. ISSN 0360-3199.
  48. ^ The ammonia economy Archived 2008-05-13 at the Wayback Machine. Memagazine.org (2003-07-10). Retrieved on 2012-01-08.
  49. ^ Mealey, Rachel. ”Automotive hydrogen membranes-huge breakthrough for cars", ABC, August 8, 2018
  50. ^ Focus Denmark. Netpublikationer.dk (2006-06-13). Retrieved on 2012-01-08.
  51. ^ Stracke, Marcelo P.; Ebeling, Günter; Cataluña, Renato; Dupont, Jairton (2007). "Hydrogen-Storage Materials Based on Imidazolium Ionic Liquids". Energy & Fuels. 21 (3): 1695–1698. doi:10.1021/ef060481t.
  52. ^ Welch, G. C.; Juan, R. R. S.; Masuda, J. D.; Stephan, D. W. (2006). "Reversible, Metal-Free Hydrogen Activation". Science. 314 (5802): 1124–6. Bibcode:2006Sci...314.1124W. doi:10.1126/science.1134230. PMID 17110572.
  53. ^ Elizabeth Wilson H2 Activation, Reversibly Metal-free compound readily breaks and makes hydrogen, Chemical & Engineering News November 20, 2006
  54. ^ Mes stands for a mesityl substituent and C6F5 for a pentafluorophenyl group, see also tris(pentafluorophenyl)boron
  55. ^ Graphene as suitable hydrogen storage substance. Physicsworld.com. Retrieved on 2012-01-08.
  56. ^ Graphene to graphane. Rsc.org. January 2009. Retrieved on 2012-01-08.
  57. ^ MOF-74 – A Potential Hydrogen-Storage Compound. Nist.gov. Retrieved on 2012-01-08.
  58. ^ Researchers Demonstrate 7.5 wt% Hydrogen Storage in MOFs. Green Car Congress (2006-03-06). Retrieved on 2012-01-08.
  59. ^ New MOF Material With hydrogen Uptake Of Up To 10 wt%. 22 February 2009
  60. ^ "Cella Energy - Website suspended". www.cellaenergy.com.
  61. ^ Compendium of Hydrogen Energy.Volume 2:hydrogen Storage, Transportation and Infrastructure. A volume in Woodhead Publishing Series in Energy 2016,Chapter 8 – Other methods for the physical storage of hydrogen doi:10.1016/B978-1-78242-362-1.00008-0
  62. ^ Sevilla, Marta; Mokaya, Robert (2014-03-21). "Energy storage applications of activated carbons: supercapacitors and hydrogen storage". Energy Environ. Sci. 7 (4): 1250–1280. doi:10.1039/c3ee43525c. hdl:10261/140713. ISSN 1754-5706.
  63. ^ Blankenship II, Troy Scott; Balahmar, Norah; Mokaya, Robert (2017-11-16). "Oxygen-rich microporous carbons with exceptional hydrogen storage capacity". Nature Communications. 8 (1): 1545. Bibcode:2017NatCo...8.1545B. doi:10.1038/s41467-017-01633-x. ISSN 2041-1723. PMC 5691040. PMID 29146978.
  64. ^ Blankenship, Troy Scott; Mokaya, Robert (2017-12-06). "Cigarette butt-derived carbons have ultra-high surface area and unprecedented hydrogen storage capacity" (PDF). Energy & Environmental Science. 10 (12): 2552–2562. doi:10.1039/c7ee02616a. ISSN 1754-5706.
  65. ^ a b R. K. Ahluwalia, T. Q. Hua, J. K. Peng and R. Kumar System Level Analysis of Hydrogen Storage Options. 2010 DOE Hydrogen Program Review, Washington, DC, June 8–11, 2010
  66. ^ Stephen Lasher Analyses of Hydrogen Storage Materials and On-Board Systems. DOE Annual Merit Review June 7–11, 2010
  67. ^ S&TR | Setting a World Driving Record with Hydrogen. Llnl.gov (2007-06-12). Retrieved on 2012-01-08.
  68. ^ Compact (L)H2 Storage with Extended Dormancy in Cryogenic Pressure Vessels. Lawrence Livermore National Laboratory June 8, 2010
  69. ^ Technical Sessions. FISITA 2010. Retrieved on 2012-01-08.
  70. ^ Florusse, L. J.; Peters, CJ; Schoonman, J; Hester, KC; Koh, CA; Dec, SF; Marsh, KN; Sloan, ED (2004). "Stable Low-Pressure Hydrogen Clusters Stored in a Binary Clathrate Hydrate". Science. 306 (5695): 469–71. Bibcode:2004Sci...306..469F. doi:10.1126/science.1102076. PMID 15486295.
  71. ^ Zhevago, N.K.; Glebov, V.I. (2007). "Hydrogen storage in capillary arrays". Energy Conversion and Management. 48 (5): 1554–1559. doi:10.1016/j.enconman.2006.11.017.
