Patent Grant
7875163
A solution of hydroxide ions, carbonate ions and/or bicarbonate ions is often required to remove protons from a solution, or buffer the pH of a solution, or precipitate an insoluble hydroxide and/or carbonate and/or bicarbonate from a solution. Conventionally, hydroxide ions can be produced by hydrolyzing a base, e.g., slaking quicklime; or, by electrolyzing a salt solution, e.g., electrolyzing an aqueous sodium chloride solution as in the Chlor-alkali process. Conventionally, carbonate ions or bicarbonate ions can be produced by dissolving carbon dioxide gas in water or by dissolving a soluble carbonate or bicarbonate salt, e.g., sodium bicarbonate, in water.
Although hydrolyzing a base or electrolyzing a salt solution can produce hydroxide ions, the conventional production of hydroxide ions consumes large amounts of energy; the conventional methods also release large amounts of carbon dioxide into the environment. Thus, for example, in producing quicklime, large amounts of fossil fuels are burned to calcine and convert limestone to calcium oxide, with the consequential release of large amounts of carbon dioxide into environment. Similarly, in producing hydroxide ions by the Chlor-alkali process, since typically at least 3V is required across the anode and cathode to drive the reaction, large amounts of energy are utilized. As this energy is derived typically from fossil fuelled power generating plants, this process also causes release of large amounts of carbon dioxide into the environment. Similarly, in producing carbonate ions and bicarbonate ions by dissolving carbon dioxide in aqueous solutions, a significant amount of energy is required to pressurize the gas for improved solubility, with the consequential release of large amounts of carbon dioxide into the environment attributable to the energy used. Thus, an energy efficient production of hydroxide ions, carbonate ions and bicarbonate ions is highly desirable.
In various embodiments, the present system and method pertain to a low-voltage, low-energy electrochemical system and method of producing hydroxide ions and/or bicarbonate ions and/or carbonate ions. In various embodiments, the system and method utilize significantly less than the typical 3V used across the conventional anode and cathode to produce the ions; consequently, the carbon dioxide emissions attributable to the present system and method are significantly reduced.
In one embodiment, the system comprises: a first electrolyte in contact with a cathode; a second electrolyte in contact with an anode; a third electrolyte separated from the first electrolyte by a first ion-exchange membrane; a fourth electrolyte separated from the second electrolyte by a second ion-exchange membrane; and a third-ion exchange membrane separating the third and fourth electrolytes.
In one embodiment, the method comprises: placing a first electrolyte in contact with a cathode; placing a second electrolyte in contact with an anode; placing a third electrolyte such that it is separated from the first electrolyte by a first ion-exchange membrane; placing a fourth electrolyte such that it is separated from the third electrolyte by an third ion-exchange membrane and is separated from the second electrolyte by a second ion-exchange membrane; and forming hydroxide ions in the first electrolyte by applying a voltage across the anode and cathode.
In another embodiment, the method comprises: placing a first electrolyte in contact with a cathode; placing second electrolyte in contact with an anode; placing a third electrolyte such that it is separated from the first electrolyte by a first ion-exchange membrane; placing a fourth electrolyte such that it is separated from the third electrolyte by an third ion-exchange membrane and is separated from the second electrolyte by a second ion-exchange membrane; and supplying carbon dioxide gas to the first electrolyte.
In various embodiments, the first ion-exchange membrane comprises a cation exchange membrane; the second ion-exchange membrane comprises a cation exchange membrane; and the third ion-exchange membrane comprises an anion exchange membrane. In various embodiments, the first electrolyte is a cathode electrolyte in contact with the cathode, and the second electrolyte is an anode electrolyte in contact with an anode.
In various embodiments, the system and method are adapted to withdraw some or all of the cathode electrolyte via an outflow stream, and/or replenishing this electrolyte via an inflow stream to the cathode electrolyte compartment. In various embodiments, the system and method are adapted to withdraw some or all of the fourth electrolyte from an outflow stream and replenishing this electrolyte via an inflow stream of the fourth electrolyte compartment. In various embodiments, the system and method are adapted for batch, semi-batch or continuous flow operation, with or without withdrawing and replenishing the electrolytes in the system.
In various embodiments, the system includes a hydrogen gas transfer system adapted for directing hydrogen gas generated at the cathode to the anode. In another embodiment, the system includes a carbon dioxide delivery system adapted for delivering carbon dioxide gas into the cathode electrolyte where it dissolves and may form bicarbonate and/or carbonate ions, depending on the pH of the electrolyte. In embodiments in which carbon dioxide is supplied to the cathode electrolyte by dissolving the gas into the cathode electrolyte, the dissolution may in some embodiments occur in one or more compartments located in the outflow stream, or in an inflow stream or in between them. In various embodiments, the system is operably connected to an industrial waste gas stream comprising combustion gases for supplying gases, e.g., carbon dioxide, to the cathode electrolyte. In various embodiments, the waste gas stream includes combustion gases from fossil fuelled electrical power generating plants, cement manufacturing plants and/or other industrial plants. In various embodiments, the waste gas includes acidic gases, e.g., oxides of nitrogen (nitrous oxide, nitric oxide) and sulfur gases (sulfur dioxide, hydrogen sulfide) that dissolve in the cathode electrolyte to form anions. In some embodiments the waste gas is treated to remove some or all of its non-carbon dioxide components before contact with the cathode electrolyte.
In various embodiments, the products of the system and method including the hydroxide ions, bicarbonate ions, carbonate ions, hydrochloric acid and a partially desalinated water from which certain cation and anions have been removed are utilized to sequester carbon dioxide and other constituents of industrial waste gases, e.g., sulfur gases, nitrogen oxide gases and other combustion gases, by contacting the waste gas with a solution comprising divalent cations and the hydroxide, bicarbonate and/or carbonate ions to precipitate divalent cation carbonates and bicarbonates as described in commonly assigned U.S. patent application Ser. No. 12/344,019 filed on Dec. 24, 2008, herein incorporated by reference in its entirety. The precipitates, comprising, e.g., calcium and magnesium carbonates and bicarbonates in various embodiments are utilized as building materials, e.g., as cements and aggregates, as described in commonly assigned U.S. patent application Ser. No. 12/126,776 filed on May 23, 2008, herein incorporated by reference in its entirety.
