US20110114502A1 - Reducing carbon dioxide to products - Google Patents

Reducing carbon dioxide to products Download PDF

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Publication number
US20110114502A1
US20110114502A1 US12/846,221 US84622110A US2011114502A1 US 20110114502 A1 US20110114502 A1 US 20110114502A1 US 84622110 A US84622110 A US 84622110A US 2011114502 A1 US2011114502 A1 US 2011114502A1
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United States
Prior art keywords
carbon dioxide
products
cathode
solution
electrolyte
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US12/846,221
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English (en)
Inventor
Emily Barton Cole
Narayanappa Sivasankar
Andrew Bocarsly
Kyle Teamey
Nety Krishna
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Liquid Light Inc
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Liquid Light Inc
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Priority to US12/846,221 priority Critical patent/US20110114502A1/en
Assigned to LIQUID LIGHT, INC. reassignment LIQUID LIGHT, INC. ASSIGNMENT OF ASSIGNORS INTEREST (SEE DOCUMENT FOR DETAILS). Assignors: KRISHNA, NETY, BOCARSLY, ANDREW, COLE, EMILY BARTON, SIVASANKAR, NARAYANAPPA, TEAMEY, KYLE
Priority to US12/875,227 priority patent/US8524066B2/en
Publication of US20110114502A1 publication Critical patent/US20110114502A1/en
Priority to AU2011282767A priority patent/AU2011282767C1/en
Priority to KR1020137005179A priority patent/KR20140012017A/ko
Priority to CN201180036854.XA priority patent/CN103140608B/zh
Priority to EP11813101.0A priority patent/EP2598671A4/de
Priority to JP2013521930A priority patent/JP2013536319A/ja
Priority to PCT/US2011/045515 priority patent/WO2012015905A1/en
Priority to CA2805840A priority patent/CA2805840A1/en
Priority to BR112013002221A priority patent/BR112013002221A2/pt
Priority to US13/542,152 priority patent/US8592633B2/en
Priority to US13/787,304 priority patent/US8845878B2/en
Priority to US13/787,481 priority patent/US20130180865A1/en
Priority to US13/956,983 priority patent/US20140021042A1/en
Priority to US14/029,444 priority patent/US20140027303A1/en
Abandoned legal-status Critical Current

