A method for catalyzing sodium borohydride to produce hydrogen at low temperature and fast
By using a combination of natural flavonoid catalysts and alcohol solvents, the problem of low activity in NaBH4 hydrolysis hydrogen production technology at low temperatures has been solved, realizing an efficient and environmentally friendly low-temperature hydrogen production method suitable for portable hydrogen supply systems.
Patent Information
- Authority / Receiving Office
- CN · China
- Patent Type
- Patents(China)
- Current Assignee / Owner
- HEFEI UNIV OF TECH
- Filing Date
- 2024-06-21
- Publication Date
- 2026-07-03
AI Technical Summary
Existing NaBH4 water electrolysis hydrogen production technology has low catalyst activity at low temperatures, making it difficult to adapt to outdoor low-temperature hydrogen production. Furthermore, traditional catalyst modification methods are complex and cause serious environmental pollution, while metal catalysts are costly and difficult to recycle.
Using natural flavonoids as catalysts and alcohols or alcohol-water mixtures as reaction solvents, the alcoholysis of NaBH4 to produce hydrogen is carried out. The catalysts are widely available, inexpensive, highly active, and can be regenerated by simple methods.
It achieves efficient catalytic hydrogen production from NaBH4 alcoholysis under low-temperature conditions. The catalyst has stable activity, high hydrogen production rate, and is easy to recover and reuse, making it suitable for portable hydrogen supply systems.
Smart Images
Figure HDA0004905557290000011 
Figure HDA0004905557290000012 
Figure HDA0004905557290000021
Abstract
Description
Technical Field
[0001] This invention belongs to the field of sodium borohydride hydrolysis hydrogen production technology, specifically relating to a catalyst for sodium borohydride hydrolysis hydrogen production and a rapid and efficient hydrogen production technology in a low-temperature environment. Background Technology
[0002] Hydrogen energy, as a carrier of clean and renewable energy, boasts advantages such as high energy density and clean, pollution-free operation. In recent years, with advancements in fuel cell and P2G technologies, hydrogen energy has seen significant development in transportation and renewable energy storage. Developing high-performance hydrogen production and storage materials remains a key technology for solving the challenges of hydrogen storage and transportation. Metal hydride and borohydride hydrolysis hydrogen production technology is an integrated hydrogen production and storage technology that can release hydrogen at room temperature and pressure and achieve recycling through off-system byproduct regeneration technology, potentially solving key issues in hydrogen storage and transportation. Sodium borohydride (NaBH4) is the closest material to practical applications for hydrolysis hydrogen production, with a hydrogen storage capacity of up to 10.8 wt%. Under normal temperature and in the presence of a suitable catalyst, it can stably and continuously produce hydrogen. Due to its non-toxicity, stability in alkaline solutions, recyclable byproducts, environmental friendliness, and high purity of produced hydrogen, NaBH4's hydrolysis hydrogen production technology is considered one of the most suitable alternatives to pressurized hydrogen storage tanks. However, the inherent stability of NaBH4 makes the hydrolysis hydrogen production rate very slow in the absence of a suitable catalyst. Over the past few decades, various catalysts for NaBH4 water electrolysis hydrogen production technology have been extensively studied, most of which are noble metal-based (such as Pt, Ru, Pd, etc.) catalysts and non-noble metal-based Co, Fe, Ni catalysts. Although metal-based catalysts have high activity, they have drawbacks such as high manufacturing cost and environmental hazards. Moreover, metal-based catalysts have very low activity at lower reaction temperatures, making them difficult to adapt to low outdoor ambient temperatures for hydrogen production, which limits the practical application of NaBH4 water electrolysis hydrogen production technology in the low-temperature outdoor environment of vehicle fuel cells. In addition, water as a reaction solution begins to freeze below 0°C, and outdoor temperatures are below 0°C for most of the year. NaBH4 methanol electrolysis hydrogen production technology can overcome the limitation of using water as a solvent. Moreover, the byproduct of NaBH4 methanol electrolysis reaction, sodium tetramethoxyboroide (NaB(OCH3)4), is readily soluble in methanol and will not inhibit the activity of the catalyst. Since methanol has a freezing point of -97°C, it is also more useful for fuel cell hydrogen supply systems in cold regions.
