US20220145477A1 - Chemical reaction devices involving acid and/or base, and related systems and methods - Google Patents

Chemical reaction devices involving acid and/or base, and related systems and methods Download PDF

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US20220145477A1
US20220145477A1 US17/438,888 US202017438888A US2022145477A1 US 20220145477 A1 US20220145477 A1 US 20220145477A1 US 202017438888 A US202017438888 A US 202017438888A US 2022145477 A1 US2022145477 A1 US 2022145477A1
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Prior art keywords
electrode
reactor
equal
acid
base
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Yet-Ming Chiang
Leah Ellis
Andres Badel
Isaac W. Metcalf
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Massachusetts Institute of Technology
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Massachusetts Institute of Technology
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Assigned to MASSACHUSETTS INSTITUTE OF TECHNOLOGY reassignment MASSACHUSETTS INSTITUTE OF TECHNOLOGY ASSIGNMENT OF ASSIGNORS INTEREST (SEE DOCUMENT FOR DETAILS). Assignors: CHIANG, YET-MING, METCALF, ISAAC W., BADEL, Andres, ELLIS, Leah
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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
    • C25B1/01—Products
    • C25B1/22—Inorganic acids
    • C—CHEMISTRY; METALLURGY
    • C01—INORGANIC CHEMISTRY
    • C01B—NON-METALLIC ELEMENTS; COMPOUNDS THEREOF; METALLOIDS OR COMPOUNDS THEREOF NOT COVERED BY SUBCLASS C01C
    • C01B13/00—Oxygen; Ozone; Oxides or hydroxides in general
    • C01B13/14—Methods for preparing oxides or hydroxides in general
    • C01B13/36—Methods for preparing oxides or hydroxides in general by precipitation reactions in aqueous solutions
    • C—CHEMISTRY; METALLURGY
    • C04—CEMENTS; CONCRETE; ARTIFICIAL STONE; CERAMICS; REFRACTORIES
    • C04B—LIME, MAGNESIA; SLAG; CEMENTS; COMPOSITIONS THEREOF, e.g. MORTARS, CONCRETE OR LIKE BUILDING MATERIALS; ARTIFICIAL STONE; CERAMICS; REFRACTORIES; TREATMENT OF NATURAL STONE
    • C04B7/00—Hydraulic cements
    • C04B7/02—Portland cement
    • C04B7/06—Portland cement using alkaline raw materials
    • Y—GENERAL TAGGING OF NEW TECHNOLOGICAL DEVELOPMENTS; GENERAL TAGGING OF CROSS-SECTIONAL TECHNOLOGIES SPANNING OVER SEVERAL SECTIONS OF THE IPC; TECHNICAL SUBJECTS COVERED BY FORMER USPC CROSS-REFERENCE ART COLLECTIONS [XRACs] AND DIGESTS
    • Y02—TECHNOLOGIES OR APPLICATIONS FOR MITIGATION OR ADAPTATION AGAINST CLIMATE CHANGE
    • Y02E—REDUCTION OF GREENHOUSE GAS [GHG] EMISSIONS, RELATED TO ENERGY GENERATION, TRANSMISSION OR DISTRIBUTION
    • Y02E60/00—Enabling technologies; Technologies with a potential or indirect contribution to GHG emissions mitigation
    • Y02E60/30—Hydrogen technology
    • Y02E60/36—Hydrogen production from non-carbon containing sources, e.g. by water electrolysis
    • Y—GENERAL TAGGING OF NEW TECHNOLOGICAL DEVELOPMENTS; GENERAL TAGGING OF CROSS-SECTIONAL TECHNOLOGIES SPANNING OVER SEVERAL SECTIONS OF THE IPC; TECHNICAL SUBJECTS COVERED BY FORMER USPC CROSS-REFERENCE ART COLLECTIONS [XRACs] AND DIGESTS
    • Y02—TECHNOLOGIES OR APPLICATIONS FOR MITIGATION OR ADAPTATION AGAINST CLIMATE CHANGE
    • Y02P—CLIMATE CHANGE MITIGATION TECHNOLOGIES IN THE PRODUCTION OR PROCESSING OF GOODS
    • Y02P40/00—Technologies relating to the processing of minerals
    • Y02P40/10—Production of cement, e.g. improving or optimising the production methods; Cement grinding
    • Y02P40/18—Carbon capture and storage [CCS]

Definitions

  • a method comprises producing base near a first electrode (e.g., a cathode) and acid near a second electrode (e.g., anode) that is electrochemically coupled to the first electrode.
  • the method comprises collecting the acid and/or base.
  • the method comprises storing the acid and/or base.
  • the method comprises reacting the acid and/or base in a chemical dissolution (e.g., reacting the acid with a metal carbonate, such as CaCO 3 , to produce metal ions, such as calcium ions, and/or carbonate ions).
  • the method comprises reacting the acid and/or base in a precipitation reaction (e.g., reacting the base with metal ions, such as calcium ions, to produce a metal hydroxide, such as Ca(OH) 2 ).
  • a precipitation reaction e.g., reacting the base with metal ions, such as calcium ions, to produce a metal hydroxide, such as Ca(OH) 2 ).
  • the metal hydroxide can be used in cement-making processes.
  • production of the acid near the second electrode and/or production of the base near the first electrode results in production of a gas (e.g., CO 2 , H 2 , and/or O 2 ).
  • a gas e.g., CO 2 , H 2 , and/or O 2
  • one or more of the gases can be collected, sold, used in a downstream process, and/or fed back into the system.
  • production of the acid near the second electrode and/or production of the base near the first electrode produces a reduced amount of gas, does not produce a gas, and/or does not produce a net amount of gas, as any produced gas is used by the system (e.g., to increase the pH gradient between the electrodes).
  • the acid produced near the second electrode and/or the base produced near the first electrode for example, during periods of low electricity cost, can be used to produce hydrogen gas and/or oxygen gas, for example, in periods of high electricity cost.
  • Inventive systems and methods for formation of precipitates in a spatially varying chemical composition gradient are also described.
  • Formation of precipitates in a spatially varying chemical composition gradient can be achieved, for example, by dissolving a chemical compound (e.g., a metal salt) in a first region (e.g., an acidic region) of the spatially varying chemical composition gradient (e.g., the spatially varying pH gradient) and collecting a precipitate comprising one or more elements (e.g., metal) from the chemical compound (e.g., the metal salt) in a second region (e.g., an alkaline region) of the spatially varying chemical composition gradient (e.g., spatially varying pH gradient).
  • a chemical compound e.g., a metal salt
  • the spatially varying chemical composition gradient (e.g., spatially varying pH gradient) is in an electrochemical cell and is established and/or maintained by electrolysis (e.g., electrolysis of water).
  • electrolysis e.g., electrolysis of water
  • the precipitate is heated within a kiln to make cement, such as Portland cement.
  • the subject matter of the present invention involves, in some cases, interrelated products, alternative solutions to a particular problem, and/or a plurality of different uses of one or more systems and/or articles.
  • the method comprises running a reactor in a first mode; wherein the first mode comprises: producing base from a first electrode; producing acid from a second electrode that is electrochemically coupled to the first electrode in the reactor; and collecting the acid and/or base.
  • the method comprises running a reactor in a first mode; wherein the first mode comprises: producing base from a first electrode; producing acid from a second electrode that is electrochemically coupled to the first electrode in the reactor; collecting the acid and/or base; and reacting the collected acid and/or base in a chemical dissolution and/or in a precipitation reaction.
  • the method comprises running a reactor in a first mode; wherein the first mode comprises: producing base and hydrogen gas from a first electrode; producing acid and oxygen gas from a second electrode that is electrochemically coupled to the first electrode in the reactor; and allowing the oxygen gas to diffuse and/or be transported to the first electrode and/or allowing the hydrogen gas to diffuse and/or be transported to the second electrode; and allowing the oxygen gas to be reduced by the first electrode and/or allowing the hydrogen gas to be oxidized by the second electrode.
  • the method comprises producing a base and a dihalide in a first reactor; producing an acid in a second reactor; collecting the acid; collecting the base; performing a chemical dissolution with the acid and/or base; and performing a precipitation reaction with the acid and/or base.
  • the system comprises a first electrode; a second electrode that is electrochemically coupled to the first electrode; and an apparatus configured to collect an acidic output near the second electrode and/or a basic output near the first electrode.
  • the system comprises a first electrode; a second electrode that is electrochemically coupled to the first electrode; a first apparatus configured to collect an acidic output near the second electrode and/or a basic output near the first electrode; and a second apparatus configured to react the collected acidic output and/or collected basic output.
  • the system comprises a first electrode configured to produce base and hydrogen gas; and a second electrode that is electrochemically coupled to the first electrode and is configured to produce acid and oxygen gas; wherein the system is configured to allow oxygen gas to diffuse and/or be transported to the first electrode and/or to allow hydrogen gas to diffuse and/or be transported to the second electrode; and wherein the system is configured to allow the oxygen gas to be reduced by the first electrode and/or to allow the hydrogen gas to be oxidized by the second electrode.
  • the system comprises a first reactor configured to produce a base, a dihalide, and hydrogen gas; a second reactor configured to produce an acid; a first apparatus configured to collect the acid near the second reactor and perform a chemical dissolution and/or precipitation reaction with the acid; and a second apparatus configured to collect the base near the first reactor and perform a chemical dissolution and/or precipitation reaction with the base.
  • FIG. 1A is, in accordance with certain embodiments, a schematic illustration of a system comprising a first electrode, a second electrode, and an apparatus.
  • FIG. 1B is, in accordance with certain embodiments, a schematic illustration of a system comprising a first electrode, a second electrode, and two apparatuses.
  • FIG. 1C is, in accordance with certain embodiments, a schematic illustration of a system comprising a first electrode, a second electrode, an apparatus, and a separator.
  • FIG. 1D is, in accordance with certain embodiments, a schematic illustration of a system comprising a first electrode, a second electrode, and three apparatuses.
  • FIG. 1E is, in accordance with certain embodiments, a schematic illustration of a system comprising a first electrode, a second electrode, and six apparatuses.
  • FIG. 1F is, in accordance with certain embodiments, a schematic illustration of a system comprising a first electrode, a second electrode, an apparatus, and a kiln.
  • FIG. 2A is, in accordance with certain embodiments, a cross-sectional schematic illustration of a system that comprises a first electrode and a second electrode, and generates hydrogen gas and oxygen gas.
  • FIG. 2B is, in accordance with certain embodiments, a cross-sectional schematic illustration of a system that comprises a first electrode, a second electrode, and a separator, and generates hydrogen gas and oxygen gas.
  • FIG. 2C is, in accordance with certain embodiments, a cross-sectional schematic illustration of a system that comprises a first electrode, a second electrode, a separator, and two apparatuses, and generates hydrogen gas and oxygen gas.
  • FIG. 2D is, in accordance with certain embodiments, a schematic illustration of a system that comprises a first electrode, a second electrode, a separator, two apparatuses, and a kiln, and generates hydrogen gas and oxygen gas.
  • FIG. 3A is, in accordance with certain embodiments, a schematic illustration of a system comprising two reactors.
  • FIG. 3B is, in accordance with certain embodiments, a schematic illustration of a system comprising two reactors, wherein the first reactor comprises a first electrode and second electrode.
  • FIG. 4A is, in accordance with certain embodiments, a schematic illustration of a system comprises two chambers.
  • FIG. 4B is, in accordance with certain embodiments, a schematic illustration of a system comprising two chambers where CaCO 3 is dissolved in one chamber and
  • FIG. 5A is, in accordance with certain embodiments, a schematic illustration of operation of a reactor in high-voltage mode.
  • FIG. 5B is a Pourbaix diagram illustrating high-voltage mode.
  • FIG. 6A is, in accordance with certain embodiments, a schematic illustration of operation of a reactor in low-voltage mode.
  • FIG. 6B is a Pourbaix diagram illustrating low-voltage mode.
  • FIG. 7 is a plot of electricity cost versus time for a 1 kW alkaline electrolyzer operating at 1.2 V (solid line) and for an electrolyzer (dotted line) consuming the same amount of current operating at 2 V when the cost of electricity is >0.05 $/kWh and at 0.4 V when the cost of electricity is ⁇ 0.05 $/kWh.
  • FIG. 8A is, in accordance with certain embodiments, a schematic illustration of operation of a reactor in low-voltage mode A.
  • FIG. 8B is a Pourbaix diagram illustrating low-voltage mode A.
  • FIG. 9A is, in accordance with certain embodiments, a schematic illustration of operation of a reactor in low-voltage mode B.
  • FIG. 9B is a Pourbaix diagram illustrating low-voltage mode B.
  • FIG. 10A is, in accordance with certain embodiments, a schematic illustration of operation of a reactor in fuel cell mode.
  • FIG. 10B is a Pourbaix diagram illustrating fuel cell mode.
  • FIG. 11 is, in accordance with certain embodiments, a flow chart showing electrolysis of neutral-pH water to make acid/base for making precipitated hydroxides, in accordance with some embodiments.
  • FIG. 12 is, in accordance with certain embodiments, a flow chart showing electrolysis of alkali halide electrolytes to make acid/base for making precipitated hydroxides, in accordance with certain embodiments.
  • FIGS. 13A-13B show that the OH ⁇ is charge-balanced by the cation in the electrolyte that crosses the diaphragm or membrane, in accordance with certain embodiments.
  • FIG. 13A is, in accordance with certain embodiments, an illustration showing that at the first electrode (e.g., the cathode) of Reactor 1, water is reduced to give OH ⁇ (an alkali solution) and H 2 (g) .
  • FIG. 13B is, in accordance with certain embodiments, an illustration showing that at the first electrode (e.g., the cathode) of Reactor 1, O 2 is reduced to give OH ⁇ (an alkali solution).
  • FIGS. 14A-14B show chemical dissolution and precipitation reactions, in accordance with certain embodiments.
  • FIG. 14A is, in accordance with certain embodiments, a schematic showing that the dihalide is reacted with hydrogen gas to produce the desired acid.
  • FIG. 14B is, in accordance with certain embodiments, a schematic showing that the dihalide is reacted with water to produce the desired acid, and oxygen as a byproduct.
  • a method comprises producing base near a first electrode (e.g., cathode) and acid near a second electrode (e.g., anode) that is electrochemically coupled to the first electrode.
  • the method comprises collecting the acid and/or base.
  • the method comprises storing the acid and/or base.
  • the method comprises reacting the acid and/or base in a chemical dissolution (e.g., reacting the acid with a metal carbonate, such as CaCO 3 , to produce metal ions, such as calcium ions, and/or carbonate ions).
  • the method comprises reacting the acid and/or base in a precipitation reaction (e.g., reacting the base with metal ions, such as calcium ions, to produce a metal hydroxide, such as Ca(OH) 2 ).
  • a precipitation reaction e.g., reacting the base with metal ions, such as calcium ions, to produce a metal hydroxide, such as Ca(OH) 2 ).
  • the metal hydroxide can be used in cement-making processes.
  • production of the acid near the second electrode and/or production of the base near the first electrode results in production of a gas (e.g., CO 2 , H 2 , and/or O 2 ).
  • a gas e.g., CO 2 , H 2 , and/or O 2
  • one or more of the gases can be collected, sold, used in a downstream process, and/or fed back into the system.
  • production of the acid near the second electrode and/or production of the base near the first electrode produces a reduced amount of gas, does not produce a gas and/or does not produce a net amount of gas, as any produced gas is used by the system (e.g., to increase the pH gradient between the electrodes).
  • the acid produced near the second electrode and/or the base produced near the first electrode for example, during periods of low electricity cost, can be used to produce hydrogen gas and/or oxygen gas, for example, in periods of high electricity cost.
  • Electrochemical reactors comprise spatially varying chemical composition gradients (e.g., spatially varying pH gradients).
  • precipitates are formed using a spatially varying chemical composition gradient (e.g., spatially varying pH gradient).
  • a chemical compound e.g., a metal salt
  • a first region e.g., an acidic region
  • a precipitate comprising one or more elements (e.g., metal) from the chemical compound (e.g., the metal salt) is formed in a second region (e.g., an alkaline region) of the spatially varying chemical composition gradient (e.g., the spatially varying pH gradient).
  • Some embodiments concern compositions, methods, and reactor designs in which an electrolytic reaction is used to produce a chemical composition gradient between the positive and negative electrodes of an electrochemical cell. Said electrolytically produced composition gradient is then employed, in some embodiments, to conduct a desired chemical reaction by feeding a reactant to the chemical environment near one electrode, and using the electrolytically produced chemical gradient to produce a product from said reactant as the reactant or its components diffuse toward the other electrode.
  • a desired chemical reaction is conducted by collecting solutions or suspensions of differing composition produced electrolytically, and using said solutions or suspensions to produce a product from said reactant in a portion of the reactor or in a separate apparatus.
  • such a reactor is directed to the production of a decomposed, mineral or metal salt through electrochemical and chemical means.
  • the use of fossil fuels for production of thermal energy, and the associated production of greenhouse gases or gases that are atmospheric pollutants is reduced or avoided through the use of such a reactor in place of traditional thermal calcination that involves heating of the mineral or metal salt to decompose it.
  • the mineral or metal salt comprises a metal carbonate, and the greenhouse gases produced are at least in part carbon dioxide.
  • the electrolytically driven chemical reactor is powered by electricity from renewable sources such as solar photovoltaics or wind energy, and thereby reduces the use of greenhouse-gas-producing energy sources in carrying out the calcination or decomposition reaction.
  • Some embodiments are related to a process for the production of cement, such as Portland cement. Concrete is today the most widely used man-made material in the world. Cement production is also the second largest industrial emitter of CO 2 in the world, accounting for about 8% of global CO 2 emissions. Traditional methods for industrial production of cement include the calcination of CaCO 3 by thermal means. In current manufacturing of cement, about 60% of the CO 2 emissions result from the calcination of CaCO 3 , and about 40% of the CO 2 emissions result from the burning of fossil fuels to carry out the calcination and sintering processes. Thus, there exists a great need for cement production processes that emit less CO 2 . Some embodiments are related to a cement production process in which thermal calcination is replaced by herein-described electrochemical processes that produce less CO 2 per quantity of cement produced than current manufacturing.
  • Cement production systems comprising electrochemical reactors, and related methods, are also described. Certain embodiments are related to inventive systems for producing cement comprising an electrochemical reactor and a kiln.
  • the electrochemical reactor is configured to receive CaCO 3 .
  • the electrochemical reactor comprises a first outlet configured to discharge Ca(OH) 2 and/or lime (CaO).
  • the electrochemical reactor comprises a second outlet configured to discharge CO 2 , O 2 , and/or H 2 gas.
  • the kiln is configured to heat the Ca(OH) 2 and/or lime (and/or a reaction product thereof) as part of a cement-making process.
  • the system is powered at least in part (e.g., at least 10%, at least 25%, at least 50%, at least 75%, at least 90%, or 100%) by renewable electricity (e.g., solar energy and/or wind energy).
  • renewable electricity e.g., solar energy and/or wind energy.
  • the system has lower net carbon emissions (e.g., at least 10% lower, at least 25% lower, at least 50% lower, at least 75% lower, or at least 90% lower) than substantially similar systems that use traditional thermal calcination instead of the electrochemical reactor.
  • the system has net-zero carbon emissions.
  • Certain embodiments are related to inventive methods in which Ca(OH) 2 and/or lime (CaO) is produced in an electrochemical reactor.
  • the Ca(OH) 2 and/or lime from the electrochemical reactor is then transported to a kiln, which heats the Ca(OH) 2 and/or lime (and/or a reaction product thereof) as part of a cement-making process.
