Process for Producing Oxalic Acid

Abstract

A process for producing oxalic acid containing or having the following steps: i) Utilizing a chemical reaction to produce an alkali metal formate and/or alkaline earth metal formate; ii) Converting the alkali metal formate and/or alkaline earth metal formate to an alkali metal oxalate and/or alkaline earth metal oxalate in a thermal reaction, preferably utilizing hydrogen in the process; iii) Converting the alkali metal oxalate and/or alkaline earth metal oxalate to oxalic acid and an alkali metal base and/or alkaline earth metal base utilizing an electrochemical process; and iv) Recycling the alkali metal base and/or alkaline earth metal base from step (iii) to step (i).

Claims

1. A method for producing oxalic acid, comprising the following steps: i) Utilizing a chemical reaction to produce an alkali metal formate and/or alkaline earth metal formate; ii) Converting the alkali metal formate and/or alkaline earth metal formate to an alkali metal oxalate and/or alkaline earth metal oxalate in a thermal reaction, preferably utilizing hydrogen in the process; iii) Converting the alkali metal oxalate and/or alkaline earth metal oxalate to oxalic acid and an alkali metal base and/or alkaline earth metal base utilizing an electrochemical process; and iv) Recycling the alkali metal base and/or alkaline earth metal base from step (iii) to step (i).

2. The method according to claim 1, wherein step (i) comprises utilizing a chemical reaction to convert carbon, carbon monoxide, carbon dioxide, methane, hydrogen or a combination of any of these to thereby produce an alkali metal formate and/or alkaline earth metal formate.

3. The method according to claim 1, wherein the alkali metal base and/or alkaline earth metal base in step (iv) is recycled from step (iii) into step (i) in addition to hydrogen, oxygen, or chlorine.

4. The method according to claim 1, wherein step (i) further includes the use of an electrochemical cell for the reduction of carbon dioxide to formate.

5. The method according to claim 1, wherein step (i) comprises reacting carbon monoxide with an alkali metal hydroxide and/or an alkaline earth metal hydroxide to thereby produce the corresponding alkali metal formate and/or alkaline earth metal formate.

6. The method according to claim 1, wherein step (i) comprises reacting carbon monoxide with an alkali metal carbonate and/or an alkaline earth metal carbonate and with water to thereby produce the corresponding alkali metal formate and/or alkaline earth metal formate and carbon dioxide.

7. The method according to claim 1, wherein step (i) comprises reacting carbon monoxide with an alkali metal bicarbonate and/or an alkaline earth metal bicarbonate to thereby produce the corresponding alkali metal formate and/or alkaline earth metal formate and carbon dioxide.

8. The method according to claim 1, wherein step (i) comprises reacting a, preferably gaseous, formaldehyde with an alkali metal hydroxide and/or an alkaline earth metal hydroxide to thereby produce the corresponding alkali metal formate and/or alkaline earth metal formate and hydrogen, optionally including a side reaction wherein the, preferably gaseous, formaldehyde is converted to methanol.

9. The method according to claim 1, wherein step (i) comprises reacting carbon monoxide with steam to make formic acid and subsequently neutralize the formic acid with an alkali metal hydroxide and/or alkaline earth metal hydroxide to thereby produce the corresponding alkali metal formate and/or alkaline earth metal formate,

10. The method according to claim 1, wherein step (i) comprises reacting an alkali metal carbonate and/or an alkaline earth metal carbonate with hydrogen to thereby produce the corresponding alkali metal formate and/or alkaline earth metal formate and water.

11. The method according to claim 1, wherein step (i) comprises reacting carbon dioxide with hydrogen to thereby produce formic acid, and optionally subsequently neutralizing the formic acid with an alkali metal hydroxide and/or alkaline earth metal hydroxide to thereby produce the corresponding alkali metal formate and/or alkaline earth metal formate.

