INTEGRATION OF DIRECT AIR CAPTURE SYSTEM INTO CO2 MINERALIZATON PROCESS OF CONCRETES AND AGGREGATES

Abstract

A method of forming a concrete product includes directly capturing CO2 from a gas source, the capturing comprising contacting the gas source with an absorption solution having a solvent and a solute, wherein the solvent and/or the solute are capable of reacting with CO2 to form an anionic compound, adjusting the pH of the absorption solution electrochemically to less than about 7 to release the CO2 as a concentrated vapor containing CO2, collecting the concentrated vapor containing CO2, regenerating the solvent and/or the solute, and optionally collecting the regenerated solvent and/or solute; flowing the concentrated vapor containing CO2 through a gas processing unit to adjust at least one of a temperature, a relative humidity, or a flow rate of the concentrated vapor containing CO2; and contacting the concentrated vapor containing CO2 with a concrete component.

Description

BACKGROUND

Traditional concrete is a mixture of calcium silicate-dominant ordinary portland cement (“OPC”), mineral aggregates, water, and chemical additives. The reaction of OPC with water (hydration) forms calcium silicate hydrate (C-S-H) compounds. The precipitation of C-S-H between proximate particles induces cohesion/hardening, and the resulting porosity reduction and refinement strengthen the concrete. Due to the significant impact of the construction industry on climate change, there is a pressing demand to implement OPC-alternative cementation solutions with significantly reduced embodied CO₂ intensities. Over 30 billion metric tons of concrete are produced per year, involving the production of over 4.5 billion metric tons of cement, with CO₂ emissions on the order of 0.8-0.9 CO₂/kg cement. Emissions associated with cement production make up over 5% of global CO₂ emissions, contributing significantly to global climate change.

Transformative technologies that can capture gigatons (Gt) of CO₂ produced from industrial processes (e.g., concrete production) are vital to mitigate climate change. Various CO₂ capture, sequestration, and storage processes (CCSS) have been investigated to manage CO₂ emissions from various sources. Current technologies for carbon capture using amines rely on a thermal swing cycle in which CO₂ is absorbed in a bubble-flow column, after which regeneration of the CO₂-rich amine solution occurs in a packed distillation column at >140° C. Although this process has been used for post-combustion capture in power generation, it suffers from large energy intensities needed to: desorb only a fraction (˜50%) of the CO₂ trapped in the amine solution at large energy intensities (1.2 MWh per tonne of CO₂ for power generation and 5.0 MWh per tonne of CO₂ for direct air capture (“DAC”).

The relatively low extent of amine regeneration leads to low working CO₂ absorption capacities (e.g., ˜0.05 and 0.25 mol CO₂ per mol MEA for DAC and power generation, respectively. (See E. S. Sanz-Pérez, et al., Direct Capture of CO₂ from Ambient Air, 116 CHEM. REV. 11840-76 (2016).) Further, the high temperatures required for amine regeneration (>140° C.) result in solvent loss via chemical degradation and evaporation. These factors can result in up to a 50% increase in capital expenditures and up to 25% increase in operating expenses, which leads to high costs of carbon capture (>$100 per tonne CO₂) and restricts the use of amine-based processes to point source emitters (e.g., fossil-fuel fired power plants).

Use of caustic solutions (e.g., KOH/K₂CO₃) for direct air capture also requires high energy intensities to produce mineral reagents for pH swing processes (e.g., 4.5 MWh per tonne CO₂ for chlor-alkali to produce NaOH and HCl). Adsorption using solid materials has also been proposed for direct air capture, however, these processes also suffer from high energy requirements for desorption (>2.0 MWh per tonne CO₂).

Therefore, there exists great interest in a more efficient and less energy-intensive processes for forming concrete products that harden via contacting concentrated vapor CO₂ from a gas source.

