WO2013134418A1 - Réduction du dioxyde de carbone en produits - Google Patents

Réduction du dioxyde de carbone en produits Download PDF

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Publication number
WO2013134418A1
WO2013134418A1 PCT/US2013/029425 US2013029425W WO2013134418A1 WO 2013134418 A1 WO2013134418 A1 WO 2013134418A1 US 2013029425 W US2013029425 W US 2013029425W WO 2013134418 A1 WO2013134418 A1 WO 2013134418A1
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Prior art keywords
cathode
carbon dioxide
cell compartment
products
cell
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PCT/US2013/029425
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English (en)
Inventor
Emily Barton Cole
Narayanappa Sivasankar
Rishi Parajuli
Kate A. Keets
Kunttal Keyshar
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Liquid Light, Inc.
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Application filed by Liquid Light, Inc. filed Critical Liquid Light, Inc.
Priority to EP13757264.0A priority Critical patent/EP2823090A4/fr
Priority to AU2013231005A priority patent/AU2013231005A1/en
Priority to KR1020147024882A priority patent/KR20140138153A/ko
Priority to CA2864611A priority patent/CA2864611A1/fr
Priority to JP2014561087A priority patent/JP2015513616A/ja
Priority to CN201380011453.8A priority patent/CN104204301A/zh
Publication of WO2013134418A1 publication Critical patent/WO2013134418A1/fr

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    • C—CHEMISTRY; METALLURGY
    • C25—ELECTROLYTIC OR ELECTROPHORETIC PROCESSES; APPARATUS THEREFOR
    • C25B—ELECTROLYTIC OR ELECTROPHORETIC PROCESSES FOR THE PRODUCTION OF COMPOUNDS OR NON-METALS; APPARATUS THEREFOR
    • C25B1/00—Electrolytic production of inorganic compounds or non-metals
    • C—CHEMISTRY; METALLURGY
    • C25—ELECTROLYTIC OR ELECTROPHORETIC PROCESSES; APPARATUS THEREFOR
    • C25B—ELECTROLYTIC OR ELECTROPHORETIC PROCESSES FOR THE PRODUCTION OF COMPOUNDS OR NON-METALS; APPARATUS THEREFOR
    • C25B3/00—Electrolytic production of organic compounds
    • C25B3/20—Processes
    • C25B3/25—Reduction
    • C—CHEMISTRY; METALLURGY
    • C25—ELECTROLYTIC OR ELECTROPHORETIC PROCESSES; APPARATUS THEREFOR
    • C25B—ELECTROLYTIC OR ELECTROPHORETIC PROCESSES FOR THE PRODUCTION OF COMPOUNDS OR NON-METALS; APPARATUS THEREFOR
    • C25B1/00—Electrolytic production of inorganic compounds or non-metals
    • C25B1/50—Processes
    • C25B1/55—Photoelectrolysis
    • C—CHEMISTRY; METALLURGY
    • C25—ELECTROLYTIC OR ELECTROPHORETIC PROCESSES; APPARATUS THEREFOR
    • C25B—ELECTROLYTIC OR ELECTROPHORETIC PROCESSES FOR THE PRODUCTION OF COMPOUNDS OR NON-METALS; APPARATUS THEREFOR
    • C25B11/00—Electrodes; Manufacture thereof not otherwise provided for
    • C25B11/04—Electrodes; Manufacture thereof not otherwise provided for characterised by the material
    • C25B11/042—Electrodes formed of a single material
    • C25B11/046—Alloys
    • C—CHEMISTRY; METALLURGY
    • C25—ELECTROLYTIC OR ELECTROPHORETIC PROCESSES; APPARATUS THEREFOR
    • C25B—ELECTROLYTIC OR ELECTROPHORETIC PROCESSES FOR THE PRODUCTION OF COMPOUNDS OR NON-METALS; APPARATUS THEREFOR
    • C25B15/00—Operating or servicing cells
    • C25B15/08—Supplying or removing reactants or electrolytes; Regeneration of electrolytes
    • C25B15/083—Separating products
    • C—CHEMISTRY; METALLURGY
    • C25—ELECTROLYTIC OR ELECTROPHORETIC PROCESSES; APPARATUS THEREFOR
    • C25B—ELECTROLYTIC OR ELECTROPHORETIC PROCESSES FOR THE PRODUCTION OF COMPOUNDS OR NON-METALS; APPARATUS THEREFOR
    • C25B9/00—Cells or assemblies of cells; Constructional parts of cells; Assemblies of constructional parts, e.g. electrode-diaphragm assemblies; Process-related cell features
    • C25B9/17—Cells comprising dimensionally-stable non-movable electrodes; Assemblies of constructional parts thereof
    • C25B9/19—Cells comprising dimensionally-stable non-movable electrodes; Assemblies of constructional parts thereof with diaphragms

Definitions

  • the present invention relates to chemical reduction generally and, more particularly, to a method and/or apparatus for implementing reducing carbon dioxide to products.
  • a mechanism for mitigating emissions is to convert carbon dioxide into economically valuable materials such as fuels and industrial chemicals. If the carbon dioxide is converted using energy from renewable sources, both mitigation of carbon dioxide emissions and conversion of renewable energy into a chemical form that can be stored for later use will be possible. Electrochemical and photochemical pathways are means for the carbon dioxide conversion.
  • the present disclosure concerns methods for reducing carbon dioxide to one or more products.
  • the methods may include steps (A) to (C).
  • Step (A) may bubble the carbon dioxide into a solution of an electrolyte and a catalyst in a divided electrochemical cell.
  • the divided electrochemical cell may include an anode in a first cell compartment and a cathode in a second cell compartment. The cathode generally reduces the carbon dioxide into the products.
  • Step (B) may adjust one or more of (a) a cathode material, (b) a surface morphology of said cathode, (c) said electrolyte, (d) a manner in which said carbon dioxide is bubbled, (e), a pH level of said solution, and (f) an electrical potential of said divided electrochemical cell, to vary at least one of (i) which of said products is produced and (ii) a faradaic yield of said products.
  • Step (C) may separate the products from the solution.
  • the present disclosure concerns a system for electrochemical reduction of carbon dioxide.
  • the system may include an electrochemical cell, which may include a first cell compartment, an anode positioned within said first cell compartment, a second cell compartment, a separator interposed between said first cell compartment and said second cell compartment.