  • the electrochemical reactor also produces CO 2 , O 2 , and/or H 2 gas.
  • the CO 2 is sequestered, used in liquid fuel, used in oxyfuel, used in enhanced oil recovery, used to produce dry ice, and/or used as an ingredient in a beverage.
  • the O 2 can be sequestered, used in oxyfuel, used in a CCS application, and/or used in enhanced oil recovery.
  • the H 2 can be sequestered and/or used as a fuel (e.g., in a fuel cell and/or to heat the system).
  • at least a portion e.g., at least 10%, at least 25%, at least 50%, at least 75%, at least 90%, or all) of the CO 2 , O 2 , and/or H 2 discharged from the system is fed into the kiln.
  • FIGS. 1A-3B Non-limiting examples of such systems are shown in FIGS. 1A-3B .
  • the system comprises a first electrode.
  • the first electrode comprises a cathode.
  • system 100 comprises first electrode 104 (e.g., cathode).
  • system 200 comprises first electrode 104 (e.g., cathode).
  • the first electrode is selected to be an electronic conductor that is stable under relatively alkaline conditions (e.g., in an alkaline region and/or base described herein).
  • the first electrode comprises a metallic electrode (such as platinum, gold, nickel, iridium, copper, iron, steel, stainless steel, manganese, and/or zinc), carbon (such as graphite or disordered carbons), or a metal carbide (such as silicon carbide, titanium carbide, and/or tungsten carbide).
  • a metallic electrode such as platinum, gold, nickel, iridium, copper, iron, steel, stainless steel, manganese, and/or zinc
  • carbon such as graphite or disordered carbons
  • a metal carbide such as silicon carbide, titanium carbide, and/or tungsten carbide.
  • the first electrode comprises a metal alloy (e.g. a nickel-chromium-iron alloy, nickel-molybdenum-cadmium alloy), a metal oxide (e.g.
  • electrocatalyst or electrode material is dispersed or coated onto a conductive support.
  • the system comprises a second electrode.
  • the second electrode comprises an anode.
  • system 100 comprises second electrode 105 (e.g., an anode).
  • system 200 comprises second electrode 105 (e.g., an anode).
  • the second electrode is electrochemically coupled to the first electrode. That is to say, the electrodes can be configured such that they are capable of participating in an electrochemical process. Electrochemical coupling can be achieved, for example, by exposing the first and second electrodes to an electrolyte that facilitates ionic transport between the two electrodes.
  • first electrode 104 is electrochemically coupled to second electrode 105 .
  • first electrode 104 is electrochemically coupled to second electrode 105 .
  • the second electrode is selected to be an electronic conductor that is stable under relatively acidic conditions (e.g., in an acidic region and/or acid described herein).
  • the second electrode comprises a metallic electrode (such as platinum, palladium, lead, and/or tin) or a metal oxide (such as a transition metal oxide).
  • the first electrode and/or the second electrode comprise catalysts.
  • the cathode catalyst is selected to be stable under alkaline conditions.
  • the cathode catalyst can comprise, in some embodiments, nickel, iron, a transition metal sulfide (such as molybdenum sulfide), and/or a transition metal oxide (such as MnO 2 , Mn 2 O 3 , Mn 3 O 4 , nickel oxide, nickel hydroxide, iron oxide, iron hydroxide, cobalt oxide), a mixed transition metal spinel oxide (such as MnCo 2 O 4 , CoMn 2 O 4 , MnFe 2 O 4 , ZnCoMnO 4 ), and the like.
  • the anode catalyst is selected to be stable under acidic conditions.
  • the anode catalyst comprises platinum, iridium or their oxides.
  • the system comprises a reactor (e.g., an electrochemical reactor).
  • system 100 comprises a reactor.
  • system 200 comprises a reactor.
  • the reactor comprises the first electrode and the second electrode.
  • the first electrode is electrochemically coupled to the second electrode in the reactor.
  • first electrode 104 is electrochemically coupled to second electrode 105 in the reactor.
  • first electrode 104 is electrochemically coupled to second electrode 105 in the reactor.
  • the method comprises running a reactor (e.g., any reactor described herein).
  • running the reactor comprises applying current to an electrode of the reactor.
  • running the reactor results in at least one chemical reaction occurring within the reactor.
  • the method comprises running a reactor in a first mode.
  • the first mode comprises producing base near the first electrode (e.g., base is produced as a result of an electrochemical reaction in the first electrode).
  • the first mode comprises producing base near first electrode 104 .
  • the first mode comprises producing base near first electrode 104 .
  • the first electrode (e.g., in the first mode) is configured to produce a basic output (e.g., any of the bases described herein).
  • the basic output is produced as a result of an electrochemical reaction in the first electrode.
  • first electrode 104 is configured to produce base.
  • first electrode 104 is configured to produce base.
  • the base may have any of a variety of suitable concentrations.
  • the base has a concentration of greater than or equal to 0.000001 M, greater than or equal to 0.00001 M, greater than or equal to 0.0001 M, greater than or equal to 0.001 M, greater than or equal to 0.01 M, greater than or equal to 0.1 M, greater than or equal to 0.5 M, greater than or equal to 1 M, greater than or equal to 3 M, greater than or equal to 5 M, greater than or equal to 7 M, greater than or equal to 10 M, greater than or equal to 15 M, or greater than or equal to 20 M.
  • the base has a concentration of less than or equal to 25 M, less than or equal to 20 M, less than or equal to 15 M, less than or equal to 10 M, less than or equal to 7 M, less than or equal to 5 M, or less than or equal to 3 M. Combinations of these ranges are also possible (e.g., greater than or equal to 0.1 M and less than or equal to 25 M or greater than or equal to 0.1 M and less than or equal to 10 M).
  • the production of the base by the first electrode results in an alkaline region (e.g., any alkaline region described herein) near the first electrode (e.g., within the half of the reactor compartment that is closest to the first electrode).
  • the fluid adjacent the first electrode e.g., the alkaline region
  • the system comprises alkaline region 106 near first electrode 104 .
  • the system comprises an alkaline region near first electrode 104 .
  • the pH near (e.g., adjacent to) the first electrode is greater than or equal to 8, greater than or equal to 9, greater than or equal to 10, greater than or equal to 11, greater than or equal to 12, or greater than or equal to 13.
  • the pH near the first electrode is less than or equal to 14, less than or equal to 13, less than or equal to 12, less than or equal to 11, or less than or equal to 10. Combinations of these ranges are also possible (e.g., greater than or equal to 8 and less than or equal to 14).
  • the second electrode is configured to produce an acidic output (e.g., any of the acids described herein).
  • the acidic output is produced as a result of an electrochemical reaction in the second electrode.
  • second electrode 105 is configured to produce acid.
  • second electrode 105 is configured to produce acid.
  • the first mode of the reactor comprises producing acid near the second electrode (e.g., acid is produced as a result of an electrochemical reaction in the second electrode).
  • the first mode comprises producing acid near second electrode 105 .
  • the first mode comprises producing acid near second electrode 105 .
  • the acid may have any of a variety of suitable concentrations.
  • the acid has a concentration of greater than or equal to 0.000001 M, greater than or equal to 0.00001 M, greater than or equal to 0.0001 M, greater than or equal to 0.001 M, greater than or equal to 0.01 M, greater than or equal to 0.1 M, greater than or equal to 0.5 M, greater than or equal to 1 M, greater than or equal to 3 M, greater than or equal to 5 M, greater than or equal to 7 M, or greater than or equal to 10 M.
  • the acid has a concentration of less than or equal to 12 M, less than or equal to 10 M, less than or equal to 7 M, less than or equal to 5 M, less than or equal to 3 M, or less than or equal to 1 M. Combinations of these ranges are also possible (e.g., greater than or equal to 0.000001 M and less than or equal to 12 M or greater than or equal to 0.1 M and less than or equal to 10 M).
  • the production of the acid by the second electrode results in an acidic region (e.g., any acidic region described herein) near the second electrode (e.g., within the half of the reactor compartment that is closest to the second electrode).
  • the fluid adjacent the second electrode e.g., the acidic region
  • the system comprises acidic region 107 near second electrode 105 .
  • the system comprises acidic region 107 near second electrode 105 .
  • the pH near (e.g., adjacent to) the second electrode has a pH of less than or equal to 6, less than or equal to 5, less than or equal to 4, less than or equal to 3, less than or equal to 2, or less than or equal to 1.
  • the pH near the second electrode has a pH of greater than or equal to 0, greater than or equal to 1, greater than or equal to 2, greater than or equal to 3, greater than or equal to 4, or greater than or equal to 5. Combinations of these ranges are also possible (e.g., greater than or equal to 0 and less than or equal to 6).
  • the first electrode e.g., cathode
  • the first electrode is configured to produce hydrogen gas, such that hydrogen gas can be produced near the first electrode (e.g., the hydrogen gas is produced as a result of an electrochemical reaction in the first electrode).
  • first electrode 104 is configured to produce hydrogen gas 108 .
  • first electrode 104 is configured to produce hydrogen gas.
  • running the reactor in the first mode comprises producing hydrogen gas (e.g., hydrogen gas and base) near the first electrode (e.g., hydrogen gas is produced as a result of an electrochemical reaction in the first electrode).
  • the hydrogen gas and/or base are produced near the first electrode by reduction of water near the first electrode.
  • the second electrode (e.g., anode) is configured to produce oxygen, such that oxygen gas can be produced near the second electrode (e.g., the oxygen gas is produced as a result of an electrochemical reaction in the second electrode).
  • second electrode 105 is configured to produce oxygen gas 109 .
  • second electrode 105 is configured to produce oxygen gas.
  • running the reactor in the first mode comprises producing oxygen gas (e.g., oxygen gas and acid) near the second electrode (e.g., oxygen gas is produced as a result of an electrochemical reaction in the second electrode).
  • the oxygen gas and/or acid are produced near the second electrode by oxidation of water near the second electrode.
  • the system is configured to allow oxygen gas to diffuse and/or be transported to a location near the first electrode (e.g., from a location near the second electrode).
  • the system is configured to allow oxygen gas to diffuse and/or be transported to fluid near the first electrode, such that the oxygen gas could be involved in an electrochemical reaction in the first electrode, from fluid near the second electrode, after the oxygen gas was produced as a result of an electrochemical reaction in the second electrode.
  • system 200 is configured to allow oxygen gas 109 to diffuse and/or be transported from second electrode 105 to first electrode 104 .
  • system 100 is configured to allow oxygen gas to diffuse and/or be transported from second electrode 105 to first electrode 104 .
  • the system is configured to allow the oxygen gas to be reduced near the first electrode (e.g., the oxygen gas is reduced as a result of an electrochemical reaction in the first electrode).
  • system 200 is configured to allow oxygen gas 109 to be reduced near first electrode 104 .
  • system 100 is configured to allow oxygen gas to be reduced near first electrode 104 .
  • reducing the oxygen gas near the first electrode comprises production of base.
  • the production of base is advantageous because it increases the overall amount of base produced at the first electrode.
  • the system is configured to allow hydrogen gas to diffuse and/or be transported to a location near the second electrode (e.g., from a location near the first electrode).
  • the system is configured to allow hydrogen gas to diffuse and/or be transported to fluid near the second electrode, such that the hydrogen gas could be involved in an electrochemical reaction in the second electrode, from fluid near the first electrode, after the hydrogen gas was produced as a result of an electrochemical reaction in the first electrode.
  • system 200 is configured to allow hydrogen gas 108 to diffuse and/or be transported from first electrode 104 to second electrode 105 .
  • system 100 is configured to allow hydrogen gas to diffuse and/or be transported from first electrode 104 to second electrode 105 .
  • the system is configured to allow the hydrogen gas to be oxidized near the second electrode (e.g., hydrogen gas is oxidized as a result of an electrochemical reaction in the second electrode).
  • system 200 is configured to allow hydrogen gas 108 to be oxidized near second electrode 105 .
  • system 100 is configured to allow hydrogen gas to be oxidized near the second electrode.
  • oxidizing the hydrogen gas near the second electrode comprises production of acid.
  • the production of acid is advantageous because it increases the overall amount of acid produced at the second electrode.
  • the system comprises a separator.
  • system 100 comprises separator 124 .
  • system 200 comprises separator 124 .
  • the separator is configured to allow oxygen gas produced at the second electrode to diffuse to the first electrode and/or to allow hydrogen gas produced at the first electrode to diffuse to the second electrode.
  • the separator is permeable to oxygen gas and/or hydrogen gas.
  • separator 124 is configured to allow oxygen gas produced at the second electrode to diffuse to the first electrode and/or to allow hydrogen gas produced at the first electrode to diffuse to the second electrode.
  • separator 124 is configured to allow oxygen gas produced at the second electrode to diffuse to the first electrode and/or to allow hydrogen gas produced at the first electrode to diffuse to the second electrode.
  • the hydrogen gas and/or oxygen gas could be transported with a syringe (e.g., if the reactor had an inlet near one electrode for a syringe and an outlet near the other electrode for a syringe, the gas could be transported from one electrode to the other with a syringe).
  • the hydrogen gas and/or oxygen gas could be transported via a conduit (e.g., a pipe, channel, needle, or tube).
  • the hydrogen gas and/or oxygen gas could be transported directly from one electrode to another, or the hydrogen gas and/or oxygen gas could be stored after removal from the reactor until it is added back into the reactor.
  • the hydrogen gas and/or oxygen gas is transported continuously or in batches.
  • the hydrogen gas and/or oxygen gas is transported automatically or manually.
  • hydrogen gas produced by hydrolysis may be electrochemically oxidized using the hydrogen oxidation reaction (HOR) in which one dihydrogen molecule reacts to form two protons and two electrons.
  • oxygen gas produced by hydrolysis may be electrochemically reduced in the oxygen reduction reaction (ORR) wherein one dioxygen molecule reacts with two water molecules and four electrons to form four hydroxyl ions.
  • the HOR reaction is used to lower the pH or increase the proton concentration of the acidic solution produced by the reactor.
  • the ORR reaction is used to increase the pH or increase the hydroxyl concentration of the basic solution produced by the reactor.
  • HOR and ORR reactions as herein described may be carried out, in some cases, using separate electrodes from those used for the electrolysis reaction of the reactor.
  • these electrodes may be located within the electrolysis reactor, for example, as a combustion electrode where the hydrogen and oxygen combustion reaction produces water that remains within the reactor.
  • the electrodes used for combustion, or for HOR or ORR may, in some instances, also be located in a separate vessel or reactor, to which the hydrogen or oxygen gas is each delivered.
  • the hydrogen produced at the cathode of the electrolysis reactor is delivered to an HOR electrode connected to the anode side of the reactor, where HOR is conducted and the protons produced thereby increase the acid concentration (lowering the pH) of the acidic solution that is produced by the reactor.
  • the oxygen produced at the anode of the electrolysis reactor is delivered to an ORR electrode connected to the cathode side of the reactor, where ORR is conducted and the hydroxyl ions produced thereby increase the hydroxyl concentration (increasing the pH) of the alkaline solution that is produced by the reactor.
  • the HOR reaction is preferentially conducted over the ORR reaction to reduce the release of hydrogen as compared to the less reactive oxygen to the external environment.
  • the electrodes used for hydrogen-oxygen combustion or HOR or ORR may, in some cases, comprise compounds that function as electrocatalysts.
  • Hydrogen-oxygen combustion catalysts have been described, for example, in “Catalytic Combustion of Hydrogen—Its Role in Hydrogen Utilization,” by M Haruta and H Sano, International Journal of Hydrogen Energy, Vol. 6, No. 6, pp. 601-608, 1981, which is hereby incorporated by reference.
  • electrocatalysts for HOR and ORR include platinum group metals such as Pt, Pd, Ru, Rh, Os, and Jr, non-platinum group metals such as Mo, Fe, Ti, W, Cr, Co, Cu, Ag, Au, and Re, used individually or as alloys or mixtures; high surface area nickel-aluminum alloys known as Raney nickel, optionally coated or doped with other catalysts.
  • electrocatalysts selective for ORR include metallic iron, iron oxides, iron sulfide, and iron hydroxide, silver alloys, oxides and nitrate, and various forms of carbons including carbon paper, carbon felt, graphite, carbon black, and nanoscale carbons.
  • the gaseous byproducts produced by electrolysis may have value and may be sold for use in other applications and processes, including combustion in a fuel cell or gas turbine or internal combustion engine for the purpose of producing energy and power, including electric power.
  • one or more of the gases produced by the reactor are recombined.
  • recombination refers to chemical or electrochemical reactions that consume one or more of the gases produced.
  • hydrogen and oxygen produced by hydrolysis are recombined using hydrogen-oxygen combustion to form water.
  • hydrogen gas 108 produced by first electrode 104 can be recombined with oxygen gas 109 to form water, as shown in FIG. 6A .
  • hydrogen gas produced by first electrode 104 can be recombined with oxygen gas to form water.
  • hydrogen-oxygen recombination may take place within or external to the reactor, and may, in some cases, use electrode materials and designs, and optionally catalysts, well-known to those skilled in the art.
  • the method does not produce net hydrogen gas (or the net amount of hydrogen gas produced is less than 5% (e.g., less than 2% or less than 1%) of the current supplied to the reactor).
  • the method does not release any hydrogen gas (or the amount of hydrogen gas released is less than 5% (e.g., less than 2% or less than 1%) of the current supplied to the reactor) to the atmosphere, as the hydrogen gas produced is recombined with oxygen to form water.
  • the method does not produce net oxygen gas (or the net amount of oxygen gas produced is less than 5% (e.g., less than 2% or less than 1%) of the current supplied to the reactor).
  • the method does not release any oxygen gas (or the net amount of oxygen gas released is less than 5% (e.g., less than 2% or less than 1%) of the current supplied to the reactor) to the atmosphere, as the oxygen gas produced is recombined with hydrogen to form water.
  • hydrolysis is carried out under conditions that produce a basic pH near the first electrode (e.g., the cathode), and an acidic pH near the second electrode (e.g., the anode), without liberating hydrogen gas or oxygen gas (or the amount of hydrogen gas or oxygen gas liberated is less than 5% (e.g., less than 2% or less than 1%) of the current supplied to the reactor), respectively.
  • O 2 could diffuse (e.g., through electrolyte 235 of FIG.
  • this reaction would occur at pH>7 and an electrode potential less than 0.8 V vs the standard hydrogen electrode.
  • H 2 could diffuse from the first electrode (e.g., the cathode), where base is produced, to the second electrode (e.g., the anode), where acid is produced and where the H 2 would be oxidized to form H + (H 2 ⁇ 2H + +2e ⁇ ). In certain instances, this would occur when the pH is ⁇ 7 and when the electrode potential is greater than ⁇ 0.41 V vs the standard hydrogen electrode. In other electrolyzers, such as an alkaline electrolyzer, this reaction is hindered by a separator that prevents the crossover of gases between the two electrodes. However, in some embodiments disclosed herein, the reactor comprises a separator that allows and/or promotes crossover of H 2 and/or O 2 , such that they can be consumed and increase the pH gradient.
  • acidic solutions are generated from neutral-pH electrolytes at electrode potentials greater than 0.8 V vs the standard hydrogen electrode.
  • the minimum electrode potential would be 1.23 V vs the standard hydrogen electrode.
  • basic solutions are generated from neutral-pH electrolytes at electrode potentials less than ⁇ 0.4 V vs the standard hydrogen electrode.
  • the maximum electrode potential would be ⁇ 0.83 V vs the standard hydrogen electrode.
  • the Nernst potential at the second electrode may be any of a variety of suitable values.