In another application, the partially desalinated water from which cation and anions have been removed, e.g., a partially desalinated water formed by removing sodium and chloride ions from the third electrolyte, is used as feed water in a desalination system where the water is further processed as described in commonly assigned U.S. patent application Ser. No. 12/163,205 filed on Jun. 27, 2008, herein incorporated by reference in its entirety.
In another embodiment, the acid produced in the fourth electrolyte and/or the base solution produced in the cathode electrolyte are utilized to dissolve minerals and waste materials comprising divalent cations, e.g., Ca++ and Mg++ to produce divalent cation solutions that are utilized in producing divalent metal ion carbonate precipitates using the present cathode electrolyte. In various embodiments, the precipitates are used as building materials e.g. cement and aggregates as described in commonly assigned U.S. patent application Ser. No. 12/126,776, herein incorporated by reference in its entirety.
The following drawings illustrate by way of examples and not by limitation embodiments of the present system and method.
Before the present methods and systems are described in detail, it is should be understood that the present system and method are not limited to particular embodiments described and illustrated herein, as such may vary. It is also to be understood that the terminology used herein is for the purpose of describing particular embodiments only, and is not limiting, since the scope are limited only by the appended claims.
Herein, where a range of values is provided. it is should understood that each intervening value, to the tenth of the unit of the lower limit (unless the context clearly dictates otherwise) between the upper and lower limit of that range and any other stated or intervening value in that stated range, is encompassed within the present system and method. The upper and lower limits of these smaller ranges may independently be included in the smaller ranges and are also encompassed within the system and method, subject to any specifically excluded limit in the stated range. Where the stated range includes one or both of the limits, ranges excluding either or both of those included limits are also included in the system and method.
Herein, ranges are presented with numerical values being preceded by the term “about.” Herein, the term “about” is used to provide literal support for the exact number that it precedes, as well as a number that is near to or approximately the number that the term precedes. In determining whether a number is near to or approximately a specifically recited number, the near or approximating un-recited number may be a number, which, in the context in which it is presented, provides the substantial equivalent of the specifically recited number.
Unless defined otherwise, all technical and scientific terms used herein have the same meaning as commonly understood by one of ordinary skill in the art to which this invention belongs. Although any methods, systems and materials similar or equivalent to those described herein can also be used in practicing the present system an method, only representative methods, systems and materials are herein described.
All publications and patents cited in this specification are herein incorporated by reference as if each individual publication or patent were specifically and individually indicated to be incorporated by reference and are incorporated herein by reference to disclose and describe the methods and/or materials in connection with which the publications are cited. The citation of any publication is for its disclosure prior to the filing date and should not be construed as an admission that the present invention is not entitled to antedate such publication by virtue of prior invention. Further, the dates of publication provided may differ from the actual publication dates that may need to be independently confirmed.
As used herein and in the appended claims, the singular forms “a,” “an,” and “the” include plural references unless the context clearly dictates otherwise. Also, the claims may be drafted to exclude any optional element. As such, this statement is intended to serve as antecedent basis for use of such exclusive terminology as “solely,” “only” and the like in connection with the recitation of claim elements, or use of a “negative” limitation.
As will be apparent to those of skill in the art, each of the embodiments described and illustrated herein comprise discrete components and features which may be readily separated from or combined with the features of any of the other several embodiments without departing from the scope of the present invention. Any recited method can be carried out in the order of events recited or in any possible logical order.
In various embodiments, the present system and method pertain to producing hydroxide and/or bicarbonate and/or carbonate ions in an aqueous solution by a low-voltage, low-energy electrochemical process. In one embodiment, and with reference to
In various embodiments, hydrogen gas obtained at the cathode is directed to the anode where the gas is oxidized. In various embodiments, sodium hydroxide produced in the cathode electrolyte and hydrochloric acid produced in the fourth electrolyte are continually removed from the system, while the cathode electrolyte and sodium chloride in the third electrolyte are continually replenished with water to maintain a continuous production operation of the system. In other embodiments, the system and method are adapted for other modes of operation, e.g., batch or semi-batch flows.
In another embodiment, bicarbonate ions and/or carbonate ions are produced in the cathode electrolyte by dissolving carbon dioxide gas in the cathode electrolyte and applying a voltage of less than 3V across the anode and cathode. The carbon dioxide gas may be dissolved in the cathode electrolyte or may be dissolved in a separate carbon dioxide compartment 152 connected to the cathode electrolyte compartment 122 to provide carbon dioxide, dissolved in a solution, to the cathode electrolyte compartment. In this embodiment, since carbon dioxide is dissolved in the cathode electrolyte, three reactions occur as follows:
2H2O+2e−=H2+2OH−
(water is reduced at the cathode),
H2O+CO2═H2CO3═H++HCO3−═H++CO32−
(carbonate and/or bicarbonate ions are formed in the cathode electrolyte, depending on the pH of the electrolyte), and
H++OH−→H2O
As these reactions are pH dependent, the overall cathode reaction is: either: 2H2O+2CO2+2e−=H2+2HCO3−,
or H2O+CO2+2e−=H2+CO32−
or a combination of both reactions, depending on the pH of the cathode electrolyte.
In this embodiment, and with reference to
In this embodiment of the system, as with the embodiment that produces hydroxide ions described above, hydrogen gas produced at the cathode is optionally directed to the anode where it is oxidized, or the gas is vented. In embodiments where the hydrogen gas is vented, another source of hydrogen gas provides the hydrogen gas to the anode. In various embodiments of this system, as with the production of hydroxide ions, the carbonate ions and/or bicarbonate ions produced in the cathode electrolyte are continually removed from the system while the cathode electrolyte and sodium chloride in the third electrolyte are continually replenished with water to maintain continuous operation of the system. In various embodiments, the system and method are adaptable for other modes of operation, e.g., batch or semi-batch flows.