  • the second cell compartment may contain an electrolyte.
  • the electrochemical cell may include a cathode within said second cell compartment.
  • the cathode may be selected from the group consisting of n-GaAs, SS304, n-Ge, C0 2 O 4 , Rh, and mixtures thereof.
  • the system may also include an energy source operably coupled with said anode and said cathode.
  • the energy source may be configured to apply a voltage between said anode and said cathode to reduce carbon dioxide at said cathode to at least one of acetate, acetic acid, glycolate, and glycolic acid.
  • the present disclosure concerns a system for electrochemical reduction of carbon dioxide.
  • the system may include an electrochemical cell, which may include a first cell compartment, an anode positioned within said first cell compartment, a second cell compartment, a separator interposed between said first cell compartment and said second cell compartment.
  • the second cell compartment may contain an electrolyte.
  • the electrochemical cell may include a cathode and a homogenous catalyst positioned within said second cell compartment.
  • the cathode may comprise tin (Sn).
  • the catalyst may include at least one of pyridine, 2-picoline or 2,6-lutidine.
  • the system may also include an energy source operably coupled with said anode and said cathode.
  • the energy source may be configured to apply a voltage between said anode and said cathode to reduce carbon dioxide at said cathode to at least one of formate or formic acid.
  • Step (A) may introduce an anolyte to a first compartment of an electrochemical cell, said first compartment including an anode.
  • Step (B) may introduce a catholyte and carbon dioxide to a second compartment of said electrochemical cell.
  • the second compartment may include a tin cathode and a catalyst.
  • the catalyst may include at least one of pyridine, 2-picoline or 2,6-lutidine.
  • Step (C) may apply an electrical potential between said anode and said cathode sufficient for said cathode to reduce said carbon dioxide to at least one of formate or formic acid.
  • FIG. 1 is a block diagram of a system in accordance with a preferred embodiment of the present invention.
  • FIGS. 2A-2C are tables illustrating relative product yields for different cathode material, catalyst, electrolyte and pH level combinations
  • FIG. 3 is a formula of an aromatic heterocyclic amine catalyst
  • FIGS. 4-6 are formulae of substituted or unsubstituted aromatic 5-member heterocyclic amines or 6-member heterocyclic amines;
  • FIG. 7 is a flow diagram of an example method used in electrochemical examples.
  • FIG. 8 is a flow diagram of an example method used in photochemical examples.
  • an electro-catalytic system that generally allows carbon dioxide to be converted at modest overpotentials to highly reduced species in an aqueous solution.
  • Some embodiments generally relate to simple, efficient and economical conversion of carbon dioxide to reduced organic products, such as methanol, formic acid and formaldehyde.
  • Inorganic products such as polymers may also be formed.
  • Carbon-carbon bonds and/or carbon-hydrogen bonds may be formed in the aqueous solution under mild conditions utilizing a minimum of energy.
  • the energy used by the system may be generated from an alternative energy source or directly using visible light, depending on how the system is implemented.
  • the reduction of carbon dioxide may be suitably catalyzed by aromatic heterocyclic amines (e.g., pyridine, imidazole and substituted derivatives).
  • Simple organic compounds have been found to be effective and stable homogenous electrocatalysts and photoelectrocatalysts for the aqueous multiple electron, multiple proton reduction of carbon dioxide to organic products, such as formic acid, formaldehyde and methanol.
  • organic products such as formic acid, formaldehyde and methanol.
  • the reduction of carbon dioxide may proceed along a electron (e-) transfer pathway.
  • High faradaic yields for the reduced products have generally been found in both electrochemical and photoelectrochemical systems at low reaction overpotentials.
  • Metal-derived multi-electron transfer was previously thought to achieve highly reduced products such as methanol.
  • simple aromatic heterocyclic amine molecules may be capable of producing many different chemical species on route to methanol through multiple electron transfers, instead of metal-based multi-electron transfers.
  • Some embodiments of the present invention thus relate to environmentally beneficial methods for reducing carbon dioxide.
  • the methods generally include electrochemically and/or photoelectrochemically reducing the carbon dioxide in an aqueous, electrolyte-supported divided electrochemical cell that includes an anode (e.g., an inert conductive counter electrode) in a cell compartment and a conductive or p-type semiconductor working cathode electrode in another cell compartment.
  • a catalyst may be included to produce a reduced product.
  • Carbon dioxide may be continuously bubbled through the cathode electrolyte solution to saturate the solution.
  • the electrode may be a suitable conductive electrode, such as Al, Au, Ag, Bi, C, Cd, Co, Cr, Cu, Cu alloys (e.g., brass and bronze), Ga, Hg, In, Mo, Nb, Ni, NiCo 2 0 4 , Ni alloys (e.g., Ni 625, NiHX), Ni-Fe alloys, Pb, Pd alloys (e.g., PdAg), Pt, Pt alloys (e.g., PtRh), Rh, Sn, Sn alloys (e.g., SnAg, SnPb, SnSb), Ti, V, W, Zn, stainless steel (SS) (e.g., SS 2205, SS 304, SS 316, SS 321), austenitic steel, ferritic steel, duplex steel, martensitic steel, Nichrome (e.g., NiCr 60: 16 (with Fe)), elgilo
  • the electrode may be a p-type semiconductor, such as p- GaAs, p-GaP, p-InN, p-InP, p-CdTe, p-GaInP 2 and p-Si, or an n-type semiconductor, such as n-GaAs, n-GaP, n-InN, n-InP, n-CdTe, n-GaInP 2 and n-Si.
  • p-type semiconductor such as p- GaAs, p-GaP, p-InN, p-InP, p-CdTe, p-GaInP 2 and p-Si
  • n-GaAs such as n-GaP, n-InN, n-InP, n-CdTe, n-GaInP 2 and n-Si.
  • the catalyst for conversion of carbon dioxide electrochemically or photoelectrochemically may be a substituted or unsubstituted aromatic heterocyclic amine.
  • Suitable amines are generally heterocycles which may include, but are not limited to, heterocyclic compounds that are 5 -member or 6-member rings with at least one ring nitrogen.
  • heterocyclic compounds that are 5 -member or 6-member rings with at least one ring nitrogen.
  • pyridines, imidazoles and related species with at least one five-member ring, bipyridines (e.g., two connected pyridines) and substituted derivatives were generally found suitable as catalysts for the electrochemical reduction and/or the photoelectrochemical reduction.