  • the Nernst potential at the second electrode e.g., the anode
  • the Nernst potential at the second electrode is greater than or equal to ⁇ 0.4 V, greater than or equal to ⁇ 0.2 V, greater than or equal to 0 V, greater than or equal to 0.5 V, greater than or equal to 0.8 V, greater than or equal to 0.9 V, greater than or equal to 1 V, greater than or equal to 1.1 V, greater than or equal to 1.2 V, greater than or equal to 1.4 V, or greater than or equal to 1.6 V vs the standard hydrogen electrode.
  • the Nernst potential at the second electrode is less than or equal to 2 V, less than or equal to 1.7 V, less than or equal to 1.5 V, less than or equal to 1.4 V, less than or equal to 1.3 V, less than or equal to 1.2 V, less than or equal to 1.1 V, less than or equal to 1 V, less than or equal to 0.9 V, less than or equal to 0.8 V, less than or equal to 0.5 V, less than or equal to 0 V, or less than or equal to ⁇ 0.2 V vs the standard hydrogen electrode.
  • Combinations of these ranges are also possible (e.g., greater than or equal to 0.8 V and less than or equal to 2 V, greater than or equal to 1.2 V and less than or equal to 2 V, greater than or equal to ⁇ 0.4 V and less than or equal to 0.5 V, or greater than or equal to 0 V and less than or equal to 0.5 V).
  • the suitable Nernst potential at the second electrode depends on the type of reaction at the electrode. For example, in some cases, the Nernst potential at the second electrode when hydrogen gas is oxidized to acid is greater than or equal to ⁇ 0.4 V vs the standard hydrogen electrode (e.g., greater than or equal to ⁇ 0.4 V and less than or equal to 0.5 V or greater than or equal to 0 V and less than or equal to 0.5 V).
  • the Nernst potential at the second electrode when water is oxidized to acid and oxygen gas is greater than or equal to 0.8 V vs the standard hydrogen electrode (e.g., greater than or equal to 0.8 V and less than or equal to 2 V or greater than or equal to 1.2 V and less than or equal to 2 V).
  • the Nernst potential at the first electrode may be any of a variety of suitable values.
  • the Nernst potential at the first electrode e.g., cathode
  • the Nernst potential at the first electrode is less than or equal to 0.8 V, less than or equal to 0.6 V, less than or equal to 0.4 V, less than or equal to 0 V, less than or equal to ⁇ 0.4 V, less than or equal to ⁇ 0.5 V, less than or equal to ⁇ 0.6 V, less than or equal to ⁇ 0.7 V, less than or equal to ⁇ 0.8 V, less than or equal to ⁇ 0.9 V, less than or equal to ⁇ 1 V, less than or equal to ⁇ 1.2 V, or less than or equal to ⁇ 1.4 V vs the standard hydrogen electrode.
  • the Nernst potential at the first electrode is greater than or equal to ⁇ 2 V, greater than or equal to ⁇ 1.7 V, greater than or equal to ⁇ 1.5 V, greater than or equal to ⁇ 1.2 V, greater than or equal to ⁇ 1 V, greater than or equal to ⁇ 0.9 V, greater than or equal to ⁇ 0.8 V, greater than or equal to ⁇ 0.7 V, greater than or equal to ⁇ 0.6 V, greater than or equal to ⁇ 0.5 V, greater than or equal to ⁇ 0.4 V, greater than or equal to 0 V, greater than or equal to 0.4 V, or greater than or equal to 0.6 V vs the standard hydrogen electrode.
  • Combinations of these ranges are also possible (e.g., greater than or equal to ⁇ 1.5 V and less than or equal to ⁇ 0.4 V, greater than or equal to ⁇ 1.5 V and less than or equal to ⁇ 0.8 V, greater than or equal to ⁇ 0.4 V and less than or equal to 0.8 V, or greater than or equal to ⁇ 0.4 V and less than or equal to 0.4 V).
  • the suitable Nernst potential at the first electrode depends on the type of reaction at the electrode. For example, in some cases, the Nernst potential at the first electrode when oxygen gas is reduced to base is less than or equal to 0.8 V vs the standard hydrogen electrode (e.g., less than or equal to 0.8 V and greater than or equal to ⁇ 0.4 V or less than or equal to 0.4 V and greater than or equal to ⁇ 0.4 V).
  • the Nernst potential at the first electrode when water is reduced to base and hydrogen gas is less than or equal to ⁇ 0.4 V vs the standard hydrogen electrode (e.g., less than or equal to ⁇ 0.4 V and greater than or equal to ⁇ 1.5 V, or less than or equal to ⁇ 0.8 V and greater than or equal to ⁇ 1.5 V).
  • the cell voltage (e.g., the voltage applied to the cell, for example, during production of acid and/or base) is greater than or equal to 0 V, greater than or equal to 0.5 V, greater than or equal to 1 V, greater than or equal to 1.23 V, greater than or equal to 1.5 V, greater than or equal to 2 V, greater than or equal to 2.06 V, or greater than or equal to 2.5 V vs the standard hydrogen electrode.
  • the cell voltage is less than or equal to 5 V, less than or equal to 4 V, less than or equal to 3 V, less than or equal to 2.5 V, less than or equal to 2.25 V, less than or equal to 2 V, less than or equal to 1.5 V, less than or equal to 1 V, or less than or equal to 0.5 V vs the standard hydrogen electrode. Combinations of these ranges are also possible (e.g., 0-5 V or 0-2.5 V).
  • the system comprises a reactor system for producing concentrated acid and base.
  • the system comprises a first reactor (e.g., any reactor described herein).
  • system 300 comprises first reactor 320 .
  • the system comprises a second reactor (e.g., any reactor described herein).
  • system 300 comprises second reactor 301 .
  • the first reactor and the second reactor are fluidically connected.
  • first reactor 320 is fluidically connected to second reactor 301 via conduit 330 .
  • a fluid e.g., a liquid or a gas
  • the method comprises diffusing and/or transporting hydrogen gas and/or dihalide from the first reactor to the second reactor.
  • the first reactor comprises an electrochemical reactor.
  • the first reactor comprises a first electrode (e.g., any first electrode described herein).
  • first reactor 320 comprises first electrode 104 .
  • the first reactor comprises a second electrode (e.g., any second electrode described herein).
  • first reactor 320 comprises second electrode 105 .
  • the second electrode is electrochemically coupled to the first electrode (e.g., the electrodes are configured such that current may flow from one electrode to the other). That is to say, the electrodes can be configured such that they are capable of participating in an electrochemical process.
  • Electrochemical coupling can be achieved, for example, by exposing the first and second electrodes to an electrolyte that facilitates ionic transport between the two electrodes.
  • first electrode 104 is electrochemically coupled to second electrode 105 .
  • the second reactor comprises a fuel cell (e.g., an H 2 /Cl 2 fuel cell).
  • the method comprises producing an acid in the second reactor.
  • second reactor 301 in FIG. 3A is configured to produce acid (e.g., any acid described herein).
  • the method comprises producing a base (e.g., any base described herein), a dihalide, and/or hydrogen gas in the first reactor.
  • first reactor 320 is configured to produce a base, a dihalide, and/or hydrogen gas.
  • the dihalide is produced near the second electrode of the first reactor (e.g., dihalide is produced as a result of an electrochemical reaction in the second electrode of the first reactor).
  • dihalide is produced near second electrode 105 of first reactor 320 .
  • the base and/or hydrogen gas is produced near the first electrode (e.g., base and/or hydrogen gas is produced as a result of an electrochemical reaction in the first electrode).
  • base and/or hydrogen gas is produced as a result of an electrochemical reaction in the first electrode.
  • base is produced near first electrode 104 .
  • the Nernst potential at the second electrode of the first reactor may be any of a variety of suitable values.
  • the Nernst potential at the second electrode (e.g., the anode) of the first reactor is greater than or equal to 1.3 V, greater than or equal to 1.5 V, greater than or equal to 1.7 V, greater than or equal to 1.9 V, greater than or equal to 2.1 V, or greater than or equal to 2.3 V vs the standard hydrogen electrode.
  • the Nernst potential at the second electrode of the first reactor is less than or equal to 2.5 V, less than or equal to 2.3 V, less than or equal to 2.1 V, less than or equal to 1.9 V, less than or equal to 1.7 V, or less than or equal to 1.5 V vs the standard hydrogen electrode. Combinations of these ranges are also possible (e.g., greater than or equal to 1.3 V and less than or equal to 2.5 V).
  • the suitable Nernst potential at the second electrode of the first reactor depends on the type of reaction at the electrode.
  • the Nernst potential at the second electrode when dihalide is produced e.g., chloride ions are being oxidized to form Cl 2
  • the standard hydrogen electrode e.g., greater than or equal to 1.3 V and less than or equal to 2.5 V.
  • Cl 2 is generated from Cl ⁇ at Nernst potentials above 1.36 V vs the standard hydrogen electrode (e.g., greater than or equal to 1.4 V, greater than or equal to 1.5 V, greater than or equal to 1.7 V, or greater than or equal to 2 V; less than or equal to 5 V, less than or equal to 3 V, less than or equal to 2 V, or less than or equal to 1.5 V; combinations are also possible) vs the standard hydrogen electrode.
  • the standard hydrogen electrode e.g., greater than or equal to 1.4 V, greater than or equal to 1.5 V, greater than or equal to 1.7 V, or greater than or equal to 2 V; less than or equal to 5 V, less than or equal to 3 V, less than or equal to 2 V, or less than or equal to 1.5 V; combinations are also possible
  • Br 2 is generated from Br ⁇ at Nernst potentials greater than 1.06 V vs the standard hydrogen electrode (e.g., greater than or equal to 1.1 V, greater than or equal to 1.2 V, greater than or equal to 1.3 V, greater than or equal to 1.5 V, or greater than or equal to 1.8 V; less than or equal to 4 V, less than or equal to 3 V, less than or equal to 2 V, or less than or equal to 1.5 V; combinations are also possible).
  • the standard hydrogen electrode e.g., greater than or equal to 1.1 V, greater than or equal to 1.2 V, greater than or equal to 1.3 V, greater than or equal to 1.5 V, or greater than or equal to 1.8 V; less than or equal to 4 V, less than or equal to 3 V, less than or equal to 2 V, or less than or equal to 1.5 V; combinations are also possible.
  • I 2 is generated from I ⁇ at Nernst potentials greater than 0.54 V vs the standard hydrogen electrode (e.g., greater than or equal to 0.6 V, greater than or equal to 0.7 V, greater than or equal to 0.8 V, greater than or equal to 0.9 V, greater than or equal to 1 V, or greater than or equal to 1.2 V; less than or equal to 3 V, less than or equal to 2 V, less than or equal to 1.5 V, less than or equal to 1.3 V, or less than or equal to 1 V; combinations are also possible).
  • the standard hydrogen electrode e.g., greater than or equal to 0.6 V, greater than or equal to 0.7 V, greater than or equal to 0.8 V, greater than or equal to 0.9 V, greater than or equal to 1 V, or greater than or equal to 1.2 V; less than or equal to 3 V, less than or equal to 2 V, less than or equal to 1.5 V, less than or equal to 1.3 V, or less than or equal to 1 V; combinations are also possible).
  • the Nernst potential at the first electrode of the first reactor may be any of a variety of suitable values.
  • the Nernst potential at the first electrode (e.g., the cathode) of the first reactor is greater than or equal to ⁇ 2 V, greater than or equal to ⁇ 1.8 V, greater than or equal to ⁇ 1.6 V, greater than or equal to ⁇ 1.4 V, greater than or equal to ⁇ 1.2 V, greater than or equal to ⁇ 1.0 V, greater than or equal to ⁇ 0.8 V, greater than or equal to ⁇ 0.6 V, greater than or equal to ⁇ 0.4 V, greater than or equal to ⁇ 0.2 V, greater than or equal to 0 V, greater than or equal to 0.2 V, greater than or equal to 0.4 V, or greater than or equal to 0.6 V vs the standard hydrogen electrode.
  • the Nernst potential at the first electrode of the first reactor is less than or equal to 0.8 V, less than or equal to 0.6 V, less than or equal to 0.4 V, less than or equal to 0.2 V, less than or equal to 0 V, less than or equal to ⁇ 0.2 V, less than or equal to ⁇ 0.4 V, less than or equal to ⁇ 0.6 V, less than or equal to ⁇ 0.8 V, less than or equal to ⁇ 1.0 V, less than or equal to ⁇ 1.2 V, less than or equal to ⁇ 1.4 V, or less than or equal to ⁇ 1.6 V vs the standard hydrogen electrode.
  • Combinations of these ranges are also possible (e.g., greater than or equal to ⁇ 2 V and less than or equal to 0.8 V, greater than or equal to ⁇ 1.4 V and less than or equal to 0.4 V, greater than or equal to ⁇ 2 V and less than or equal to ⁇ 0.4 V, or greater than or equal to ⁇ 2 V and less than or equal to ⁇ 0.8 V).
  • the suitable Nernst potential at the first electrode of the first reactor depends on the type of reaction at the electrode. For example, in some cases, the Nernst potential at the first electrode when oxygen is reduced to form base is less than or equal to 0.8 V vs the standard hydrogen electrode (e.g., greater than or equal to ⁇ 2 V and less than or equal to 0.8 V or greater than or equal to ⁇ 1.4 V and less than or equal to 0.4 V).
  • the Nernst potential at the first electrode when water is reduced to hydrogen gas and base is less than or equal to ⁇ 0.4 V vs the standard hydrogen electrode (e.g., greater than or equal to ⁇ 2 V and less than or equal to ⁇ 0.4 V, or greater than or equal to ⁇ 2 V and less than or equal to ⁇ 0.8 V).
  • the first reactor produces a base/alkaline solution, a dihalide, and hydrogen gas from an electrolyte containing a halide salt.
  • FIG. 11 shows, in accordance with certain embodiments, a neutral water electrolyzer based reactor as disclosed herein, whereby electrolysis or hydrolysis produces an acidic solution and an alkaline solution, the acidic solution being then used to decarbonate a starting metal carbonate, and the alkaline solution being then used to precipitate a metal hydroxide from the dissolved metal ions of the starting metal carbonate.
  • the volume concentrations of reactants on which such a reactor operates are determined by the pH values produced by the electrolyzer.
  • an alternative reactor concept is shown in FIG. 12 .
  • this reactor is capable of producing higher concentrations of acid and base than the reactor in FIG. 11 .
  • the system comprises a first reactor that electrolytically oxidizes a near-neutral solution of a dissolved metal salt to produce an alkaline solution, hydrogen, and a compound enriched in the anion of the metal salt.
  • the metal salt is an alkali halide salt or an alkaline earth halide salt, and said compound produced is a dihalide.
  • a second reactor produces, in accordance with certain embodiments, an acidic solution by reacting said compound and hydrogen with water.
  • Said acidic solution produced by the second reactor, and said alkaline solution produced by the first reactor are then used, in some embodiments, to, respectively, dissolve said metal carbonate releasing CO 2 , and precipitate said metal hydroxide.
  • the reactor of FIG. 12 can reach concentrations of 3 molar, 5 molar, or even higher, in certain embodiments.
  • the first reactor comprises a second electrode (e.g., the anode), a first electrode (e.g., the cathode), a semi-permeable membrane between the two electrodes, inlets for the electrolyte, and outlets for the products of electrolysis (H 2 , a dihalide, and an alkaline solution).
  • a second electrode e.g., the anode
  • a first electrode e.g., the cathode
  • a semi-permeable membrane between the two electrodes inlets for the electrolyte, and outlets for the products of electrolysis (H 2 , a dihalide, and an alkaline solution).
  • H 2 a dihalide
  • an alkaline solution e.g., a semi-permeable membrane between the two electrodes
  • inlets for the electrolyte e.g., the cathode
  • a semi-permeable membrane between the two electrodes
  • inlets for the electrolyte e.g.,
  • the aqueous solution comprises halide anions (for example, F ⁇ , Cl ⁇ , Br ⁇ , I ⁇ ) and the corresponding cations (for example, Li + , Na + , K+, NH 4 + , Mg 2+ , Ca 2+ ).
  • the concentration of halide salt in the electrolyte may be anywhere from 0.01-50% by weight.
  • the electrolyte is introduced to the second electrode (e.g., the anode) by an inlet.
  • the active material on the second electrode's surface may comprise platinum, graphite, platinized titanium, mixed metal oxides, mixed metal oxide-clad titanium, platinized metal oxides (e.g. platinized lead oxide, manganese dioxide), platinized ferrosilicon, platinum-iridium alloys, ruthenium oxides, titanium oxides, ruthenium and/or titanium mixed metal oxides.
  • halide anions are oxidized to produce dihalides (e.g. Cl 2 . Br 2 , I 2 ).
  • dihalides e.g. Cl 2 . Br 2 , I 2
  • oxidation of dissolved Cl ⁇ gives Cl 2 gas.
  • oxidation of Br ⁇ gives Br 2
  • a fuming liquid gives 12
  • oxidation of I ⁇ gives 12, a solid.
  • the dihalide is collected from the electrolyzer, in some cases, through an outlet and is used to make acid in a subsequent step, described below.
  • the electrolyte containing a cation e.g. Li + , Na + , K + , NH 4 +
  • the semipermeable membrane a diaphragm, or an ion-exchange membrane
  • the diaphragm or membrane prevents the alkali solution generated at the first electrode from increasing the pH at the second electrode.
  • the first electrode's surface may comprise electrocatalytic compounds.
  • electrocatalytic compounds include platinum, platinized titanium, mixed metal oxide-clad titanium, platinized metal oxides (e.g. platinized lead oxide, manganese dioxide), platinized ferrosilicon, platinum-iridium alloys, stainless steel, graphite, unalloyed titanium, stainless steel, nickel, nickel oxides.
  • the second electrode comprises a metallic electrode, such as platinum, gold, nickel, iridium, copper, iron, steel, stainless steel, manganese, and zinc, or a carbon, such as graphite or disordered carbons, or a metal carbide, such as silicon carbide, titanium carbide, or tungsten carbide.
  • the second electrode comprises a metal alloy (e.g. a nickel-chromium-iron alloy, nickel-molybdenum-cadmium alloy), a metal oxide (e.g. iridium oxide, nickel iron cobalt oxide, nickel cobalt oxide, lithium cobalt oxide, lanthanum strontium cobalt oxide, barium strontium ferrous oxide, manganese molybdenum oxide, ruthenium dioxide, iridium ruthenium tantalum oxide), a metal organic framework, or a metal sulfide (e.g. molybdenum sulfide).
  • the electrocatalyst or electrode material is dispersed or coated onto a conductive support.
  • the first electrode e.g., the cathode
  • water is reduced to give OH ⁇ (an alkali solution) and H 2(g) :
  • O 2 is reduced to give OH ⁇ (an alkali solution); see FIG. 13A .
  • the OH ⁇ is charge-balanced by the cation in the electrolyte that crosses the diaphragm or membrane, as shown, for example, in FIG. 13 .
  • the alkali hydroxide solution e.g. NaOH, KOH
  • the H 2 is collected from the reactor from a different outlet.
  • Reactor 1 produces an alkaline solution at one electrode, and hydrogen and a dihalide (in the instance where the metal salt is a metal halide) at the other electrode.
  • Reactor 2 is a reactor that produces an acid by reacting the hydrogen gas and dihalide produced at the anode of Reactor 1, or by reacting the dihalide with water.
  • the reactor comprises a first chamber, an inlet through which H 2 is introduced to the first chamber, a second inlet through which the dihalide is introduced to the first chamber, and an outlet through which the hydrogen halide (e.g.
