Patent Grant
12286349
The present disclosure is directed toward green energy production methods, and more particularly, relates to a method of synthesizing a nanocomposite material for green energy generation and storage.
The “background” description provided herein is for the purpose of generally presenting the context of the disclosure. Work of the presently named inventors, to the extent it is described in this background section, as well as aspects of the description which may not otherwise qualify as prior art at the time of filing, are neither expressly nor impliedly admitted as prior art against the present disclosure.
The rapid industrialization and population growth in recent decades have increased global energy demand, highlighting the need for alternative energy sources. The depletion of non-renewable resources, coupled with rising environmental concerns such as climate change and pollution, emphasizes the urgency of transitioning to clean, renewable energy solutions. One such renewable energy source is solar energy, which is inexpensive to generate, however, solar energy generation faces challenges in storage due to the reliance on costly and difficult-to-dispose battery-based storage systems. In contrast, hydrogen may be considered a desirable alternative, offering the potential to reduce dependency on fossil fuels and lower environmental impacts, particularly when used in fuel cells that emit water vapor only. Hydrogen energy offers several advantages such as cleaner energy generation process, ease of storage due to compressible nature of hydrogen and complete elimination of battery needs. Further, hydrogen energy offers several advantages over traditional battery systems as it has a higher energy density, allowing it to store more energy in a smaller volume, which may be beneficial for applications like transportation where space and weight should be optimized. Hydrogen-powered vehicles may be refueled in a shorter time period, similar to gasoline vehicles, whereas electric vehicles require much longer charging times. Hydrogen fuel cells also provide longer operational ranges compared to battery electric vehicles, making them suitable for heavy-duty and long-distance applications. Despite these benefits, large-scale hydrogen production faces challenges such as use of energy-intensive methods and complexities in storage and transportation of hydrogen, which must be addressed for hydrogen to become a viable mainstream energy solution.
Nanocomposites, particularly metal oxide-based materials, are highly suitable for hydrogen production due to their desirable catalytic properties, including high surface area, tunable porosity, and improved electron conductivity. The aforementioned properties enable efficient hydrogen generation, making hydrogen production a promising solution for large-scale energy storage from renewable sources like solar and wind power. However, the synthesis of nanocomposites for hydrogen generation involves high temperatures and long processing times, often leading to irregular particle sizes and inconsistent porosity, which may negatively affect the performance of the process. Many current synthesis techniques contribute to high operational costs and material inefficiency, with extensive milling and post-treatment steps required for non-uniform particle size distribution. Hence, in order to achieve an efficient nanocomposite material, issues related to production costs, infrastructure, and energy conversion efficiency must be addressed.
Accordingly, one object of the present disclosure is to provide an efficient method for hydrogen generation using a nanocomposite catalyst that may circumvent the drawbacks and limitations such as high cost, high lead times, low efficiency, and poor environmental performance of methods and materials known in the art.
In an exemplary embodiment, a method for synthesizing a MoO3@Al2O3—MgO nanocomposite material is described. The method includes adding distilled water and nitric acid (HNO3) to a mixture of (NH4)2MoO4, Al(NO3)3·9H2O, Mg(Ac)2·4H2O, and sucrose to form a reaction mixture and heating the reaction mixture to a reaction temperature ranging from 150° C. to 220° C. until a carbonized product is formed. The method further includes grinding the carbonized product to form a ground carbonized product and calcining the ground carbonized product at a temperature in a range of 700° C. to 800° C. for a period of 2 to 4 hours to form the MoO3@Al2O3—MgO nanocomposite material. The MoO3 content of the MoO3@Al2O3—MgO nanocomposite material ranges from 1 percent by weight (wt. %) to 20 wt. % of the total weight of the MoO3@Al2O3—MgO nanocomposite material and the MoO3@Al2O3—MgO nanocomposite material has a hydrogen generation rate of greater than or equal to 400 milliliter per minute per gram (mL·min−1·g−1) when used to generate hydrogen from NaBH4.
In some embodiments, the MoO3 content of the MoO3@Al2O3—MgO nanocomposite material is in a range from 5 wt. % to 15 wt. % of the total weight of the MoO3@Al2O3—MgO nanocomposite material.
In some embodiments, the MoO3 content of the MoO3@Al2O3—MgO nanocomposite material is in a range from 8 wt. % to 12 wt. % of the total weight of the MoO3@Al2O3—MgO nanocomposite material.
In some embodiments, the MoO3 content of the MoO3@Al2O3—MgO nanocomposite material is 10 wt. % of the total weight of the MoO3@Al2O3—MgO nanocomposite material.