12. The method according to claim 1, wherein step (i) comprises reacting an alkali metal bicarbonate and/or an alkaline earth metal bicarbonate with hydrogen to thereby produce the corresponding alkali metal formate and/or alkaline earth metal formate and water.

13. The method according to claim 5, wherein the carbon monoxide is produced or obtained by: a reaction of carbon or biomass with carbon dioxide; a reaction of carbon or biomass with oxygen; a reaction of methane with water; and/or a reaction of carbon dioxide with hydrogen.

14. The method according to claim 8, wherein the hydrogen is produced or obtained by: a reaction of methane with water; and/or a reaction of carbon monoxide with water.

15. The method according to claim 1, wherein step (ii) comprises reacting the alkali metal formate and/or alkaline earth metal formate with molten hydroxide and carbon dioxide to thereby produce the corresponding alkali metal oxalate and/or alkaline earth metal oxalate.

16. The method according to claim 1, wherein step (i) comprises: making a mixture of alkali metal bicarbonate or carbonate and/or an alkaline earth metal bicarbonate or carbonate with an alkali metal hydroxide; melting the mixture; and bubbling hydrogen, carbon monoxide or carbon dioxide through the mixture or react the mixture in a reactor where pressurized hydrogen, carbon monoxide or carbon dioxide is introduced into the reactor to thereby produce the corresponding alkali metal formate and/or alkaline earth metal formate,

17. The method according to claim 1, wherein the oxalic acid is subsequently converted into mono-ethylene-glycol.

18. A method for the production of formic acid from CO.sub.2 and lactic acid from glycerol, comprising: a stage 1, wherein a metal M is reacted with carbon dioxide and water to thereby produce a metal oxide and formic acid; and a stage 2, wherein the metal oxide is reacted with glycerol to thereby produce metal, lactic acid and water, wherein the metal M is Iron, Zinc, Aluminium or Manganese and optionally an additional metal promotor is used.

19. A chemical method, comprising: utilizing syngas, carbon monoxide produced from carbon dioxide and hydrogen, and/or hydrogen in first producing an alkali metal formate-containing reaction product; separating the alkali metal formate from the alkali metal formate reaction product and converting the alkali metal formate into alkali metal formate solids or concentrated solutions; converting the alkali metal formate solids or concentrated solutions into alkali metal oxalates using a thermal reaction, which optionally produces byproduct hydrogen; dissolving the alkali metal oxalates in an aqueous solution and converting the oxalate to oxalic acid and an alkali metal hydroxide in an electrochemical process; converting the oxalic acid to monoethylene glycol (MEG) by esterification and hydrogenation.

20. The method of claim 19, wherein the electrochemical process comprises electrochemical acidification or electrodialysis.

Description

BRIEF DESCRIPTION OF THE DRAWINGS

[0017] The processes and systems of the invention are illustrated by the accompanying figures in which:

[0018] FIG. 1 illustrates an example of an integrated thermal and electrochemical process according to the invention using syngas to produce formate. It illustrates the use of syngas in a series flow through two separate CO and H.sub.2 formate reactors.

[0019] FIG. 2 illustrates an example of an integrated thermal and electrochemical process according to the invention using hydrogen (H.sub.2) to produce formate.

[0020] FIG. 3 illustrates an example of an integrated thermal and electrochemical process according to the invention using carbon monoxide (CO) to produce formate.

[0021] FIG. 4 shows alternative routes to formate using hydrogen

[0022] FIG. 5 shows alternative routes to formate using carbon monoxide.

DETAILED DESCRIPTION OF THE INVENTION

[0023] The present disclosure describes a process and system for a combined chemical and electrochemical process for the production of oxalic acid from carbon dioxide that can be subsequently converted to a downstream product such as monoethylene glycol (MEG).