In various embodiments, as will be appreciated by one ordinarily skilled in the art, the voltage across the anode and cathode is dependent on the pH of the anode electrolyte and cathode electrolyte, as well as the pH difference between these electrolytes. Thus, in various embodiments, hydroxide ions, carbonate ions and/or bicarbonate ions are produced in the cathode electrolyte when the voltage applied across the anode and cathode is less than 3, 2.9 2.8, 2.7, 2.6 2.5, 2.4, 2.3, 2.2, 2.1, 2.0, 1.9, 1.8, 1.7, 1.6, 1.5, 1.4, 1.3, 1.2, 1.1, 1.0, 0.9, 0.8, 0.7, 0.6, 0.5, 0.4, 0.3, 0.2, or 0.1 V or less, while the pH of difference between the anode electrolyte and the cathode electrolyte, is 0, 1, 2, 3, 4, 5, 6, 7, 8, 9, 10, 11, 12, 13, 14 pH units or greater; and while the pH of the anode electrolyte varies from 1 to 7 pH units and the pH of the cathode electrolytes varies from 7 to 14 pH units or greater.
In various embodiments, and with reference to
Similarly, and with reference to
In various embodiments, and with reference to
Thus, in embodiments where the third electrolyte 110 is initially charged with sodium chloride, sodium ions will migrate from the third electrolyte to the cathode electrolyte 102 to form sodium hydroxide or sodium bicarbonate or sodium carbonate, depending on the pH of the cathode electrolyte 102. Similarly, chloride ions will migrate from the third electrolyte 110 to the fourth electrolyte to form hydrochloric acid 148 with protons that migrate from the anode electrolyte 106. Consequently, in various embodiments, a partially desalinated water 150 from which sodium ions and chloride are removed is produced in the third electrolyte 110.
In various embodiments where hydrogen gas is not provided for oxidation at the anode, the system and method is adaptable to produce a gas at the anode, e.g., oxygen or chlorine, while producing hydroxide, bicarbonate and carbonate ions in the cathode electrolyte and hydrogen gas at the cathode. As with other embodiments, in this embodiment the system and method are adaptable to form an acid in the fourth electrolyte and a partially desalinated water in the third electrolyte, while forming a gas, e.g., oxygen or chlorine, at the anode. In this embodiment, however, since hydrogen gas is not oxidized at the anode, a higher voltage is generally required across the cathode and anode to drive the electrochemical reaction in the system.
In various embodiments, and with reference to
In the following exemplary description of a specific embodiment of the system and method, for illustrative purposes, a system is configured as in
Thus in this system, on applying a voltage across the anode 108 and cathode 104, sodium ions will migrate from the third electrolyte 110 to the cathode electrolyte 102, and chloride ions will migrate from the third electrolyte to the fourth electrolyte 116; hydroxide ions, or carbonate ions or bicarbonate ions will be produced in the cathode electrolyte 102 (depending on whether carbon dioxide gas is added to the electrolyte); hydrogen gas will be produced at the cathode 104; hydrogen gas supplied to the anode 108 will be oxidized to protons at the anode; and the protons will migrate into the anode electrolyte 106 from where they will migrate across the second cation exchange membrane 118 to the fourth electrolyte 116 where they accumulate, as the anion exchange membrane 120 will block their further migration to the third electrolyte 110.
Consequently, in various embodiments, on applying a voltage across the anode and cathode in this system, sodium hydroxide will be produced in the cathode electrolyte; hydrochloric acid will be produced in the fourth electrolyte; the concentration of sodium chloride in the third electrolyte will decrease; hydrogen gas will be oxidized at the anode; and hydrogen gas will be generated at the cathode.
In an embodiment of this system where carbon dioxide gas is dissolved in the cathode electrolyte, the system and method additionally will produce bicarbonate and/or carbonate ions in the cathode electrolyte; hence, in this embodiment, sodium bicarbonate and/or sodium carbonate will be produced in the cathode electrolyte, depending on the pH of the cathode electrolyte. In this embodiment, as with the embodiment wherein carbon dioxide is not dissolved in the cathode electrolyte, the system and method will produce hydrochloric acid in the fourth electrolyte; the concentration of sodium chloride in the third electrolyte will decrease; hydrogen gas will be oxidized at the anode; and hydrogen gas will be generated at the anode.
As will be appreciated by one ordinarily skilled in the art, the present system and method are not limited to this exemplary use of sodium chloride solution as the third electrolyte, but are adaptable for using an equivalent ionic salt solution in the third electrolyte, e.g., a potassium sulfate. Thus, for example, if potassium sulfate were used, sulfuric acid will be produced in the fourth electrolyte and potassium hydroxide, bicarbonate and/or carbonate will be produced in the cathode electrolyte. As can be appreciated, the system and method with potassium sulfate as the third electrolyte will produce protons at the anode by oxidizing hydrogen gas supplied to the anode; hydrogen gas will form at the cathode; and the third electrolyte will be depleted of potassium and sulfate ions. In embodiments where carbon dioxide gas is dissolved in the cathode electrolyte, the system and method with potassium sulfate as the third electrolyte will produce bicarbonate and carbonate ions in the cathode electrolyte. Hence, in this equivalent system, potassium hydroxide, potassium bicarbonate and/or potassium carbonate will be produced in the cathode electrolyte, depending on the pH of the cathode electrolyte. Other electrolytes that can be used to produce the electrolytes in the present system include seawater, brackish water and brines. Such equivalent systems and methods are therefore within the scope of the present system and method.
Also as will be appreciated by one skilled in the art, in the embodiment where carbon dioxide is dissolved in the cathode electrolyte to produce bicarbonate and carbonate anions, other equivalent gases that react dissolve and ionize in water will produce equivalent results. Thus, for example, acidic gases such as sulfur dioxide and oxides of nitrogen that are soluble in the cathode electrolyte will produce equivalent anions in the cathode electrolyte. Therefore, to the extent that an equivalent gas is dissolved in the third electrolyte to produce equivalent anions as with carbon dioxide, such systems and methods are also within by the scope of the present system and method.