In some embodiments, the MoO3@Al2O3—MgO nanocomposite material has a hydrogen generation rate of greater than or equal to 500 mL·min−1·g−1 when used to generate hydrogen from NaBH4 at a temperature of 30° C.
In some embodiments, the MoO3@Al2O3—MgO nanocomposite material has a hydrogen generation rate of greater than or equal to 550 mL·min−1·g−1 when used to generate hydrogen from NaBH4 at a temperature of 30° C.
In some embodiments, the MoO3@Al2O3—MgO nanocomposite material has a hydrogen generation rate of greater than or equal to 600 mL·min−1·g−1 when used to generate hydrogen from NaBH4 at a temperature of 35° C.
In some embodiments, the MoO3@Al2O3—MgO nanocomposite material has a hydrogen generation rate of greater than or equal to 800 mL·min−1·g−1 when used to generate hydrogen from NaBH4 at a temperature of 40° C.
In some embodiments, the MoO3@Al2O3—MgO nanocomposite material has a hydrogen generation rate of greater than or equal to 1000 mL·min−1·g−1 when used to generate hydrogen from NaBH4 at a temperature of 45° C.
In some embodiments, the MoO3@Al2O3—MgO nanocomposite material has a hydrogen generation rate of greater than or equal to 1200 mL·min−1·g−1 when used to generate hydrogen from NaBH4 at a temperature of 45° C.
In another exemplary embodiment, a method of hydrogen generation from NaBH4 is described. The method includes hydrolyzing NaBH4 in the presence of a MoO3@Al2O3—MgO nanocomposite. The NaBH4 is hydrolyzed to evolve H2 gas and the MoO3@Al2O3—MgO nanocomposite material catalyzes the hydrolysis. The method further includes collecting the H2 gas. The MoO3 content of the MoO3@Al2O3—MgO nanocomposite material ranges from 1 wt. % to 20 wt. % of the total weight of the MoO3@Al2O3—MgO nanocomposite material. The hydrogen generation rate is greater than or equal to 400 mL·min−1·g−1.
In some embodiments, the MoO3 content of the MoO3@Al2O3—MgO nanocomposite material is in a range from 5 wt. % to 15 wt. % of the total weight of the MoO3@Al2O3—MgO nanocomposite material.
In some embodiments, the MoO3 content of the MoO3@Al2O3—MgO nanocomposite material is in a range from 8 wt. % to 12 wt. % of the total weight of the MoO3@Al2O3—MgO nanocomposite material.
In some embodiments, the MoO3 content of the MoO3@Al2O3—MgO nanocomposite material is 10 wt. % of the total weight of the MoO3@Al2O3—MgO nanocomposite material.
In some embodiments, the hydrogen generation rate is greater than or equal to 500 mL·min−1·g−1 at a reaction temperature of 30° C.
In some embodiments, the hydrogen generation rate is greater than or equal to 550 mL·min−1·g−1 at a reaction temperature of 30° C.
In some embodiments, the hydrogen generation rate is greater than or equal to 600 mL·min−1·g−1 at a reaction temperature of 35° C.
In some embodiments, the hydrogen generation rate is greater than or equal to 800 mL·min−1·g−1 at a reaction temperature of 40° C.
In some embodiments, the hydrogen generation rate is greater than or equal to 1000 mL·min−1·g−1 at a reaction temperature of 45° C.
In some embodiments, the hydrogen generation rate is greater than or equal to 1200 mL·min−1·g−1 at a reaction temperature of 45° C.
The foregoing general description of the illustrative embodiments and the following detailed description thereof are merely exemplary aspects of the teachings of this disclosure, and are not restrictive.
A more complete appreciation of this disclosure and many of the attendant advantages thereof will be readily obtained as the same becomes better understood by reference to the following detailed description when considered in connection with the accompanying drawings, wherein:
In the following description, it is understood that other embodiments may be utilized, and structural and operational changes may be made without departure from the scope of the present embodiments disclosed herein.
Reference will now be made in detail to specific embodiments or features, examples of which are illustrated in the accompanying drawings. Wherever possible, corresponding or similar reference numbers will be used throughout the drawings to refer to the same or corresponding parts. Moreover, references to various elements described herein, are made collectively or individually when there may be more than one element of the same type. However, such references are merely exemplary in nature. It may be noted that any reference to elements in the singular may also be construed to relate to the plural and vice-versa without limiting the scope of the disclosure to the exact number or type of such elements unless set forth explicitly in the appended claims.