[0003] In contrast, emerging environmentally friendly non-metallic catalysts have attracted increasing attention. Currently, much research focuses on amylating or acidifying non-metallic materials such as microcrystalline cellulose, diatomaceous earth, and carbon black to graft specific active functional groups, thereby catalyzing the methanol hydrolysis of NaBH4 to produce hydrogen. However, catalyst modification methods are complex, using large amounts of organic solvents and inorganic acids, causing environmental pollution. Furthermore, the grafted active functional groups participate in the reaction during catalysis, resulting in poor recyclability. Summary of the Invention
[0004] To address the shortcomings of existing technologies, this invention provides a method for rapid low-temperature hydrogen production using sodium borohydride catalyzed by natural flavonoids. The selected catalyst is characterized by its wide availability, low price, high catalytic activity, ease of use, and convenient recycling. This method enables hydrogen production in low-temperature environments, laying the foundation for the application of controllable hydrogen systems in the field of portable hydrogen supply during the winter in northern regions and in the low-temperature environments of the North and South Poles.
[0005] To achieve its objectives, the present invention employs the following technical solution:
[0006] A method for rapid low-temperature hydrogen production from sodium borohydride catalyzed by natural flavonoids is characterized by using natural flavonoids as a catalyst, alcohols or alcohol-water mixtures as reaction solvents, and NaBH4 as a raw material for hydrogen production, to carry out the alcoholysis reaction of NaBH4 to produce hydrogen.
[0007] Furthermore, the natural flavonoids include at least one of flavonoids, flavonols, and isoflavones.
[0008] Furthermore, the flavonoids include at least one of the natural plant extracts baicalin, baicalin, naringin, and naringin; the flavonols include at least one of the natural quercetin, rutin, and silymarin; and the isoflavones include at least one of the natural daidzein, puerarin, and rotenone.
[0009] Furthermore, the alcohols include at least one of methanol, ethanol, ethylene glycol, and glycerol.
[0010] Furthermore, the reaction temperature for the alcoholysis to hydrogen production reaction is -30℃ to 40℃.
[0011] Furthermore, the mass ratio of the catalyst to NaBH4 is 0.05 to 1:1, indicating that the amount of catalyst used is small and the activity is high.
[0012] Furthermore, natural flavonoids can be regenerated by acid precipitation after repeated catalytic reactions with NaBH4, and still retain high catalytic activity after regeneration.
[0013] Based on the above-mentioned low-temperature rapid hydrogen production method, this invention also proposes the application of natural flavonoids as catalysts for the low-temperature rapid hydrogen production of sodium borohydride.
[0014] Compared with the prior art, the present invention has the following beneficial effects:
[0015] 1. The catalyst used in this invention is a non-metallic flavonoid compound, which is widely found in the plant kingdom, mainly derived from plant flowers, leaves, fruits, and roots. It has the advantages of abundant sources and low cost, making it a renewable and green catalyst. Furthermore, this catalyst can be directly used to catalyze the alcoholysis of NaBH4 to produce hydrogen without any modification or reduction treatment, exhibiting excellent catalytic activity.
[0016] 2. The method of the present invention is simple and has commercial application prospects.
[0017] 3. The catalyst involved in this invention can catalyze the rapid alcoholysis of sodium borohydride to produce hydrogen under low temperature conditions. It has stable catalytic performance, high hydrogen production rate, good catalytic durability, and can be reused.
[0018] 4. The reaction solution used in the hydrogen production method of the present invention is methanol, ethanol, ethylene glycol, glycerol or alcohol-water mixture. Since the freezing point of alcohol solution or alcohol-water mixture is very low, the system can still catalyze the rapid alcoholysis of NaBH4 to produce hydrogen at low temperature (<-30℃). The reaction temperature range is wide (-30℃ to 40℃), and it has excellent hydrogen production performance. Each 1g of NaBH4 consumed produces about 2500mL of hydrogen.