  • HCl, HBr, HI is removed from the first chamber, an inlet through which the hydrogen halide is introduced to a second chamber, an inlet through which water is introduced to a second chamber, and an outlet through which an aqueous, acidic solution of the hydrogen halide is removed from the second chamber.
  • the dihalide reacts with H 2 to form a hydrogen halide.
  • the reaction between H 2 and the dihalide may be assisted by heating or irradiation by electromagnetic waves. For example, in some embodiments, if the dihalide is Cl 2 , the following reaction takes place in Reactor 2:
  • the hydrogen halide in the second chamber, is dissolved in water to make an acidic solution.
  • HCl could be dissolved in water to make protons.
  • the dihalide is reacted with water to produce the desired acid, and oxygen as a byproduct.
  • the exemplary reactor comprises a first chamber, an inlet through which H 2 O is introduced to the first chamber, and a second inlet through which the dihalide is introduced to the first chamber.
  • the reactor also comprises an outlet through which the hydrogen halide (e.g. HCl, HBr, HI) is removed from the first chamber, and an outlet through which O 2 is removed from the first chamber.
  • the reaction between chlorine as an exemplary dihalide and water is:
  • the relative amounts of the dihalide and water will determine whether the pure hydrogen halide, or an admixture of the hydrogen halide and water, including for example a solution of the hydrogen halide in water, is produced.
  • the reactor may comprise a second chamber where the hydrogen halide is dissolved in water to make an acidic solution with an inlet through which the hydrogen halide is introduced, an inlet through which water is introduced to the second chamber, and an outlet through which an aqueous, acidic solution of the hydrogen halide is removed from the reactor, as shown in FIG. 14B .
  • the system comprises an apparatus.
  • the system comprises first apparatus 118 .
  • the system comprises first apparatus 118 .
  • the apparatus is a container (e.g., a container that is not open to the atmosphere).
  • the apparatus is configured to collect one or more products or byproducts of the reactor (e.g., acid, base, hydrogen gas, oxygen gas, and/or carbon dioxide gas, etc.), store one or more of the one or more products or byproducts, and/or react one or more of the one or more products or byproducts (e.g., in a chemical dissolution and/or precipitation reaction).
  • the reactor e.g., acid, base, hydrogen gas, oxygen gas, and/or carbon dioxide gas, etc.
  • react one or more of the one or more products or byproducts e.g., in a chemical dissolution and/or precipitation reaction.
  • the system comprises multiple apparatuses. In some embodiments, the system comprises greater than or equal to 1, greater than or equal to 2, greater than or equal to 3, greater than or equal to 4, or greater than or equal to 5 apparatuses. In some cases, the system comprises less than or equal to 6, less than or equal to 5, less than or equal to 4, less than or equal to 3, or less than or equal to 2 apparatuses. Combinations of these ranges are also possible (e.g., 1-6 apparatuses). In some embodiments, the system comprises a first apparatus and a second apparatus. For example, in FIG. 1B , in some embodiments, the system comprises first apparatus 118 and second apparatus 119 . Similarly, referring to FIG.
  • the system comprises first apparatus 118 and second apparatus 119 .
  • the system comprises first apparatus 118 and second apparatus 119 .
  • Each apparatus may independently have one or more functions. Any apparatus, or configuration of apparatuses, disclosed herein may be used with any system disclosed herein.
  • the apparatus is fluidically connected to the reactor.
  • the apparatus is connected to the reactor by a conduit (e.g., a pipe, channel, needle, or tube) through which fluid can flow.
  • a conduit e.g., a pipe, channel, needle, or tube
  • apparatus 118 is fluidically connected to the reactor by a conduit.
  • apparatus 118 is fluidically connected to the reactor by a conduit.
  • apparatus 118 is fluidically connected to the reactor by a conduit.
  • an apparatus is fluidically connected to one or more other apparatuses (e.g., by a conduit, such as a pipe, channel, needle, or tube).
  • a conduit such as a pipe, channel, needle, or tube.
  • first apparatus 118 is fluidically connected to third apparatus 120 by a conduit.
  • first apparatus 118 could be fluidically connected to a third apparatus (e.g., by a conduit).
  • first apparatus 118 could be fluidically connected to a third apparatus (e.g., by a conduit).
  • FIG. 3A in some cases, first apparatus 118 could be fluidically connected to a third apparatus (e.g., by a conduit).
  • FIG. 3A in some cases, first apparatus 118 could be fluidically connected to a third apparatus (e.g., by a conduit).
  • first apparatus 118 is fluidically connected to third apparatus 120 (e.g., by a conduit), which is fluidically connected to fifth apparatus 122 (e.g., by a conduit), while second apparatus 119 is fluidically connected to fourth apparatus 121 (e.g., by a conduit), which is fluidically connected to sixth apparatus 123 (e.g., by a conduit).
  • the method comprises collecting the acid and/or base.
  • the method comprises removing the acid and/or base from the vessel in which it was produced (e.g., the reactor).
  • a non-limiting example of a suitable method of collecting the acid and/or base comprises moving the acid and/or base through a conduit (e.g., a pipe, channel, needle, or tube) into a separate container.
  • Other suitable examples of collecting the acid and/or base include moving the acid and/or base directly into a separate container (e.g., a container connected to the reactor by a panel that can be moved to block or allow diffusion of fluids).
  • the acid and/or base is collected continuously or in batches.
  • the acid and/or base is collected automatically or manually.
  • an apparatus is configured to collect an acid near the second electrode (and/or second reactor) and/or a base near the first electrode (and/or first reactor) (e.g., collect an acid from the acidic region and/or collect a base from the alkaline region).
  • the system comprises first apparatus 118 , which is configured to collect a base near first electrode 104 .
  • the system comprises first apparatus 118 , which is configured to collect a base near first electrode 104 .
  • the system comprises first apparatus 118 , which is configured to collect a base near first electrode 104 .
  • system 300 comprises first apparatus 118 , which is configured to collect a base near first reactor 320 (e.g., near first electrode 104 of first reactor 320 ).
  • first apparatus 118 could be configured to collect an acid near the second electrode (and/or second reactor), in addition to, or instead of collecting a base near the first electrode (and/or first reactor).
  • the second apparatus is configured to collect an acid near the second electrode (and/or second reactor) and/or a base near the first electrode (and/or first reactor).
  • the first apparatus is configured to collect a base near the first electrode
  • the second apparatus is configured to collect an acid near the second electrode.
  • the system comprises first apparatus 118 and second apparatus 119 , and, in certain cases, first apparatus 118 is configured to collect a base near first electrode 104 and second apparatus 119 is configured to collect an acid near second electrode 105 .
  • first apparatus 118 is configured to collect a base near first electrode 104
  • second apparatus 119 is configured to collect an acid near second electrode 105 .
  • the system comprises first apparatus 118 and second apparatus 119 , and, in certain cases, first apparatus 118 is configured to collect a base near first electrode 104 and second apparatus 119 is configured to collect an acid near second electrode 105 .
  • system 300 comprises first apparatus 118 and second apparatus 119 , and, in certain cases, first apparatus 118 is configured to collect a base near first reactor 320 (e.g., first electrode 104 ) and apparatus 119 is configured to collect an acid near second reactor 301 .
  • the second apparatus may be configured to collect a base near the first electrode (and/or first reactor).
  • collecting the acid comprises collecting acid produced by an electrode from a vicinity close enough to the electrode that the acid has not been significantly diluted and/or reacted (e.g., the pH of the collected acid is within 1 pH unit of the acid with the lowest pH in the reactor).
  • collecting the base comprises collecting the base produced by the electrode from a vicinity close enough to the electrode that the base has not been significantly diluted and/or reacted (e.g., the pH of the collected base is within 1 pH unit of the base with the highest pH in the reactor).
  • the method comprises storing the acid and/or base. For example, in certain embodiments, once the acid and/or base are collected in a separate container, the method comprises keeping the acid and/or base in the separate container for at least some period of time. In some embodiments, the method comprises storing the acid and/or base for greater than or equal to 5 minutes, greater than or equal to 15 minutes, greater than or equal to 30 minutes, greater than or equal to 1 hour, greater than or equal to 5 hours, greater than or equal to 12 hours, greater than or equal to 1 day, greater than or equal to 2 days, greater than or equal to 3 days, greater than or equal to 1 week, greater than or equal to 2 weeks, or greater than or equal to 1 month.
  • the method comprises storing the acid and/or base for less than or equal to 1 year, less than or equal to 6 months, less than or equal to 3 months, less than or equal to 2 months, less than or equal to 1 month, less than or equal to 2 weeks, less than or equal to 1 week, less than or equal to 3 days, less than or equal to 2 days, less than or equal to 1 day, or less than or equal to 12 hours. Combinations of these ranges are also possible (e.g., greater than or equal to 5 minutes and less than or equal to 1 year, greater than or equal to 5 hours and less than or equal to 1 day, or greater than or equal to 1 week and less than or equal to 1 year).
  • an apparatus e.g., the first apparatus and/or the second apparatus
  • first apparatus 118 is configured to store the base.
  • first apparatus 118 is configured to store the base.
  • first apparatus 118 is configured to store the base.
  • second apparatus 119 is configured to store the acid.
  • second apparatus 119 is configured to store the acid.
  • second apparatus 119 is configured to store the acid.
  • second apparatus 119 is configured to store the acid.
  • the second apparatus is configured to store the acid.
  • the system comprises first apparatus 118 and second apparatus 119 , and, in certain cases, first apparatus 118 is configured to store the base, and second apparatus 119 is configured to store the acid.
  • the system comprises first apparatus 118 and second apparatus 119 , and, in certain cases, first apparatus 118 is configured to store the base, and second apparatus 119 is configured to store the acid.
  • first apparatus 118 is configured to store the base
  • second apparatus 119 is configured to store the acid.
  • the system comprises first apparatus 118 and second apparatus 119 , and, in certain cases, first apparatus 118 is configured to store the base, and second apparatus 119 is configured to store the acid.
  • first apparatus 118 is configured to store the base
  • second apparatus 119 is configured to store the acid.
  • the second apparatus may be configured to store the base.
  • the method comprises reacting the acid and/or base in a chemical dissolution and/or in a precipitation reaction.
  • the chemical dissolution is before the precipitation reaction (e.g., the product of the chemical dissolution is used in the precipitation reaction).
  • the precipitation reaction is before the chemical dissolution (e.g., the product of the precipitation reaction is used in the chemical dissolution).
  • the chemical dissolution and precipitation reaction are simultaneous and/or unrelated (e.g., the product of one is not used in the other, and vice versa).
  • an apparatus e.g., the first apparatus and/or the second apparatus
  • second apparatus 119 is configured to react the acid (e.g., in a chemical dissolution and/or in a precipitation reaction).
  • second apparatus 119 is configured to react the acid (e.g., in a chemical dissolution and/or in a precipitation reaction).
  • second apparatus 119 is configured to react the acid (e.g., in a chemical dissolution and/or in a precipitation reaction).
  • second apparatus 119 is configured to react the acid (e.g., in a chemical dissolution and/or in a precipitation reaction).
  • an apparatus e.g., the first apparatus and/or the second apparatus
  • first apparatus 118 is configured to react the base in a chemical dissolution and/or in a precipitation reaction.
  • first apparatus 118 is configured to react the base (e.g., in a chemical dissolution and/or in a precipitation reaction).
  • first apparatus 118 is configured to react the base (e.g., in a chemical dissolution and/or in a precipitation reaction).
  • first apparatus 118 is configured to react the base (e.g., in a chemical dissolution and/or in a precipitation reaction).
  • first apparatus 118 is configured to react the base (e.g., in a chemical dissolution and/or in a precipitation reaction).
  • the second apparatus is configured to react an acid (e.g., in a chemical dissolution and/or in a precipitation reaction).
  • the system comprises first apparatus 118 and second apparatus 119 , and, in certain cases, first apparatus 118 is configured to react a base (e.g., in a chemical dissolution and/or in a precipitation reaction), and second apparatus 119 is configured to react an acid (e.g., in a chemical dissolution and/or in a precipitation reaction).
  • first apparatus 118 is configured to react a base (e.g., in a chemical dissolution and/or in a precipitation reaction)
  • second apparatus 119 is configured to react an acid (e.g., in a chemical dissolution and/or in a precipitation reaction).
  • the system comprises first apparatus 118 and second apparatus 119 , and, in certain cases, first apparatus 118 is configured to react a base (e.g., in a chemical dissolution and/or in a precipitation reaction), and second apparatus 119 is configured to react an acid (e.g., in a chemical dissolution and/or in a precipitation reaction).
  • first apparatus 118 is configured to react a base (e.g., in a chemical dissolution and/or in a precipitation reaction)
  • second apparatus 119 is configured to react an acid (e.g., in a chemical dissolution and/or in a precipitation reaction).
  • the system comprises first apparatus 118 and second apparatus 119 , and, in certain cases, first apparatus 118 is configured to react a base (e.g., in a chemical dissolution and/or in a precipitation reaction), and second apparatus 119 is configured to react an acid (e.g., in a chemical dissolution and/or in a precipitation reaction).
  • first apparatus 118 is configured to react a base
  • second apparatus 119 is configured to react an acid (e.g., in a chemical dissolution and/or in a precipitation reaction).
  • the second apparatus may be configured to react a base.
  • an apparatus e.g., first apparatus and/or second apparatus
  • first apparatus may be configured to (i) collect an acid near the second electrode and/or a base near the first electrode; (ii) store the acid and/or base; and/or (iii) react the acid and/or base (e.g., in a chemical dissolution and/or in a precipitation reaction).
  • first apparatus 118 is configured to (i) collect a base near the first electrode; (ii) store the base; and (iii) react the base (e.g., in a chemical dissolution and/or in a precipitation reaction).
  • FIG. 1A in some embodiments, first apparatus 118 is configured to (i) collect a base near the first electrode; (ii) store the base; and (iii) react the base (e.g., in a chemical dissolution and/or in a precipitation reaction).
  • FIG. 1A in some embodiments, first apparatus 118 is configured to (i) collect a base near the first electrode; (i
  • first apparatus 118 is configured to (i) collect a base near the first electrode; (ii) store the base; and (iii) react the base (e.g., in a chemical dissolution and/or in a precipitation reaction).
  • first apparatus 118 is configured to (i) collect a base near the first electrode; (ii) store the base; and (iii) react the base (e.g., in a chemical dissolution and/or in a precipitation reaction).
  • second apparatus 119 is configured to (i) collect an acid near the second electrode; (ii) store the acid; and (iii) react the acid (e.g., in a chemical dissolution and/or in a precipitation reaction).
  • second apparatus 119 is configured to (i) collect an acid near the second electrode; (ii) store the acid; and (iii) react the acid (e.g., in a chemical dissolution and/or in a precipitation reaction).
  • second apparatus 119 is configured to (i) collect an acid near the second electrode; (ii) store the acid; and (iii) react the acid (e.g., in a chemical dissolution and/or in a precipitation reaction).
  • each apparatus may have only one function.
  • a first apparatus is configured to collect a base near the first electrode
  • a second apparatus is configured to collect an acid near the second electrode
  • a third apparatus is configured to react the base and/or acid (e.g., in a chemical dissolution and/or in a precipitation reaction).
  • first apparatus 118 is configured to collect a base near first electrode 104
  • second apparatus 119 is configured to collect an acid near second electrode 105
  • third apparatus 120 is configured to react the base (e.g., in a chemical dissolution and/or in a precipitation reaction).
  • a first apparatus is configured to collect a base near the first electrode and store the base; a second apparatus is configured to collect an acid near the second electrode, store the acid, and react the acid (e.g., in a chemical dissolution and/or in a precipitation reaction); and a third apparatus is configured to react the base (e.g., in a chemical dissolution and/or in a precipitation reaction).
  • a first apparatus is configured to collect a base near the first electrode and store the base;
  • a second apparatus is configured to collect an acid near the second electrode, store the acid, and react the acid (e.g., in a chemical dissolution and/or in a precipitation reaction); and a third apparatus is configured to react the base (e.g., in a chemical dissolution and/or in a precipitation reaction).
  • first apparatus 118 is configured to collect a base near first electrode 104 and store the base; second apparatus 119 is configured to collect an acid near second electrode 105 , store the acid, and react the acid (e.g., in a chemical dissolution and/or in a precipitation reaction); and third apparatus 120 is configured to react the base (e.g., in a chemical dissolution and/or in a precipitation reaction).
  • a first apparatus is configured to collect a base near the first electrode
  • a second apparatus is configured to collect an acid near the second electrode
  • a third apparatus is configured to store the base
  • a fourth apparatus is configured to store the acid
  • a fifth apparatus is configured to react the base (e.g., in a chemical dissolution and/or in a precipitation reaction)
  • a sixth apparatus is configured to react the acid (e.g., in a chemical dissolution and/or in a precipitation reaction).
  • first apparatus 118 is configured to collect a base near first electrode 104
  • second apparatus 119 is configured to collect an acid near second electrode 105
  • third apparatus 120 is configured to store the base
  • fourth apparatus 121 is configured to store the acid
  • fifth apparatus 122 is configured to react the base (e.g., in a chemical dissolution and/or in a precipitation reaction)
  • sixth apparatus 123 is configured to react the acid (e.g., in a chemical dissolution and/or in a precipitation reaction).
  • the acid and/or base described herein is reacted in a chemical dissolution and/or precipitation reaction. In certain cases, the acid and/or base is reacted in a chemical dissolution.
  • the chemical dissolution comprises the dissolution of a solid to form two solubilized ions.
  • the solid comprises a metal, metal alloy, metalloid, metal salt, a metal oxide, a metal hydroxide, and/or a silicate. In certain embodiments, the solid is crystalline, amorphous, nanocrystalline, and/or a mixture thereof.
  • the solid comprises Ag, Al, As, Au, Ba, Ca, Cd, Cl, Co, Cr, Cu, Fe, Hg, K, Mg, Mn, Mo, Na, Ni, P, Pb, S, Sb, Se, Si, Sn, Ti, Tl, V, W and/or Zn (e.g., in elemental form or as a salt).
  • the metal and/or metal alloy comprises iron, a ferrous alloy, a stainless steel, a nonferrous metal, a nonferrous alloy, aluminum, brass, bronze, copper, zinc, tin, and/or a coin alloy.
  • metal salts, metal oxides, and metal hydroxides include salts, oxides, and hydroxides of calcium, magnesium, barium, strontium, manganese, iron, cobalt, zinc, cadmium, lead, and/or nickel.
  • the metal salt comprises a metal carbonate.
  • suitable metal carbonates include calcium carbonate, magnesium carbonate, barium carbonate, strontium carbonate, manganese carbonate, iron carbonate, cobalt carbonate, zinc carbonate, cadmium carbonate, lead carbonate, and/or nickel carbonate.
  • suitable metal oxides include calcium oxide, magnesium oxide, strontium oxide, manganese oxide, iron oxide, cobalt oxide, nickel oxide, zinc oxide, cadmium oxide, lead oxide, silicon dioxide, and/or aluminum oxide.
  • suitable metal hydroxides include calcium hydroxide, magnesium hydroxide, strontium hydroxide, manganese hydroxide, iron oxide, cobalt hydroxide, nickel hydroxide, zinc hydroxide, cadmium hydroxide, lead hydroxide, silicon hydroxide, and/or aluminum hydroxide.
  • the acid is reacted in a chemical dissolution of a metal, metal alloy, metalloid, metal salt, metal oxide, and/or metal hydroxide.
  • the base is reacted in a chemical dissolution of a metal oxide (e.g., silicon dioxide and/or aluminum oxide) and/or metal hydroxide (e.g., silicon hydroxide and/or aluminum hydroxide).
  • the acid and/or base is reacted in a precipitation reaction.