Furthermore, the terms “approximately,” “approximate,” “about,” and similar terms generally refer to ranges that include the identified value within a margin of 20%, 10%, or preferably 5%, and any values therebetween.
Aspects of the present disclosure are directed toward a catalyst system designed to enhance the hydrolysis of sodium borohydride (NaBH4) for efficient hydrogen generation. It utilizes a solid catalyst composed of low-cost materials, which is easy to prepare and offers a high hydrogen generation rate (HGR) in a short time. This catalyst system facilitates the safe and rapid release of hydrogen from NaBH4, making it an efficient solution for clean hydrogen production. The present disclosure circumvents the drawbacks of prior art by addressing limitations such as high catalyst costs, slow reaction rates, and environmental concerns. Traditional catalysts often require expensive materials and result in inefficient or slow hydrogen production. In contrast, the present disclosure uses a cost-effective catalyst that promotes faster hydrogen generation without relying on toxic or scarce materials. The simplicity of its preparation and its high catalytic activity also enable scalability and practical applicability, making it a more efficient and sustainable alternative to existing methods.
At step 52, the method 50 includes adding distilled water and ammonium molybdate to a powder mixture of Al(NO3)3·9H2O, Mg(Ac)2·4H2O, and sucrose to form a reaction mixture. The Al(NO3)3·9H2O provides the Al3+ ions needed to form Al2O3; the Mg(Ac)2·4H2O supplies the Mg2+ ions, (NH4)2MoO4 provides the molybdenum oxide precursor. The sucrose acts as a carbon source to potentially aid in creating a porous structure. The sucrose acts as a carbon source to potentially aid in creating a porous structure. In some embodiments, glucose, citric acid, glycerol, tannic acid, polyvinyl alcohol (PVA), humic acid may also be used in place of sucrose to serve as the carbon source.
In some embodiments, the sucrose is present in the reaction mixture in a range from 0.1 to 1 M, more preferably 0.45 to 0.65 M, and yet more preferably about 0.584 M. In some embodiments, the concentration of (NH4)2MoO4 in the reaction mixture in a range from 0.1 to 1.0 M, preferably about 0.2 to 0.5 M. In some embodiments, the concentration of Al(NO3)3·9H2O present in the reaction mixture is in a range from 0.5 to 1.5 M, more preferably 0.9 to 0.95 M, and yet more preferably 0.930 M. In some embodiments, the concentration of Mg(Ac)2·4H2O in the reaction mixture is in the range from 2.0 to 2.7 M, more preferably 2.2 to 2.5 M, and yet more preferably 2.36 M.
At step 54, the method 50 includes heating the reaction mixture to a reaction temperature in a range of 150 to 220° C. to form a carbonized product. In some embodiments, heating of the reaction mixture can be performed by using heating appliances such as ovens, microwaves, autoclaves, hot plates, heating mantles and tapes, oil baths, salt baths, sand baths, air baths, hot-tube furnaces, and hot-air guns. The heating is varied out till all the water is evaporated, and causes degradation of the carbon source, preferably sucrose.
At step 56, the method 50 includes grinding the carbonized product to form a ground carbonized product. The grinding may be carried out using any suitable means, for example, ball milling, blending, etc., using manual method (e.g., mortar) or machine-assisted methods such as using a mechanical blender, or any other apparatus known to those of ordinary skill in the art. In a preferred embodiment, the carbonized product is ground in a motor to obtain the ground carbonized product.
At step 58, the method 50 includes calcining the ground carbonized product at a temperature in a range from 700 to 800° C., more preferably 720 to 780° C., more preferably 750° C. for a period of 2 to 4 hours, 2.5 to 3.5 hours, and yet more preferably 3 hours to form the MoO3@Al2O3—MgO nanocomposite material. The calcination is carried out by heating it to a high temperature under a restricted supply of ambient oxygen. This is performed to remove impurities or volatile substances and to incur thermal decomposition. Typically, the calcination is carried out in a furnace, preferably equipped with a temperature control system, which may provide a heating rate of up to 50° C./min, preferably up to 40° C./min, preferably up to 30° C./min, preferably up to 20° C./min, preferably up to 10° C./min, preferably up to 5° C./min. During calcination, any carbon source material left further decomposes, leaving behind a porous structure, and the metal salts convert to oxides, forming the MoO3@Al2O3—MgO nanocomposite material.