[0019] 5. The catalyst involved in this invention is sparingly soluble in water in neutral or acidic solutions. It can be separated from the alcoholysis products by simple filtration or centrifugation, making it easy to recover and reuse. The catalyst recovered after acid treatment can be directly reused for catalytic hydrogen production from the alcoholysis of NaBH4. The catalytic efficiency of the regenerated catalyst can reach more than 99% of the original, overcoming the disadvantages of metal nanocatalysts that are easy to disperse, difficult to recover, and cannot be recycled. Attached Figure Description
[0020] Figure 1 The kinetic curves of the sodium borohydride alcoholysis hydrogen production reaction in Examples 1-10 are shown. Figure 1 (a~c) and catalytic hydrogen production rate (HGR) values ( Figure 1 (d) in the middle.
[0021] Figure 2 The hydrogen production reaction curves of NaBH4 catalyzed by quercetin in Example 11 in different reaction solutions include: (a) methanol, (b) ethylene glycol, (c) glycerol, (d) ethanol and (e) water.
[0022] Figure 3The kinetic curves for hydrogen production from alcoholysis under different catalyst dosages in Example 12 are shown below. Figure 3 (a) in the figure corresponds to the reaction rate and HGR value. Figure 3 (b) in the middle.
[0023] Figure 4 The kinetic curves for hydrogen production from the alcoholysis of different amounts of NaBH4 in Example 13 are shown. Figure 4 (a) and the corresponding HGR value ( Figure 4 (b) in the middle.
[0024] Figure 5 The figures are kinetic curves of NaBH4 alcoholysis to hydrogen production at different methanol concentrations in Examples 14 and 15, where (a) corresponds to Example 14 and (b) corresponds to Example 15.
[0025] Figure 6 The graph shows the kinetics of quercetin-catalyzed NaBH4 alcoholysis to hydrogen production at different reaction temperatures in Example 16. Figure 6 (a) and the corresponding calculated activation energy fitting curve ( Figure 6 (b) in the middle.
[0026] Figure 7 The graph shows the performance of quercetin in five catalytic hydrogen production cycles in Example 17. Figure 7 (a) and a comparison chart of the percentage of catalytic activity after multiple cycles ( Figure 7 (b) in the middle.
[0027] Figure 8 The kinetic curve for hydrogen production from NaBH4 catalyzed by regenerated quercetin in Example 18 is shown. Detailed Implementation
[0028] The present invention will be further described clearly, in detail and completely below with reference to specific embodiments and accompanying drawings. The listed embodiments are only for further explanation of the present invention and do not limit the present invention as such:
[0029] Example 1
[0030] The steps for the hydrogen production reaction of NaBH4 via alcoholysis catalyzed by quercetin are as follows:
[0031] 50 mg of quercetin and 0.1 g of NaBH4 were placed in a reaction tube, and 5 mL of methanol was added to carry out the alcoholysis reaction at room temperature. The volume of hydrogen produced was recorded over time using the water displacement method. The kinetic curve of hydrogen production from the alcoholysis of NaBH4 catalyzed by quercetin is shown below. Figure 1Curve (1) in (a) shows that the reaction can produce 250±1mL of hydrogen gas within 3min. The hydrogen production rate (HGR) of NaBH4 alcoholysis catalysis per unit mass catalyst is 13483mLH2 / (g·min), and the hydrogen production conversion rate reaches 100%.
[0032] Example 2
[0033] The alcoholysis reaction of NaBH4 to produce hydrogen, catalyzed by rutin as a catalyst, proceeds as follows:
[0034] 50 mg of rutin and 0.1 g of NaBH4 were placed in a reaction tube, and 5 mL of methanol was added to carry out the alcoholysis reaction at room temperature. The volume of hydrogen produced was recorded over time using the water displacement method. The kinetic curve of rutin-catalyzed NaBH4 alcoholysis for hydrogen production is shown below. Figure 1 Curve (2) in (a) shows that the reaction can produce 250±1mL of hydrogen gas within 3min, the hydrogen production conversion rate reaches 100%, and its HGR value is 8727mLH2 / (g·min).