SUMMARY OF THE INVENTION

In one aspect, which may be combined with any other aspect or embodiment, the present disclosure relates to a method of forming a concrete product, comprising capturing CO₂ from a gas source. In some embodiments, capturing the CO₂ comprises contacting the gas source with an absorption solution having a solvent and a solute. In some embodiments, the solvent and/or solute are capable of reacting with CO₂ to form an anionic compound. In some embodiments, capturing the CO₂ further comprises adjusting the pH of the absorption solution electrochemically to less than about 7 to release the CO₂ as a concentrated vapor containing CO₂, collecting the concentrated vapor containing CO₂, regenerating the solvent and/or the solute, and optionally collecting the regenerated solvent and/or solute. In some embodiments, adjusting the pH of the absorption solution occurs at ambient temperature. In some embodiments, the method further comprises flowing the concentrated vapor containing CO₂ through a gas processing unit to adjust at least one of a temperature, a relative humidity, or a flow rate of the concentrated vapor containing CO₂. In some embodiments, the method further comprises reacting the concentrated vapor containing CO₂ with a concrete component. In some embodiments, the concrete component is a green body.

In some embodiments, including any of the foregoing, the concentrated vapor comprises about 2-99% (v/v) CO₂. In some of these embodiments, the concentrated vapor comprises greater than or equal to 2% (v/v) CO₂. In certain embodiments, the concentrated vapor comprises less than or equal to 5% (v/v) CO₂. In some embodiments, the concentrated vapor comprises 2.0% to 5.0% (v/v) CO₂. In some embodiments, the concentrated vapor comprises 2.0, 2.5, 3.0, 3.5, 4.0, 4.5, or 5.0% (v/v) CO₂. In certain embodiments, the concentrated vapor comprises 2.0 (v/v) CO₂. In certain other embodiments, the concentrated vapor comprises 2.5% (v/v) CO₂. In certain embodiments, the concentrated vapor comprises 3.0% (v/v) CO₂. In certain other embodiments, the concentrated vapor comprises 3.5% (v/v) CO₂. In certain embodiments, the concentrated vapor comprises 4.0% (v/v) CO₂. In certain other embodiments, the concentrated vapor comprises 4.5% (v/v) CO₂. In certain embodiments, the concentrated vapor comprises 5.0% (v/v) CO₂. In some embodiments, the concentrated vapor containing CO₂ has a relative humidity that ranges from 10% to 30%.