  • the precipitation reaction comprises the combination of two solubilized ions to form a solid precipitate.
  • the solid precipitate comprises a metal hydroxide.
  • suitable metal hydroxides include calcium hydroxide, magnesium hydroxide, barium hydroxide, strontium hydroxide, manganese hydroxide, iron hydroxide, cobalt hydroxide, zinc hydroxide, cadmium hydroxide, lead hydroxide, and/or nickel hydroxide.
  • the base is reacted in a precipitation reaction to form a metal hydroxide.
  • the acid is reacted in a precipitation reaction to form a metal hydroxide.
  • the reactor is intermittently run when in the first mode (e.g., as described above). In some cases, the reactor is continuously run in the first mode. In certain instances, the reactor is run intermittently in a first mode, while the reactions with the collected acid and or base (e.g., the chemical dissolution and/or precipitation reaction) are run continuously. For example, in some embodiments, the reactor produces enough acid and/or base when run in the first mode that it only needs to be run intermittently to produce enough acid and/or base to continuously perform the reactions (e.g., the chemical dissolution and/or precipitation reaction).
  • the reactor produces enough acid and/or base when run in the first mode that it only needs to be run intermittently to produce enough acid and/or base to continuously perform the reactions (e.g., the chemical dissolution and/or precipitation reaction).
  • a desired chemical reaction is conducted by collecting solutions or suspensions of differing compositions produced electrolytically, and using said solution or solutions to produce a product from said reactant in a portion of the reactor or in a separate apparatus.
  • FIGS. 4A-4B shows, in accordance with certain embodiments, a reactor in which an electrolyzer produces solutions of low and high pH that are directed to a separate zone of the reactor or to a separate reactor.
  • the acidic solution is used to dissolve CaCO 3 in a first chamber, releasing CO 2 gas in the process (see FIG. 4B ).
  • the dissolved solution reacts with the alkaline solution produced by the electrolyzer to produce Ca(OH) 2 (see FIG.
  • the two chambers are storage tanks for acidic and for alkaline solutions.
  • the acid storage tank comprises a polymer material, or a glass lining.
  • the alkaline storage tank comprises a polymer material, or a metal.
  • the metal tank comprises iron or steel.
  • a byproduct of the precipitation reaction is fed back into the system (e.g., first reactor).
  • the system is configured to feed a byproduct from the precipitation reaction into the system (e.g., first reactor).
  • the byproduct has a neutral pH.
  • the byproduct has a pH of greater than 6, greater than or equal to 6.25, greater than or equal to 6.5, greater than or equal to 6.75, or greater than or equal to 6.9.
  • the byproduct has a pH of less than 8, less than or equal to 7.75, less than or equal to 7.5, less than or equal to 7.25, or less than or equal to 7.1. Combinations of these ranges are also possible (e.g., greater than 6 and less than 8 or greater than or equal to 6.9 and less than or equal to 7.1).
  • the byproduct has a pH of 7.
  • the byproduct comprises an alkali halide (e.g., the byproduct in the precipitation of an alkali hydroxide) (e.g., NaCl).
  • the byproduct comprises an alkali salt (e.g., NaClO 4 , NaNO 3 , sodium triflate, and/or sodium acetate).
  • the method comprises running the reactor in a second mode.
  • the polarity of the reactor is reversed in the second mode compared to the polarity of the reactor in the first mode.
  • running the reactor in the first mode uses more electricity than running the reactor in the second mode.
  • running the reactor in the first mode uses at least 10%, at least 20%, at least 30%, or at least 40% more electricity than running the reactor in the second mode.
  • running the reactor in the first mode uses less than or equal to 50%, less than or equal to 40%, less than or equal to 30%, or less than or equal to 20% more electricity than running the reactor in the second mode. Combinations of these ranges are also possible (e.g., at elast 10% and less than or equal to 50%) Any embodiment related to the second mode can be applied to any of the systems described herein.
  • running the reactor in the second mode comprises adding base to the reactor near the second electrode.
  • running the reactor in the second mode comprises adding base to the reactor in such a way that the base can be used in an electrochemical reaction in the second electrode.
  • running the reactor in the second mode comprises adding base near second electrode 105 .
  • running the reactor in the second mode comprises adding base near second electrode 105 .
  • the base added to the reactor was collected from near the first electrode when the reactor was run in the first mode and stored until the reactor was run in the second mode.
  • running the reactor in the second mode comprises oxidizing the added base (e.g., the base that had been stored) near the second electrode to produce oxygen gas.
  • running the reactor in the second mode comprises oxidation of the added base to oxygen gas by the second electrode.
  • running the reactor in the second mode comprises adding acid to the reactor near the first electrode.
  • running the reactor in the second mode comprises adding acid to the reactor in such a way that the acid can be used in an electrochemical reaction in the first electrode.
  • running the reactor in the second mode comprises adding acid near first electrode 104 .
  • running the reactor in the second mode comprises adding acid near first electrode 104 .
  • the acid added to the reactor was collected from near the second electrode when the reactor was run in the first mode and stored until the reactor was run in the second mode.
  • running the reactor in the second mode comprises reducing the added acid (e.g., the acid that had been stored) near the first electrode to produce hydrogen gas.
  • running the reactor in the second mode comprises reduction of the added acid to hydrogen gas by the first electrode.
  • running the reactor in the first mode comprises adding a near-neutral input solution to the reactor.
  • the near-neutral input solution has a pH of greater than 6, greater than or equal to 6.25, greater than or equal to 6.5, greater than or equal to 6.75, or greater than or equal to 6.9.
  • the near-neutral input solution has a pH of less than 8, less than or equal to 7.75, less than or equal to 7.5, less than or equal to 7.25, or less than or equal to 7.1. Combinations of these ranges are also possible (e.g., greater than 6 and less than 8 or greater than or equal to 6.9 and less than or equal to 7.1).
  • the near-neutral input solution has a pH of 7.
  • the near-neutral input solution comprises a salt.
  • suitable salts include an alkali sulfate, alkali chlorate, alkali halide, alkali nitrate, alkali perchlorate, alkali acetate, alkali nitrite, and/or alkali triflate.
  • the cost of electricity and/or availability of electricity from the power provider may fluctuate, and it may be advantageous to run the reactor in the first mode when the cost of electricity is low and/or the availability of electricity is high and then run the reactor in the second mode when the cost of electricity is high and/or the availability of electricity is low.
  • the electricity is from a renewable source, such as solar energy or wind energy
  • a renewable source such as solar energy or wind energy
  • there may be fluctuations in the availability of electricity such that it may be advantageous to run the reactor in the first mode when the availability of electricity is high (e.g., during the day and/or during the summer for solar energy or during windy periods for wind energy) and then run the reactor in the second mode when the availability of electricity is low (e.g., during the night and/or during the winter for solar energy or during periods without significant wind).
  • the reactor is run in the first mode when the cost of electricity is a first cost and the availability of electricity is a first availability
  • the reactor is run in the second mode when the cost of electricity is a second cost and the availability of electricity is a second availability, wherein the second cost is greater than the first cost (e.g., at least 10%, 25%, 50%, or 100% greater) and/or the first availability is greater than the second availability (e.g., at least 10%, 25%, 50%, or 100% greater).
  • the acidic and/or basic solutions produced by the electrolysis reactor are at least partially collected and/or stored during periods of high electricity availability and/or low electricity cost, permitting the chemical dissolution reaction in the acid producing CO 2 and the chemical precipitation reaction occurring in the base to be conducted during periods of reduced or low electrolyzer operation or electricity availability and/or high electricity cost.
  • the storage of acidic and basic solutions functions as chemical storage, allowing the output of the chemically reacted product, which may generally be solid, liquid or gaseous, to be less variable, or to be smoothed, compared to the output rate of the electrolyzer.
  • the stored acidic or basic solutions are of a size or volume permitting the chemically reacted product to be produced at a rate that does not fully deplete the stored acidic or basic solutions during periods of reduced or low electrolyzer operation or electricity availability and/or high electricity cost.
  • a system comprises a source of variable electricity, said electrolyzer, and said chemical storage tanks and chemical reactor.
  • a method comprises operating such a system so as to produce a less variable, or constant or relatively constant, flow of a chemical reaction product from a more variable or intermittent electricity source.
  • the method comprises producing acid and base in a low-voltage mode (e.g., at a lower voltage than a high-voltage mode described herein). Any embodiment related to the low voltage mode may be used with any system disclosed herein.
  • the method does not produce oxygen gas and/or hydrogen gas.
  • the electrolytic reactions occurring in the low-voltage mode may be the oxidation of hydrogen at the second electrode (H 2 ⁇ 2H + +2e ⁇ ) and the reduction of water at the first electrode (2H 2 O+2e ⁇ ⁇ H 2 +2OH ⁇ ), such that oxygen gas is not produced.
  • the electrolytic reactions occurring in the low-voltage mode may be the oxidation of water at the first electrode (2H 2 O ⁇ O 2 +4H + +4e ⁇ ) and the reduction of oxygen at the second electrode (O 2 +2H 2 O+4e ⁇ ⁇ 4OH ⁇ ), such that hydrogen gas is not produced.
  • System 1 Exemplary Systems for Producing Low-Cost H 2 at a Constant Rate Using Intermittent Renewable Energy
  • the system may comprise a reactor comprising a region comprising a spatially varying chemical composition gradient (e.g., a spatially varying pH gradient).
  • the reactor may comprise a first electrode and a second electrode, one or more inlets supplying liquids and/or a gas that undergoes an electrolytic reaction or reactions, and a portion of the reactor or a separate apparatus in which the solutions are stored after undergoing electrolytic reactions.
  • the method comprises running a reactor in a first mode (e.g., a high-voltage mode, as shown in FIGS. 5A-5B ); wherein the first mode comprises: producing base near a first electrode; producing acid near a second electrode that is electrochemically coupled to the first electrode in the reactor; collecting the acid and/or base; and reacting the collected acid and/or base in a chemical dissolution and/or in a precipitation reaction.
  • a first mode e.g., a high-voltage mode, as shown in FIGS. 5A-5B )
  • the first mode comprises: producing base near a first electrode; producing acid near a second electrode that is electrochemically coupled to the first electrode in the reactor; collecting the acid and/or base; and reacting the collected acid and/or base in a chemical dissolution and/or in a precipitation reaction.
  • the electrolytic reactions may produce H 2 , O 2 , an acidic solution, and a basic solution.
  • This is an example of a high-voltage mode, which requires a higher voltage than a low-voltage mode.
  • a non-limiting example of an electrolytic reaction occurring in the high-voltage mode is the oxidation of water at the second electrode (2H 2 O ⁇ O 2 +4H + +4e ⁇ ) and the reduction of water at the first electrode (2H 2 O+2e ⁇ ⁇ H 2 +2OH ⁇ ); this reaction requires a minimum voltage of 2 V when the pH at the second electrode is 0 and the pH at the first electrode is 14 (see FIGS. 5A-5B ).
  • the acidic and basic solutions produced at the electrodes may be collected and stored separately.
  • the method comprises running the reactor in a second mode (e.g., a low-voltage mode, as shown in FIGS. 6A-6B ).
  • the polarity of the reactor is reversed in the second mode compared to the polarity of the reactor in the first mode.
  • the second mode comprises adding the collected and/or stored base to the reactor near the second electrode.
  • the second mode comprises oxidizing the added base near the second electrode to produce oxygen gas.
  • the second mode comprises adding the collected and/or stored acid to the reactor near the first electrode.
  • the second mode comprises reducing the added acid near the first electrode to produce hydrogen gas.
  • the electrolytic reactions may neutralize an acidic and a basic solution while producing H 2 and O 2 .
  • This is an example of a low-voltage mode, which requires a lower voltage than the aforementioned high-voltage mode.
  • a non-limiting example of an electrolytic reaction occurring in the low-voltage mode is the oxidation of hydroxide ions at the second electrode (e.g., anode) (4OH ⁇ ⁇ O 2 +2H 2 O+4e ⁇ ) and the reduction of protons at the first electrode (e.g., cathode) (2H+ + 2e ⁇ ⁇ H 2 ); this reaction requires a minimum voltage of 0.4 V when the pH at the second electrode is 14 and the pH at the first electrode is 0 (see FIGS. 6A-6B ).
  • the inlets of the reactor may supply a solution of pH greater than 8 to the second electrode and a solution of pH less than 6 to the first electrode.
  • different reactors may be operated in high-voltage and low-voltage modes.
  • a single reactor may be configured such that it can be operated in the high-voltage mode or in the low-voltage mode.
  • the reactor may be switched from the high-voltage mode to the low-voltage mode by changing the pH of the liquid that flows to the electrode. For example, to switch to low-voltage mode from high-voltage mode an alkaline solution could be introduced to the second electrode, while an acidic solution could be introduced to the first electrode.
  • the decision to switch between a high-voltage mode (e.g., producing H 2 /O 2 while creating acid/base) and the low voltage mode (e.g., producing H 2 /O 2 while neutralizing acid/base) may be based on the cost or availability of electricity, which may fluctuate throughout a day, month or year.
  • a reactor may be run in high-voltage mode (e.g., consuming more power while producing H 2 , O 2 , acid and base); when the cost of electricity is above a certain value, the reactor may be run in low-voltage mode (e.g., consuming less power, while using the acidic and basic solutions to produce H 2 and O 2 ).
  • the system may effectively arbitrage the electricity cost of producing H 2 : when electricity is inexpensive the system uses more of it by operating in high-voltage mode, in which some of the inexpensive electrical energy is converted into chemical energy that may be physically stored (e.g., in the form of acidic and basic solutions); when electricity is expensive the system may use less of it by operating in low-voltage mode, in which the stored chemical energy (e.g., the acidic and basic solutions) may be used to lower the energy requirement for producing H 2 and O 2 .
  • the system may serve to decrease the electricity cost of producing H 2 and O 2 .
  • the system may serve to produce hydrogen and oxygen at a constant rate using electricity that fluctuates in price or availability.
  • FIG. 7 illustrates a non-limiting example in which a system reduces the energy cost of producing H 2 using intermittent renewable electricity by 20%.
  • the cost of renewable energy fluctuates between 0.02 $/kWh and 0.07 $/kWh (according to the energy-production rate of a typical wind turbine on a typical day).
  • Electricity cost vs. time for a 1 kW alkaline or PEM electrolyzer, operating at fixed voltage (1.2 V, 32 kWh/kg H 2 ) is shown in FIG. 7 .
  • variable-voltage electrolyzer 7 also shows the energy cost of a variable-voltage electrolyzer that operates in high-voltage mode (2 V, 54 kWh/kg H 2 ) when the cost of electricity is below average (0.05 $/kWh) and in low-voltage mode (0.4 V, 10 kWh/kg H 2 ) when the cost of electricity is above average, in accordance with some embodiments.
  • both electrolyzers produce H 2 at the same rate and use the same amount of energy on average (32 kWh/kg H 2 ), however, the energy costs of running the two cells are different.
  • the variable-voltage electrolyzer uses less of the expensive electricity (by operating in low-voltage mode) and more of the inexpensive electricity (by operating in high-voltage mode).
  • the average energy cost for the fixed-voltage electrolyzer is 0.05 $/kWh
  • the average energy cost for the variable-voltage electrolyzer is 0.04 $/kWh (20% less).
  • the amount of cost savings possible with the variable-voltage electrolyzer is proportional to the magnitude of the cost fluctuations: the larger the variation in the electricity cost, the larger the cost savings.
  • the system may comprise a reactor comprising a region comprising a spatially varying chemical composition gradient (e.g., a spatially varying pH gradient).
  • the reactor may comprise a first electrode and a second electrode, one or more inlets supplying a liquid and/or a gas that undergoes electrolytic reaction or reactions, and a portion of the reactor or a separate apparatus in which the solutions are stored after undergoing electrolytic reactions.
  • the electrolytic reactions may produce a pH less than about six in the vicinity of the second electrode and a pH greater than about eight in the vicinity of the first electrode; the solutions of high and low pH may be collected and stored separately.
  • the electrodes may be configured to perform one or more of the electrolytic reactions to produce high or low pH solutions.
  • the electrolytic reactions may produce H 2 , O 2 , an acidic solution, and a basic solution.
  • This is an example of a high-voltage mode, which requires a higher voltage than a low-voltage mode.
  • a non-limiting example of an electrolytic reaction occurring in the high-voltage mode is the oxidation of water at the second electrode (e.g., anode) (2H 2 O ⁇ O 2 +4H + +4e ⁇ ) and the reduction of water at the first electrode (e.g., cathode) (2H 2 O+2e ⁇ ⁇ H 2 +2OH ⁇ ); this reaction requires a minimum voltage of 2 V when the pH at the second electrode is 0 and the pH at the first electrode is 14 (see FIGS. 5A-5B ).
  • the acidic and basic solutions produced at the electrodes may be collected and stored separately.
  • the reactor at times may produce acidic and basic solutions in a low-voltage mode that requires a lesser voltage than the high-voltage mode.
  • electrolytic reactions producing acidic and basic solutions in the low-voltage mode include the following.
  • the electrolytic reactions occurring in the low-voltage mode may be the oxidation of hydrogen at the second electrode (e.g., anode) (H 2 ⁇ 2H + +2e ⁇ ) and the reduction of water at the first electrode (e.g., cathode) (2H 2 O+2e ⁇ ⁇ H 2 +2OH ⁇ ) (e.g., HRR/HER reactions); this reaction requires a minimum voltage of 0.8 V when the pH at the second electrode is 0 and the pH at the first electrode is 14 (see FIGS. 8A-8B ).
  • the second electrode e.g., anode
  • the reduction of water at the first electrode e.g., cathode
  • HRR/HER reactions e.g., HRR/HER reactions
  • the electrolytic reactions occurring in the low-voltage mode may be the oxidation of water at the second electrode (e.g., anode) (2H 2 O ⁇ O 2 +4H + +4e ⁇ ) and the reduction of oxygen at the first electrode (e.g., cathode) (O 2 +2H 2 O+4e ⁇ ⁇ 4OH ⁇ ) (e.g., OER/ORR reactions); this reaction requires a minimum voltage of 0.8 V when the pH at the second electrode is 0 and the pH at the first electrode is 14 (see FIGS. 9A-9B ).
  • the second electrode e.g., anode
  • the reduction of oxygen at the first electrode e.g., cathode
  • O 2 +2H 2 O+4e ⁇ ⁇ 4OH ⁇ e.g., OER/ORR reactions
  • the decision to switch between the high-voltage mode (e.g., creating acid/base with the co-generation of H 2 /O 2 ) or a low voltage mode (e.g., creating acid/base without producing a net amount of gas) may be based on the cost or availability of electricity, which may fluctuate throughout a day, month or year.
  • a reactor may be run in the high-voltage mode (e.g., consuming more power while producing H 2 , O 2 , acid and base).
  • the reactor may be run in the low-voltage mode (e.g., consuming less power, producing acid and base only).
  • the system may take advantage of low electricity prices by co-producing H 2 and O 2 along with the acidic and basic solutions: when electricity is inexpensive the system may use more of it by operating in high-voltage mode, which produces acid, base, H 2 and O 2 ; when electricity is expensive the system may use less of it by operating in the low-voltage modes, which produce acid and base, but do not produce a net amount of H 2 or O 2 . In some embodiments, the system serves to decrease the electricity cost of producing H 2 and O 2 .
  • System 3 Exemplary Systems for Producing Low-Cost Acid/Base at a Constant Rate Using Intermittent Renewable Energy
  • the system may comprise a reactor comprising a region comprising a spatially varying chemical composition gradient (e.g., a spatially varying pH gradient).