[0024] Preferably the process according to the invention is an alternative process for producing oxalic acid having the following process steps: [0025] In a first step, utilizing of one or more chemical route reactions in producing alkali metal formate from a carbon, carbon dioxide, or methane and their combinations [0026] In a second step, converting of the alkali metal formate to an alkali metal oxalate in a thermal reaction and utilizing any co-products, such as hydrogen, in the process [0027] In a third step, converting the alkali metal oxalate to oxalic acid and an alkali metal base utilizing various electrochemical processs [0028] In a fourth step, recycling the alkali metal base from the electrochemical system back into the formate chemical route as needed in addition to any other suitable process co-products such as hydrogen, oxygen, or chlorine depending on the electrochemical cell anode and cathode reactions and its chemical feed(s)

[0029] That is, the process is preferably a process, wherein the alkali metal base and/or alkaline earth metal base in step (iv) is recycled from step (iii) into step (i) in addition to hydrogen, oxygen, or chlorine.

[0030] It is contemplated that the process may employ full or partial use of the electrochemical formate cells for the reduction of carbon dioxide to formate. That is, preferably the process is a process wherein step (i) further includes the use of an electrochemical cell for the reduction of carbon dioxide to formate.

[0031] In addition, the process may preferably consume more CO.sub.2 than may be produced using the process feed options available. The process raw materials may be chosen such that the entire process may be operated on a commercial scale and may have suitable economics. The formation and use of alkali metal formate may be preferred, but the formation and use of alkaline earth formates using reagents such as calcium hydroxide or calcium carbonate, may also be employed, so as long as a good process of separation and recycle of the alkaline earth metals with minimal generation of wastes may be designed. Hence, hereafter, wherever an alkali metal compound is described, an alkaline earth metal compound, although less preferred, may also be used.

[0032] Chemical Reactants for Formate Formation

[0033] Various chemical feed stocks may be suitable in the chemical formation of alkali metal formate. The chemical reactions with proposed and theorized chemical reactions are summarized below.

[0034] CO Reactions

[0035] Carbon monoxide (CO) is a very reactive reagent that is useful in carbonylation reactions.

a. CO Reaction with Alkali Metal Hydroxide, for example:

CO+KOH.fwdarw.KCO.sub.2H

[0036] This is a reaction for producing alkali metal formate. The CO source may be from various sources such as Syngas, RWGS reaction, and the like. The reaction operating temperature may range from 50 C. to 300 C. at pressures between 50 to 2,000 psig. Processs to increase the reaction rate may employ packed bed towers with counter flow of CO as well as employing reactive spray drying equipment. Catalysts may be optionally employed and the reaction may employ an aqueous or an aqueous system with an added solvent, such as an alcohol, to help improve the reaction rate. The solvent would be recovered and recycled in a separate step. Solid state reactions with a wetted alkali metal hydroxide may also be suitable with a sufficient mixing/reaction system.

That is, step (i) of the process according to the invention may comprise or consist of reacting carbon monoxide with an alkali metal hydroxide and/or an alkaline earth metal hydroxide to thereby produce the corresponding alkali metal formate and/or alkaline earth metal formate.
b. CO Reaction with Alkali Metal Carbonate, for example:

K.sub.2CO.sub.3+2CO+H.sub.2O.fwdarw.2KCO.sub.2H+CO.sub.2

[0037] The reaction operating temperature for this reaction may range from 100 C. to 300 C. at pressures between 50 to 2,000 psig. Processs of increasing the reaction rate may employ packed bed towers with counter flow of CO as well as employing reactive spray drying equipment. Catalysts may be optionally employed and the reaction may employ an aqueous or an aqueous system with an added solvent, such as an alcohol, to help improve the reaction rate. The solvent would be recovered and recycled in a separate step. Solid state reactions with a wetted alkali metal carbonate may also be suitable with a sufficient mixing/reaction system.