[0035] Example 3
[0036] The alcoholysis reaction of NaBH4 to produce hydrogen was catalyzed by silymarin as a catalyst, and the steps are as follows:
[0037] 50 mg of silymarin and 0.1 g of NaBH4 were placed in a reaction tube and subjected to alcoholysis with 5 mL of methanol at room temperature. The volume of hydrogen produced was recorded over time using the water displacement method. The kinetic curve of hydrogen production from the alcoholysis of NaBH4 catalyzed by silymarin is shown below. Figure 1 As shown in curve (3) in (a), the reaction produces 237 mL of hydrogen gas within 3 min, with a conversion rate of over 95% and an HGR value of 3582 mLH2 / (g·min). The hydrogen production conversion rate can reach 100% within 8 min of the reaction.
[0038] Example 4
[0039] The alcoholysis reaction of NaBH4 to produce hydrogen, catalyzed by baicalin as a catalyst, proceeds as follows:
[0040] 50 mg of baicalin and 0.1 g of NaBH4 were placed in a reaction tube, and 5 mL of methanol was added to carry out the alcoholysis reaction at room temperature. The change in the volume of hydrogen produced over time was recorded using the water displacement method. The kinetic curve of hydrogen production from the alcoholysis of NaBH4 catalyzed by baicalin is shown below. Figure 1 Curve (1) in (b) shows that the reaction can produce 250±1mL of hydrogen gas within 3min, with a hydrogen production conversion rate of 100% and an HGR value of 7500mLH2 / (g·min).
[0041] Example 5
[0042] The alcoholysis reaction of NaBH4 to produce hydrogen, catalyzed by naringenin as a catalyst, proceeds as follows:
[0043] 50 mg of naringenin and 0.1 g of NaBH4 were placed in a reaction tube, and 5 mL of methanol was added to carry out the alcoholysis reaction at room temperature. The change in the volume of hydrogen produced over time was recorded using the water displacement method. The kinetic curve of hydrogen production from the alcoholysis of Naingenin catalyzed by NaBH4 is shown below. Figure 1 Curve (2) in (b) shows that the reaction can produce 250±1mL of hydrogen gas within 5min, with a hydrogen production conversion rate of 100% and an HGR value of 8000mLH2 / (g·min).
[0044] Example 6
[0045] The alcoholysis reaction of NaBH4 to produce hydrogen, catalyzed by baicalin as a catalyst, proceeds as follows:
[0046] 50 mg of baicalein and 0.1 g of NaBH4 were placed in a reaction tube, and 5 mL of methanol was added to carry out the alcoholysis reaction at room temperature. The change in the volume of hydrogen produced over time was recorded using the water displacement method. The kinetic curve of hydrogen production from the alcoholysis of NaBH4 catalyzed by baicalein is shown below. Figure 1 As shown in curve (3) in (b), the reaction produces 238 mL of hydrogen gas within 3 min, with a hydrogen production conversion rate of over 95% and an HGR value of 3692 mLH2 / (g·min). The hydrogen production conversion rate can reach 100% within 8 min of the reaction.
[0047] Example 7
[0048] The alcoholysis reaction of NaBH4 to produce hydrogen, catalyzed by naringin as a catalyst, proceeds as follows:
[0049] 50 mg of naringin and 0.1 g of NaBH4 were placed in a reaction tube, and 5 mL of methanol was added to carry out the alcoholysis reaction at room temperature. The change in the volume of hydrogen produced over time was recorded using the water displacement method. The kinetic curve of hydrogen production from the alcoholysis of Naingin catalyzed by NaBH4 is shown below. Figure 1 As shown in curve (4) in (b), the reaction produces 196 mL of hydrogen gas within 3 min, with a hydrogen production conversion rate of over 78% and an HGR value of 1244 mLH2 / (g·min). The hydrogen production conversion rate can reach 98% within 10 min of the reaction.
