METHOD FOR SIMULTANEOUS CONVERSION OF HYDROGEN SOURCE AND A CARBON DIOXIDE SOURCE INTO FORMATE WITH IMPROVED YIELD

Abstract

Proposed is a high-yield simultaneous conversion method for a hydrogen source and a carbon dioxide source. The method significantly increases a yield of a formate through conversion of carbon dioxide. To this end, a carbon dioxide source and a hydrocarbon containing one or more hydroxy groups undergo a simultaneous conversion reaction in the presence of a solvent containing one or more alcohols and having a pH of 10 to 14.

Claims

1. A method for simultaneous conversion of a hydrogen source and a carbon dioxide source into a formate with an improved yield, the method using a simultaneous conversion reaction of the hydrogen source and the carbon dioxide source, wherein the hydrogen source is a hydrocarbon containing one or more hydroxy groups, the carbon dioxide source is one or more materials selected from among carbon dioxide molecules, metal carbonates, and metal bicarbonates, the simultaneous conversion reaction is performed in an aqueous solution containing one or more alcohols having 1 to 4 carbon atoms, and the solution in which the hydrogen source and the carbon dioxide source are dissolved is adjusted to have a pH within a range of 10 to 14.

2. The method of claim 1, wherein the metal carbonate and the metal bicarbonate are carbon dioxide derivatives formed by a reaction between carbon dioxide and a metal and/or metal salt.

3. The method of claim 1, wherein the simultaneous conversion is performed in the presence of a catalyst, and the catalyst has a form in which one or more metals selected from among ruthenium (Ru), iridium (Ir), rhodium (Rh), platinum (Pt), palladium (Pd), and gold (Au) are supported on a support.

4. The method of claim 1, wherein a basic material is further added to adjust the pH of the solution.

5. The method of claim 1, wherein the carbon dioxide source has a concentration of 0.01 M to 1 M in the solution.

6. The method of claim 1, wherein the hydrogen source and the carbon dioxide source are mixed in a ratio in a range of 0.1 to 10 in the solution in terms of moles of hydrogen and carbon dioxide.

7. The method of claim 1, wherein the metal in the metal carbonate salt and the metal in the metal bicarbonate salt are K, Na, Li, Rb, or Cs.

8. The method of claim 1, wherein the one or more alcohols in the aqueous solution have a concentration within a range of 10% to 90% by weight.

9. The method of claim 1, wherein the reaction is performed at a temperature in a range of 0° C. to 50° C. and at a pressure in a range of 1 to 50 bar.

10. A method for simultaneous conversion of a hydrogen source and a carbon dioxide source, the method using a simultaneous conversion reaction of the hydrogen source and the carbon dioxide source, wherein the hydrogen source is a hydrocarbon containing at least one hydroxyl group, the carbon dioxide source is a metal carbonate, the metal is at least one of K, Rb, and Cs, and the simultaneous conversion reaction is performed in an aqueous solution containing at least one of ethanol, n-propanol, isopropanol, t-butanol.

Description

DESCRIPTION OF THE PREFERRED EMBODIMENTS

[0026] Hereinafter, preferred embodiments of the present disclosure that can be easily implemented by those skilled in the art will be described in detail. In describing the principles employed in the preferred embodiments of the present invention, well-known functions or constructions will not be described in detail when they may obscure the gist of the present invention.

[0027] The present disclosure relates to simultaneous conversion of carbon dioxide and a hydrogen source that is a hydrocarbon containing one or more hydroxy groups. One or more forms selected from among carbon dioxide molecules, a metal carbonate derived from carbon dioxide, and a metal bicarbonate derived from carbon dioxide may be introduced into the simultaneous conversion reaction as the carbon dioxide. The reaction according to the present disclosure improves the selectivity of formates among products obtained by the reaction.

[0028] As such, the embodiment of the present disclosure can convert sugars and carbon dioxide into formates with high yields by simultaneous conversion of sugars and carbon dioxide. Therefore, the present disclosure can be widely used in the field of carbon dioxide fixation, capture, conversion, or storage.

[0029] In another embodiment of the present disclosure, any hydrocarbons including one or more hydroxy groups can be used as the hydrogen source without particular limitations, but the hydrogen source will be preferably a sugar derived from biomass. More preferably, one or more sugars selected from among glucose, galactose, and lactose may be used as the hydrogen source, and most preferably, glucose may be used.