That is, step (i) of the process according to the invention may comprise or consist of reacting carbon monoxide with an alkali metal carbonate and/or an alkaline earth metal carbonate and with water to thereby produce the corresponding alkali metal formate and/or alkaline earth metal formate and carbon dioxide.
c. CO Reaction with Alkali Metal Bicarbonate (also referred to as Akali Metal Hydrogen Carbonate), for example:

KHCO.sub.3+CO.fwdarw.KCO.sub.2H+CO.sub.2

[0038] This reaction may or may not require a catalyst. If both CO and hydrogen are used as the reactant gas (a water gas composition), the reaction may occur with or without a nickel catalyst which may help with the reaction with hydrogen, and then both gases may react to form formate, and requiring less CO in the reaction. The reaction operating temperature may range from 100 C. to 350 C. at pressures between 50 to 5,000 psig. Catalysts may be optionally employed and the reaction may employ an aqueous or an aqueous system with an added solvent, such as an alcohol to help improve the reaction rate. The solvent would be recovered and recycled in a separate step. Solid state reactions with wetted alkali metal bicarbonate may be suitable with a sufficient mixing/reaction system.

That is, step (i) of the process according to the invention may comprise or consist of reacting carbon monoxide with an alkali metal bicarbonate and/or an alkaline earth metal bicarbonate to thereby produce the corresponding alkali metal formate and/or alkaline earth metal formate and carbon dioxide.
d. Formaldehyde (gas) Reaction with Alkali Metal Hydroxide

HCHO(g)+KOH.fwdarw.KCO.sub.2H+H.sub.2

HCHO(g).fwdarw.CH.sub.3OH(aq) Side reaction

[0039] This reaction operating temperature may range from 20 C. to 150 C. at pressures between 0.1 and 500 psig. The reaction of formaldehyde forming methanol is a side reaction that may be minimized using lower reaction temperatures. Catalysts may be optionally employed and the reaction may employ an aqueous or an aqueous system with an added solvent, such as an alcohol to help improve the reaction rate. The system may also be totally non-aqueous using one or more solvents. The solvent would be recovered and recycled in a separate step. That is, step (i) of the process according to the invention may comprise or consist of reacting a, preferably gaseous, formaldehyde with an alkali metal hydroxide and/or an alkaline earth metal hydroxide to thereby produce the corresponding alkali metal formate and/or alkaline earth metal formate and hydrogen, optionally including a side reaction wherein the, preferably gaseous, formaldehyde is converted to methanol.

e. CO Reaction with Steam to Make Formic Acid and Neutralize with Alkali Metal Hydroxide

[0040] This reaction requires a high temperature and pressure in addition to a catalyst in the formation of the formic acid. The reaction operating temperature may range from 100 C. to 350 C. at pressures between 50 to 5,000 psig. Catalysts such as the phosphates of zinc, calcium, magnesium, sodium, potassium, copper, and cerium as well as the acid salts of these formed with the oxides of tungsten and molybdenum and mixtures.

CO+H.sub.2O.fwdarw.HCO.sub.2H (with Catalyst)Reaction 1

HCO.sub.2H+KOH.fwdarw.KCO.sub.2H+H.sub.2OReaction 2

That is, step (i) of the process according to the invention may comprise or consist of reacting carbon monoxide with steam to make formic acid and subsequently neutralize the formic acid with an alkali metal hydroxide and/or alkaline earth metal hydroxide to thereby produce the corresponding alkali metal formate and/or alkaline earth metal formate.
f. Alkali Metal Carbonate with Hydrogen

K.sub.2CO.sub.3+2H.sub.2.fwdarw.2KCO.sub.2H+H.sub.2O

[0041] This reaction operating temperature may range from 100 C. to 300 C. at pressures between 50 to 2,000 psig. The reaction may require a catalyst to work efficiently. The catalyst may be a homogeneous or heterogeneous type.

That is, step (i) of the process according to the invention may comprise or consist of reacting an alkali metal carbonate and/or an alkaline earth metal carbonate with hydrogen to thereby produce the corresponding alkali metal formate and/or alkaline earth metal formate and water.