In various embodiments, the system and method are adapted to withdraw some or the entire cathode electrolyte from an outflow to an inflow stream of the cathode compartment. Also, the system and method are adapted to withdraw some or the entire fourth electrolyte from an outflow stream to an inflow stream of the fourth electrolyte. In various embodiments, the system and method are adapted for batch, semi-batch or continuous flow operation, with or without directing hydrogen gas generated at the cathode for oxidation at the anode, and with or without withdrawing and replenishing the electrolytes in the system.
In various embodiments, the system includes a hydrogen gas transfer system for circulating hydrogen gas from the cathode to the anode. In another embodiment, the system includes a carbon dioxide delivery system for dissolving carbon dioxide gas in the cathode electrolyte. In various embodiments, the system is operably connected to an industrial waste gas stream comprising combustion gases for supplying gases, e.g., carbon dioxide, to the cathode electrolyte. In various embodiments, the waste gas stream includes combustion gases from fossil fuelled electrical power generating plants, cement manufacturing plants and other industrial plants. In various embodiments, the waste gas includes acidic gases, e.g., oxides of nitrogen (nitrous oxide, nitric oxide) and sulfur gases (sulfur dioxide, hydrogen sulfide) that dissolve in the cathode electrolyte to form anions analogous to the production of bicarbonate and carbonate ions when carbon dioxide is dissolved in the cathode electrolyte.
Referring to
In the system illustrated in
Also with reference to
In various embodiments, the system includes a cathode electrolyte withdrawal and replenishing system 138 adapted for withdrawing all of, or a portion of, the cathode electrolyte 102 from the first cell 122 containing the cathode electrolyte. In various embodiments the system includes a fourth electrolyte withdrawal and replenishing system 140 for withdrawing and replenishing all of, or a portion of, the fourth electrolyte 116 to the fourth cell 132 containing the fourth electrolyte. In various embodiments, the system includes a salt supply system for providing a salt solution 142, e.g., concentrated sodium chloride, to the third electrolyte cell 130. In various embodiments the system includes a gas supply system 144 for providing a gas, e.g., carbon dioxide, to the cathode electrolyte 102. In various embodiments the system includes a carbon dioxide mixing system 152 in which carbon dioxide is supplied to the cathode electrolyte by dissolving the gas into the cathode in one or more compartments located in the outflow stream, or in an inflow stream or in between them. In various embodiments, the system includes inlet ports (not shown) for introducing fluids into the cells (122, 126, 130, 132) and outlet ports (not shown) for removing fluids from the cells.
In various operating modes, e.g., continuous flow, batch flow or mixed modes, the system when charged with sodium chloride solution 142 will produce a solution of sodium hydroxide 146 in the cathode electrolyte 102, hydrochloric acid 148 in the fourth electrolyte 116, and an a partially desalinated aqueous solution 150 in which the cation and anion content is reduced. In various embodiments, the aqueous partially desalinated solution 150 is utilized feed water to a desalinated water treatment plant (not shown) for further processing to remove e.g., other ions present in the solution. In other embodiments, the aqueous solution 150 is used to prepare the initial electrolyte solutions for charging the first cell 122, second cell 126, third cell 130 and fourth cell 132 with an electrolyte.
As can be appreciated, in various embodiments and with reference to
Thus, for example, with reference to
H2=2H++2e− (anode, oxidation reaction)
2H2O+2e−=H2+20H− (cathode, reduction reaction)
As will be appreciated by one ordinarily skilled in the art and with reference to
Further, as can be appreciated by one skilled in the art, in the present system since a gas does not form at the anode, the system will produce hydroxide ions in the cathode electrolyte and hydrogen gas at the anode when less than 3V is applied across the anode and cathode, in contrast to the higher voltage that is required in conventional systems that does generate gas, e.g., chlorine at the anode. For example, in various embodiments, hydroxide ions are produced when less than 2.0, 1.5, 1.4, 1.3, 1.2, 1.1, 1.0, 0.9, 0.8, 0.7, 0.6, 0.5, 0.4, 0.3, 0.2, 0.1 V or less is applied across the anode and cathode.
Further, as will be appreciated by those ordinarily skilled in the art and with reference to
However, as is illustrated in
Similarly with reference to protons generated at the anode 108, under the applied voltage 134 across the cathode 104 and anode 108, the protons will enter the anode electrolyte 106 and migrate to the fourth electrolyte through the second cation exchange membrane 118. However, since the anion exchange membrane 120 between the fourth electrolyte 116 and the third electrolyte 110 will block the movement of cations from the fourth electrolyte 116 to the third electrolyte 116, consequently, protons in the fourth electrolyte 116 will be prevented from migrating from the fourth electrolyte to the third electrolyte 110. Consequently, on applying the voltage 134 across the anode and cathode, the protons produced at the anode will be contained in the fourth electrolyte 116. Thus, depending on the flow rate of fluids into and out of the fourth electrolyte the pH of the fourth electrolyte will adjust, e.g., the pH may increase, decrease or remain the same.
With reference to the third electrolyte 110 that is initially charged with a concentrated solution of sodium and chloride ions and contained in the third cell 130 by the anion exchange membrane 120 and the first cation exchange membrane 112, on applying a voltage across the anode 108 and cathode 104, anions in the third electrolyte 110, e.g., chloride ions, will attempt to migrate to the anode 108, while cations, e.g., sodium ions in the third electrolyte, will attempt to migrate to the cathode 104. Since the anion exchange membrane 120 will allow the migration of anions from the third electrolyte 110 to the fourth electrolyte 116, chloride ions present in the third electrolyte 110 will migrate to the fourth electrolyte where they will form an acid, e.g., hydrochloric acid, with the protons from the anode.