  • Amines that have sulfur or oxygen in the rings may also be suitable for the reductions.
  • Amines with sulfur or oxygen may include thiazoles or oxazoles.
  • Other aromatic amines e.g., quinolines, adenine, azoles, indoles, benzimidazole and 1, 10-phenanthroline
  • Carbon dioxide may be photochemically or electrochemically reduced to formic acid with formaldehyde and methanol being formed in smaller amounts.
  • Catalytic hydrogenation of carbon dioxide using heterogeneous catalysts generally provides methanol together with water as well as formic acid and formaldehyde.
  • the reduction of carbon dioxide to methanol with complex metal hydrides, such as lithium aluminum hydrides, may be costly and therefore problematic for bulk production of methanol.
  • Current reduction processes are generally highly energy-consuming and thus are not efficient ways for a high yield, economical conversion of carbon dioxide to various products.
  • the use of processes for converting carbon dioxide to reduced organic and/or inorganic products in accordance with some embodiments of the invention generally has the potential to lead to a significant reduction of carbon dioxide, a major greenhouse gas, in the atmosphere and thus to the mitigation of global warming.
  • some embodiments may advantageously produce methanol and related products without adding extra reactants, such as a hydrogen source.
  • the resultant product mixture may use little in the way of further treatment.
  • a resultant 1 molar (M) methanol solution may be used directly in a fuel cell.
  • simple removal of the electrolyte salt and water may be readily accomplished.
  • process steps may be carried out over a range of temperatures (e.g., approximately 10°C (Celsius) to 50°C) and a range of pressures (e.g., approximately 1 to 10 atmospheres) unless otherwise specified.
  • Numerical ranges recited herein generally include all values from the lower value to the upper value (e.g., all possible combinations of numerical values between the lowest value and the highest value enumerated are considered expressly stated). For example, if a concentration range or beneficial effect range is stated as 1% to 50%, it is intended that values such as 2% to 40%, 10% to 30%, or 1% to 3%, etc., are expressly enumerated. The above may be simple examples of what is specifically intended.
  • a use of electrochemical or photoelectrochemical reduction of carbon dioxide may produce methanol and related products in a high yield of about 60% to about 100%, based on the amount of carbon dioxide, suitably about 75% to 90%, and more suitably about 85% to 95%.
  • methanol may be produced with good faradaic efficiency at the cathode.
  • the reactions at the cathode and anode may be represented as follows:
  • the reduction of the carbon dioxide may be suitably achieved efficiently in a divided electrochemical or photoelectrochemical cell in which (i) a compartment contains an anode that is an inert counter electrode and (ii) another compartment contains a working cathode electrode and a catalyst.
  • the compartments may be separated by a porous glass frit or other ion conducting bridge. Both compartments generally contain an aqueous solution of an electrolyte. Carbon dioxide gas may be continuously bubbled through the cathodic electrolyte solution to saturate the solution.
  • carbon dioxide may be continuously bubbled through the solution.
  • an external bias may be impressed across the cell such that the potential of the working electrode is held constant.
  • the electrode may be suitably illuminated with light. An energy of the light may be matching or greater than a bandgap of the semiconductor during the electrolysis.
  • a modest bias e.g., about 500 millivolts
  • the working electrode potential is generally held constant relative to the SCE.
  • the electrical energy for the electrochemical reduction of carbon dioxide may come from a normal energy source, including nuclear and alternatives (e.g., hydroelectric, wind, solar power, geothermal, etc.), from a solar cell or other nonfossil fuel source of electricity, provided that the electrical source supply at least 1.6 volts across the cell. Other voltage values may be adjusted depending on the internal resistance of the cell employed.
  • the carbon dioxide may be obtained from any sources (e.g., an exhaust stream from fossil-fuel burning power or industrial plants, from geothermal or natural gas wells or the atmosphere itself).
  • the carbon dioxide may be obtained from concentrated point sources of generation prior to being released into the atmosphere.
  • high concentration carbon dioxide sources may frequently accompany natural gas in amounts of 5% to 50%, exist in flue gases of fossil fuel (e.g., coal, natural gas, oil, etc.) burning power plants and nearly pure carbon dioxide may be exhausted from cement factories and from fermenters used for industrial fermentation of ethanol.
  • Certain geothermal steams may also contain significant amounts of carbon dioxide.
  • the carbon dioxide emissions from varied industries, including geothermal wells may be captured on-site. Separation of the carbon dioxide from such exhausts is known.
  • the capture and use of existing atmospheric carbon dioxide in accordance with some embodiments of the present invention generally allow the carbon dioxide to be a renewable and unlimited source of carbon.
  • the carbon dioxide may be readily reduced in an aqueous medium with a conductive electrode. Faradaic efficiencies have been found high, some reaching about 100%.
  • the carbon dioxide may be readily reduced with a p-type semiconductor electrode, such as p-GaP, p-GaAs, p-InP, p- InN, p-WSe 2 , p-CdTe, p-GaInP 2 and p-Si.
  • Aromatic heterocyclic amines may include, but are not limited to, unsubstituted and substituted pyridines and imidazoles.
  • Substituted pyridines and imidazoles may include, but are not limited to mono and disubstituted pyridines and imidazoles.
  • suitable catalysts may include straight chain or branched chain lower alkyl (e.g., C1-C10) mono and disubstituted compounds such as 2-methylpyridine, 4-tertbutyl pyridine, 2,6-dimethylpyridine (2,6- lutidine); bipyridines, such as 4,4'-bipyridine; amino-substituted pyridines, such as 4- dimethylamino pyridine; and hydroxyl-substituted pyridines (e.g., 4-hydroxy-pyridine) and substituted or unsubstituted quinoline or isoquinolines.
  • straight chain or branched chain lower alkyl e.g., C1-C10
  • mono and disubstituted compounds such as 2-methylpyridine, 4-tertbutyl pyridine, 2,6-dimethylpyridine (2,6- lutidine)
  • bipyridines such as 4,4'-bipyridine
  • amino-substituted pyridines such
  • the catalysts may also suitably include substituted or unsubstituted dinitrogen heterocyclic amines, such as pyrazine, pyridazine and pyrimidine.
  • Other catalysts generally include azoles, imidazoles, indoles, oxazoles, thiazoles, substituted species and complex multi-ring amines such as adenine, pterin, pteridine, benzimidazole, phenonthroline and the like.