  • the reactor may comprise a first electrode and a second electrode, one or more inlets supplying a liquid and/or a gas that undergoes electrolytic reaction or reactions, and a portion of the reactor or a separate apparatus in which the solutions are stored after undergoing electrolytic reactions.
  • the electrolytic reactions may produce a pH less than about six in the vicinity of the second electrode and a pH greater than about eight in the vicinity of the first electrode; the solutions of high and low pH may be collected and stored separately.
  • the electrodes may be configured to perform one or more of the electrolytic reactions to produce high or low pH solutions.
  • the electrolytic reactions may produce H 2 , O 2 , an acidic solution, and a basic solution.
  • This is an example of an electrolytic mode, as it requires a higher voltage than the fuel cell mode which will be described later.
  • a non-limiting example of an electrolytic reaction occurring in the electrolytic mode is the oxidation of water at the second electrode (e.g., anode) (2H 2 O ⁇ O 2 +4H + +4e ⁇ ) and the reduction of water at the first electrode (e.g., cathode) (2H 2 O+2e ⁇ ⁇ H 2 +2OH ⁇ ); this reaction requires a minimum voltage of 2 V when the pH at the second electrode is 0 and the pH at the first electrode is 14 (see FIGS. 5A-5B ).
  • the acidic and basic solutions produced at the electrodes may be collected and stored separately.
  • the reactions occurring in the fuel cell mode may be the oxidation of hydrogen at the second electrode (e.g., anode) (H 2 ⁇ 2H + +2e ⁇ ) and the reduction of oxygen at the first electrode (e.g., cathode) (O 2 +2H 2 O+4e ⁇ ⁇ 4OH ⁇ ) (e.g., HRR/ORR reactions); this results in a spontaneous reaction that produces energy (see FIGS. 10A-10B ).
  • the second electrode e.g., anode
  • oxygen at the first electrode e.g., cathode
  • O 2 +2H 2 O+4e ⁇ ⁇ 4OH ⁇ e.g., HRR/ORR reactions
  • the system may effectively arbitrage the electricity cost of producing acidic and basic solutions: when electricity is inexpensive the system uses more of it by operating in electrolytic mode, in which some of the inexpensive electrical energy is converted into chemical energy that may be physically stored (in the form of H 2 and O 2 gases); when electricity is expensive the system may use less of it by operating in fuel cell mode, in which the stored chemical energy (H 2 and O 2 gases) may be used for creating acid, base and electricity.
  • the system serves to decrease the electricity cost of producing solutions of acid and base.
  • this system serves to produce acidic and basic solutions at a constant rate using electricity that fluctuates in price or availability.
  • the chemical dissolution and/or precipitation reaction occur inside of the reactor.
  • the reactor comprises a spatially varying chemical composition gradient between the first electrode and the second electrode.
  • the spatially varying chemical composition gradient comprises a spatially varying pH gradient.
  • system 200 comprises alkaline region 106 near first electrode 104 and acidic region 107 near second electrode 105 ; thus, system 200 comprises a spatially varying chemical composition gradient (e.g., spatially varying pH gradient) between the first electrode and the second electrode.
  • a first region comprises the acidic region.
  • a second region comprises the alkaline region.
  • the first region comprises an alkaline region and the second region comprises an acidic region.
  • the reactor is configured such that the spatially varying chemical composition gradient (e.g., the spatially varying pH gradient) is established and/or maintained, at least in part, by electrolysis.
  • system 200 comprises a spatially varying chemical composition gradient (e.g., a spatially varying pH gradient) comprising alkaline region 106 and acidic region 107 .
  • this spatially varying chemical composition gradient (e.g., spatially varying pH gradient) is established and/or maintained by electrolysis.
  • Electrolysis of a neutral electrolyte can produce, in accordance with some embodiments, a spatially varying chemical composition gradient (e.g., spatially varying pH gradient) between electrodes, such as first electrode 104 and second electrode 105 .
  • a spatially varying chemical composition gradient e.g., spatially varying pH gradient
  • an electrolysis reaction is used to produce a chemical composition gradient between the positive and negative electrodes of an electrochemical cell.
  • the electrolytically produced chemical composition gradient can be employed to conduct a desired chemical reaction by feeding a reactant to the chemical environment near one electrode, and using the electrolytically produced chemical composition gradient to produce a product from said reactant as the reactant or its components diffuse towards the other electrode.
  • the electrolysis comprises hydrolysis.
  • hydrolysis refers to the electrolysis of water.
  • the reaction taking place in the cathode converts 2 H 2 O molecules and 2 electrons to H 2 and 2OH ⁇
  • the reaction taking place in the anode converts 2 H 2 O molecules to 4 electrons, O 2 , and 4 protons.
  • the generation of hydroxide ions near first electrode 104 establishes and/or maintains an alkaline pH near first electrode 104 , establishing and/or maintaining alkaline region 106
  • the generation of protons near second electrode 105 establishes an acidic pH near second electrode 105 , establishing and/or maintaining acidic region 107 .
  • the reactor is configured such that the spatially varying chemical composition gradient (e.g., spatially varying pH gradient) is established and/or maintained, at least in part, by hydrolysis.
  • the reactor comprises an inlet connected to a first region (e.g., an acidic region) of the spatially varying chemical composition gradient (e.g., spatially varying pH gradient).
  • a first region e.g., an acidic region
  • the spatially varying chemical composition gradient e.g., spatially varying pH gradient.
  • the electrochemical reactor and/or inlet is configured to receive a solid (e.g., CaCO 3 ).
  • the reactor comprises a reactor outlet.
  • the reactor outlet is configured to discharge Ca(OH) 2 (e.g., solid calcium hydroxide) and/or lime (CaO).
  • the reactor comprises an outlet connected to a second region (e.g., an alkaline region) of the spatially varying chemical composition gradient (e.g., spatially varying pH gradient).
  • the outlet is configured such that solids can be expelled from the reactor.
  • the reactor comprises a solids handling apparatus associated with the outlet and configured to remove solid from the reactor.
  • solids handling apparatus is configured to remove solids (such as solid metal hydroxides, such as solid nickel hydroxide, solid calcium hydroxide, or solid magnesium hydroxide) from the reactor.
  • solids handling apparatuses include, but are not limited to, conveyor belts, augers, pumps, chutes, or any other device capable of transporting solids away from the reactor.
  • the solids handling apparatus separates the solid from the liquid using one or a combination of fluid flow, filtering, sedimentation, centrifugal force, electrophoresis, dielectrophoresis, or magnetic separation.
  • the reactor comprises more than one reactor outlet (e.g., at least 1, at least 2, at least 3, at least 4, less than or equal to 5, less than or equal to 4, less than or equal to 3, or less than or equal to 2; combinations of these ranges are also possible).
  • the reactor comprises a second outlet.
  • the second outlet is configured to discharge a gas (e.g., CO 2 , O 2 , and/or H 2 ).
  • a gas e.g., CO 2 , O 2 , and/or H 2
  • the CO 2 is to be sequestered, used in a liquid fuel, used in an oxyfuel, used in enhanced oil recovery, used to produce dry ice, and/or used as an ingredient in a beverage.
  • the O 2 is to be sequestered, used as oxyfuel, used in a CCS application, and/or used in enhanced oil recovery.
  • the H 2 is to be sequestered and/or used as a fuel (e.g., in a fuel cell and/or to heat the system).
  • At least a portion e.g., at least 10%, at least 25%, at least 50%, at least 75%, at least 90%, or all
  • the CO 2 , O 2 , and/or H 2 discharged from the system is fed into a kiln.
  • the reactor comprises a third outlet and/or a fourth outlet.
  • the second outlet, third outlet, and/or fourth outlet is configured to discharge CO 2 , O 2 , and/or H 2 .
  • the second outlet is configured to discharge CO 2 and O 2 while the third outlet is configured to discharge H 2 .
  • the second outlet is configured to discharge CO 2
  • the third outlet is configured to discharge O 2
  • the fourth outlet is configured to discharge H 2 .
  • the reactor further comprises one or more membranes selectively permeable to ions between the first electrode and the second electrode.
  • the one or more membranes selectively permeable to ions comprises two membranes selectively permeable to ions.
  • the two membranes selectively permeable to ions are different from each other.
  • the one or more membranes selectively permeable to ions is configured to prevent solid from precipitating on the first electrode, prevent solid from passivating the first electrode, and/or prevent two different solids from contaminating each other.
  • a membrane selectively permeable to ions allows ions to pass through while restricting (or eliminating) the passage of solids.
  • a metal ion e.g., Ca 2+
  • a solid metal salt e.g., a solid metal carbonate, such as solid CaCO 3
  • a precipitate e.g., solid metal hydroxide, such as solid Ca(OH) 2
  • the membrane selectively permeable to ions allows ions to pass through but restricts (or eliminates) the passage of non-ionic compounds. In certain embodiments, the membrane selectively permeable to ions allows ions to pass through at a first rate and allows non-ionic compounds to pass through at a second rate, which is slower than the first rate. In some embodiments, the membrane selectively permeable to ions allows certain ions to pass through but restricts (or eliminates) the passage of other ions. In certain embodiments, the membrane selectively permeable to ions allows certain ions to pass through at a first rate and allows other ions to pass through at a second rate, which is slower than the first rate.
  • membranes selectively permeable to ions may allow certain metal ions to pass through but restricts (or eliminates) the passage of others (or allows certain metal ions to pass through faster than others), may allow H + to pass through but restricts (or eliminates) the passage of OH ⁇ (or allows H + to pass through faster than OH ⁇ ) may allow OH ⁇ to pass through but restricts (or eliminates) the passage of H + (or allows OH ⁇ to pass through faster than H + ), may allow metal ions to pass through but restricts (or eliminates) the passage of H + and/or OH ⁇ (or allows metal ions to pass through faster than H + and/or OH ⁇ ), and/or may allow H + and/or OH ⁇ ions to pass through but restricts (or eliminates) the passage of metal ions (or allows H + and/or OH ⁇ ions to pass through faster than metal ions).
  • the membrane selectively permeable to ions is permeable to OH ⁇ ions but relatively less permeable to Ca 2+ ions, while the membrane selectively permeable to ions is permeable to Ca 2+ ions but relatively less permeable to OH ⁇ ions.
  • Ca 2+ from the first region e.g., acidic region
  • the second region e.g., alkaline region
  • OH ⁇ ions from the second region could diffuse through the membrane selectively permeable to ions into the separate chamber, but could not diffuse through the membrane selectively permeable to ions.
  • Ca 2+ and OH ⁇ would only be able to react, forming solid Ca(OH) 2 , in the separate chamber, preventing solid Ca(OH) 2 from forming on the cathode or anode.
  • the one or more membranes selectively permeable to ions could prevent solid (e.g., solid metal hydroxide, such as solid Ca(OH) 2 ) from precipitating on the first electrode (e.g., cathode), prevent solid (e.g., solid metal hydroxide, such as solid Ca(OH) 2 ) from passivating the first electrode (e.g., cathode); and/or prevent two different solids—the chemical compound (e.g., a metal salt, such as a solid metal carbonate, such as solid calcium carbonate) and the precipitate (e.g., a solid hydroxide, such as a solid metal hydroxide, such as solid Ca(OH) 2 ) from contaminating each other.
  • solid e.g., solid metal hydroxide, such as solid Ca(OH) 2
  • the chemical compound e.g., a metal salt, such as a solid metal carbonate, such as solid calcium carbonate
  • the precipitate e.g., a solid hydroxide,
  • the reactor is directed toward the production of a calcined, or decomposed, mineral or metal salt (e.g., metal carbonate) through electrochemical and chemical means.
  • a calcined, or decomposed, mineral or metal salt e.g., metal carbonate
  • the use of fossil fuels for production of thermal energy, and the associated production of greenhouse gases (e.g., CO 2 ) or gases that are atmospheric pollutants is reduced or avoided through the use of such a reactor in place of traditional thermal calcination that involves heating of the mineral or metal salt to decompose it.
  • the system comprises a reactor.
  • the reactor comprises any of the reactor embodiments disclosed above or elsewhere herein, or combinations thereof.
  • the system (e.g., any system described herein) comprises a kiln.
  • the system comprises an electrochemical reactor and kiln 150 .
  • the system comprises an electrochemical reactor and kiln 150 .
  • the kiln comprises a kiln inlet.
  • the kiln is attached directly to the reactor and/or to an apparatus (e.g., an apparatus configured to react acid and/or base in a precipitation reaction).
  • a kiln (e.g., any kiln described herein) may be used in any system described herein.
  • the kiln is downstream from the reactor, reactor outlet, and/or one or more apparatuses.
  • the system further comprises a heater between the reactor, reactor outlet, and/or one or more apparatuses and the kiln inlet. Examples of heaters include devices that heat or dehydrate the substance placed inside it.
  • the reactor outlet is attached directly to the kiln inlet.
  • a direct attachment exists between a first unit and a second unit (and the two units are said to be “attached directly to” each other) when they are connected to each other and the composition of the material being transferred between the units does not substantially change (i.e., no component changes in relative abundance by more than 5%) as it is transported from the first unit to the second unit.
  • a conduit that connects first and second units, and in which the pressure and temperature of the contents of the conduit are adjusted but the composition of the contents is not altered, would be said to directly attach the first and second units.
  • the conduit would not be said to directly connect the first and second units.
  • two units that are attached directly to each other are configured such that there is no phase change of the material as it is transported from the first unit to the second unit.
  • the kiln inlet is configured to receive at least a portion of the solid calcium hydroxide and/or solid calcium oxide derived from at least a portion of the solid calcium hydroxide.
  • calcium hydroxide is collected from the reactor, reactor outlet, and/or more apparatuses and the reactor, reactor outlet, and/or more apparatuses is attached directly to the kiln inlet, such that the kiln inlet is configured to receive at least a portion of the solid calcium hydroxide.
  • calcium hydroxide is collected from the reactor, reactor outlet, and/or more apparatuses, and is transported to the heater.
  • the heater converts the calcium hydroxide to calcium oxide, in full or in part.
  • the kiln inlet is configured to receive at least a portion of the solid calcium hydroxide and/or solid calcium oxide derived from at least a portion of the solid calcium hydroxide from the heater.
  • the kiln is configured to heat the Ca(OH) 2 (e.g., solid calcium hydroxide) and/or lime (e.g., solid calcium oxide) and/or a reaction product thereof as part of a cement-making process.
  • heating the Ca(OH) 2 and/or lime as part of a cement-making process comprises heating the Ca(OH) 2 and/or lime in the kiln with other compounds.
  • the Ca(OH) 2 and/or lime could be heated in the kiln with SiO 2 or other minerals.
  • the system has lower net carbon emissions (e.g., at least 10% lower, at least 25% lower, at least 50% lower, at least 75% lower, or at least 90% lower) than substantially similar systems that use traditional thermal calcination instead of the electrochemical reactor. In some instances, the system has net-zero carbon emissions.
  • Certain aspects are related to methods of forming precipitates in a spatially varying chemical composition gradient (e.g., spatially varying pH gradient). According to some embodiments, the method is performed in a reactor and/or system as described in association with any of the embodiments disclosed above or elsewhere herein, or combinations thereof.
  • the method comprises transporting a chemical compound (e.g., a metal salt) to a first region (e.g., an acidic region) of the spatially varying chemical composition gradient (e.g., the spatially varying pH gradient).
  • a chemical compound e.g., a metal salt
  • the metal salt comprises metal carbonate.
  • the metal carbonate comprises calcium carbonate, magnesium carbonate, and/or nickel carbonate.
  • the method comprises transporting calcium carbonate to a first region (e.g., an acidic region) of the spatially varying pH gradient.
  • the chemical compound e.g., the metal salt
  • a liquid within the spatially varying chemical composition gradient e.g., spatially varying pH gradient.
  • liquids include non-aqueous or aqueous solutions.
  • non-aqueous solutions include solutions comprising a non-aqueous solvent and an electrolyte salt and/or solutions comprising an ionic liquid.
  • aqueous solutions include solutions comprising water and an electrolyte salt.
  • electrolyte salts include NaSO 4 and NaClO 4 .
  • the chemical compound e.g., the metal salt
  • the spatially varying chemical composition gradient e.g., the spatially varying pH gradient
  • calcium carbonate is dissolved and/or reacted in a liquid within the spatially varying chemical composition gradient (e.g., the spatially varying pH gradient).
  • calcium carbonate is dissolved and reacted within the liquid within the spatially varying chemical composition gradient (e.g., the spatially varying pH gradient).
  • the chemical compound e.g., metal salt
  • the chemical compound e.g., calcium carbonate
  • the chemical compound e.g., metal salt
  • the protons in the first region e.g., acidic region
  • the chemical compound e.g., metal salt
  • the chemical compound e.g., calcium carbonate
  • the one or more elements moves to the second region (e.g., alkaline region), where it reacts with the hydroxide ions in the second region (e.g., alkaline region), forming a precipitate (e.g., a metal precipitate, such as Ca(OH) 2 ).
  • a metal such as Ca 2+
  • the first region comprises an acidic region.
  • the second region comprises an alkaline region.
  • the chemical compound e.g., metal salt
  • the one or more elements e.g., a metal, such as Ca 2+
  • the first region comprises an alkaline region.
  • the second region comprises an acidic region.
  • the chemical compound e.g., metal salt
  • the one or more elements e.g., a metal, such as Ca 2+
  • the method comprises collecting a precipitate from a second region (e.g., an alkaline region) of the spatially varying chemical composition gradient (e.g., spatially varying pH gradient).
  • the precipitate comprises a metal precipitate, such as a metal hydroxide.
  • metal hydroxides include nickel hydroxide, calcium hydroxide, and magnesium hydroxide.
  • the one or more elements moves to the second region (e.g., alkaline region), where it reacts with the hydroxide ions in the second region (e.g., alkaline region), forming a precipitate (e.g., a metal precipitate, such as Ca(OH) 2 ).
  • the method comprises collecting solid calcium hydroxide from an alkaline region of the spatially varying chemical composition gradient (e.g., spatially varying pH gradient).
  • Non-limiting examples of ways in which the one or more elements (e.g., the metal) can move to the second region (e.g., alkaline region) include diffusion, transportation by convection, and/or transportation by flow.
  • the precipitate comprises one or more elements (e.g., metal) from the chemical compound (e.g., the metal salt) dissolved and/or reacted within the spatially varying chemical composition gradient (e.g., spatially varying pH gradient).
  • the one or more elements comprises a metal element.
  • Metal refers to metallic metal or a metal ion.
  • the precipitate comprises a metal cation from the metal salt that was dissolved and/or reacted within the spatially varying chemical composition gradient (e.g., spatially varying pH gradient), and that metal cation is ionically bonded to an anion within the precipitate.
  • the solid calcium hydroxide comprises calcium from the calcium carbonate dissolved and/or reacted within the spatially varying chemical composition gradient (e.g., spatially varying pH gradient).
  • the method is a method of making cement.
  • the method comprises heating the Ca(OH) 2 (e.g., solid calcium hydroxide) and/or lime (e.g., solid calcium oxide) and/or a reactant product thereof within a kiln to make cement.
  • this comprises taking the calcium hydroxide from the reactor and placing it directly in the kiln.
  • there are steps in between collecting the calcium hydroxide and heating in the kiln e.g., a heater.
  • the heater converts the calcium hydroxide to its calcium oxide, and then the calcium hydroxide and/or the oxide calcium oxide are heated in the kiln.