Further, since the first cation exchange membrane 112 will allow the migration of cations from the third electrolyte 110 to the cathode electrolyte 102, sodium ions present in the third electrolyte 110 will migrate to the cathode electrolyte 102 where they will form sodium hydroxide with the hydroxide ions generated at the cathode 104. Consequently, as is illustrated in
In various embodiments and as is illustrated in
In other embodiments, depending on the ionic species desired, alternative reactants can be dissolved in the cathode electrolyte to produce the desired ions. Thus, for example, in various embodiments, carbon dioxide is added to the cathode electrolyte to produce carbonate and bicarbonate ions. The carbon dioxide gas can be added to the electrolyte by bubbling it directly into the electrolyte; alternatively, the carbon dioxide gas may be dissolved in the cathode electrolyte or may be dissolved in a separate compartment 152 connected to the cathode compartment by a conduit to feed the solution with carbon dioxide dissolved into the cathode compartment as noted above.
In embodiments where carbon dioxide is dissolved in the cathode electrolyte, as discussed above and with reference to
At the cathode 104, water is reduced to hydroxide ions and hydrogen gas as follows:
2H2O+2e−=H2+2OH− (water is reduced at the cathode).
In the cathode electrolyte 102, the carbon dioxide gas will dissolve to form carbonic acid, protons, bicarbonate ions, and carbonate ions, depending on the pH of the electrolyte, as follows:
H2O+CO2═H2CO3═H++HCO3−=2H++CO32−
As the dissolution of carbon dioxide and the concentration of bicarbonate and carbonate ions in the cathode electrolyte 102 are pH dependant, the overall reaction in the first (cathode) cell 122 is either:
2H2O+2CO2+2e−=H2+2HCO3−; or Scenario 1
H2O+CO2+2e−=H2+CO32− Scenario 2
or a combination of both, depending on the pH of the cathode electrolyte 102, as is illustrated in
For either scenario the overall cell potential can be determined through the Gibbs energy change of the reaction by the formula:
Ecell=−ΔG/nF
Or, at standard temperature and pressure conditions:
Eocell=−ΔGo/nF
where, Ecell is the cell voltage, ΔG is the Gibbs energy of reaction, n is the number of electrons transferred, and F is the Faraday constant (96485 J/Vmol). The Ecell of each of these reactions is pH dependent based on the Nernst equation as demonstrated for Scenario 1 in
For either scenario the overall cell potential can be determined through the combination of Nernst equations for each half cell reaction:
E=Eo−RTIn(Q)/nF
where, Eo is the standard reduction potential, R is the universal gas constant, (8.314 J/mol K) T is the absolute temperature, n is the number of electrons involved in the half cell reaction, F is Faraday's constant (96485 J/V mol), and Q is the reaction quotient so that:
Etotal=Ecathode+Eanode.
When hydrogen is oxidized to protons at the anode as follows:
H2=2H++2e−,
Eo is 0.00 V, n is 2, and Q is the square of the activity of H+ so that:
Eanode=−0.059 pHa,
where pHa is the pH of the anode electrolyte.
When water is reduced to hydroxide ions and hydrogen gas at the cathode as follows:
2H2O+2e−=H2+2OH−,
Eo is −0.83 V, n is 2, and Q is the square of the activity of OH− so that:
Ecathode=−0.059 pHc,
where pHc is the pH of the cathode electrolyte.
For either Scenario, the E for the cathode and anode reactions varies with the pH of the anode and cathode electrolytes. Thus, for Scenario 1 if the anode reaction, which is occurring in an acidic environment, is at a pH of 0, then the E of the reaction is 0 V for the half cell reaction. For the cathode reaction, if the generation of bicarbonate ions occur at a pH of 7, then the theoretical E is 7×(0.059 V)=0.413 V for the half cell reaction where a negative E means energy is needed to be input into the half cell or full cell for the reaction to proceed. Thus, if the anode pH is 0 and the cathode pH is 7 then the overall cell potential would be 0.413 V, where:
Etotal=0.059(pHa−pHc)=0.059 ΔpH.
For Scenario 2 in which carbonate ions are produced, if the anode pH is 0 and the cathode pH is 10, this would represent an E of 0.59 V.
Thus, in various embodiments, an effect of directing CO2 into the cathode electrolyte (to lower the pH of the cathode electrolyte and to produce bicarbonate ions and/or carbonate ions in the cathode electrolyte) is a lowering of the required voltage across the anode and cathode of the system to produce the hydroxide, carbonate and bicarbonate in the cathode electrolyte. In Scenario 1, it can be appreciated that if the cathode electrolyte was allowed to increase to a pH of 14 or greater, the difference between the anode half-cell potential (represented as the thin dashed horizontal line) and the cathode half cell potential (represented as the thick solid sloping line) would increase to 0.83V. With increased duration of cell operation without CO2 addition or other intervention, e.g., diluting with water, the required cell potential would continue to increase. It can thus be appreciated that operation of the electrochemical cell with the cathode pH at 7 or greater provides a significant energy savings.
Thus, as can be appreciated by one ordinarily skilled in the art, for different pH values in the cathode electrolyte and the anode electrolyte, hydroxide ions, carbonate ions and/or bicarbonate ions are produced in the cathode electrolyte when the voltage applied across the anode and cathode is less than 3, 2.9 2.8, 2.7, 2.6 2.5, 2.4, 2.3, 2.2, 2.1, 2.0, 1.9, 1.8, 1.7, 1.6, 1.5, 1.4, 1.3, 1.2, 1.1, 1.0, 0.9, 0.8, 0.7, 0.6, 0.5, 0.4, 0.3, 0.2, or 0.1 V or less, while the pH difference between the anode electrolyte and the cathode electrolyte is greater 0, 1, 2, 3, 4, 5, 6, 7, 8, 9, 10, 11, 12, 13, 14 or greater.
Also as will be appreciated by one skilled in the art, in embodiments wherein it is desired to produce bicarbonate and/or carbonate ions, the system as illustrated in
Thus, in producing carbonate/bicarbonate ions in the cathode electrolyte 102, as with the embodiment that produces hydroxide ions in the cathode electrolyte without the addition of carbon dioxide to the cathode electrolyte as described above, the anode 108, the first cation exchange membrane 118, the anion exchange membrane 120, the first cation exchange membrane 112, the anode electrolyte, the fourth electrolyte and the third electrolyte are functionally identical.