  • FIG. 1 a block diagram of a system 100 is shown in accordance with a preferred embodiment of the present invention.
  • the system (or apparatus) 100 generally comprises a cell (or container) 102, a liquid source 104, a power source 106, a gas source 108, an extractor 110 and an extractor 112.
  • a product may be presented from the extractor 110.
  • An output gas may be presented from the extractor 112.
  • Another output gas may be presented from the cell 102.
  • the cell 102 may be implemented as a divided cell.
  • the divided cell may be a divided electrochemical cell and/or a divided photochemical cell.
  • the cell 102 is generally operational to reduce carbon dioxide (C0 2 ) and protons into one or more organic products and/or inorganic products. The reduction generally takes place by bubbling carbon dioxide into an aqueous solution of an electrolyte in the cell 102.
  • a cathode in the cell 102 may reduce the carbon dioxide into one or more compounds.
  • the cell 102 generally comprises two or more compartments (or chambers)
  • the anode 1 18 may be disposed in a given compartment (e.g., 1 14a).
  • the cathode 120 may be disposed in another compartment (e.g., 114b) on a side of the separator 1 16 opposite the anode 1 18.
  • An aqueous solution 122 may fill both compartments 1 14a-l 14b.
  • a catalyst 124 may be added to the compartment 1 14b containing the cathode 120.
  • the liquid source 104 may implement a water source.
  • the liquid source 104 may be operational to provide pure water to the cell 102.
  • the power source 106 may implement a variable voltage source.
  • the source may implement a variable voltage source.
  • the 106 may be operational to generate an electrical potential between the anode 1 18 and the cathode 120.
  • the electrical potential may be a DC voltage.
  • the gas source 108 may implement a carbon dioxide source.
  • the source 108 is generally operational to provide carbon dioxide to the cell 102.
  • the carbon dioxide is bubbled directly into the compartment 1 14b containing the cathode 120 and the electrolyte 122.
  • a carbon dioxide-saturated electrolyte is introduced to the cell 102.
  • the electrolyte 122 may include one or more of Na 2 S0 4 , KHC0 3 ,KC1, NaNOs, NaCl, NaF, NaC10 4 , KC10 4 , K 2 Si0 3 , CaCl 2 , a guanidinium cation, a H + ion, an alkali metal cation, an ammonium cation, an alkylammonium cation, a halide ion, an alkyl amine, a borate, a carbonate, a guanidinium derivative, a nitrite, a nitrate, a phosphate, a polyphosphate, a perchlorate, a silicate, a sulfate, and a tetraalkyl ammonium salt.
  • the extractor 1 10 may implement an organic product and/or inorganic product extractor.
  • the extractor 110 is generally operational to extract (separate) products (e.g., formic acid, acetone, glyoxal, isopropanol, formaldehyde, methanol, polymers and the like) from the electrolyte 122.
  • the extracted products may be presented through a port 126 of the system 100 for subsequent storage and/or consumption by other devices and/or processes.
  • the extractor 1 12 may implement an oxygen extractor.
  • the extractor 1 12 is generally operational to extract oxygen (e.g., (3 ⁇ 4) byproducts created by the reduction of the carbon dioxide and/or the oxidation of water.
  • the extracted oxygen may be presented through a port 128 of the system 100 for subsequent storage and/or consumption by other devices and/or processes.
  • Chlorine and/or oxidatively evolved chemicals may also be byproducts in some configurations.
  • the organic pollutants may be rendered harmless by oxidization. Any other excess gases (e.g., hydrogen) created during the reduction of the carbon dioxide may be vented from the cell 102 via a port 130.
  • water may be oxidized (or split) to protons and oxygen at the anode 1 18 while the carbon dioxide is reduced to organic products at the cathode 120.
  • the electrolyte 122 in the cell 102 may use water as a solvent with any salts that are water soluble and with a pyridine or pyridine-derived catalyst 124.
  • the catalysts 124 may include, but are not limited to, nitrogen, sulfur and oxygen containing heterocycles. Examples of the heterocyclic compounds may be pyridine, imidazole, pyrrole, thiazole, furan, thiophene and the substituted heterocycles such as amino-thiazole and benzimidazole.
  • Cathode materials generally include any conductor.
  • any anode material may be used.
  • the overall process is generally driven by the power source 106.
  • Combinations of cathodes 120, electrolytes 122, catalysts 124, introduction of carbon dioxide to the cell 102, introduction of divalent cations (e.g., Ca 2+ , Mg 2+ , Zn 2+ ) to the electrolytes 122, pH levels and electric potential from the power source 106 may be used to control the reaction products of the cell 102.
  • the pH of electrolyte solution may be maintained between about pH 1 and pH 8 with a suitable range depending on what product or products are desired.
  • Organic products and inorganic products resulting from the reaction may include, but are not limited to, acetaldehyde, acetate, acetic acid, acetone, 1-butanol, 2-butanol, 2-butanone, carbon, carbon monoxide, carbonates, ethane, ethanol, ethylene, formaldehyde, formate, formic acid, glycolate, glycolic acid, glyoxal, glyoxylate, glyoxylic acid, graphite, isopropanol, lactate, lactic acid, methane, methanol, oxalate, oxalic acid, a polymer containing carbon dioxide, 1 - propanal, 1-propanol, and propionic acid.
  • the cell 102 includes a tin (Sn) cathode for the production of formate.
  • a catalyst is preferably used, with the catalyst preferably including one or more of pyridine, 2-picoline and 2,6-lutadine.
  • the preferred catalyst concentration is between about lppm and lOOmM, and more preferably between about O.OlmM and 30mM.
  • the electrolyte in the cell 102 may include potassium chloride with a concentration of 0.5 M, however other electrolytes may be utilized, including but not limited to, another chloride electrolyte (e.g., LiCl, CsCl, NH 4 C1), a perchlorate electrolyte, a phosphate electrolyte, a bicarbonate electrolyte, and a sulfate electrolyte.
  • another chloride electrolyte e.g., LiCl, CsCl, NH 4 C1
  • a perchlorate electrolyte e.g., LiCl, CsCl, NH 4 C1
  • a perchlorate electrolyte e.g., LiCl, CsCl, NH 4 C1
  • a perchlorate electrolyte e.g., LiCl, CsCl, NH 4 C1
  • a perchlorate electrolyte e.g.,
  • an acidic solution may be introduced to the cathode compartment, where additional protons may be made available at the cathode surface to neutralize the hydroxide to water.