  • the heater converts 100% (by weight) of the calcium hydroxide to its calcium oxide and only the calcium oxide is heated in the kiln. In other embodiments, the heater converts 10% or more, 20% or more, 30% or more, 40% or more, 50% or more, up to 90%, up to 95%, or up to 99% (by weight) of the calcium hydroxide to calcium oxide. Combinations of these ranges are also possible (e.g., 10% to 100% (by weight) inclusive). In some embodiments, both the calcium hydroxide and calcium oxide are heated in the kiln. Examples of heaters include devices that heat or dehydrate the substance placed inside it.
  • heating the Ca(OH) 2 (e.g., solid calcium hydroxide) and/or lime (e.g., solid calcium oxide) and/or a reactant product thereof within a kiln to make cement comprises heating the s Ca(OH) 2 (e.g., solid calcium hydroxide) and/or lime (e.g., solid calcium oxide) and/or a reactant product thereof in the kiln with other compounds.
  • the Ca(OH) 2 (e.g., solid calcium hydroxide) and/or lime (e.g., solid calcium oxide) and/or a reactant product thereof could be heated in the kiln with SiO 2 or other minerals.
  • the method is part of a batch process.
  • the precipitate e.g., a metal hydroxide, such as Ca(OH) 2
  • the method is performed continuously.
  • the chemical compound e.g., a metal salt, such as a metal carbonate, such as CaCO 3
  • the precipitate e.g., a metal hydroxide, such as Ca(OH) 2
  • the precipitate is collected continuously or periodically.
  • Non-limiting examples of collecting the precipitate (e.g., a metal hydroxide, such as Ca(OH) 2 ) include collecting it with a flow stream and/or allowing it to deposit on a surface from which it is continuously or periodically collected.
  • the method produces a byproduct different from the precipitate.
  • the method produces a byproduct different from the solid calcium hydroxide and/or the solid calcium oxide.
  • the byproduct comprises CO 2 , O 2 , and/or H 2 .
  • hydrolysis is performed in the reactor, and the reaction taking place in the cathode converts 2 H 2 O molecules and 2 electrons to H 2 (g) and 2 OH ⁇ , while the reaction taking place in the anode converts 2 H 2 O molecules to O 2 (g), 4 electrons, and 4 protons.
  • the chemical compound e.g., metal salt
  • a metal carbonate such as calcium carbonate
  • the chemical compound e.g., metal salt
  • the protons in the first region e.g., acidic region
  • the chemical compound e.g., metal salt
  • the net reaction between CaCO 3 and two protons results in the formation of H 2 O, Ca 2+ , and CO 2 (g).
  • the method further comprises collecting the byproduct.
  • the byproduct comprises CO 2 , O 2 , and H 2 .
  • collecting the byproduct comprises collecting each of the CO 2 , O 2 , and H 2 ; collecting only the CO 2 , collecting only the O 2 ; collecting only the H 2 ; collecting CO 2 and O 2 ; collecting CO 2 and H 2 , or collecting O 2 and H 2 .
  • the byproduct comprises CO 2 and the collecting the byproduct comprises sequestering the CO 2 .
  • the byproduct is used as fuel.
  • the H 2 can be used as a fuel. Non-limiting examples include burning the H 2 directly or using it with a fuel, such as natural gas.
  • the O 2 and CO 2 are used to support combustion of a fuel, such as a fossil fuel.
  • the byproducts are used as fuel for a kiln.
  • the O 2 and CO 2 are fed into the kiln to support combustion of a fuel, such as a fossil fuel.
  • the H 2 , O 2 , and CO 2 are reacted in a fuel cell, such as a solid oxide fuel cell.
  • H 2 and O 2 are reacted in a fuel cell to produce electric power.
  • the reactors, systems, and methods described herein display one or more beneficial properties and have one or more applications.
  • some embodiments of the reactors, systems, and methods described herein may be used for producing cement (e.g., Portland cement).
  • the reactor is used in place of calcination in a traditional cement production process.
  • certain embodiments of the reactors, systems, and methods described herein may be used for producing cement with reduced production of atmospheric pollutants or greenhouse gases, such as CO 2 , than traditional cement production processes.
  • Traditional cement production processes include calcination of CaCO 3 by thermal means, which accounts for about 60% of the CO 2 emissions while about 40% of the CO 2 emissions results from the burning of fossil fuels to carry out the calcination and sintering processes.
  • Ca(OH) 2 produced by the methods, reactors, and/or systems described herein can be used to produce CaO for cement making, instead of traditional calcination of CaCO 3 to CaO.
  • the thermal dehydration of Ca(OH) 2 to CaO has a 25% lower minimum energy requirement (71.2 kJ/mol) than thermal calcination of CaCO 3 to CaO (97.0 kJ/mol).
  • the reactor and/or system is powered, in part or in full, by renewable electricity (e.g., solar energy, wind energy, and/or hydroelectric power.).
  • renewable electricity e.g., solar energy, wind energy, and/or hydroelectric power.
  • byproducts such as CO 2 , H 2 , and/or O 2 are generated, which have many possible uses, including for oxy-combustion, improved kiln efficiency, reduced NO x emissions, and/or as flue gas suitable for carbon capture and sequestration (CCS).
  • CCS carbon capture and sequestration
  • the electrolytically-driven chemical reactor comprises an electrolysis cell for the electrolysis of water.
  • a cell when performing electrolysis, produces a high pH at the cathode, where a hydrogen evolution reaction (HER) is taking place and producing OH ⁇ , and produces a low pH at the anode, where an oxygen evolution reaction (OER) is taking place and producing H + .
  • a gradient in pH is therefore produced, in accordance with certain embodiments, between the cathode and anode.
  • a gradient in other species may be produced depending on the nature of the electrolysis reaction.
  • said pH gradient is used to dissolve a metal carbonate at low pH in the vicinity of the anode, and to precipitate a metal hydroxide as the metal ion diffuses towards the higher pH environment at the cathode.
  • a metal carbonate as the metal carbonate is dissolved near the anode, CO 2 gas is produced, and metal cations of the carbonate are produced in solution. These then diffuse, in accordance with some such embodiments, or are optionally transported by convection or flow, toward the high pH environment produced by HER at the cathode.
  • reaction of the metal ion with OH ⁇ ions produced at the cathode results in the precipitation of the metal hydroxide.
  • any metal carbonate or mixtures of metal carbonates may be converted to its hydroxide or hydroxides through such a process, with non-limiting examples of metal carbonates including CaCO 3 , MgCO 3 , and NiCO 3 .
  • metal carbonates including CaCO 3 , MgCO 3 , and NiCO 3 .
  • hydrogen gas is liberated at the cathode and a mixture of oxygen gas and carbon dioxide gas is liberated at the anode.
  • the reactor is operated in a batch manner whereby the product metal hydroxide is periodically collected. In one or more embodiments, the reactor is operated in a continuous manner such that additional metal carbonate is added continuously or periodically at the anode, and the precipitated metal hydroxide is continuously or periodically removed from the reaction zone. For example, precipitated metal hydroxide may be removed from the reaction zone using a flow stream and collected, or the precipitate may be allowed to deposit on a surface from which it is continuously or periodically removed while the reactor continues to operate.
  • the hydrogen and/or oxygen gas produced by the electrochemical reactor is beneficially used or sold.
  • the hydrogen and oxygen are reacted in a fuel cell to produce electric power.
  • the hydrogen is combusted as a fuel or as a component of a fuel for the purpose of heating a reactor or kiln or furnace.
  • the electric power to carry out said electrolytically-driven chemical reactor is produced from renewable resources, including but not limited to solar energy, wind energy, or hydroelectric power.
  • said electrochemically-driven chemical reactor is used to decarbonize CaCO 3 and produce Ca(OH) 2 as a precursor for the production of cement, such as Portland cement. It is useful to compare both the total energy consumption, and to consider the form of the energy consumed and its carbon intensity. For simplicity, it is assumed that the high temperature heat treatment that reacts CaO with aluminosilicates and other components to form Portland cement is identical for the two processes.
  • the energy consumption to bring CaO produced by thermal calcination of CaCO 3 , and by electrochemical decarbonization followed by thermal dehydration of Ca(OH) 2 , to the same starting temperature of 900 C has been considered.
  • the energy per mole input to heat the reactant or product to a given temperature has been calculated from its heat capacity.
  • the energy per mole to carry out the decomposition reactions has been given as the standard free energy of reaction (i.e., gas partial pressures are 1 atm).
  • the electrochemical process also includes the decarbonation reaction in which CaCO 3 is converted to Ca(OH) 2 with a standard free energy of 74.3 kJ/mole; this is an additional energy consumption for the electrochemical process.
  • this exemplary process, as well as the electrolysis reaction can be powered by electricity from low or zero-carbon renewable resources at nearly zero marginal cost of electricity.
  • the electrolysis reaction necessary to operate the reactor, in this exemplary process requires 237.1 kJ/mole; however, this energy firstly can be generated by low carbon sources as well, and secondly, yields hydrogen and oxygen that can be used remotely as a value-added product, or can be used to power the cement production process, for example by using a fuel cell to provide electrical power, or through a combustion process to provide reaction heat.
  • the energy produced may be used to operate the electrolyser, or to heat the high temperature kiln.
  • the calcium hydroxide also known as slaked lime, and/or calcium oxide, which is reacted with water to produce slaked lime, produced herein (e.g., from a precipitation reaction) can be used in applications including but not limited to paper making, flue gas treatment carbon capture, plaster mixes and masonry (including Pozzolan cement), soil stabilization, pH adjustment, water treatment, waste treatment, and sugar refining.
  • the following are non-limiting examples of uses of calcium hydroxide (also known as slake lime) and/or calcium oxide (also known as lime).
  • slaked lime and/or lime produced by the reactors, systems, and/or methods disclosed herein is used in the making of iron and/or steel.
  • lime can be used as a flux, to form slag that prevents the iron and/or steel from oxidizing, and to remove impurities such as silica, phosphates, manganese and sulfur.
  • slaked lime dry, or as a slurry
  • lime or slaked lime is also used to neutralize acidic wastes.
  • slaked lime and/or lime produced by the reactors, systems, and/or methods disclosed herein is used in the making of nonferrous metals including, but not limited to, copper, mercury, silver, gold, zinc, nickel, lead, aluminum, uranium, magnesium and/or calcium.
  • Lime may be used, in some cases, as a fluxing agent, to remove impurities (such as silica, alumina, phosphates, carbonates, sulfur, sulfates) from ores.
  • impurities such as silica, alumina, phosphates, carbonates, sulfur, sulfates
  • lime and slaked lime can be used in the flotation or recovery of non-ferrous ores.
  • lime acts as a settling aid, to maintain proper alkalinity, and/or to remove impurities (such as sulfur and/or silicon).
  • slaked lime is used to neutralize sulfurous gases and/or to prevent the formation of sulfuric acid.
  • lime and/or slaked lime is also used as a coating on metals to prevent the reaction with sulfurous species.
  • lime and/or slaked lime is used to remove impurities (such as silica and/or carbonate) from bauxite ore, and/or is used to regulate pH.
  • lime is used to maintain alkaline pH for the dissolution of gold, silver, and/or nickel in cyanide extraction.
  • lime is used as a reducing agent in certain cases.
  • magnesium and/or calcium oxides are reduced at high temperatures to form magnesium and/or calcium metal.
  • slaked lime and/or lime produced by the reactors, systems, and/or methods disclosed herein is used for making masonry mortars, plasters, stuccos, whitewashes, grouts, bricks, boards, and/or non-Portland cements.
  • lime and/or slaked lime may be mixed with other additives and exposed to carbon dioxide to produce calcium carbonate, lime and/or slaked lime may be reacted with other additives (such as aluminosilicates) to form a cementitious material, and/or lime and/or slaked lime may be used as a source of calcium.
  • lime and/or slaked lime is mixed with additives and/or aggregates (such as sand) to form a paste/slurry that hardens as water evaporates and as the lime and/or slaked lime reacts with atmospheric carbon dioxide to form calcium carbonate.
  • additives and/or aggregates such as sand
  • lime and/or slaked lime is reacted with aluminates, silicates, and/or other pozzolanic materials (e.g., pulverized fuel ash, volcanic ash, blast furnace slag, and/or calcined clay), to form a water-based paste/slurry that hardens as insoluble calcium aluminosilicates are formed.
  • aluminates, silicates, and/or other pozzolanic materials e.g., pulverized fuel ash, volcanic ash, blast furnace slag, and/or calcined clay
  • lime and/or slaked lime is reacted at high temperature with sources of silica, alumina, and/or other additives such that cementitious compounds are formed, including dicalcium silicate, calcium aluminates, tricalcium silicate, and/or mono calcium silicate.
  • sources of silica, alumina, and/or other additives such that cementitious compounds are formed, including dicalcium silicate, calcium aluminates, tricalcium silicate, and/or mono calcium silicate.
  • sandlime bricks are made by reacting slaked lime with a source of silica (e.g., sand, crushed siliceous stone, and/or flint) and/or other additives at temperatures required to form calcium silicates and/or calcium silicate hydrates.
  • lightweight concrete e.g., aircrete
  • lightweight concrete is made by reacting lime and/or slaked lime with reactive silica, aluminum powder, water, and/or other additives; the reaction between slaked lime and silicates/aluminates causes calcium silicates/aluminates and/or calcium silicate hydrates to form, while the reaction between water, slaked lime and aluminum causes hydrogen bubbles to form within the hardening paste.
  • Whitewash is a white coating made from a suspension of slaked lime, which hardens and sets as slaked lime reacts with carbon dioxide from the atmosphere.
  • Calcium silicate boards, concrete, and other cast calcium silicate products are formed, in some cases, when calcium silicate-forming materials (e.g., lime, slaked lime, silica, and/or cement) and additives (e.g., cellulose fiber and/or fire retardants) and water are mixed together, cast or pressed into shape. In some cases, high temperatures are used to react the lime, slaked lime, and/or silica, and/or to hydrate the cement.
  • calcium silicate-forming materials e.g., lime, slaked lime, silica, and/or cement
  • additives e.g., cellulose fiber and/or fire retardants
  • slaked lime and/or lime produced by the reactors, systems, and/or methods disclosed herein is used to stabilize, harden, and/or dry soils.
  • lime and/or slaked lime may be applied to loose or fine-grained soils before the construction of roads, runways, and/or railway tracks, and/or to stabilize embankments and/or slopes.
  • a pozzolanic reaction may occur between the clay and the lime to produce calcium silicate hydrates, and/or calcium aluminate hydrates, which strengthen and/or harden the soil.
  • lime and/or slaked lime applied to soils may also react with carbon dioxide to produce solid calcium carbonate, which may also strengthen and/or harden soil.
  • lime may also be used to dry wet soils at construction sites, as lime reacts readily with water to form slaked lime.
  • slaked lime and/or lime produced by the reactors, systems, and/or methods disclosed herein is used to make and/or recycle asphalt.
  • slaked lime is added to hot mix asphalt as a mineral filler and/or antioxidant, and/or to increase resistance to water stripping.
  • slaked lime can react with aluminosilicates and/or carbon dioxide to create a solid product that improves the bond between the binder and aggregate in asphalt.
  • lime may increase the viscosity of the binder, the stiffness of the asphalt, the tensile strength of the asphalt, and/or the compressive strength of the asphalt.
  • lime may reduce moisture sensitivity and/or stripping, stiffen the binder so that it resists rutting, and/or improve toughness and/or resistance to fracture at low temperature.
  • lime and/or slaked lime added to recycled asphalt results in greater early strength and/or resistance to moisture damage.
  • slaked lime and/or lime produced by the reactors, systems, and/or methods disclosed herein is used for the removal of acid gases (such as hydrogen chloride, sulfur dioxide, sulfur trioxide, and/or hydrogen fluoride) and/or carbon dioxide from a gas mixture (e.g. flue gas, atmospheric air, air in storage rooms, and/or air in closed breathing environments such as submarines).
  • acid gases such as hydrogen chloride, sulfur dioxide, sulfur trioxide, and/or hydrogen fluoride
  • carbon dioxide e.g. flue gas, atmospheric air, air in storage rooms, and/or air in closed breathing environments such as submarines.
  • lime and/or slaked lime is exposed to flue gas, causing the reaction of lime and/or slaked lime with components of the flue gas (such as acid gases, including hydrogen chloride, sulfur dioxide and/or carbon dioxide), resulting in the formation of non-gaseous calcium compounds (such as calcium chloride, calcium sulfite, and/or calcium carbonate).
  • flue gas such as acid gases, including hydrogen chloride, sulfur dioxide and/or carbon dioxide
  • non-gaseous calcium compounds such as calcium chloride, calcium sulfite, and/or calcium carbonate
  • exposure of gas to slaked lime is done by spraying slaked lime solutions and/or slurries onto gas, and/or by reacting gas streams with dry lime and/or slaked lime.
  • the gas stream containing acid gas or gases is first reacted with a solution of alkali metal hydroxides (e.g.
  • the calcium carbonate formed from the reaction of lime and/or slaked lime with carbon dioxide or alkali carbonate is returned to the reactors, systems, and/or methods disclosed herein, so that the lime and/or slaked lime can be regenerated and/or so that the carbon dioxide can be sequestered.
  • slaked lime and/or lime produced by the reactors, systems, and/or methods disclosed herein is used to treat wastes such as biological wastes, industrial wastes, wastewaters, and/or sludges.
  • lime and/or slaked lime may be applied to the waste to create an alkaline environment, which serves to neutralize acid waste, inhibit pathogens, deter flies or rodents, control odors, prevent leaching, and/or stabilize and/or precipitate pollutants (such as heavy metals, chrome, copper, and/or suspended/dissolved solids) and/or dissolved ions that cause scaling (calcium and/or magnesium ions).
  • pollutants such as heavy metals, chrome, copper, and/or suspended/dissolved solids
  • dissolved ions that cause scaling (calcium and/or magnesium ions).
  • lime may be used to de-water oily wastes.
  • slaked lime may be used to precipitate certain species, such as phosphates, nitrates, and/or sulfurous compounds, and/or prevent leaching.
  • lime and/or slaked lime may be used to hasten the decomposition of organic matter, by maintaining alkaline conditions that favor hydrolysis.
  • slaked lime and/or lime produced by the reactors, systems, and/or methods disclosed herein is used to treat water.
  • lime and/or slaked lime may be used, in some cases, to create an alkaline environment, which serves to disinfect, remove suspended/colloidal material, reduce hardness, adjust pH, precipitate ions contributing to water hardness, precipitate dissolved metals (such as iron, aluminum, manganese, barium, cadmium, chromium, lead, copper, and/or nickel), and/or precipitate other ions (such as fluoride, sulfate, sulfite, phosphate, and/or nitrate).
  • dissolved metals such as iron, aluminum, manganese, barium, cadmium, chromium, lead, copper, and/or nickel
  • precipitate other ions such as fluoride, sulfate, sulfite, phosphate, and/or nitrate.
  • slaked lime and/or lime produced by the reactors, systems, and/or methods disclosed herein is used for agriculture.
  • lime and/or slaked lime may be used alone, or as an additive in fertilizer, to adjust the pH of the soil and/or of the fertilizer mixture to give optimum growing conditions and/or improve crop yield, in some cases.
  • slaked lime and/or lime produced by the reactors, systems, and/or methods disclosed herein is used to refine sugar.
  • lime and/or slaked lime is used to raise the pH of raw sugar juice, destroy enzymes in the raw sugar juice, and/or react with inorganic and/or organic species to form precipitates.
  • Excess calcium may be precipitated with carbon dioxide, in certain instances.
  • the precipitated calcium carbonate that results may be returned to the reactors, systems, and/or methods disclosed herein, to regenerate slaked lime.
  • slaked lime and/or lime produced by the reactors, systems, and/or methods disclosed herein is used to make leather and/or parchment.