As with the production of hydroxide ions, in the production of carbonates and or bicarbonates, hydrogen gas 136 produced at the cathode 104 is optionally directed for oxidization of the hydrogen gas at the anode 108; a desalinated water 150 depleted of sodium chloride is obtained from the third electrolyte 110, and hydrochloric acid 148 is produced in the fourth electrolyte. Also, in various embodiments as with the production of hydroxide ions, the carbonate ions or bicarbonate ions produced in the cathode electrolyte can be continually removed from the system while water in the cathode electrolyte and sodium chloride in the third electrolyte are continually replenished to maintain a continuous operation of the system. In various embodiments, the system and method are adaptable for other modes of operation, e.g., batch or semi-batch flows.
As can be appreciated by one skilled in the art, in various embodiments, the system can be configured to operate in various production modes including batch mode, semi-batch mode, continuous flow mode, with or without the option to withdraw portions of the sodium hydroxide produced in the cathode electrolyte, or withdraw all or a portions of the acid produced in the fourth electrolyte, or direct the hydrogen gas produced at the cathode to the anode where it may be oxidized.
In various embodiments, the hydroxide ions, bicarbonate ions and/or carbonate ion solutions are produced in the cathode electrolyte when the voltage applied across the anode and cathode is less than 3, 2.9 or less, 2.8 or less, 2.7 or less, 2.6 or less, 2.5 or less, 2.4 or less, 2.3 or less, 2.2 or less, 2.1 or less, 2.0 or less, 1.9 or less, 1.8 or less, 1.7 or less, 1.6, or less 1.5 or less, 1.4 or less, 1.3 or less, 1.2 or less, 1.1 or less, 1.0 or less, 0.9 or less or less, 0.8 or less, 0.7 or less, 0.6 or less, 0.5 or less, 0.4 or less, 0.3 or less, 0.2 or less, or 0.1 V or less.
In another embodiment, the system and method is adaptable to allow for formation of a gas at the anode, e.g., oxygen or chlorine, while hydroxide ions, carbonate ions and bicarbonate ions are produced in the cathode electrolyte and hydrogen gas is generated at the cathode. However, in this embodiment, hydrogen gas is not supplied to the anode. While with this embodiment protons will be produced at the anode, and sodium hydroxide, sodium carbonate, and/or sodium bicarbonate will be produced in the cathode electrolyte, in general the voltage across the anode and cathode will be higher compared to the embodiment when a gas does not form at the anode but, instead, hydrogen gas is oxidized at the anode.
In various embodiments, and with reference to
Examples of suitable cation exchange membranes include, e.g., a Teflon™-based membranes available from Asahi Kasei of Tokyo, Japan. In general, exemplary cation exchange membrane should be capable of use in strong basic solutions in a temperature range from about 0° C. to about 120° C. and higher. However, with reference to
Similarly, typical hydrocarbon based anion exchange membranes are also available from Membrane International of Glen Rock, N.J., USA. In general, such anion exchange membranes should exhibit high ion selectivity, low ionic resistance, high burst strength, and high stability in an acidic electrolytic solution temperature range from about 0° C. to about 100° C. or higher.
As will be appreciated by one skilled in the art, since a cation exchange membrane is selective to migrating cations between two adjacent electrolytes, when a cation exchange membrane is positioned between two electrolytes in an electrochemical system as is illustrated in
Also as will be appreciated by those skilled in the art, since an anion exchange membrane is selective to migrating anions between two adjacent electrolytes, when an anion exchange membrane is positioned between two electrolytes in an electrochemical system as is illustrated in
Thus, for example, and with reference to
With reference to
In various embodiments, method 200 further comprises, a step of e.g., directing carbon dioxide 144 gas into the cathode electrolyte 102; a step of e.g., directing carbon dioxide gas 144 into the cathode electrolyte before or after the cathode electrolyte is placed in contact with the cathode 104; a step of e.g., applying a voltage 134 of less than 3 V, or less than 2V, or less than 1.5V, or less than 1V, or less than 0.5V across the cathode 104 and anode 108; a step of e.g., forming hydrogen gas 136 at the cathode; a step of e.g., forming oxidizing hydrogen to form protons at the anode 108; e.g., a step of forming a pH differential of 1, 2, 3, 4, 5, 6, 7, 8, 9, 10, 11, 12, 13, 14 pH units or greater between the anode and cathode electrolytes without forming a gas at the anode by applying a voltage of less than 3 V, or less than 2V, or less than 1.5V, or less than 1V, or less than 0.5V across the anode and the cathode; a step of forming pH differential of between 1, 2, 3, 4, 5, 6, 7, 8, 9, 10, 11, 12, 13, 14 pH units or greater between the fourth electrolyte 116 and the cathode electrolyte 102 by applying a voltage of 3V or less, or less than 2V, or less than 1.5V, or less than 1.0V, or less than 0.5V across the anode and the cathode; a step of e.g., forming hydroxide ions, bicarbonate ions, carbonate ions and/or a combination thereof in the cathode electrolyte 102; a step of e.g., forming sodium hydroxide, sodium bicarbonate or sodium carbonate in the cathode electrolyte 102; a step of e.g., migrating protons from the anode electrolyte 106 across the second cation exchange membrane 118 to the fourth electrolyte 116; a step of e.g., a step of migrating anions from the third electrolyte 110 across the anion exchange membrane 120 to the fourth electrolyte 116; a step of e.g., migrating chloride ions from the third electrolyte 110 across the anion exchange membrane 120 to the fourth electrolyte 116; a step of e.g., forming an acid 148 in the fourth electrolyte; a step of e.g., forming hydrochloric acid 148 in the fourth electrolyte; a step of e.g., migrating cations from the third electrolyte 110 across the first cation exchange membrane 112 to the cathode 104; a step of e.g., migrating sodium ions from the third electrolyte 110 across the first cation exchange membrane 112 to the cathode electrolyte 102; a step of e.g., directing hydrogen gas formed at the cathode 104 for oxidation of the gas at the anode 108; a step of e.g., removing cathode electrolyte 102 via an outflow and replenishing cathode electrolyte via an inflow stream to the cathode electrolyte; a step of e.g., removing fourth cathode electrolyte 116 via an outflow stream and replenishing the fourth electrolyte via an inflow stream of the fourth electrolyte.