  72. ^ Zhevago, N.K.; Denisov, E.I.; Glebov, V.I. (2010). "Experimental investigation of hydrogen storage in capillary arrays". International Journal of Hydrogen Energy. 35: 169–175. doi:10.1016/j.ijhydene.2009.10.011.
  73. ^ Dan Eliezer et al. A New Technology for Hydrogen Storage in Capillary Arrays. C.En & BAM
  74. ^ Zhevago, N. K.; Chabak, A. F.; Denisov, E. I.; Glebov, V. I.; Korobtsev, S. V. (2013). "Storage of cryo-compressed hydrogen in flexible glass capillaries". International Journal of Hydrogen Energy. 38 (16): 6694–6703. doi:10.1016/j.ijhydene.2013.03.107.
  75. ^ Glass microsphere diffusion Archived 2008-06-24 at the Wayback Machine. Ceer.alfred.edu (2001-05-15). Retrieved on 2012-01-08.
  76. ^ G.G. Wicks; L.K. Heung; R.F. Schumacher. "SRNL's porous, hollow glass balls open new opportunities for hydrogen storage, drug delivery and national defense" (PDF). American Ceramic Society Bulletin. 87 (6): 23. Archived from the original (PDF) on November 15, 2008.
  77. ^ "R&D of large stationary hydrogen/CNG/HCNG storage vessels" (PDF).
  78. ^ a b "COMMISSION STAFF WORKING DOCUMENT: Energy storage – the role of electricity" (PDF). European Commission. 1 Feb 2017. Retrieved 22 April 2018.
  79. ^ 1994 – ECN abstract. Hyweb.de. Retrieved on 2012-01-08.
  80. ^ "European Renewable Energy Network Study" (PDF). Brussels: European Union. January 2012. pp. 86, 188.
  81. ^ "Why storing large scale intermittent renewable energies with hydrogen?". Hyunder. Retrieved 2018-11-25.
  82. ^ "Storing renewable energy: Is hydrogen a viable solution?" (PDF).
  83. ^ "Bringing North Sea Energy Ashore Efficiently" (PDF). World Energy Council Netherlands. Retrieved 22 April 2018.
  84. ^ Gerdes, Justin (2018-04-10). "Enlisting Abandoned Oil and Gas Wells as 'Electron Reserves'". Greentech Media. Retrieved 22 April 2018.
  85. ^ Rathi, Akshat. "Batteries can't solve the world's biggest energy-storage problem. One startup has a solution". qz.com. Quartz. Retrieved 22 April 2018.
  86. ^ "Munich-based clean-tech startup Electrochaea and Hungarian utility MVM establish power-to-gas joint venture". MVM Group. 24 October 2016. Retrieved 22 April 2018.
  87. ^ "SoCalGas and Opus 12 Successfully Demonstrate Technology That Simplifies Conversion of Carbon Dioxide into Storable Renewable Energy". prnewswire.com. prnewswire. Retrieved 22 April 2018.
  88. ^ Ambrose, Jillian (2018-01-06). "Energy networks prepare to blend hydrogen into the gas grid for the first time". The Telegraph. Retrieved 22 April 2018.
  89. ^ Anscombe, Nadya (4 June 2012). "Energy storage: Could hydrogen be the answer?". Solar Novus Today. Retrieved 3 November 2012.
  90. ^ Naturalhy Archived 2012-01-18 at the Wayback Machine
  91. ^ "DOE National Center for Carbon-Based Hydrogen Storage". National Renewable Energy Laboratory (NREL). Archived from the original on 2007-01-27. Retrieved October 1, 2006.. See also "Targets for On-Board Hydrogen Storage Systems" (PDF). Office of Energy Efficiency & Renewable Energy. Archived from the original (PDF) on 2007-04-18. Retrieved April 1, 2007.
  92. ^ Hydrogen Storage Technologies Roadmap. uscar.org. November 2005
  93. ^ Yang, Jun; Sudik, A; Wolverton, C; Siegel, DJ (2010). "High capacity hydrogen storage materials: attributes for automotive applications and techniques for materials discovery". Chemical Society Reviews. 39 (2): 656–675. CiteSeerX 10.1.1.454.1947. doi:10.1039/b802882f. PMID 20111786.
  94. ^ FCT Hydrogen Storage: Current Technology. Office of Energy Efficiency & Renewable Energy|access
  95. ^ "Hydrogen Storage". U.S. Department of Energy.
  96. ^ "DOE Technical Targets for Onboard Hydrogen Storage for Light-Duty Vehicles". U.S. Department of Energy.
  97. ^ a b Hussein, A.K. (2015). "Applications of nanotechnology in renewable energies—A comprehensive overview and understanding". Renewable and Sustainable Energy Reviews. 42: 460–476. doi:10.1016/j.rser.2014.10.027.
  98. ^ Evans, Scarlett (August 20, 2018). "Researchers to create hydrogen energy source using nanotechnology". United Kingdom.

External links

Wikimedia Commons has media related to Hydrogen storage.
Retrieved from "https://en.wikipedia.org/w/index.php?title=Hydrogen_storage&oldid=929490202"