  • a pH buffer may be utilized to maintain a preferred pH range in the cathode compartment of between about 1 and 7, with a more preferable pH range of between 3 and 6, and even more preferable pH range of between 3 and 4.5.
  • the pH buffer is a phosphate buffer, which may be a 0.2M phosphate buffer.
  • a cation mixture may also be introduced to the catholyte compartment which also may address the formation of the surface hydroxide development.
  • Preferred cations include mixture of cations such as K+/Cs+, Li+/K+ and Li+/Cs+ combinations, which may be introduced in a molar ratio between about 1 : 1000 and 1000: 1. Na+ works equally good in place of K+.
  • the solvent may include methanol, acetonitrile, and/or other nonaqueous solvents.
  • the electrolytes 122 generally include tetraalkyl ammonium salts and a heterocyclic catalyst.
  • a primary product may be oxalate in a completely nonaqueous system.
  • the products In a system containing a nonaqueous catholyte and an aqueous anolyte, the products generally include all of the products seen in aqueous systems with higher yields.
  • the process is generally controlled to get a desired product by using combinations of specific cathode materials, catalysts, electrolytes, surface morphology of the electrodes, introduction of reactants relative to the cathode, introduction of divalent cations to the electrolyte, adjusting pH levels and/or adjusting electrical potentials. Faradaic yields for the products generally range from less than 1% to more than 90% with the remainder being hydrogen, though methane, carbon monoxide and/or ethylene may also be produced as gaseous byproducts.
  • FIGS. 2A-2C tables illustrating relative product yields for different cathode material, catalyst, electrolyte, pH level and cathode potential combinations are shown.
  • the combinations listed in the tables generally are not the only combinations providing a given product.
  • the combinations illustrated may demonstrate high yields of the products at the lowest potential.
  • the cathodes tested generally include all conductive elements on the periodic table, steels, nickel alloys, copper alloys such as brass and bronze and elgiloy. Most of the conductors may be used with heterocyclic catalysts 124 to reduce the carbon dioxide.
  • the products created may vary based on which cathode material is used.
  • a W cathode 120 with pyridine catalyst 124 may give acetone as a product whereas a Sn cathode 120 with pyridine may primarily give formic acid and methanol as products.
  • a product yield may also be changed by the manner in which the carbon dioxide was bubbled into the cell 102. For instance, with a stainless steel 2205 cathode 120 in a KC1 electrolyte 122, if the carbon dioxide bubbles directly contact the cathode 120, the product mix may switch to methanol and isopropanol, rather than formic acid and acetone when the carbon dioxide bubbles avoid contact with the cathode 120 (i.e., the carbon dioxide bubbles circumvent the cathode 120 in the cell 102).
  • Cell design and cathode treatment may affect both product yields and current density at the cathode.
  • a divided cell 102 with a stainless steel 2205 cathode 120 in a KC1 electrolyte 122 generally has higher yields with a heavily scratched (rough) cathode 120 than an unscratched (smooth) cathode 120.
  • the roughness or smoothness of a cathode surface may be determined by a comparison between a surface area measurement and the geometric surface area of the cathode, where the greater the difference between the surface area measurement and the geometric surface area, the rougher the cathode. Matte tin generally performs different than bright tin. Maintaining carbon dioxide bubbling only on the cathode side of the divided cell 102 (e.g., in compartment 1 14b) may also increase yields.
  • Raising or lowering the cathode potential may also alter the reduced products.
  • ethanol is generally evolved at lower potentials between -0.8 volts and -1 volt using the duplex steel/pyridine/KCl, while methanol is favored beyond -1 volt.
  • Faradaic yields for the products may be improved by controlling the electrical potential of the reaction. By maintaining a constant potential at the cathode 120, hydrogen evolution is generally reduced and faradaic yields of the products increased. Addition of hydrogen inhibitors, such as acetonitrile, certain heterocycles, alcohols, and other chemicals may also increase yields of the products.
  • stability may be improved with cathode materials known to poison rapidly when reducing carbon dioxide. Copper and copper-alloy electrodes commonly poison in less than an hour of electrochemically reducing carbon dioxide.
  • copper-based alloys were operated for many hours without any observed degradation in effectiveness. The effects were particularly enhanced by using sulfur containing heterocycles. For instance, a system with a copper cathode and 2-amino thiazole catalyst showed very high stability for the reduction of carbon dioxide to carbon monoxide and formic acid.
  • Heterocycles other than pyridine may catalytically reduce carbon dioxide in the electrochemical process using many aforementioned cathode materials, including tin, steels, nickel alloys and copper alloys.
  • Nitrogen-containing heterocyclic amines shown to be effective include azoles, indoles, 4,4'-bipyridines, picolines (methyl pyridines), lutidines (dimethyl pyridines), hydroxy pyridines, imidazole, benzimidazole, methyl imidazole, pyrazine, pyrimidine, pyridazine, pyridazineimidazole, nicotinic acid, quinoline, adenine and 1, 10-phenanthroline.
  • Sulfur containing heterocycles include thiazole, aminothiazoles, thiophene.
  • Oxygen containing heterocycles include furan and oxazole.
  • the combination of catalyst, cathode material and electrolyte may be used to control product mix.
  • Some process embodiments of the present invention for making/converting hydrocarbons generally consume a small amount of water (e.g., approximately 1 to 3 moles of water) per mole of carbon. Therefore, the processes may be a few thousand times more water efficient than existing production techniques.
  • the ring structure may be an aromatic 5-member heterocyclic ring or 6-member heterocyclic ring with at least one ring nitrogen and is optionally substituted at one or more ring positions other than nitrogen with R.
  • L may be C or N.
  • Rl may be H.
  • R2 may be H if L is N or R2 is R if L is C.
  • R3 may be H.
  • R4, R5, R7 and R8 are generally independently H, straight chain or branched chain lower alkyl, hydroxyl, amino, or taken together are a fused six-member aryl ring.
  • R6 may be H, straight chain or branched chain lower alkyl, hydroxyl, amino or pyridyl.
  • one of LI, L2 and L3 may be N, while the other L's may be C.