With reference to
In various embodiments, method 300 as with method 200 does not form a gas at the anode 108 when the voltage applied across the anode and cathode is less than 3, 2.9, 2.8, 2.7, 2.6, 2.5, 2.4, 2.3, 2.2, 2.1, 2.0, 1.9, 1.8, 1.7, 1.6, 1.5, 1.4, 1.3, 1.2, 1.1, 1.0, 0.9, 0.8, 0.7, 0.6, 0.5, 0.4, 0.3, 0.2, or 0.1 V or less, while hydrogen gas is provided to the anode where it is oxidized to protons. As will be appreciated by one ordinarily skilled in the art, by not forming a gas at the anode and by providing hydrogen gas to the anode for oxidation at the anode, hydroxide ions are produced in the cathode electrolyte with the present voltages. In various embodiments, method 300 in conjunction with the system of
In various embodiments, bicarbonate ions and carbonate ions are produced where the voltage applied across the anode and cathode is less than 3.0, 2.9, 2.8, 2.7, 2.6, 2.5, 2.4, 2.3, 2.2, 2.1, 2.0, 1.9, 1.8, 1.7, 1.6, 1.5, 1.4, 1.3, 1.2, 1.1, 1.0, 0.9, 0.8, 0.7, 0.6, 0.5, 0.4, 0.3, 0.2, 0.1V or less without the formation of gas at the anode. In various embodiments, the method is adapted to withdraw and replenish at least a portion of the cathode electrolyte and the acid in the fourth electrolyte back into the system in either a batch, semi-batch or continuous mode of operation.
With reference to
Exemplary results achieved with the present system are summarized in Table 1, below. Using 270 cm2 20-mesh Ni gauze for cathode and a 50 cm2 100-mesh Pt gauze as anode, several 24-hr runs were done where hydrogen gas flow to the anode was controlled at a rate of 20 mL/min at room temperature while various voltages were applied across the anode and cathode. A Solartron™ potentiostat was used for electrochemical measurements, and a PC Acid and a PC SK ion exchange membrane from GMbH™ Membranes of Germany were chosen as the anion exchange membrane and cation exchange membrane, respectively.
For example, in particular embodiments the method and system are capable of producing a pH difference of more than 0.5 pH units between the anode electrolyte solution and a cathode electrolyte solution, and the two electrolyte solutions are separated, e.g., by one or more ion exchange membranes, when a voltage of 3V or less, 2.9 V or less or 2.5 V or less, or 2 V or less is applied across the anode and cathode. In some embodiments the method and system are capable of producing a pH difference of more than 1.0 pH units, or 2 pH units, or 4 pH units, or 6 pH units, or 8 pH units, or 10 pH units, or 12 pH units, or 14 pH units between a first electrolyte solution and a second electrolyte solution where the first electrolyte solution contacts an anode and the second electrolyte solution contacts a cathode, and the two electrolyte solutions are separated, e.g., by one or more ion exchange membranes, when a voltage of 0.1V or less is applied across the anode and cathode. In some embodiments the invention provides a system that is capable of producing a pH difference of more than 2.0 pH units between a first electrolyte solution and a second electrolyte solution where the first electrolyte solution contacts an anode and the second electrolyte solution contacts a cathode, and the two electrolyte solutions are separated, e.g., by one or more ion exchange membranes, when a voltage of 0.2V or less is applied across the anode and cathode.
In other embodiments, the method and system are capable of producing a pH difference of more than 4.0 pH units between a first electrolyte solution and a second electrolyte solution where the first electrolyte solution contacts an anode and the second electrolyte solution contacts a cathode, and the two electrolyte solutions are separated, e.g., by one or more ion exchange membranes, when a voltage of 0.4V or less is applied across the anode and cathode. In some embodiments the invention provides a system that is capable of producing a pH difference of more than 6 pH units between a first electrolyte solution and a second electrolyte solution where the first electrolyte solution contacts an anode and the second electrolyte solution contacts a cathode, and the two electrolyte solutions are separated, e.g., by one or more ion exchange membranes, when a voltage of 0.6V or less is applied across the anode and cathode. In some embodiments the invention provides a system that is capable of producing a pH difference of more than 8 pH units between a first electrolyte solution and a second electrolyte solution where the first electrolyte solution contacts an anode and the second electrolyte solution contacts a cathode, and the two electrolyte solutions are separated, e.g., by one or more exchange membranes, when a voltage of 0.8V or less is applied across the anode and cathode. in particular embodiments the invention provides a system that is capable of producing a pH difference of more than 8 pH units between a first electrolyte solution and a second electrolyte solution where the first electrolyte solution contacts an anode and the second electrolyte solution contacts a cathode, and the two electrolyte solutions are separated, e.g., by one or more ion exchange membranes, when a voltage of 1.0 V or less is applied across the anode and cathode. In some embodiments the invention provides a system that is capable of producing a pH difference of more than 10 pH units between a first electrolyte solution and a second electrolyte solution where the first electrolyte solution contacts an anode and the second electrolyte solution contacts a cathode, and the two electrolyte solutions are separated, e.g., by one or more ion exchange membranes, when a voltage of 1.2V or less is applied across the anode and cathode.
As will be appreciated by one skilled in the art, the voltage need not be kept constant and the voltage applied across the anode and the cathode may be very low, e.g., 0.05V or less, when the two electrolytes are the same pH or close in pH, and that the voltage may be increased as needed as the pH difference increases. In this way, the desired pH difference or production of hydroxide ions, carbonate ions and bicarbonate ions may be achieved with the minimum average voltage. Thus in some embodiments described in the previous paragraph, the average voltage may be less than 80%, 70%, 60%, or less than 50% of the voltages given in previous paragraph for particular embodiments.