In some embodiments, the MoO3 content of the MoO3@Al2O3—MgO nanocomposite material is in a range from 1 to 20 wt. %, preferably 5 to 15 wt. %, preferably 8 to 12 wt. %, and yet more preferably 10 wt. % of the total weight of the MoO3@Al2O3—MgO nanocomposite material.
In some embodiments, the MoO3@Al2O3—MgO nanocomposite material has a hydrogen generation rate of greater than or equal to 400 milliliters per minute per gram (mL·min−1·g−1) when used to generate hydrogen from NaBH4 as described below. In some embodiments, the MoO3@Al2O3—MgO nanocomposite material has a hydrogen generation rate of greater than or equal to 500 mL min−1·g−1, preferably 510 mL·min−1·g−1, preferably 520 mL·min−1·g−1, preferably 530 mL·min−1·g−1, preferably 540 mL·min−1·g−1, preferably 550 mL·min−1·g−1, preferably 560 mL·min−1·g−1, preferably 570 mL·min−1·g−1, and yet more preferably 580 mL·min−1·g−1 when used to generate hydrogen from NaBH4 at a temperature of 30° C. In some embodiments, the MoO3@Al2O3—MgO nanocomposite material has a hydrogen generation rate of greater than or equal to 550 mL·min−1·g−1 when used to generate hydrogen from NaBH4 at a temperature of 30° C.
In some embodiments, the MoO3@Al2O3—MgO nanocomposite material has a hydrogen generation rate of greater than or equal to 600 mL·min−1·g−1, preferably 610 mL·min−1·g−1, preferably 620 mL·min−1·g−1, and yet more preferably 630 mL·min−1·g−1 when used to generate hydrogen from NaBH4 at a temperature of 35° C. as described below.
In some embodiments, the MoO3@Al2O3—MgO nanocomposite material has a hydrogen generation rate of greater than or equal to 800 mL·min−1·g−1, preferably 810 mL·min−1·g−1, preferably 820 mL·min−1·g−1, preferably 830 mL·min−1·g−1, preferably 840 mL·min−1·g−1, preferably 850 mL·min−1·g−1, preferably 860 mL·min−1·g−1, preferably 870 mL·min−1·g−1, and preferably 880 mL·min−1·g−1, preferably 890 mL·min−1·g−1, preferably 900 mL·min−1·g−1, preferably 910 mL·min−1·g−1, preferably 920 mL·min−1·g−1, preferably 930 mL·min−1·g−1, and yet more preferably 940 mL·min−1·g−1, when used to generate hydrogen from NaBH4 at a temperature of 40° C. as described below.
In some embodiments, the MoO3@Al2O3—MgO nanocomposite material has a hydrogen generation rate of greater than or equal to 1000 mL·min−1·g−1 when used to generate hydrogen from NaBH4 at a temperature of 45° C. as described below. In some embodiments, the MoO3@Al2O3—MgO nanocomposite material has a hydrogen generation rate of greater than or equal to 1200 mL·min−1·g−1, preferably 1210 mL·min−1·g−1, preferably 1220 mL·min−1·g−1, preferably 1230 mL·min−1·g−1, preferably 1240 mL·min−1·g−1, preferably 1250 mL·min−1·g−1, preferably 1260 mL·min−1·g−1, preferably 1270 mL·min−1·g−1, and preferably 1280 mL·min−1·g−1, preferably 1290 mL·min−1·g−1, preferably 1300 mL·min−1·g−1, preferably 1310 mL·min−1·g−1, preferably 1320 mL·min−1·g−1, preferably 1330 mL·min−1·g−1, preferably 1340 mL·min−1·g−1, preferably 1350 mL·min−1·g−1, preferably 1360 mL·min−1·g−1, preferably 1370 mL·min−1·g−1, preferably 1380 mL·min−1·g−1, preferably 1390 mL·min−1·g−1, and yet more preferably 1400 mL·min−1·g−1 when used to generate hydrogen from NaBH4 at a temperature of 45° C.
NaBH4+4H2O→NaBO2+4H2
This reaction provides a way to generate hydrogen efficiently, with sodium borohydride being a high-density hydrogen carrier. The hydrogen gas produced can be used in fuel cells or other applications that require clean, on-demand hydrogen generation. The process is particularly attractive due to NaBH4's high hydrogen content and the fact that the byproducts (such as sodium metaborate) are relatively benign compared to those from fossil fuel-based methods. The order in which the method 70 is described is not intended to be construed as a limitation, and any number of the described method steps can be combined in any order to implement the method 70. Additionally, individual steps may be removed or skipped from the method 70 without departing from the spirit and scope of the present disclosure.