[0050] Example 8
[0051] The hydrogen production reaction catalyzed by the alcoholysis of NaBH4 using daidzein as a catalyst is as follows:
[0052] 50 mg of daidzein and 0.1 g of NaBH4 were placed in a reaction tube, and 5 mL of methanol was added to carry out the alcoholysis reaction at room temperature. The volume of hydrogen produced was recorded over time using the water displacement method. The kinetic curve of hydrogen production from the alcoholysis of daidzein and NaBH4 is shown below. Figure 1 Curve (1) in (c) shows that the reaction can produce 250±1mL of hydrogen gas within 3min, with an HGR value of 13953mL H2 / (g·min) and a hydrogen production conversion rate of 100%.
[0053] Example 9
[0054] The hydrogen production reaction of NaBH4 via alcoholysis catalyzed by puerarin is as follows:
[0055] 50 mg of puerarin and 0.1 g of NaBH4 were placed in a reaction tube, and 5 mL of methanol was added to carry out the alcoholysis reaction at room temperature. The volume of hydrogen produced was recorded over time using the water displacement method. The kinetic curve of hydrogen production from the alcoholysis of NaBH4 catalyzed by puerarin is shown below. Figure 1 As shown in curve (2) in (c), the reaction can produce 250±1mL of hydrogen gas within 3min, with an HGR value of 9231mLH2 / (g·min) and a hydrogen production conversion rate of 100%.
[0056] Example 10
[0057] The alcoholysis reaction of NaBH4 to produce hydrogen, catalyzed by rotenone as a catalyst, proceeds as follows:
[0058] 50 mg of rotenone and 0.1 g of NaBH4 were placed in a reaction tube, and 5 mL of methanol was added to carry out the alcoholysis reaction at room temperature. The change in the volume of hydrogen produced over time was recorded using the water displacement method. The kinetic curve of hydrogen production from the alcoholysis of NaBH4 catalyzed by rotenone is shown below. Figure 1 As shown in curve (3) in (c), the reaction produces 117 mL of hydrogen gas within 5 min, with a hydrogen production conversion rate of 46.8% and an HGR value of 334 mLH2 / (g·min). The hydrogen production conversion rate can reach 75% within 10 min of the reaction.
[0059] Example 11
[0060] The hydrogen production reaction of NaBH4 in different reaction solutions was catalyzed by quercetin as a catalyst, and the steps are as follows:
[0061] Mix 50 mg of quercetin with 0.1 g of NaBH4 and place the mixture in a reaction tube. Add 5 mL of a reaction solution (containing methanol, ethanol, ethylene glycol, glycerol, and water) to the reaction tube and allow the alcoholysis reaction to proceed at room temperature. Record the change in hydrogen production volume over time using the water displacement method. The NaBH4 hydrolysis / alcohololysis hydrogen production kinetic curves for different types of reaction solutions are shown below. Figure 2 As shown in (ae), the reaction rate of NaBH4 in each reaction solution, from highest to lowest, is: ethylene glycol > methanol > glycerol > ethanol > water, and the alcoholysis conversion rate is: methanol > ethylene glycol > glycerol > ethanol > water.
[0062] Example 12
[0063] The experiments on hydrogen production from NaBH4 via alcoholysis under different catalyst dosages are as follows:
[0064] Quercetin at concentrations of 10, 15, 20, 25, 30, 50, 70, and 100 mg were mixed with 0.1 g of NaBH4, and placed in separate reaction tubes. 5 mL of methanol was added to initiate the hydrogen production reaction at room temperature. The volume of hydrogen produced was recorded over time using the water displacement method. The kinetic curves for hydrogen production from the alcoholysis of NaBH4 catalyzed by different amounts of quercetin are shown below. Figure 3 As shown in (a), the corresponding alcoholysis hydrogen production reaction rate and the hydrogen production rate per unit mass of catalyst catalyzing NaBH4 (HGR) are as follows: Figure 3 As shown in (b), the reaction rate increases linearly with increasing catalyst dosage, but the HGR value decreases exponentially with increasing catalyst dosage.