In various embodiments and with reference to
In some embodiments, divalent cations are removed from the electrolyte solutions, e.g., in magnesium or calcium, during parts of the process where the electrolytes are in contact with the ion exchange membranes. This is done to prevent scaling of the membranes, if necessary for that particular membrane. Thus, in various embodiments the total concentration of divalent cations in the electrolyte solutions when they are in contact with the ion exchange membrane or membranes for any appreciable time is less than 0.06 mol/kg solution, or less than 0.06 mol/kg solution, or less than 0.04 mol/kg solution, or less than 0.02 mol/kg solution, or less than 0.01 mol/kg solution, or less than 0.005 mol/kg solution, or less than 0.001 mol/kg solution, or less than 0.0005 mol/kg solution, or less than 0.0001 mol/kg solution, or less than 0.00005 mol/kg solution.
In embodiments where carbon dioxide gas is dissolved in the cathode electrolyte, as protons are removed from the cathode electrolyte more carbon dioxide may be dissolved to form bicarbonate and/or carbonate ions. Depending on the pH of the cathode electrolyte the balance is shifted toward bicarbonate or toward carbonate, as is well understood in the art and as is illustrated in the carbonate speciation diagram, above. In these embodiments the pH of the cathode electrolyte solution may decrease, remain the same, or increase, depending on the rate of removal of protons compared to rate of introduction of carbon dioxide. It will be appreciated that no hydroxide, carbonate or bicarbonate ion are formed in these embodiments, or that hydroxide, carbonate, bicarbonate may not form during one period but form during another period.
In another embodiment, the present system and method are integrated with a carbonate and/or bicarbonate precipitation system (not illustrated) wherein a solution of divalent cations, when added to the present cathode electrolyte, causes formation of precipitates of divalent carbonate and/or bicarbonate compounds e.g., calcium carbonate or magnesium carbonate and/or their bicarbonates. In various embodiments, the precipitated divalent carbonate and/or bicarbonate compounds are utilized as building materials, e.g., cements and aggregates as described for example in commonly assigned U.S. patent application Ser. No. 12/126,776 filed on May 23, 2008, herein incorporated by reference in its entirety.
In an alternative embodiment, the present system and method are integrated with a mineral and/or material dissolution and recovery system (not illustrated) wherein the acidic fourth electrolyte solution 116 or the basic cathode electrolyte 102 is utilized to dissolve calcium and/or magnesium-rich minerals e.g., serpentine or olivine, or waste materials e.g., fly ash, red mud and the like, to form divalent cation solutions that are utilized to precipitate carbonates and/or bicarbonates as described herein. In various embodiments, the precipitated divalent carbonate and/or bicarbonate compounds are utilized as building materials, e.g., cements and aggregates as described for example in commonly assigned U.S. patent application Ser. No. 12/126,776 filed on May 23, 2008, herein incorporated by reference in its entirety.
In an alternative embodiment, the present system and method are integrated with an industrial waste gas treatment system (not illustrated) for sequestering carbon dioxide and other constituents of industrial waste gases, e.g., sulfur gases, nitrogen oxide gases, metal and particulates, wherein by contacting the flue gas with a solution comprising divalent cations and the present cathode electrolyte comprising hydroxide, bicarbonate and/or carbonate ions, divalent cation carbonates and/or bicarbonates are precipitated as described in commonly assigned U.S. patent application Ser. No. 12/344,019 filed on Dec. 24, 2008, herein incorporated by reference in its entirety. The precipitates, comprising, e.g., calcium and/or magnesium carbonates and bicarbonates in various embodiments are utilized as building materials, e.g., as cements and aggregates, as described in commonly assigned U.S. patent application Ser. No. 12/126,776 filed on May 23, 2008, herein incorporated by reference in its entirety.
In another embodiment, the present system and method are integrated with an aqueous desalination system (not illustrated) wherein the partially desalinated water 150 of the third electrolyte of the present system is used as feed-water for the desalination system, as described in commonly assigned U.S. patent application Ser. No. 12/163,205 filed on Jun. 27, 2008, herein incorporated by reference in its entirety.
In an alternative embodiment, the present system and method are integrated with a carbonate and/or bicarbonate solution disposal system (not illustrated) wherein, rather than producing precipitates by contacting a solution of divalent cations with the first electrolyte solution to form precipitates, the system produces a slurry or suspension comprising carbonates and/or bicarbonates. In various embodiments, the slurry/suspension is disposed of in a location where it is held stable for an extended periods of time, e.g., the slurry/suspension is disposed in an ocean at a depth where the temperature and pressure are sufficient to keep the slurry stable indefinitely, as described in U.S. patent application Ser. No. 12/344,019 filed on Dec. 24, 2008, herein incorporated by reference in its entirety.
While several embodiments of the system and method have been shown and described herein, it will be obvious to those skilled in the art that such embodiments are provided by way of example and not by limitation. Thus, variations, changes, and substitutions will occur to those skilled in the art that are within the scope of the appended claims.
Under 35 U.S.C. §119 (e), this application claims priority to commonly assigned U.S. Provisional Patent Application No. 61/081,299 filed Jul. 16, 2008, title: “Low Energy pH Modulation for Carbon Sequestration Using Hydrogen Absorptive Metal Catalysts”; and commonly assigned U.S. Provisional Patent Application No. 61/091,729 filed Aug. 25, 2008, title: “Low Energy Absorption of Hydrogen Ion from an Electrolyte Solution into a Solid Material”, both of which are herein incorporated by reference in their entirety. Under 35 U.S.C §119 (a) and under 35 U.S.C §365, this application is a continuation-in-part of and claims priority to commonly assigned PCT Patent Application no. PCT/US08/88242, titled “Low-energy Electrochemical Hydroxide System and Method” filed on Dec. 23, 2008, and is a continuation-in-part of and claims priority to commonly assigned PCT Patent Application no PCT/US09/32301 titled “Low-energy Electrochemical Bicarbonate Ion Solution” filed on Jan. 28, 2009, both of which are herein incorporated by reference in their entirety.
| Filing Document | Filing Date | Country | Kind | 371c Date |
|---|---|---|---|---|
| PCT/US2009/048511 | 6/24/2009 | WO | 00 | 3/5/2010 |
| Publishing Document | Publishing Date | Country | Kind |
|---|---|---|---|
| WO2010/008896 | 1/21/2010 | WO | A |
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