  • lime is used, in some cases, to remove hair and/or keratin from hides, split fibers, and/or remove fat.
  • slaked lime and/or lime produced by the reactors, systems, and/or methods disclosed herein is used to make glue and/or gelatin.
  • animal bones and/or hides are soaked in slaked lime, causing collagen and other proteins to hydrolyze, forming a mixture of protein fragments of different molecular weights.
  • slaked lime and/or lime produced by the reactors, systems, and/or methods disclosed herein is used to make dairy products.
  • slaked lime is used to neutralize acidity of cream before pasteurization.
  • slaked lime is used to precipitate calcium caseinate from acidic solutions of casein.
  • slaked lime is added to fermented skim milk to produce calcium lactate.
  • slaked lime and/or lime produced by the reactors, systems, and/or methods disclosed herein is used in the fruit industry.
  • slaked lime and/or lime is used, in some cases, to remove carbon dioxide from air in fruit storage.
  • slaked lime is used to neutralize waste citric acid and to raise the pH of fruit juices.
  • slaked lime and/or lime produced by the reactors, systems, and/or methods disclosed herein is used as an additive in fungicides and/or insecticides.
  • slaked lime may be mixed with coper sulfate to form tetracupric sulfate, a pesticide.
  • lime may also be used as a carrier for other kinds of pesticides, as it forms a film on foliage as it carbonates, retaining the insecticide on the leaves.
  • slaked lime is used to control infestations of starfish on oyster beds.
  • slaked lime and/or lime produced by the reactors, systems, and/or methods disclosed herein is used as a food additive.
  • lime and/or slaked lime may be used as an acidity regulator, as a pickling agent, to remove cellulose (e.g. from kernels such as maize), and/or to precipitate certain anions (such as carbonates) from brines.
  • slaked lime and/or lime produced by the reactors, systems, and/or methods disclosed herein is used to make chemicals.
  • lime and/or slaked lime may be used as a source of calcium and/or magnesium, an alkali, a desiccant, causticizing agent, saponifying agent, bonding agent, flocculant and/or precipitant, fluxing agent, glass-forming product, degrader of organic matter, lubricant, filler, and/or hydrolyzing agent, among other things.
  • slaked lime and/or lime produced by the reactors, systems, and/or methods disclosed herein is used to make precipitated calcium carbonate.
  • a solution and/or slurry of slaked lime, and/or a solution of calcium ions is reacted with carbon dioxide, and/or an alkali carbonate, so that a precipitate of calcium carbonate and/or magnesium carbonate forms.
  • the precipitated alkali metal carbonate may be used as a filler, to reduce shrinkage, improve adhesion, increase density, modify rheology and/or to whiten/brighten plastics (such as PVC and latex), rubber, paper, paints, inks, cosmetics, and/or other coatings.
  • Precipitated carbonates in some cases, may be used as flame retarders or dusting powder.
  • precipitated calcium carbonate may be used as an alkalizer, for agriculture, as an antiseptic agent, flour additive, brewing additive, digestive aid, and/or additive for bituminous products), an abrasive (in cleaners, detergents, polishes and/or toothpastes), a dispersant in pesticides, and/or a desiccant.
  • slaked lime and/or lime produced by the reactors, systems, and/or methods disclosed herein is used to make calcium hypochlorite, a bleach, by reacting chlorine with lime and/or slaked lime.
  • slaked lime and/or lime produced by the reactors, systems, and/or methods disclosed herein is used to make calcium carbide, a precursor to acetylene, by reacting lime with carbonaceous matter (e.g. coke) at high temperature.
  • carbonaceous matter e.g. coke
  • slaked lime and/or lime produced by the reactors, systems, and/or methods disclosed herein is used to make calcium phosphates (monocalcium phosphate, dicalcium phosphate, and/or tricalcium phosphate) by reacting phosphoric acid with slaked lime, and/or aqueous calcium ions, in the appropriate ratios.
  • monocalcium phosphate may be used as an additive in self-rising flour, mineral enrichment foods, as a stabilizer for milk products and/or as a feedstuff additive.
  • dicalcium phosphate dihydrate is used in toothpastes, as a mild abrasive, for mineral enrichment of foodstuffs, as a pelletizing aid and/or as a thickening agent.
  • tricalcium phosphate is used in toothpastes, and/or as an anti-caking agent in foodstuffs and/or fertilizers.
  • slaked lime and/or lime produced by the reactors, systems, and/or methods disclosed herein is used to make calcium bromide. This is done, in some cases, by reacting lime and/or slaked lime with hydrobromic acid and/or bromine and a reducing agent (e.g. formic acid and/or formaldehyde).
  • a reducing agent e.g. formic acid and/or formaldehyde
  • slaked lime and/or lime produced by the reactors, systems, and/or methods disclosed herein is used to make calcium hexacyanoferrate, by reacting lime and/or slaked lime with hydrogen cyanide in an aqueous solution of ferrous chloride. Calcium hexacyanoferrate can then be converted to the alkali metal salt, or hexacyanoferrates. These are used as pigments and anti-caking agents.
  • slaked lime and/or lime produced by the reactors, systems, and/or methods disclosed herein is used to make calcium silicon, by reacting lime, quartz and/or carbonaceous material at high temperatures.
  • calcium silicon is used as a de-oxidizer, as a de-sulfurizer, and/or to modify non-metallic inclusions in ferrous metals.
  • slaked lime and/or lime produced by the reactors, systems, and/or methods disclosed herein is used to make calcium dichromate, by roasting chromate ores with lime.
  • slaked lime and/or lime produced by the reactors, systems, and/or methods disclosed herein is used to make calcium tungstate, by reacting lime and/or slaked lime with sodium tungstate, to be used in the production of ferrotungsten and/or phosphors for items such as lasers, fluorescent lamps and/or oscilloscopes.
  • slaked lime and/or lime produced by the reactors, systems, and/or methods disclosed herein is used to make calcium citrate, by reacting lime and/or slaked lime with citric acid.
  • the calcium citrate may be reacted with sulfuric acid to regenerate pure citric acid.
  • slaked lime and/or lime produced by the reactors, systems, and/or methods disclosed herein is used to make calcium soaps, by reacting slaked lime with aliphatic acids, wax acids, unsaturated carboxylic acids (e.g. oleic acid, linoleic acid, ethylhexanoate acids), napthenic acids, and/or resin acids.
  • calcium soaps are used as lubricants, stabilizers, mold-release agents, waterproofing agents, coatings, and/or additives in printing inks.
  • slaked lime and/or lime produced by the reactors, systems, and/or methods disclosed herein is used to make calcium lactate, by reacting slaked lime with lactic acid.
  • the lactic acid may be reacted in a second step with sulfuric acid to produce pure lactic acid.
  • these chemicals act as coagulants and foaming agents.
  • calcium lactate is used as a source of calcium in pharmaceutical agents and/or foodstuffs, and/or as a buffer.
  • slaked lime and/or lime produced by the reactors, systems, and/or methods disclosed herein is used to make calcium tartrate, by reacting slaked lime with alkali bitartarates.
  • the calcium bitartarate may be reacted in a second step with sulfuric acid to produce pure tartaric acid.
  • tartaric acid is used in foodstuffs, pharmaceutical preparations, and/or as an additive in plaster and/or metal polish.
  • slaked lime and/or lime produced by the reactors, systems, and/or methods disclosed herein is used to make aluminum oxide.
  • Lime is used to precipitate impurities (e.g., silicates, carbonates, and/or phosphates) from processed bauxite ore in the preparation of aluminum oxide.
  • slaked lime and/or lime produced by the reactors, systems, and/or methods disclosed herein is used to make alkali carbonates and/or bicarbonates from alkali chlorides in the ammonia-soda process.
  • lime and/or slaked lime is reacted with ammonium chloride (and/or ammonium chlorides, such as isopropylammonium chloride) to regenerate ammonia (and/or amines, such as isopropyl amine) after the reaction of ammonia (and/or the amine) with an alkali chloride.
  • the resulting calcium chloride can be reacted with the alkaline stream from the reactors, systems, and/or methods disclosed herein, to regenerate the slaked lime.
  • slaked lime and/or lime produced by the reactors, systems, and/or methods disclosed herein is used to make strontium carbonate.
  • lime and/or slaked lime is used to re-generate ammonia from ammonium sulfate, which forms after the ammonia has been carbonated and reacted with strontium sulfate.
  • slaked lime and/or lime produced by the reactors, systems, and/or methods disclosed herein is used to make calcium zirconate.
  • lime and/or slaked lime reacts with zircon, ZrSiO 4 , to produce a calcium silicate and zirconate, which is further purified.
  • slaked lime and/or lime produced by the reactors, systems, and/or methods disclosed herein is used to make alkali hydroxides from alkali carbonates, in a process often called causticizing or re-causticizing.
  • slaked lime is reacted with alkali carbonates to produce alkali hydroxides and calcium carbonate.
  • the process of causticizing alkali carbonates is a feature of several other processes, in some instances, including the purification of bauxite ore, the processing of carbolic oil, and the Kraft liquor cycle (in which “green liquor”, containing sodium carbonate, reacts with slaked lime to form “white liquor”, containing sodium hydroxide).
  • slaked lime and/or lime produced by the reactors, systems, and/or methods disclosed herein is used to make magnesium hydroxide.
  • the addition of slaked lime to solutions containing magnesium ions causes magnesium hydroxide to precipitate from solution.
  • slaked lime and/or lime produced by the reactors, systems, and/or methods disclosed herein is used to make alkene oxides.
  • lime is used to saponify or dehydrochlorinate propylene and/or butene chlorohydrins to produce the corresponding oxides.
  • the oxides may then be converted to the glycols by acidic hydrolysis, in some instances.
  • slaked lime and/or lime produced by the reactors, systems, and/or methods disclosed herein is used to make diacetone alcohol.
  • slaked lime is used as an alkaline catalyst to promote the self-condensation of acetone to form diacetone alcohol, which is used as a solvent for resins, and/or as in intermediate in the production of mesityl oxide, methyl isobutyl ketone and/or hexylene glycol.
  • slaked lime and/or lime produced by the reactors, systems, and/or methods disclosed herein is used as a basic catalyst to make hydroxypivalic acid neopentyl glycol ester, and/or pentaerythritol.
  • slaked lime and/or lime produced by the reactors, systems, and/or methods disclosed herein is used as a basic reagent, to replace a sulfonic acid group with a hydroxide, in the making of anthraquinone dyes and/or intermediates.
  • slaked lime and/or lime produced by the reactors, systems, and/or methods disclosed herein is used to remove a chlorine from tetrachloroethane to form trichloroethylene.
  • slaked lime and/or lime produced by the reactors, systems, and/or methods disclosed herein is used as a binder, bonding and/or stabilizing agent in the fabrication of silica, silicon carbide and/or zirconia refractories.
  • slaked lime and/or lime produced by the reactors, systems, and/or methods disclosed herein is used as a source of lime in the fabrication of soda-lime glass.
  • lime and/or slaked lime is heated to high temperatures with other raw materials, including silica, sodium carbonate and/or additives such as alumina and/or magnesium oxide.
  • the molten mixture forms a glass upon cooling.
  • slaked lime and/or lime produced by the reactors, systems, and/or methods disclosed herein is used to make whiteware pottery and/or vitreous enamels.
  • slaked lime is blended with clays to act as a flux, a glass-former, to help bind the materials, and/or to increase the whiteness of the final product.
  • slaked lime and/or lime produced by the reactors, systems, and/or methods disclosed herein is used as a lubricant for casting and/or drawing of materials (such as iron, aluminum, copper, steel and/or noble metals).
  • materials such as iron, aluminum, copper, steel and/or noble metals.
  • calcium-based lubricants can be used at high temperature to prevent the metal from sticking to the mold.
  • lubricants can be calcium soaps, blends of lime and other materials (including silicilic acid, aluminia, carbon and/or fluxing agents such as fluorospar and/or alkali oxides).
  • Slaked lime is used as a lubricant carrier, in some cases.
  • the slaked lime bonds to the surface of the wire increases surface roughness and/or improves adhesion of the drawing compound.
  • slaked lime and/or lime produced by the reactors, systems, and/or methods disclosed herein is used in drilling mud formulations to maintain high alkalinity and/or to keep clay in a non-plastic state.
  • Drilling mud may, in some cases, be pumped through a hollow drill tube when drilling through rock for oil and gas. In certain instances, the drilling mud carries fragments of rock produced by the drill bit to the surface.
  • slaked lime and/or lime produced by the reactors, systems, and/or methods disclosed herein is used as an oil additive and/or lubricating grease.
  • lime is reacted with alkyl phenates and/or organic sulfonates to make calcium soaps, which are blended with other additives to make oil additives and/or lubricating greases.
  • the lime-based additives prevent sludge build-up and to reduce acidity from products of combustion, especially at high temperature.
  • slaked lime and/or lime produced by the reactors, systems, and/or methods disclosed herein is used in the pulp and/or paper industry.
  • slaked lime is used in the Kraft process to re-causticize the sodium carbonate into sodium hydroxide.
  • the calcium carbonate that forms from this reaction can be returned to the reactors, systems and/or methods disclosed herein to regenerate the slaked lime.
  • slaked lime can also be used as a source of alkali in the sulfite process of pulping, to prepare the liquor.
  • slaked lime is added to a solution of sulfurous acid to form a bisulfite salt. The mixture of sulfurous acid and bisulfite is used, in some cases, to digest the pulp.
  • Slaked lime can also be used to precipitate calcium lignosulfonates from spent sulfite liquor, in certain instances.
  • slaked lime and/or lime produced by the reactors, systems, and/or methods disclosed herein is used as a source of calcium and/or alkalinity for marine aquariums and/or reef growth.
  • thermochemical energy storage e.g. for a self-heating food container and/or for solar heat storage.
  • calcium and/or magnesium hydroxide produced by the reactors, systems, and/or methods disclosed herein is used as a fire retardant, an additive to cable insulation, and/or insulation of plastics.
  • slaked lime and/or lime produced by the reactors, systems, and/or methods disclosed herein is used as an antimicrobial agent.
  • lime and/or slaked lime is used to treat disease contaminated areas, such as walls, floors, bedding, and/or animal houses.
  • This example describes a system run in the first mode where the produced acid and base were collected.
  • a near-neutral solution of 1M Na 2 SO 4 was fed to the anode (made from carbon felt) and the cathode (also carbon felt) of a flow cell at a rate of 10 mL per minute, and solution was taken out from the anode and from the cathode.
  • a voltage of 2.5 V was applied to the cell the pH of the solution coming from the anode was 1.5, and the pH of the solution coming from the cathode was 12.5.
  • This example describes a system run in the first mode where the produced acid and base are collected and reacted.
  • a hydrolysis reaction is run in an electrochemical cell comprising a first electrode and second electrode, such that base and hydrogen gas are produced at the first electrode (cathode) and acid and oxygen gas are produced at the second electrode (anode).
  • the base is collected from the reactor through a conduit to a first apparatus in fluidic connection with the reactor, and the base is stored in the apparatus.
  • the acid is collected from the reactor through a conduit to a second apparatus in fluidic connection with the reactor, and the acid is stored in that apparatus.
  • the base is transferred to a third apparatus in fluidic connection with the first apparatus and the acid is transferred to a fourth apparatus in fluidic connection with the second apparatus.
  • the acid is then used to dissolve CaCO 3 in a chemical dissolution in the fourth apparatus to form Ca 2+ ions and CO 3 2 ⁇ ions.
  • the Ca 2+ ions are then transported to the third apparatus (which is in fluidic connection with the fourth apparatus), where the base is used in a precipitation reaction with the Ca 2+ ions to form Ca(OH) 2 .
  • the Ca(OH) 2 may optionally be used in a cement-making process, for example, with a kiln and/or a heater.
  • This example describes a system run in the first mode where the produced oxygen gas and hydrogen gas are transported and reduced and oxidized, respectively.
  • a hydrolysis reaction is run in an electrochemical cell comprising a first electrode and second electrode, such that base and hydrogen gas are produced at the first electrode (cathode) and acid and oxygen gas are produced at the second electrode (anode).
  • the hydrogen gas is transported from the cathode to the anode through a conduit, where it is oxidized, producing acid.
  • the production of acid decreases the pH at the anode further.
  • the oxygen gas is transported from the anode to the cathode through a conduit, where it is reduced, producing base.
  • the production of base increases the pH at the cathode further.
  • the acid and base are optionally collected and/or reacted as described in Example 1.
  • This example describes a system run in the first mode where the produced oxygen and gas may be collected and sold or used, or recombined to form water.
  • a hydrolysis reaction is run in an electrochemical cell comprising a first electrode and second electrode, such that base and hydrogen gas are produced at the first electrode (cathode) and acid and oxygen gas are produced at the second electrode (anode).
  • the hydrogen gas and oxygen gas may be collected and sold or used, or recombined to form water if production of gas is not desired.
  • This example describes a system run alternatively in the first mode and second mode.
  • Example 1 The system or method of Example 1 is used in times of low electricity cost and/or high electricity availability, but some or all of the acid and base is stored, rather than used in chemical dissolution and/or precipitation reactions.
  • the system is switched to a second mode, where the polarity of the electrodes is reversed from that in Example 1.
  • the stored base from Example 1 is then added to the anode where it is oxidized to form oxygen gas.
  • the stored acid is then added to the cathode where it is reduced to produce hydrogen gas.
  • the hydrogen gas and oxygen gas may optionally be collected and sold or used.
  • This examples describes running a system comprising two reactors to produce acid and base, which can be used in chemical dissolution and/or precipitation reactions.
  • a system comprising two reactors in fluidic connection are run.
  • the first reactor produces base, dihalide (e.g., Cl 2 ), and hydrogen gas.
  • the first reactor and second reactor are in fluidic connection, and hydrogen gas and dihalide produced in the first reactor are transported to the second reactor.
  • Water is also added to the second reactor, and the second reactor produces acid (e.g., HCl).
  • the base is collected from the first reactor with a first apparatus and the acid is collected from the second reactor with a second apparatus.
  • the acid is used in a chemical dissolution in the second apparatus, such as the chemical dissolution of solid CaCO 3 to Ca 2+ and CO 3 2 ⁇ ions.
  • the second apparatus is in fluidic connection with the first apparatus, and the Ca 2+ ions from the second apparatus are transported to the first apparatus, where they react with the base in a precipitation reaction to form Ca(OH) 2 .
  • the Ca(OH) 2 may optionally be used in a cement-making process, for example, with a kiln and/or a heater.
  • a reference to “A and/or B,” when used in conjunction with open-ended language such as “comprising” can refer, in one embodiment, to A without B (optionally including elements other than B); in another embodiment, to B without A (optionally including elements other than A); in yet another embodiment, to both A and B (optionally including other elements); etc.
  • the phrase “at least one,” in reference to a list of one or more elements, should be understood to mean at least one element selected from any one or more of the elements in the list of elements, but not necessarily including at least one of each and every element specifically listed within the list of elements and not excluding any combinations of elements in the list of elements.
  • This definition also allows that elements may optionally be present other than the elements specifically identified within the list of elements to which the phrase “at least one” refers, whether related or unrelated to those elements specifically identified.
  • “at least one of A and B” can refer, in one embodiment, to at least one, optionally including more than one, A, with no B present (and optionally including elements other than B); in another embodiment, to at least one, optionally including more than one, B, with no A present (and optionally including elements other than A); in yet another embodiment, to at least one, optionally including more than one, A, and at least one, optionally including more than one, B (and optionally including other elements); etc.

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CN114751369B (zh) * 2022-05-19 2023-07-04 重庆大学 一种MnCo2O4.5-MgH2复合储氢材料及其制备方法

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