At step 72, the method 70 includes hydrolyzing NaBH4 in the presence of a MoO3@Al2O3—MgO nanocomposite. The NaBH4 is hydrolyzed to evolve H2 gas in the presence of the 003@Al2O3—MgO nanocomposite material. MoO3 of the MoO3@Al2O3—MgO nanocomposite material is effective in promoting the hydrolysis of NaBH4 by lowering the activation energy of the reaction. Al2O3 and MgO when combined with MoO3, form a nanocomposite that enhances the overall catalytic activity and durability. The MoO3@Al2O3—MgO nanocomposite is a composite material where MoO3 is anchored onto the surface or dispersed into a Al2O3 and MgO matrix, forming a hybrid catalyst. The design improves the interaction between the catalyst and the NaBH4, providing more active sites for the reaction to take place. In the presence of the MoO3@Al2O3—MgO nanocomposite material, the hydrolysis process becomes faster, more efficient, and can operate under milder conditions (e.g., lower temperatures or pressures), which is beneficial for hydrogen production systems.
At step 74, the method 70 includes collecting the H2 gas. In some embodiments, methods for collecting hydrogen may include, but are not limited to, water displacement, gas collection bags, pressure collection in cylinders or tanks, cold trap collection, siphon collection, absorption into metal hydrides, membrane separation, and cryogenic collection. Any other applicable system of hydrogen collection may be used. Also, any typical method of hydrogen storage may be employed after the method to store hydrogen safely.
In some embodiments, the MoO3 content of the MoO3@Al2O3—MgO nanocomposite material is in a range from 1 to 20 wt. %, preferably 5 to 15 wt. %, preferably 8 to 12 wt. %, and yet more preferably 10 wt. % of the total weight of the MoO3@Al2O3—MgO nanocomposite material.
In some embodiments, the MoO3@Al2O3—MgO nanocomposite material has a hydrogen generation rate of greater than or equal to 400 milliliters per minute per gram (mL·min−1·g−1) when used to generate hydrogen from NaBH4. In some embodiments, the MoO3@Al2O3—MgO nanocomposite material has a hydrogen generation rate of greater than or equal to 500 mL·min−1·g−1, preferably 510 mL·min−1·g−1, preferably 520 mL·min−1·g−1, preferably 530 mL·min−1·g−1, preferably 540 mL·min−1·g−1, preferably 550 mL·min−1·g−1, preferably 560 mL·min−1·g−1, preferably 570 mL·min−1·g−1, and yet more preferably 580 mL·min−1·g−1 when used to generate hydrogen from NaBH4 at a temperature of 30° C. In some embodiments, the MoO3@Al2O3—MgO nanocomposite material has a hydrogen generation rate of greater than or equal to 550 mL·min−1·g−1 when used to generate hydrogen from NaBH4 at a temperature of 30° C.
In some embodiments, the MoO3@Al2O3—MgO nanocomposite material has a hydrogen generation rate of greater than or equal to 600 mL·min−1·g−1, preferably 610 mL·min−1·g−1, preferably 620 mL·min−1·g−1, and yet more preferably 630 mL·min−1·g−1 when used to generate hydrogen from NaBH4 at a temperature of 35° C.
In some embodiments, the MoO3@Al2O3—MgO nanocomposite material has a hydrogen generation rate of greater than or equal to 800 mL·min−1·g−1, preferably 810 mL·min−1·g−1, preferably 820 mL·min−1·g−1, preferably 830 mL·min−1·g−1, preferably 840 mL·min−1·g−1, preferably 850 mL·min−1·g−1, preferably 860 mL min−1·g−1, preferably 870 mL·min−1·g−1, and preferably 880 mL·min−1·g−1, preferably 890 mL·min−1·g−1, preferably 900 mL·min−1·g−1, preferably 910 mL·min−1·g−1, preferably 920 mL·min−1·g−1, preferably 930 mL·min−1·g−1, and yet more preferably 940 mL·min−1·g−1, when used to generate hydrogen from NaBH4 at a temperature of 40° C.