  • R9 may be H. If LI is N, R10 may be H. If L2 is N, Rl 1 may be H. If L3 is N, R12 may be H. If LI, L2 or L3 is C, then R10, Rl l, R12, RI3 and R14 may be independently selected from straight chain or branched chain lower alkyl, hydroxyl, amino, or pyridyl.
  • R15 and R16 may be H.
  • R17, R18 and R19 are generally independently selected from straight chain or branched chain lower alkyl, hydroxyl, amino, or pyridyl.
  • the concentration of aromatic heterocyclic amine catalysts is about 1 millimolar (mM) to 1 M.
  • the electrolyte may be suitably a salt, such as KC1, KHC0 3 ,NaN0 3 , Na 2 S0 4 , NaC10 4 , NaF, NaC10 4 , KC10 4 , K 2 Si0 3 , or CaCl 2 at a concentration of about 0.5 M.
  • Other electrolytes may include, but are not limited to, all group 1 cations (e.g., H, Li, Na, K, Rb and Cs) except Francium (Fr), Ca, ammonium cations, alkylammonium cations and alkyl amines.
  • Additional electrolytes may include, but are not limited to, all group 17 anions (e.g., F, CI, Br, I and At), borates, carbonates, nitrates, nitrites, perchlorates, phosphates, polyphosphates, silicates and sulfates.
  • Na generally performs as well as K with regard to best practices, so NaCl may be exchanged with KC1.
  • NaF may perform about as well as NaCl, so NaF may be exchanged for NaCl or KC1 in many cases. Larger anions tend to change the chemistry and favor different products. For instance, sulfate may favor polymer or methanol production while CI may favor products such as acetone.
  • the pH of the solution is generally maintained at about pH 3 to 8, suitably about 4.7 to 5.6.
  • formic acid and formaldehyde were found to be intermediate products along the pathway to the 6 e- reduced product of methanol, with an aromatic amine radical (e.g., the pyridinium radical, playing a role in the reduction of both intermediate products).
  • the intermediate products have generally been found to also be the final products of the reduction of carbon dioxide at conductive electrodes or p-type semiconductor electrodes, depending on the particular catalyst used.
  • Other C-C couple products may also be possible.
  • reduction of carbon dioxide may suitably yield formaldehyde, formic acid, glyoxal, methanol, isopropanol, or ethanol, depending on the particular aromatic heterocyclic amine used as the catalyst.
  • the products of the reduction of carbon dioxide are generally substitution-sensitive. As such, the products may be selectively produced.
  • use of 4,4'-bipyridine as the catalyst may produce methanol and/or 2- propanol.
  • Lutidines and amino-substituted pyridines may produce 2-propanol.
  • Hydroxy- pyridine may produce formic acid.
  • the effective electrochemical/photoelectrochemical reduction of carbon dioxide disclosed herein may provide new methods of producing methanol and other related products in an improved, efficient, and environmentally beneficial way, while mitigating carbon dioxide-caused climate change (e.g., global warming).
  • the methanol product of reduction of carbon dioxide may be advantageously used as (1) a convenient energy storage medium, which allows convenient and safe storage and handling, (2) a readily transported and dispensed fuel, including for methanol fuel cells and (3) a feedstock for synthetic hydrocarbons and corresponding products currently obtained from oil and gas resources, including polymers, biopolymers and even proteins, that may be used for animal feed or human consumption.
  • the use of methanol as an energy storage and transportation material generally eliminates many difficulties of using hydrogen for such purposes.
  • the safety and versatility of methanol generally makes the disclosed reduction of carbon dioxide further desirable.
  • Example 1 General Electrochemical Methods.
  • Electrochemical system The electrochemical system was composed of a standard two-compartment electrolysis cell 102 to separate the anode 118 and cathode 120 reactions. The compartments were separated by a porous glass frit or other ion conducting bridge 1 16.
  • the electrolytes 122 were used at concentrations of 0.1 M to 1 M, with 0.5 M being a typical concentration. A concentration of between about 1 mM to 1 M of the catalysts 124 were used.
  • the particular electrolyte 122 and particular catalyst 124 of each given test were generally selected based upon what product or products were being created.
  • the method (or process) 140 generally comprises a step (or block) 142, a step (or block) 144, a step (or block) 146, a step (or block) 148 and a step (or block) 150.
  • the method 140 may be implemented using the system 100.
  • the electrodes 118 and 120 may be activated where appropriate. Bubbling of the carbon dioxide into the cell 102 may be performed in the step 144. Electrolysis of the carbon dioxide into organic and/or inorganic products may occur during step 146. In the step 148, the products may be separated from the electrolyte. Analysis of the reduction products may be performed in the step 150.
  • the working electrode was of a known area. All potentials were measured with respect to a saturated calomel reference electrode (Accumet). Before and during all electrolysis, carbon dioxide (Airgas) was continuously bubbled through the electrolyte to saturate the solution. The resulting pH of the solution was maintained at about pH 3 to pH 8 with a suitable range depending on what product or products were being made. For example, under constant carbon dioxide bubbling, the pH levels of 10 mM solutions of 4-hydroxy pyridine, pyridine and 4-tertbutyl pyridine were 4.7, 5.28 and 5.55, respectively.
  • NMR Nuclear Magnetic Resonance
  • the photoelectrochemical system was composed of a Pyrex three-necked flask containing 0.5 M KC1 as supporting electrolyte and a 1 mM to 1 M catalyst (e.g., 10 mM pyridine or pyridine derivative).
  • the photocathode was a single crystal p-type semiconductor etched for approximately 1 to 2 minutes in a bath of concentrated HN03:HC1, 2: 1 v/v prior to use. An ohmic contact was made to the back of the freshly etched crystal using an indium/zinc (2 wt. % Zn) solder.
  • the contact was connected to an external lead with conducting silver epoxy (Epoxy Technology H31) covered in glass tubing and insulated using an epoxy cement (Loctite 0151 Hysol) to expose only the front face of the semiconductor to solution. All potentials were referenced against a saturated calomel electrode (Accumet).
  • the three electrode assembly was completed with a carbon rod counter electrode to minimize the reoxidation of reduced carbon dioxide products.
  • carbon dioxide gas Airgas
  • the resulting pH of the solution was maintained at about pH 3 to 8 (e.g., pH 5.2).
  • the method (or process) 160 generally comprises a step (or block) 162, a step (or block) 164, a step (or block) 166, a step (or block) 168 and a step (or block) 170.