[0030] Hereinafter, a method for simultaneous conversion of carbon dioxide and a saccharide according to the present disclosure will be described in detail.

[0031] The simultaneous conversion reaction according to the present disclosure is carried out in the presence of a solvent, in which the solvent is an aqueous solution containing an alcohol having 1 to 4 carbon atoms. In this case, a catalyst may be used to promote the reaction. The catalyst may be a catalyst in which at least one type of noble metal is supported on a support as an active metal. The catalyst promotes a reaction between a hydrocarbon containing one or more hydroxy groups as a hydrogen source and one or more substances selected from among carbon dioxide, metal carbonates, and metal bicarbonates as a carbon dioxide source, and the reaction produces a formate.

[0032] In addition, as the active metal component in the catalyst, one or more noble metals selected from among ruthenium (Ru), iridium (Ir), rhodium (Rh), platinum (Pt), palladium (Pd), and gold (Au) may be used. Preferably, the noble metal may be platinum (Pt), rhodium (Rh), or palladium (Pd).

[0033] In addition, the support in the catalyst is a solid phase enabling a catalytic material to be dispersed and stably maintaining the dispersed catalytic material. The support is a carrier that holds the catalyst material in a highly dispersed manner so that the exposed surface area of the catalytic material can be maximized. To this end, the support usually refers to a material that is porous or has a large surface area and is mechanically, thermally, and chemically stable. The selection of the support is made depending on the diameter and volume of the pores in the support, the surface area, the strength, the chemical stability, and the shape. Since there are cases that the activity of the catalyst varies depending on the type of support, the support may be appropriately selected according to the type of active metal and the type of reaction.

[0034] Examples of the support according to the present disclosure include: activated carbon; carbon-phase materials such as graphite carbon; molecular sieves such as zeolite, metal-organic frameworks (MOF), etc.; ceramic materials such as hydrotalcite, perovskite, spinel (for example, CoAl.sub.2O.sub.4), etc.; metal oxides such as alumina, silica, etc.; sulfate-treated metal oxides such as ZrO.sub.2—SO.sub.4 or SnO.sub.2—SO.sub.4; and metal oxyhydroxides such as AlOOH, ZrO(OH).sub.2, CoOOH, etc. Preferably, the support may be made of activated carbon or graphite carbon.

[0035] The support may be purchased from among commercially available products or may be self-manufactured for use. For example, a carbon body formed as a support provided in a catalyst composite may be obtained by firing a metal-organic framework (MOF) used as a starting material.

[0036] In order to prepare the catalyst composite according to the present disclosure, the active metal may be supported using one of the methods known in the art. For example, impregnation, coprecipitation, solid phase crystallization, vapor deposition, washcoating, sol-gel, in-situ synthesis, etc., may be used.

[0037] In the most preferred embodiment, the catalyst comprises at least one of a carrier in which platinum (Pt) is supported on a carbon support and a carrier in which palladium (Pd) is supported on a carbon support. Preferably, the catalyst comprises a mixture of the carrier in which Pt is supported on a carbon support and the carrier in which Pd is supported on the carbon support.

[0038] In the carbon dioxide-derived metal carbonate and the carbon dioxide-derived metal bicarbonate, the metal may be sodium (Na), potassium (K), lithium (Li), rubidium (Rb), or cesium (Cs). Preferably, the metal is potassium (K).

[0039] In addition, in the simultaneous conversion method according to the disclosure, the content of alcohol included in the aqueous solution is in a range of 10% to 90% by weight. The content of alcohol is preferably in a range of 30% to 70% by weight and is more preferably in a range of 40% to 60% by weight.

[0040] In addition, according to the present disclosure, the pH of a solution containing a solvent, a carbon dioxide source, and a hydrogen source needs to be adjusted to be within a range of 10 to 14 and preferably within a range of 11 to 13. The yield of a formate is lowered when the pH of the solution is outside the range of 10 to 14.

[0041] The pH of the solution may be adjusted by adding a basic material to the solution. Non-limiting examples of the basic material include one or more materials selected from among metal hydroxides such as KOH, NaOH, Ca(OH).sub.2, metal alkoxides, and amines.

[0042] The concentration of the carbon dioxide source in the solution may be in a range of 0.01 to 1 M in terms of the concentration of carbon dioxide. The molar ratio of the hydrogen source to the carbon dioxide source may be in a range of 0.1 to 10 when the moles of the hydrogen source and the carbon dioxide source are converted into the moles of hydrogen and carbon dioxide, respectively.