[0065] Example 13
[0066] The steps of the alcoholysis hydrogen production experiment under different concentrations of NaBH4 are as follows:
[0067] 50 mg of quercetin was mixed with different masses of NaBH4 and placed in reaction tubes. 5 mL of methanol was then injected into the reaction tubes to achieve NaBH4 concentrations of 8, 20, 30, and 40 mg / mL. The alcoholysis reaction was initiated at room temperature, and the volume of hydrogen produced was recorded over time using the water displacement method. The kinetic curves for hydrogen production from the alcoholysis of different amounts of NaBH4 are shown below. Figure 4 As shown in (a), the corresponding HGR values are listed in Figure 4 (b). As can be seen from the figure, the HGR value increases linearly with the increase of NaBH4 concentration, and the kinetics follow the first-order reaction.
[0068] Example 14
[0069] The steps for the alcoholysis hydrogen production experiments under different alcohol-water mixing ratios are as follows:
[0070] Mix 50 mg of quercetin with 0.1 g of NaBH4 and place the mixture in a reaction tube. Add 5 mL of a methanol-water mixture (methanol volume percentages of 100 vol.%, 90 vol.%, 80 vol.%, 60 vol.%, 40 vol.%, and 20 vol.%) to the reaction tube. Initiate the alcoholysis reaction at room temperature and record the change in hydrogen production volume over time using the water displacement method. The kinetic curves for NaBH4 alcoholysis hydrogen production with different proportions of methanol-water mixtures as the reaction solution are shown below. Figure 5 As shown in (a), the reaction rate and hydrogen production yield both decrease with decreasing methanol content.
[0071] Example 15
[0072] The steps for the alcoholysis hydrogen production experiment with different mixing ratios of methanol and ethanol are as follows:
[0073] Mix 50 mg of quercetin with 0.1 g of NaBH4 and place the mixture in a reaction tube. Add 5 mL of a methanol-ethanol mixture (methanol volume percentages of 100 vol.%, 90 vol.%, 80 vol.%, 60 vol.%, 40 vol.%, and 20 vol.%) to the reaction tube. Initiate the alcoholysis reaction at room temperature and record the change in hydrogen production volume over time using the water displacement method. The kinetic curves for NaBH4 alcoholysis hydrogen production with different proportions of methanol-ethanol mixtures as the reaction solution are shown below. Figure 5 As shown in (b), the reaction rate and hydrogen production yield both decrease with decreasing methanol content, but the hydrogen production rate and yield are higher than those of the methanol-water system with the same methanol content.
[0074] Example 16
[0075] The hydrogen production rate and activation energy of quercetin-catalyzed NaBH4 under different temperature conditions were tested, and the steps are as follows:
[0076] Hydrogen production from sodium borohydride was catalytically carried out at different temperatures (25, 15.5, -10, and -25°C) using quercetin as a catalyst, following the method of Example 1. The hydrogen release volume over time is shown in the curves below. Figure 6 As shown in (a), the reaction starts rapidly, and the conversion rate of the alcoholysis reaction reaches 100% within 1.5, 2, 3.5, 10 and 20 min, respectively. Figure 6 (b) The Arrhenius activation energy fitting curve for the hydrogen production by sodium borohydride alcoholysis is given. The calculated activation energy is 17.2 kJ / mol, which is lower than the activation energy of NaBH4 alcoholysis reaction in the presence of most metal catalysts.