  • the method 160 may be implemented using the system 100.
  • the photoelectrode may be activated. Bubbling of the carbon dioxide into the cell 102 may be performed in the step 164. Electrolysis of the carbon dioxide into the products may occur during step 166. In the step 168, the products may be separated from the electrolyte. Analysis of the reduction products may be performed in the step 170.
  • Light sources Four different light sources were used for the illumination of the p-type semiconductor electrode.
  • a Hg-Xe arc lamp (USHIO UXM 200H) was used in a lamp housing (PTI Model A-1010) and powered by a PTI LTS-200 power supply.
  • a Xe arc lamp (USHIO UXL 151H) was used in the same housing in conjunction with a PTI monochromator to illuminate the electrode at various specific wavelengths.
  • a fiber optic spectrometer (Ocean Optics S2000) or a silicon photodetector (Newport 818-SL silicon detector) was used to measure the relative resulting power emitted through the monochromator.
  • the flatband potential was obtained by measurements of the open circuit photovoltage during various irradiation intensities using the 200 watt (W) Hg-Xe lamp (3 W/cm 2 - 23 W/cm 2 ). The photovoltage was observed to saturate at intensities above approximately 6 W/cm 2 .
  • electrolysis was performed under illumination by two different light-emitting diodes (LEDs).
  • a blue LED (Luxeon V Dental Blue, Future Electronics) with a luminous output of 500 milliwatt (mW) +/- 50 mW at 465 nanometers (nm) and a 20 nm full width at half maximum (FWHM) was driven at to a maximum rated current of 700 mA using a Xitanium Driver (Advance Transformer Company).
  • a Fraen collimating lens (Future Electronics) was used to direct the output light.
  • the resultant power density that reached the window of the photoelectrochemical cell was determined to be 42 mW/cm 2 , measured using a Scientech 364 thermopile power meter and silicon photodetector.
  • the measured power density was assumed to be greater than the actual power density observed at the semiconductor face due to luminous intensity loss through the solution layer between the wall of the photoelectrochemical cell and the electrode.
  • Example 3 Analysis of Products of Electrolysis.
  • Electrochemical experiments were generally performed using a CH Instruments potentiostat or a DC power supply with current logger to run bulk electrolysis experiments..
  • Mass spectrometry Mass spectral data was also collected to identify all organic compounds. Nuclear Magnetic Resonance. NMR spectra of electrolyte volumes after bulk electrolysis were also obtained using an automated Bruker UltrashieldTM 500 Plus spectrometer.
  • NiFe pyr 0.5M KC1 IC Trace formate ⁇ 0.1%
  • PdAg pyr 0.5M KC1 IC Trace formate, 4% acetate
  • Table 2 shows faradaic efficiencies for formate (HCOO ) production, with a system employing a controlled potential electrolysis at -1.37V vs. SCE in CO 2 saturated water with a 0.5M KC1 electrolyte.
  • the catalyst concentration in the cathode compartment was 30mM.
  • the anode compartment contained water with 0.17M K 2 SO 4 .
  • the electrolysis was carried out in a three chambered glass cell with separated cathode and anode chambers. Carbon dioxide was continuously bubbled on the cathode chamber.
  • j(mA/cm 2 ) represents average current density
  • FY(%) represents Faradaic Yield, which was calculated from the ppm of the formate measured by IC analysis on the catholyte solution collected after the electrolysis, and the total charge passed during the electrolysis.
  • Table 3 illustrates faradaic efficiencies for formate production using tin cathodes with 30mM 2-picoline catalyst in the cathode compartment, with various electrolytes. The electrolytes were saturated with carbon dioxide and present in 0.5M concentrations.
  • Table 4 illustrates faradaic efficiencies for formate production using tin cathodes obtained from electrolysis in a divided H-Cell, with a controlled potential at -1.37V vs. SCE, in SCE in C0 2 saturated water with a 0.5M KC1 electrolyte.
  • the cathode compartment included a catalyst of 30mM 2-picoline, with the anode compartment including water with 0.17M K 2 SO 4 .
  • the cathode compartment and anode compartment were separated by a proton exchange membrane (Selemion HSF). The pH was monitored continuously in situ by a glass electrode immersed in the cathode compartment.
  • Table 5 illustrates the effects of 2-picoline concentrations on faradaic efficiencies for formate production using tin electrodes. Without use of 2-picoline as a catalyst, the average faradaic yield may be about 25% for the electrolysis in the CO 2 saturated KCl solution.
  • Table 6 illustrates the effects of pH for formate production using tin cathodes.
  • the pH was adjusted using HC1 or KOH solution after saturating with CO 2 .
  • Table 7 illustrates faradaic efficiencies for formate production using tin cathodes buffered at 4.5 pH.
  • the system employed a controlled potential electrolysis (-1.37V vs. SCE) in C0 2 saturated 0.5M KCl prepared in 0.2M phosphate buffer pH 4.5 (Alfa Aesar).
  • the catalyst in the cathode compartment was ImM 2-picoline, with 0.17M K2SO4 in the anode compartment.
  • the cathode compartment and anode compartment were separated by a proton exchange membrane.
  • Table 8 illustrates faradaic efficiencies for formate production using tin cathodes in water with an electrolyte including 0.25M KC1 and 0.25M CsCl.
  • the cathode compartment included 30mM 2-picoline as a homogenous catalyst.
  • the system employed a controlled potential electrolysis (- 1.37V vs. SCE) in C0 2 saturated 0.5M KC1.
  • the anode compartment included 0.17M K 2 SO 4 .
  • the cathode compartment and anode compartment were separated by a proton exchange membrane. Without use of 2-picoline as a catalyst, the average faradaic yield may be about 17.2% for the electrolysis in the CO 2 saturated KC1 and CsCl solution.
  • Carbon dioxide may be efficiently converted to value-added products, using either a minimum of electricity (that may be generated from an alternate energy source) or directly using visible light.
  • Some processes described above may generate high energy density fuels that are not fossil-based as well as being chemical feedstock that are not fossil or biologically based.
  • the catalysts for the processes may be substituents-sensitive and provide for selectivity of the value-added products.
  • a fixed cathode e.g., stainless steel 2205
  • the cathodes may be swapped out with different materials to change the product mix.
  • the anode may use different photovoltaic materials to change the product mix.