[0043] In the simultaneous conversion reaction of a carbon dioxide source and a hydrocarbon containing one or more hydroxy groups, the reaction temperature is preferably in a range of 0° C. to 50° C., and the reaction pressure is preferably in a range of 1 to 50 bar.

[0044] In addition, preferably, the reactants participating in the reaction include 0.1 to 10 parts by weight of the catalyst per 100 parts by weight of the solvent.

[0045] In the simultaneous conversion reaction of a carbon dioxide source and a saccharide, the simultaneous conversion reaction may further include a step of converting carbon dioxide into a metal carbonate and/or a metal bicarbonate by reacting a metal, a metal salt, or both with carbon dioxide before reacting the hydrogen source with the carbon dioxide source.

[0046] Hereinafter, the effects of the present disclosure will be described in more detail with reference to examples.

Experimental Examples 1 to 5

[0047] 0.2162 g of glucose (Sigma Aldrich, G8270) as a hydrogen source and 0.0829 g of K.sub.2CO.sub.3 (Sigma Aldrich, 209619) as a carbon dioxide source were added to an aqueous solution of 2.651 g of alcohol and 2.651 g of distilled water as described in Table 1 below to prepare solutions containing 0.2 M of glucose and 0.1 M of K.sub.2CO.sub.3. Next, the pH of each of the solutions was measured. In Experimental Examples 1 to 5, the pH of each of the solutions was about 11.8. Next, 0.02 g of Pt/C (Sigma Aldrich, 205931) in which Pt is contained in an amount of 5% by weight, 0.08 g of Pd/C (Sigma Aldrich, 205680) in which Pd is contained in an amount of 5% by weight, and a magnetic bar were added to each of the solution, and the resulting solutions were stirred at 25° C. for 24 hours to obtain reaction products. The resulting samples were analyzed using HPLC (Shodex Sugar SH1101) and the results are shown in Table 1 below. Cony. in Table 1 below represents the conversion rate of glucose, and the numerical values of Gluconate (%) and the like represents yields calculated as follows:

Glucose Cony.={(initial glucose mole number)−(post-reaction glucose mole number)/(initial glucose mole number)}×100(%)

Gluconate Yield={(number of moles of gluconate produced)/(number of moles of glucose initially added)}×100(%)

Sorbitol Yield{(number of sorbitol moles produced)/(number of moles of glucose initially added)}×100(%)

Formic Acid(FA)Yield={(number of moles of FA produced)/(number of moles of CO.sub.2)}×100(%)

TABLE-US-00001 TABLE 1 Yield (%) Classification Solvent Conv.(%) Gluconate Sorbitol FA Experimental H.sub.2O 48.0 35.6 5.8 2.3 Example 1 Experimental 50% by 53.6 40.6 5.7 6.1 Example 2 weight of MeOH Experimental 50% by 54.6 44.3 6.6 23.2 Example 3 weight of EtOH Experimental 50% by 53.2 40.2 7.4 15.2 Example 4 weight of 1-propanol Experimental 50% by 53.8 42.5 6.3 30.5 Example 5 weight of IPA Experimental 50% t-BuOH 49.1 43.5 5.1 18.3 Example 6

[0048] The results of simultaneous conversion using glucose and K.sub.2CO.sub.3 are shown in Table 1. The yield of formic acid increased when a 50% aqueous alcohol solution was used as the solvent compared to the case where water was used as the solvent. When 50% IPA was used as the solvent, the yield was best (i.e., 30.5%).

Experimental Examples 7 to 12

[0049] Except for using 0.0636 g of Na.sub.2CO.sub.3 (Sigma Aldrich, 223530) as the carbon dioxide source, the experiments were performed in the same manner as in Examples 1 to 6, respectively, and the results are shown in Table 2 below. In Experimental Examples 7 to 12, the pH of each of the solutions was about 11.5.

TABLE-US-00002 TABLE 2 Yield (%) Classification Solvent Conv.(%) Gluconate Sorbitol FA Experimental H.sub.2O 48.0 35.6 5.8 0.5 Example 7 Experimental 50% by 55.8 23.4 20.9 2.0 Example 8 weight of MeOH Experimental 50% by 50.3 38.6 5.7 4.7 Example 9 weight of EtOH Experimental 50% by 42.0 31.3 3.1 2.6 Example 10 weight of 1-propanol Experimental 50% by 49.8 38.4 5.8 14.9 Example 11 weight of IPA Experimental 50% t-BuOH 39.6 34.5 4.8 13.3 Example 12

[0050] Table 2 shows the results of using Na.sub.2CO.sub.3 as the carbon dioxide source instead of K.sub.2CO.sub.3. The yield of formic acid increased when using a 50% alcohol aqueous solution was used as the solvent as in Experiment Examples 1 to 5, but the increase in this case was lower than the in the case of using K.sub.2CO.sub.3.