[0077] Example 17
[0078] The steps for testing the catalyst recycling performance are as follows:
[0079] At room temperature, 0.1 g of NaBH4 was weighed and placed in the solution after the alcoholysis reaction in Example 1 to begin the second alcoholysis reaction for hydrogen production. The change in hydrogen production volume over time was recorded using the water displacement method. After the reaction was completed, another 0.1 g of NaBH4 was added to the solution, and this process was repeated 5 times. The recycling performance of lignin-catalyzed NaBH4 alcoholysis for hydrogen production was recorded.
[0080] The kinetic curves for hydrogen production from alcoholysis after 5 cycles are shown below. Figure 7 As shown in (a). Figure 7(b) is a comparison chart of the percentage of catalytic activity of quercetin in NaBH4 after multiple cycles. As the number of uses increases, the catalytic activity of lignin gradually decreases. After 5 cycles, the catalytic activity of lignin decreases to 83% of the initial value.
[0081] Example 18
[0082] The regenerated quercetin was used in the catalytic alcoholysis of NaBH4 to produce hydrogen, and the steps are as follows:
[0083] A 10-20% sulfuric acid solution was slowly added dropwise to the product from multiple cycles of hydrogen production experiments in Example 17 until the pH reached 3-4. The product was then centrifuged, washed, and dried. The resulting solid powder was used as a regenerated catalyst for the catalytic alcoholysis of NaBH4 to produce hydrogen. The steps for the regenerated quercetin-catalyzed NaBH4 alcoholysis hydrogen production were the same as in Example 1. Figure 8 The figures show a comparison of the kinetic curves for the catalytic hydrogen production from NaBH4 using quercetin and regenerated quercetin in Example 1. As can be seen from the figures, the regenerated quercetin still exhibits high catalytic activity, reaching over 99% of the activity of the original quercetin.
[0084] The embodiments described above are merely for illustrating the technical ideas and features of the present invention. Their purpose is to enable those skilled in the art to understand the content of the present invention and implement it accordingly. They should not be used to limit the patent scope of the present invention. That is, all equivalent changes or modifications made in accordance with the spirit disclosed in the present invention should still be covered within the patent scope of the present invention.
Claims
1. A method for rapid low-temperature hydrogen production using sodium borohydride catalyzed by natural flavonoids, characterized in that: Using natural flavonoids as catalysts, alcohols or a mixture of alcohol and water as reaction solvents, and NaBH4 as a raw material for hydrogen production, the alcoholysis of NaBH4 is carried out to produce hydrogen.
2. The method for catalytic sodium borohydride low-temperature rapid hydrogen production of natural flavonoids according to claim 1, characterized in that: The natural flavonoids include at least one of flavonoids, flavonols, and isoflavones.
3. The method for catalyzing sodium borohydride to produce hydrogen at low temperature and fast according to claim 2, characterized in that: The flavonoids are at least one of baicalin, baicalin, naringin, and naringin.
4. The method for producing hydrogen by catalyzing sodium borohydride at low temperature according to claim 2, characterized in that: The flavonols are at least one of quercetin, rutin, and silymarin.
5. The method for catalyzing sodium borohydride to produce hydrogen at low temperature and fast according to claim 2, characterized in that: The isoflavones are at least one of daidzein, puerarin, and rotenone.
6. The method for producing hydrogen by catalyzing sodium borohydride at low temperature according to claim 1, characterized in that: The alcohols include at least one of methanol, ethanol, ethylene glycol, and glycerol.
7. The method for producing hydrogen by catalyzing sodium borohydride at low temperature according to claim 1, characterized in that: The reaction temperature for the alcoholysis hydrogen production reaction is -30℃ to 40℃.
8. The method for rapid low-temperature hydrogen production using sodium borohydride catalyzed by natural flavonoids according to claim 1, characterized in that: The mass ratio of the catalyst to NaBH4 is 0.05 to 1:
1.
9. The method for producing hydrogen by catalyzing sodium borohydride at low temperature according to claim 1, characterized in that: Natural flavonoids can be regenerated by sulfuric acid precipitation after repeated catalysis with NaBH4.
10. The application of a natural flavonoid compound as a catalyst for the rapid low-temperature hydrogen production from sodium borohydride.