  • Some embodiments of the present invention generally provide for new cathode materials, new electrolyte materials and new sulfur and oxygen-containing heterocyclic catalysts.
  • Specific combinations of cathode materials, electrolytes, catalysts, pH levels and/or electrical potentials may be used to get a desired product.
  • the organic products may include, but are not limited to, acetaldehyde, acetone, carbon, carbon monoxide, carbonates, ethanol, ethylene, formaldehyde, formic acid, glyoxal, glyoxylic acid, graphite, isopropanol, methane, methanol, oxalate, oxalic acid.
  • Inorganic products may include, but are not limited to, polymers containing carbon dioxide. Specific process conditions may be established that maximize the carbon dioxide conversion to specific chemicals beyond methanol.
  • Cell parameters may be selected to minimize unproductive side reactions like
  • heterocyclic amine pyridine catalysts with engineered functional groups may be utilized in the system 100 to achieve high faradaic rates. Process conditions described above may facilitate long life (e.g., improved stability), electrode and cell cycling and product recovery.
  • the organic products created may include methanol, formaldehyde, formic acid, glyoxal, acetone, and isopropanol using the same pyridine catalyst with different combinations of electrolytes, cathode materials, bubbling techniques and cell potentials.
  • Heterocyclic amines related to pyridine may be used to improve reaction rates, product yields, cell voltages and/or other aspects of the reaction.
  • Heterocyclic catalysts that contain sulfur or oxygen may also be utilized in the carbon dioxide reduction.
  • Some embodiments of the present invention may provide cathode and electrolyte combinations for reducing carbon dioxide to products in commercial quantities.
  • Catalytic reduction of carbon dioxide may be achieved using steel or other low cost cathodes.
  • High faradaic yields e.g., >20%) of organic products with steel and nickel alloy cathodes at ambient temperature and pressure may also be achieved.
  • Copper-based alloys used at the electrodes may remain stable for long-term reduction of carbon dioxide.
  • the relative low cost and abundance of the combinations described above generally opens the possibility of commercialization of electrochemical carbon dioxide reduction.

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Abstract

L'invention concerne un procédé de réduction de dioxyde de carbone en un ou plusieurs produits et pouvant comprendre les étapes A) à C). L'Étape (A) peut faire buller ledit dioxyde de carbone dans une solution d'un électrolyte et d'un catalyseur dans une cellule électrochimique divisée. La cellule électrochimique divisée peut comprendre une anode dans un premier compartiment de cellule et une cathode dans un second compartiment de cellule. La cathode peut réduire ledit dioxyde de carbone dans lesdits produits. L'étape (B) peut ajuster un ou plusieurs des (a) un matériau de cathode, (b) une morphologie de surface de ladite cathode, (c) ledit électrolyte, (d) une manière dans laquelle ledit dioxyde de carbone est introduit sous forme de bulles, (e), un niveau de pH de ladite solution et (f) un potentiel électrique de ladite cellule électrochimique divisée, à faire varier au moins l'un (i) desdits produits qui est produit et (ii) un rendement faradique de ces produits. L'étape (C) peut séparer lesdits produits à partir de ladite solution.
PCT/US2013/029425 2012-03-06 2013-03-06 Réduction du dioxyde de carbone en produits WO2013134418A1 (fr)

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EP13757264.0A EP2823090A4 (fr) 2012-03-06 2013-03-06 Réduction du dioxyde de carbone en produits
AU2013231005A AU2013231005A1 (en) 2012-03-06 2013-03-06 Reducing carbon dioxide to products
KR1020147024882A KR20140138153A (ko) 2012-03-06 2013-03-06 이산화탄소를 생성물로 환원시키는 방법
CA2864611A CA2864611A1 (fr) 2012-03-06 2013-03-06 Reduction du dioxyde de carbone en produits
JP2014561087A JP2015513616A (ja) 2012-03-06 2013-03-06 二酸化炭素の生成物への還元
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EP3014695A4 (fr) * 2013-06-27 2017-01-11 The Board of Trustees of the University of Illionis Catalyseurs pour la conversion de dioxyde de carbone
US10465303B2 (en) 2015-09-15 2019-11-05 Kabushiki Kaisha Toshiba Producing system of reduction product
CN110492203A (zh) * 2019-07-08 2019-11-22 南京航空航天大学 一种新型锂-二氧化碳电池及其正极材料的制备
US10815577B2 (en) 2015-07-14 2020-10-27 Korea Institute Of Energy Research Method and apparatus for preparing reduction product of carbon dioxide by electrochemically reducing carbon dioxide
CN112023934A (zh) * 2020-10-09 2020-12-04 北京化工大学 一种铜铟双金属单原子催化剂的制备方法
US10978703B2 (en) 2014-12-14 2021-04-13 The Board Of Trustees Of The University Of Illinois Catalyst system for advanced metal-air batteries
CN113795611A (zh) * 2019-05-05 2021-12-14 多伦多大学管理委员会 在电解池中碳酸盐转化为合成气或c2+产物

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JP7316339B2 (ja) * 2021-10-18 2023-07-27 本田技研工業株式会社 二酸化炭素処理装置、二酸化炭素処理方法及び炭素化合物の製造方法
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US10370768B2 (en) 2013-06-27 2019-08-06 The Board Of Trustees Of The University Of Illinois Catalysts for carbon dioxide conversion
CN104328046A (zh) * 2014-09-28 2015-02-04 南京工业大学 微生物电化学系统还原二氧化碳产乙酸的装置与方法
US10978703B2 (en) 2014-12-14 2021-04-13 The Board Of Trustees Of The University Of Illinois Catalyst system for advanced metal-air batteries
US10815577B2 (en) 2015-07-14 2020-10-27 Korea Institute Of Energy Research Method and apparatus for preparing reduction product of carbon dioxide by electrochemically reducing carbon dioxide
US10465303B2 (en) 2015-09-15 2019-11-05 Kabushiki Kaisha Toshiba Producing system of reduction product
CN113795611A (zh) * 2019-05-05 2021-12-14 多伦多大学管理委员会 在电解池中碳酸盐转化为合成气或c2+产物
CN110492203A (zh) * 2019-07-08 2019-11-22 南京航空航天大学 一种新型锂-二氧化碳电池及其正极材料的制备
CN110492203B (zh) * 2019-07-08 2022-05-03 南京航空航天大学 一种锂-二氧化碳电池及其正极材料的制备
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