[0042] Hydrogen Reactions

[0043] Hydrogen is a reactive reagent that has been used for the reduction of many chemicals.

a. Carbon Dioxide (CO.sub.2) Reaction with Hydrogen (H.sub.2)

CO.sub.2+H.sub.2.fwdarw.HCO.sub.2H

[0044] The reaction operating temperature of this reaction may range from 100 C. to 500 C. at pressures between 50 to 5,000 psig. The reaction requires a catalyst for the reaction to work efficiently. The catalyst may be a homogeneous or heterogeneous type. The use of a base, such as carbonate, hydroxide, tertiary amine and the like helps promote the reaction.

That is, step (i) of the process according to the invention may comprise or consist of reacting carbon dioxide with hydrogen to thereby produce formic acid, and optionally subsequently neutralizing the formic acid with an alkali metal hydroxide and/or alkaline earth metal hydroxide to thereby produce the corresponding alkali metal formate and/or alkaline earth metal formate.
b. Alkali Metal Carbonate Reaction with Hydrogen

K.sub.2CO.sub.3+2H.sub.22KCO.sub.2H+H.sub.2O

[0045] As described above, the reaction operating temperature of this reaction may range from 100 C. to 300 C. at pressures between 50 to 2,000 psig. Catalysts may be optionally employed and the reaction may employ an aqueous or an aqueous system with an added solvent, such as an alcohol to help improve the reaction rate. The system may also be totally non-aqueous using one or more solvents. The solvent would be recovered and recycled in a separate step. The catalyst may be a homogeneous or heterogeneous type. A heterogeneous catalyst is preferred such that little or no catalyst may end up in the final product.

c. Alkali Metal Bicarbonate Reaction with Hydrogen

KHCO.sub.3+H.sub.2.fwdarw.KCO.sub.2H+H.sub.2O

[0046] The reaction operating temperature of this reaction may range from 100 C. to 300 C. at pressures between 50 to 2,000 psig. Catalysts may be optionally employed and the reaction may employ an aqueous or an aqueous system with an added solvent, such as an alcohol to help improve the reaction rate. The system may also be totally non-aqueous using one or more solvents. The solvent would be recovered and recycled in a separate step. The catalyst may be a homogeneous or heterogeneous type. A heterogeneous catalyst is preferred such that little or no catalyst may end up in the final product.

That is, step (i) of the process according to the invention may comprise or consist of reacting an alkali metal bicarbonate and/or an alkaline earth metal bicarbonate with hydrogen to thereby produce the corresponding alkali metal formate and/or alkaline earth metal formate and water.

[0047] CO and Hydrogen From Syngas and Water Gas Reactions

a. Carbon or biomass may advantageously be converted to CO utilizing CO.sub.2 using the Boudouard reaction as follows:

C(s)+CO.sub.2.fwdarw.2CO

b. Carbon or biomass may be converted to CO utilizing pure O2, such as from the electrochemical cells or using PSA (Pressure Swing Absorption) to generate it from air as follows:

C(s)+O.sub.2.fwdarw.2CO

c. Syngas formation from methane as follows, generating both CO and H.sub.2 which can be further processed:

CH.sub.4+H.sub.2O.fwdarw.CO+3H.sub.2

d. Reverse Water Gas Shift (RWGS) Reaction as follows, making CO from CO.sub.2 and hydrogen:

CO.sub.2+H.sub.2.fwdarw.CO+H.sub.2O

e. Water Gas Shift Reaction (WGSR) as follows, making H2 from CO and water:

CO+H.sub.2O.fwdarw.CO.sub.2+H.sub.2

That is, the carbon monoxide that may potentially be used in the process according to the invention may conveniently be produced or obtained by:

[0048] a reaction of carbon or biomass with carbon dioxide;

[0049] a reaction of carbon or biomass with oxygen;

[0050] a reaction of methane with water; and/or

[0051] a reaction of carbondioxide with hydrogen.

In addition, the hydrogen that may potentially be used in the process according to the invention may conveniently be produced or obtained by:

[0052] a reaction of methane with water; and/or

[0053] a reaction of carbon monoxide with water.