Experimental Examples 13 to 19

[0051] Experimental Examples 13 to 19 used carbon dioxide sources other than K.sub.2CO.sub.3 and Na.sub.2CO.sub.3 which were used as the carbon dioxide sources in Experimental Examples 1 to 12.

[0052] Experimental Examples 13 to 19 used Rb.sub.2CO.sub.3, Cs.sub.2CO.sub.3, (NH.sub.4).sub.2CO.sub.3, NaHCO.sub.3, KHCO.sub.3, NH.sub.4HCO.sub.3, and KHCO.sub.3, respectively, in an amount of 0.1 M. Experimental Example 19 was performed in the same manner as in Experimental Example 1 except that 0.1 M of KOH was used and an aqueous solution of 50% by weight of water and 50% by weight of isopropanol was used as the solvent.

TABLE-US-00003 TABLE 3 CO.sub.2 Conv. Yield (%) Classification source pH (%) Gluconate Sorbitol FA Experimental R.sub.2CO.sub.3 11.7  52.8 45.5 5.8 29.8  Example 13 Experimental CS.sub.2CO.sub.3 11.8  55.8 43.4 5.9 26.7  Example 14 Experimental (NH.sub.4).sub.2CO.sub.3 8.8 30.3 16.3 2.5 0.5 Example 15 Experimental NaHCO.sub.3 8.0 18.2 14.0 4.1 0.4 Example 16 Experimental KHCO.sub.3 8.0 22.5 14.4 7.8 0.7 Example 17 Experimental NH.sub.4HCO.sub.3 7.8 23.2 16.9 2.1 0.4 Example 18 Experimental KHCO.sub.3 + 12.0  47.6 35.2 4.2 24.3  Example 19 KOH

[0053] Referring to Table 3, the yield of formic acid was high to be about 30% when Rb.sub.2CO.sub.3 or Cs.sub.2CO.sub.3 was used. When (NH).sub.4CO.sub.3, NaHCO.sub.3, KHCO.sub.3, or NH.sub.4HCO.sub.3 was used, the pH of the solution was low, resulting in that the glucose conversion rate and the yield of all products were extremely low.

[0054] When KOH was added to KHCO.sub.3 to adjust the pH of the solution to fall within the range presented by the present disclosure, the glucose conversion rate and the yield of all products were increased. From this result, it is confirmed that the pH of the solution during the reaction as well as the type of solvent is a principal factor.

Experimental Examples 20 to 24

[0055] Experimental Examples 20 to 24 were performed to check change in the yield with changing concentrations of alcohol. The total volume of the solvent was fixed to be the same as in Experimental Example 1, and an aqueous solution of water and isopropanol was used as the solvent. The results of the experiments were obtained by varying the weight ratio of isopropanol in the aqueous solution. (Experimental Example 1: 6 g of water, Experimental Example 20: 5.257 g of water and 0.584 g IPA, Experimental Example 21: 3.912 g of water and 1.677 g of IPA, Experimental Example 5: 2.641 g of water and 2.641 g of IPA, Experimental Example 22: 1.536 g of water and 3.585 g of IPA, Experimental Example 23: 0.482 g of water and 4.337 g of IPA, Experimental Example 24: 4.716 g of IPA). K.sub.2CO.sub.3 was used as the carbon dioxide source. In Experimental Examples 20 to 24, the pH of each of the solutions was about 11.8.

TABLE-US-00004 TABLE 4 Conv. Yield (%) Classification Solvent (%) Gluconate Sorbitol FA Experimental  0% by 48.0 35.6  5.8 2.3 Example 1  weight of IPA Experimental  10% by 45.9 35.4  3.8 9.2 Example 20 weight of IPA Experimental  30% by 51.5 41.0  5.0 18.0  Example 21 weight of IPA Experimental  50% by 53.8 42.5  6.3 30.5  Example 5  weight of IPA Experimental  70% by 46.9 32.8  4.7 18.2  Example 22 weight of IPA Experimental  90% by 51.8 21.4  5.1 4.2 Example 23 weight of IPA Experimental 100% by 22.2 8.7 2.2 1.0 Example 24 weight of IPA

[0056] Referring to the results of Table 4, the yield of FA changed according to the IPA content. The highest yield was obtained at 50% by weight of IPA. When the IPA content was reduced or increased than 50% by weight, the yield of FA decreased.