In some embodiments, the MoO3@Al2O3—MgO nanocomposite material has a hydrogen generation rate of greater than or equal to 1000 mL·min−1·g−1 when used to generate hydrogen from NaBH4 at a temperature of 45° C. In some embodiments, the MoO3@Al2O3—MgO nanocomposite material has a hydrogen generation rate of greater than or equal to 1200 mL·min−1·g−1, preferably 1210 mL·min−1·g−1, preferably 1220 mL·min−1·g−1, preferably 1230 mL·min−1·g−1, preferably 1240 mL·min−1·g−1, preferably 1250 mL·min−1·g−1, preferably 1260 mL·min−1·g−1, preferably 1270 mL·min−1·g−1, and preferably 1280 mL·min−1·g−1, preferably 1290 mL·min−1·g−1, preferably 1300 mL·min−1·g−1, preferably 1310 mL·min−1·g−1, preferably 1320 mL·min−1·g−1, preferably 1330 mL·min−1·g−1, preferably 1340 mL·min−1·g−1, preferably 1350 mL·min−1·g−1, preferably 1360 mL·min−1·g−1, preferably 1370 mL·min−1·g−1, preferably 1380 mL·min−1·g−1, preferably 1390 mL·min−1·g−1, and yet more preferably 1400 mL·min−1·g−1 when used to generate hydrogen from NaBH4 at a temperature of 45° C.
The following examples demonstrate a method for synthesis of a MoO3@Al2O3—MgO nanocomposite material and a method for hydrogen generation by use thereof. The examples are provided solely for illustration and are not to be construed as limitations of the present disclosure, as many variations thereof are possible without departing from the spirit and scope of the present disclosure.
According to the present disclosure, the 10% MoO3@MgAl2O4 nanocomposite material was synthesized by mixing about 10.0 grams (g) of sucrose, 17.46 g of Al(NO3) 3.9H2O, and 25.41 g of Mg(Ac)2·4H2O, in a 500 milliliter (mL) beaker. Further, ammonium molybdate and 30 mL distilled water (DW) were added to the powder mixture and heated to 100° C. till the contents of the beaker turned into a clear solution. Further, the temperature was raised to about 150° C. to 200° C. and heated until the sucrose was carbonized. The obtained black product was ground in a mortor, calcined at a temperature of about 750° C. for 3.0 hours, and the 10% MoO3@MgAl2O4 nanocomposite material was collected. The 10% MoO3@MgAl2O4 nanocomposite material may be referred to as ‘catalyst’, ‘composite’, or ‘nanocomposite’, hereinafter without any limitations.
According to the present disclosure, the 10% MoO3@MgAl2O4 nanocomposite material was prepared as per the method described above. The nanocomposite material included low-cost materials, prepared through an efficient method. The solid catalyst efficiently hydrolyzed sodium borohydride (NaBH4) into clean and pure hydrogen (H2) within minutes at a high hydrogen generation rate (HGR). In general, NaBH4 is a safe, stable, and lightweight hydrogen storage material, which may offer a high hydrogen storage capacity of about 10.8 weight percent. The hydrolysis results of NaBH4 with and without the 2.5% to 10% MoO3@MgAl2O4 nanocomposite material were evaluated and depicted in
The impact of weight of NaBH4 and reaction temperature on the catalytic hydrolysis of NaBH4 over 10% MoO3@MgAl2O4 was analyzed, the results are depicted in
The aspects of the present disclosure provide a method of synthesis for the MoO3@MgAl2O4 nanocomposite material and the use thereof in hydrogen generation. In particular, the MoO3@MgAl2O4 nanocomposite material is prepared from low-cost using an efficient method. The nanocomposite as synthesized herein was able to hydrolyze the NaBH4 into clean and pure hydrogen, within a few minutes and with a desirable hydrogen generation rate (HGR). The concentrations and strength of the MoO3@MgAl2O4 nanocomposite material may be adjusted as per the requirements in a particular application. Production of the MoO3@MgAl2O4 nanocomposite material is economically feasible and may provide enhancement in various fields where hydrogen is required, including clean and green energy applications. Further, the methods described herein and the synthesized MoO3@MgAl2O4 nanocomposite material are environmentally friendly in nature and may provide sustainable energy development solutions.
Numerous modifications and variations of the present disclosure are possible in light of the above teachings. It is therefore to be understood that within the scope of the appended claims, the invention may be practiced otherwise than as specifically described herein.
| Number | Name | Date | Kind |
|---|---|---|---|
| 2692293 | Heinemann | Oct 1954 | A |
| 20100178240 | Capron | Jul 2010 | A1 |
| Number | Date | Country |
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| 102824913 | Aug 2014 | CN |
| 109289846 | Mar 2021 | CN |
| 110252356 | Apr 2022 | CN |
| 118022811 | May 2024 | CN |
| 2002153760 | May 2002 | JP |
| WO-2007001164 | Jan 2007 | WO |
| 2008093286 | Aug 2008 | WO |
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