[0054] Step (ii) of the process according to the invention may conveniently comprise or consist of reacting the alkali metal formate and/or alkaline earth metal formate with molten hydroxide and carbon dioxide to thereby produce the corresponding alkali metal oxalate and/or alkaline earth metal oxalate.

[0055] Molten hydroxide may react with CO.sub.2 and alkali metal formate to produce alkali metal oxalate. The addition of CO.sub.2 is added as a reactant gas in a pressurized reactor and elevated temperature to produce oxalate. The reaction that may occur is the reaction of one formate, perhaps as the dianion, with one CO2 or one alkali metal carbonate to produce one oxalate. The reaction may be more effective than reacting two formates to make one oxalate.

[0056] The alkali metal formate (or formate dianion) in step (i) may also be produced in different alternative manners.

[0057] For example by a carbon dioxide (CO.sub.2) reaction with a thermal melt. That is, one may: make a mixture of alkali metal bicarbonate or carbonate with an alkali metal hydroxide; melt the mixture; and bubble CO.sub.2 through the mixture or react the mixture in a reactor where pressurized CO.sub.2 is introduced into the reactor. In this embodiment, the alkali metal formate (or formate dianion) is produced in the reactor mix.

[0058] Or for example by a carbon monoxide (CO) reaction with a thermal melt. That is, one may: make a mixture of alkali metal bicarbonate or carbonate with an alkali metal hydroxide; melt the mixture; and bubble CO through the mixture or react the mixture in a reactor where pressurized CO is introduced into the reactor. The reaction may occur in a pressurized packed bed reactor. Formate may be produced which would react and convert to make alkali metal oxalate. The formate may also react with the carbonate and bicarbonate in the presence of the hydroxide to produce oxalate.

[0059] Or for example by a hydrogen reaction with a thermal melt. That is, one may: make a mixture of mixture of alkali metal bicarbonate or carbonate with an alkali metal hydroxide; melt the mixture; and bubble hydrogen through the mixture or react the mixture in a reactor where pressurized hydrogen is introduced into the reactor. The reaction may occur in a pressurized packed bed reactor. Formate may be produced which would react and convert to make alkali metal oxalate. The formate may also react with the carbonate and bicarbonate in the presence of the hydroxide to produce oxalate.

[0060] Or for example by a carbon monoxide (CO) and hydrogen reaction with a thermal melt. That is, one may: make a mixture of mixture of alkali metal bicarbonate or carbonate with an alkali metal hydroxide; melt the mixture; and bubble a mixture of CO and hydrogen through the mixture or react the mixture in a reactor where pressurized CO and hydrogen is introduced into the reactor. The reaction may occur in a pressurized packed bed reactor. Formate may be produced which would react and convert to make alkali metal oxalate. The formate may also react with the carbonate and bicarbonate in the presence of the hydroxide to produce oxalate.

[0061] All of the embodiments may utilize a catalyst, a homogeneous or heterogeneous catalyst. The reaction may also include other additives such as organics that may improve the yield of the reaction or to conceptually produce C2and higher organic compounds from the reaction mixture. In addition, the reaction may alternatively occur in an aqueous solution mixture which may also include some amount of an organic solvent, such as an alcohol, or may be mainly a nonaqueous solution. The temperatures of the reaction may be lower, and the solvents may be recovered or may be part of the reactions to do CC coupling.

[0062] The invention further advantageously provides several routes to value added chemicals from CO.sub.2 and bio-glycerol with non-precious metal/metal oxide redox cycles

[0063] Hydrogenation of CO.sub.2 will not only reduce the amount of CO.sub.2 linked to environmental problems but also produce the useful chemicals and fuels. A carbon redox cycle that couples CO.sub.2 hydrogenation with simultaneous oxidation of bio-based renewables (e.g. glycerol) into industrially important chemicals possess additional advantages of monetizing two wastes without requiring direct electrical energy. Thus, reducing CO.sub.2 with biochemical reductants will have major impact on the energy landscape from a number of viewpoints and will also provide sustainable green chemicals for numerous industries.