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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
    • 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
    • C25B1/01—Products
    • C25B1/23—Carbon monoxide or syngas
    • 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
    • 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 invention concerns a method for reducing carbon dioxide to one or more products.
  • the method 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 vary at least one of (i) which of the products is produced and (ii) a faradaic yield of the products by adjusting one or more of (a) a cathode material and (b) a surface morphology of the cathode.
  • Step (C) may separate the products from the solution.
  • the objects, features and advantages of the present invention include providing a method and/or apparatus for implementing reducing carbon dioxide to products that may (i) catalytically reduce carbon dioxide using steel cathodes or other low cost cathode materials, (ii) produce high faradaic yields (e.g., >20%), (iii) produce organic products with steel and nickel alloy cathodes at ambient temperature and pressure, (iv) provide stabile long-term reduction of carbon dioxide using copper-based alloy electrodes and/or (v) provide for commercialization of electrochemical carbon dioxide reduction.
  • 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.
  • 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.
  • 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 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.
  • 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.
  • An example of an overall reaction for the reduction of carbon dioxide 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 as
  • 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.
  • 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 (CO 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) 114 a - 114 b , a separator (or membrane) 116 , an anode 118 and a cathode 120 .
  • the anode 118 may be disposed in a given compartment (e.g., 114 a ).
  • the cathode 120 may be disposed in another compartment (e.g., 114 b ) on an opposite side of the separator 116 as the anode 118 .
  • An aqueous solution 122 may fill both compartments 114 a - 114 b .
  • a catalyst 124 may be added to the compartment 114 b 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 106 may be operational to generate an electrical potential between the anode 118 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 114 b containing the cathode 120 .
  • the extractor 110 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 112 may implement an oxygen extractor.
  • the extractor 112 is generally operational to extract oxygen (e.g., O 2 ) 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 by 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 118 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 , pH levels and electric potential from the power source 106 may be used to control the reaction products of the cell 102 .
  • 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, 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 KCl electrolyte 122 , if the carbon dioxide bubbles directly hit the cathode 120 , the product mix may switch to methanol and isopropanol, rather than formic acid and acetone when the carbon dioxide bubbles miss the cathode 120 .
  • 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 KCl electrolyte 122 generally has higher yields with a heavily scratched (rough) cathode 120 than an unscratched (smooth) cathode 120 .
  • 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 114 b ) 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.
  • 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.
  • R1 may be H.
  • R2 may be H if L is N or R2 is R if L is C.
  • one of L1, L2 and L3 may be N, while the other L's may be C.
  • R9 may be H. If L1 is N, R10 may be H. If L2 is N, R11 may be H. If L3 is N, R12 may be H. If L1, L2 or L3 is C, then R10, R11, R12, R13 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 KCl, NaNO 3 , Na 2 SO 4 , NaCl, NaF, NaClO 4 , KClO 4 , K 2 SiO 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, Cl, 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 KCl.
  • NaF may perform about as well as NaCl, so NaF may be exchanged for NaCl or KCl in many cases. Larger anions tend to change the chemistry and favor different products. For instance, sulfate may favor polymer or methanol production while Cl 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.
  • 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 116 .
  • 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 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 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 .
  • 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 52000) 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.
  • Electrochemical experiments were generally performed using a CH Instruments potentiostat or a DC power supply with current logger to run bulk electrolysis experiments.
  • the CH Instruments potentiostat was generally used for cyclic voltammetry.
  • Electrolysis was run under potentiostatic conditions from approximately 6 hours to 30 hours until a relatively similar amount of charge was passed for each run.
  • Spectrophotometry The presence of formaldehyde and formic acid was also determined by the chromotropic acid assay. Briefly, a solution of 0.3 g of 4,5-dihydroxynaphthalene-2,7-disulfonic acid, disodium salt dihydrate (Aldrich) was dissolved in 10 mL deionized water before diluting to 100 mL with concentrated sulfuric acid. For formaldehyde, an aliquot of 1.5 mL was then added to 0.5 mL of the sample. The presence of formaldehyde (absorbency at 577 nm) was detected against a standard curve using an HP 8453 UV-Vis spectrometer.
  • Mass spectrometry Mass spectral data was also collected to identify all organic compounds. In a typical experiment, the sample was directly leaked into an ultrahigh vacuum chamber and analyzed by an attached SRS Residual Gas Analyzer (with the ionizer operating at 70 electron-volts and an emission current of 1 mA). Samples were analyzed against standard methanol spectra obtained at the same settings to ensure comparable fragmentation patterns. Mass spectral data confirmed the presence of methanol and proved that the initial solution before electrolysis contained no reduced CO 2 species. Control experiments also showed that after over 24 hours under illumination the epoxy used to insulate the backside of the electrode did not leach any organic material that would give false results for the reduction of CO 2 .
  • NMR spectra of electrolyte volumes after illumination were obtained using an automated Bruker UltrashieldTM 500 Plus spectrometer with an excitation sculpting pulse technique for water suppression. Data processing was achieved using MestReNova software. For methanol standards and electrolyte samples, the representative signal for methanol was observed between 3.18 to 3.30 parts per million (ppm).
  • NMR spectra of electrolyte volumes after bulk electrolysis were also obtained using an automated Bruker UltrashieldTM 500 Plus spectrometer with an excitation sculpting pulse technique for water suppression. Data processing was achieved using MestReNova software. The concentrations of formate and methanol present after bulk electrolysis were determined using acetone as the internal standard.
  • 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 H 2 evolution from water electrolysis.
  • Choice of specific configurations of 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 stabile 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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US12/846,221 US20110114502A1 (en) 2009-12-21 2010-07-29 Reducing carbon dioxide to products
US12/875,227 US8524066B2 (en) 2010-07-29 2010-09-03 Electrochemical production of urea from NOx and carbon dioxide
BR112013002221A BR112013002221A2 (pt) 2010-07-29 2011-07-27 "reduzido dióxido de carbono em produtos"
KR1020137005179A KR20140012017A (ko) 2010-07-29 2011-07-27 이산화탄소를 생성물로 환원시키는 방법
EP11813101.0A EP2598671A4 (de) 2010-07-29 2011-07-27 Reduzierung des kohlendioxidanteils in produkten
CA2805840A CA2805840A1 (en) 2010-07-29 2011-07-27 Reducing carbon dioxide to products
CN201180036854.XA CN103140608B (zh) 2010-07-29 2011-07-27 还原二氧化碳成产物
AU2011282767A AU2011282767C1 (en) 2010-07-29 2011-07-27 Reducing carbon dioxide to products
JP2013521930A JP2013536319A (ja) 2010-07-29 2011-07-27 二酸化炭素の生成物への還元
PCT/US2011/045515 WO2012015905A1 (en) 2010-07-29 2011-07-27 Reducing carbon dioxide to products
US13/542,152 US8592633B2 (en) 2010-07-29 2012-07-05 Reduction of carbon dioxide to carboxylic acids, glycols, and carboxylates
US13/787,304 US8845878B2 (en) 2010-07-29 2013-03-06 Reducing carbon dioxide to products
US13/787,481 US20130180865A1 (en) 2010-07-29 2013-03-06 Reducing Carbon Dioxide to Products
US13/956,983 US20140021042A1 (en) 2010-07-29 2013-08-01 Electrochemical Production of Urea from NOx and Carbon Dioxide
US14/029,444 US20140027303A1 (en) 2010-07-29 2013-09-17 Reduction of Carbon Dioxide to Carboxylic Acids, Glycols, and Carboxylates

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US13/787,481 Continuation-In-Part US20130180865A1 (en) 2010-07-29 2013-03-06 Reducing Carbon Dioxide to Products
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