Experimental Examples 25 to 28

[0057] Experimental examples 25 to 28 were measurements of changes in the yield of FA according to the concentration of K.sub.2CO.sub.3 and the concentration of glucose. The solvent was an alcohol aqueous solution containing 50% by weight of water and 50% by weight of IPA. The total weight (g) of the solvent was fixed to be the same as in Experiment Example 1, and the concentration of K.sub.2CO.sub.3 and the concentration of glucose in the alcohol aqueous solution were changed as shown in Table 5 below.

TABLE-US-00005 TABLE 5 Conv. Yield (%) Classification Glucose K.sub.2CO.sub.3 pH (%) Gluconate Sorbitol FA Experimental 0.2 M 0.05 M 11.6 47.0 41.9 2.9 1.2 Example 25 Experimental 0.2 M  0.2 M 11.9 80.5 59.7 21.3  24.0  Example 26 Experimental 0.4 M  0.2 M 11.9 58.5 35.3 22.3  20.3  Example 27 Experimental   1 M  0.5 M 12.1 51.4 17.1 32.4  25.7  Example 28

[0058] Referring to Table 5, when the concentration of K.sub.2CO 3 was low, the pH was low and the ability to receive hydrogen was low, resulting in a low yield of formic acid. When the concentration of K.sub.2CO.sub.3 was high, the pH was high, resulting in a high yield of formic acid.

Experimental Examples 29 to 34

[0059] Experimental Examples 29 to 34 were performed in the same manner as in Experimental Examples 1 to 6 except that galactose or lactose was used as the hydrogen source. The results are shown in Table 6. In Experimental Examples 29 to 34, the pH of each of the solutions was about 11.8.

TABLE-US-00006 TABLE 6 Yield (%) Classification Solvent Conv.(%) Galactonate Dulcitol FA Experimental H.sub.2O 48.6 33.4 7.3 2.1 Example 29 Experimental 50% by 50.2 34.9 9.0 10.9 Example 30 weight of MeOH Experimental 50% by 54.9 37.4 10.5 20.8 Example 31 weight of EtOH Experimental 50% by 52.0 37.8 10.4 17.7 Example 32 weight of 1-propanol Experimental 50% by 55.9 39.5 12.0 22.5 Example 33 weight of IPA Experimental 50% by 50.0 36.0 10.3 14.6 Example 34 weight of t-BuOH

[0060] Referring to Table 6, the yield of formic acid was higher in a 50% alcohol solution than in water, as was the case with glucose, and similar tendencies were observed depending on the type of alcohol.

Experimental Examples 35 to 40

[0061] Experimental Examples 35 to 40 were performed in the same manner as in Experimental Examples 1 to 6 except that lactose was used as the hydrogen source. The results are shown in Table 7. In Experimental Examples 35 to 40, the pH of each of the solutions was about 11.8.

TABLE-US-00007 TABLE 7 Yield (%) Classification Solvent Conv.(%) Lactobionate Lactitol FA Experimental H.sub.2O 43.0 41.9 0.1 2.0 Example 35 Experimental 50% by 47.2 46.7 0.0 7.3 Example 36 weight of MeOH Experimental 50% by 64.9 44.5 4.5 17.5 Example 37 weight of EtOH Experimental 50% by 41.5 33.8 5.3 17.6 Example 38 weight of 1-propanol Experimental 50% by 45.8 35.7 6.1 20.4 Example 39 weight of IPA Experimental 50% by 41.2 37.8 3.3 17.6 Example 40 weight of t-BuOH

[0062] Referring to Table 7, even when lactose was used as the hydrogen source, as was the case with glucose or galactose, the yield of formic acid was higher in a 50% alcohol aqueous solution than in water, and similar tendencies were observed depending on the type of alcohol.

[0063] While the present disclosure has been described with reference to examples presented above, those skilled in the art will appreciate that the examples are presented only for illustrative purposes. On the contrary, it will be understood that various modifications and equivalents to the examples are possible. Accordingly, the technical scope of the present disclosure should be defined by the following claims.