[0064] The present invention further provides a process for the production of formic acid from CO.sub.2 and lactic acid from glycerol. Below indicative steps are provided for such process. These steps or stages are not intended to be limiting, but indicative only.

[0065] Indicative Step/Stage 1: CO.sub.2 to Formic acid/Formate:

[0066] A hydrothermal reactor may produce (formic acid) or potassium formate by oxidizing earth abundant non-precious metal(s) as reductant(s). Metal oxide formed after the reaction may be used in a glycerol reactor and formate produced on the cathode is moved further to make MEG.

[0067] Indicative Step/Stage 2: Lactic acid production

[0068] Metal oxide from Step/Stage 1 may be used for the catalytic oxidation of glycerol to form lactic acid. Alkali metal hydroxide may be required as a catalyst for this reaction. Lactic acid can be further processed to make biopolymers.

[0069] Without wishing to be bound by any kind of theory, it is believed that indicative reactions and stoichiometry could be:

M+CO.sub.2+H.sub.2O.fwdarw.MO.sub.x+HCOOHStep/Stage 1.

MO.sub.x+C.sub.3H.sub.8O.sub.3.fwdarw.M+C.sub.3H.sub.6O.sub.3+H.sub.2OStep/Stage 2.

CO.sub.2+C.sub.3H.sub.8O.sub.3.fwdarw.HCOOH+C.sub.3H.sub.6O.sub.3Overall:

M=Fe, Zn, Al, Mn and additional metal promotor can be used to improve reaction rate and efficiency.

[0070] Without wishing to be bound by any kind of theory it is believed that CO or carbon monoxide is a very reactive reagent that can be useful in carbonylation reactions.

[0071] There are a number of advantages which may include:

[0072] Options for using CO.sub.2 directly to obtain formic acid or Alkali hydroxide (e.g. KOH from EA cell)+CO.sub.2 to obtain formate salt in step 1.

[0073] The reducing agent for CO.sub.2 is glycerol (or any other bio-organics that can reduce metal oxide to metal)

[0074] KOH from the EA cell can be utilized as a catalyst

[0075] Step 1 proceeds through quantitative H2 production from water and reacted in-situ with CO.sub.2.

[0076] The present invention further provides a chemical process utilizing syngas, carbon monoxide produced from carbon dioxide and hydrogen, and/or hydrogen in first producing an alkali metal formate product. The chemical reactions may be as follows: [0077] a. reacting of CO with an alkali metal carbonate to produce the corresponding alkali metal formate. The CO may be produced from the RWGS reaction of carbon dioxide with hydrogen. Reactions may include: [0078] i. CO reaction with alkali metal carbonate:

K.sub.2CO.sub.3+2CO+H.sub.2O.fwdarw.2KCO.sub.2H+CO.sub.2 [0079] ii. CO reaction with alkali metal bicarbonate

KHCO.sub.3+CO.fwdarw.KCO.sub.2H+CO.sub.2 [0080] iii. RWGS Reaction:

CO.sub.2 +H.sub.2.fwdarw.CO+H.sub.2O [0081] b. reacting of an alkali metal bicarbonate with hydrogen to produce the corresponding alkali metal formate, using a catalyst as needed. Alkali metal carbonate may also be converted to alkali metal formate, but may not be as reactive.

KHCO.sub.3+H.sub.2.fwdarw.KCO.sub.2H+H.sub.2O These reactions a. and b. are preferably operated in reactions using an aqueous phase, but the aqueous solution may include other non-reactive solvents. Ionic liquids, amines, and other added components may be used in the solution to promote the reaction. [0082] c. utilization of methane, that may be converted to syngas, which is a product mixture typically containing CO and H.sub.2 with the basic reaction as follows using a catalyst:

CH.sub.4+H.sub.2O.fwdarw.CO+3H.sub.2

[0083] Preferably the alkali metal formate is separated from the reaction product mixtures and converted to alkali metal formate solids or concentrated solutions.

[0084] The alkali metal formate solids or concentrated solutions (used in a spray drying conversion process) can suitably be converted into alkali metal oxalates using a thermal reaction, which may also produce byproduct hydrogen that can be recovered for use in the other process steps.

[0085] The alkali metal oxalates can be dissolved in an aqueous solution and the oxalate can be converted to oxalic acid and an alkali metal hydroxide in an electrochemical process such as electrochemical acidification or electrodialysis.

[0086] The electrochemical acidification cell can produce oxalic acid, an anolyte co-product, an alkali metal hydroxide, and hydrogen from the catholyte.

[0087] The electrodialysis cell can produce oxalic acid and alkali metal hydroxide and can utilize bipolar membranes.

[0088] Conveniently the oxalic acid can then be converted to monoethylene glycol (MEG) via an esterification route followed by hydrogenation.

[0089] In one embodiment, the process may employ methane as a feedstock, which may be from a biological source, which may be converted to Syngas. The gas from the reactor may then be passed through a set of CO and H.sub.2 based formate reactors in a series flow arrangement. The reactors may be set up with separate alkali metal carbonate and alkali metal bicarbonate feeds so that the CO in the Syngas may react with the alkali metal carbonate in a first reactor and the remaining gas, containing hydrogen and some unreacted CO, and may then be passed onto a second reactor containing alkali metal bicarbonate, with a heterogeneous catalyst as needed, to form alkali metal formate. The gases may be recycled around each reactor to enable high conversion of the Syngas components. Two CO.sub.2 reactors may be used to provide the alkali metal carbonate and bicarbonate feed to the corresponding reactor from the alkali metal hydroxide. The alkali metal formate production of each reactor is related to the ratio of the CO to H.sub.2 in the Syngas gas stream. The CO and H.sub.2 alkali formate reactors may operate at pressures between 10 to 5,000 psig and at temperatures ranging from 50 C. to 500 C.

[0090] In another embodiment, biological sourced CO.sub.2 may be converted to CO in a separate RWGS reactor to convert alkali metal carbonate to alkali metal formate. The hydrogen from the electrochemical acidification cell may be used in a separate reactor to convert alkali metal bicarbonate to alkali metal formate. The production of the alkali metal formate may depend on the quantities of hydrogen and CO available in the process.

[0091] In a further embodiment, a carbon source, such as carbon or biomass may be converted to CO utilizing CO.sub.2 using the Boudouard reaction as follows:

C(s)+CO.sub.2.fwdarw.2CO

[0092] In another embodiment, a carbon source, such as carbon or biomass may be converted to CO utilizing a limited amount of O.sub.2. The oxygen source may be from the electrochemical acidification cell anolyte reaction or from pressure swing absorption oxygen enrichment units (PSA).

C(s)+O.sub.2.fwdarw.2CO

[0093] The processes of the invention are further illustrated by the following non-limiting figures.

[0094] FIG. 1, shows one embodiment where syngas may be produced from methane, where the methane to the Syngas reactor may be from a biological or biomass source.

[0095] FIG. 2, shows an integrated process via hydrogen.

[0096] FIG. 3, shows an integrated process via carbon monoxide

[0097] FIG. 4 illustrates alternative thermal routes to formate using hydrogen

[0098] FIG. 5 illustrates alternative thermal routes to formate using carbon monoxide.

[0099] As described above, carbon monoxide and hydrogen from Syngas and water-gas shift reaction may also be used.

[0100] It may be believed that the present disclosure and many of its attendant advantages will be understood by the foregoing description, and it will be apparent that various changes may be made in the form, construction and arrangement of the components without departing from the subject matter or without sacrificing all of its material advantages. The form described may be merely explanatory.