In some embodiments, including any of the foregoing, the absorption solution comprises one or more amines. In some embodiments, the one or more amines are selected from monoethanolamine (MEA), 2-ethylaminoethanol, 2-methylaminoethanol, ethylenediamine, benzylamine), diethanolamine (DEA), pyrrolidine, morpholine, 2,6-dimethylmorpholine, monoisopropanolamine, piperazine (PZ), 2-(dimethylamino)ethanol (DMAE), N-tert-butyldiethanolamine (tBDEA), 3-dimethylamino-1-propanol (DMA-1P), 3-(dimethylamino)-1,2-propanediol (DMA-1,2-PD), 2-diethylaminoethanol (DEAE), 3-diethylamino-1,2-propanediol (DEA-1,2-PD), 3-diethylamino-1-propanol (DEA-1P), triethanolamine (TEA), 1-dimethylamino-2-propanol (DMA-2P), 1-(2-hydroxyethyl)pyrrolidine [1-(2HE)PRLD], 1-diethylamino-2-propanol (DEA-2P), 3-pyrrolidino-1,2-propanediol (PRLD-1,2-PD), 2-(diisopropylamino)ethanol (DIPAE), 1-(2-hydroxyethyl)piperidine [1-(2HE)PP], 2-(dimethylamino)-2-methyl-1-propanol (DMA-2M-1P), 3-piperidino-1,2-propanediol (3PP-1,2-PD), 3-dimethylamino-2,2-dimethyl-1-propanol (DMA-2,2-DM-1P), 3-hydroxy-1-methylpiperidine (3H-1MPP), N-ethyldiethanolamine, 1-ethyl-3-hydroxypiperidine); and mixtures thereof. In some of these embodiments, the one or more amines are selected from monoethanolamine (MEA), 2-ethylaminoethanol, 2-methylaminoethanol, ethylenediamine, benzylamine, diethanolamine (DEA), pyrrolidine, morpholine, 2,6-Dimethylmorpholine, monoisopropanolamine, piperazine (PZ), and combinations thereof. In some other of these embodiments, the one or more amines are selected from monoethanolamine (MEA), piperazine (PZ), and combinations thereof. In some of these embodiments, the one or more amines comprise monoethanolamine (MEA). In some of these embodiments, the one or more amines comprise 2-ethylaminoethanol. In some of these embodiments, the one or more amines comprise 2-methylaminoethanol. In some of these embodiments, the one or more amines comprise ethylenediamine. In some of these embodiments, the one or more amines comprise benzylamine. In some of these embodiments, the one or more amines comprise diethanolamine (DEA). In some of these embodiments, the one or more amines comprise pyrrolidine. In some of these embodiments, the one or more amines comprise morpholine. In some of these embodiments, the one or more amines comprise 2,6-dimethylmorpholine. In some of these embodiments, the one or more amines comprise monoisopropanolamine. In some of these embodiments, the one or more amines comprise piperazine (PZ). In some of these embodiments, the one or more amines comprise 2-(dimethylamino)ethanol (DMAE). In some of these embodiments, the one or more amines comprise N-tert-butyldiethanolamine (tBDEA). In some of these embodiments, the one or more amines comprise 3-dimethylamino-1-propanol (DMA-1P). In some of these embodiments, the one or more amines comprise 3-(dimethylamino)-1,2-propanediol (DMA-1,2-PD). In some of these embodiments, the one or more amines comprise 2-diethylaminoethanol (DEAE). In some of these embodiments, the one or more amines comprise 3-diethylamino-1,2-propanediol (DEA-1,2-PD). In some of these embodiments, the one or more amines comprise 3-diethylamino-1-propanol (DEA-1P). In some of these embodiments, the one or more amines comprise triethanolamine (TEA). In some of these embodiments, the one or more amines comprise 1-dimethylamino-2-propanol (DMA-2P), 1-(2-hydroxyethyl)pyrrolidine [1-(2HE)PRLD]. In some of these embodiments, the one or more amines comprise 1-diethylamino-2-propanol (DEA-2P). In some of these embodiments, the one or more amines comprise 3-pyrrolidino-1,2-propanediol (PRLD-1,2-PD). In some of these embodiments, the one or more amines comprise 2-(diisopropylamino)ethanol (DIPAE). In some of these embodiments, the one or more amines comprise 1-(2-hydroxyethyl)piperidine [1-(2HE)PP]. In some of these embodiments, the one or more amines comprise 2-(dimethylamino)-2-methyl-1-propanol (DMA-2M-1P). In some of these embodiments, the one or more amines comprise 3-piperidino-1,2-propanediol (3PP-1,2-PD). In some of these embodiments, the one or more amines comprise 3-dimethylamino-2,2-dimethyl-1-propanol (DMA-2,2-DM-1P). In some of these embodiments, the one or more amines comprise 3-hydroxy-1-methylpiperidine (3H-1MPP). In some of these embodiments, the one or more amines comprise N-ethyldiethanolamine. In some of these embodiments, the one or more amines comprise 1-ethyl-3-hydroxypiperidine).

In some embodiments, reacting the concentrated vapor containing CO₂ with the concrete component further comprises providing a carbonatable concrete mixture, hydrating/reacting the concrete mixture to form the concrete component, and contacting the concrete component with the concentrated vapor CO₂ to harden the concrete mixture via the formation of carbonate minerals.

In some embodiments, reacting the concentrated vapor containing CO₂ with the concrete component further comprises providing a carbonatable concrete mixture, hydrating the concrete mixture to form the concrete component, and contacting the concrete component with the concentrated vapor CO₂ to harden the concrete mixture via the formation of carbonate minerals.

In some embodiments, reacting the concentrated vapor containing CO₂ with the concrete component further comprises providing a carbonatable concrete mixture, reacting the concrete mixture to form the concrete component, and contacting the concrete component with the concentrated vapor CO₂ to harden the concrete mixture via the formation of carbonate minerals.

In some embodiments, reacting the concentrated vapor containing CO₂ with the concrete component further comprises providing a carbonatable concrete mixture, hydrating the concrete mixture to form the concrete component and reacting the concrete mixture to form the concrete component, and contacting the concrete component with the concentrated vapor CO₂ to harden the concrete component via the formation of carbonate minerals.

In some embodiments, the concrete mixture comprises portland cement and the concrete component comprises virgin portlandite or portlandite residues. In some embodiments, the concrete mixture comprises portland cement and the concrete component comprises a combination of virgin portlandite and portlandite residues. In some embodiments, the concrete mixture comprises at least one of portlandite, coal combustion residues, recycled concrete aggregates, slag, portland cement, lime, portlandite residues, or natural alkaline rocks. In some embodiments, the concentrated vapor containing CO₂ contacts aggregate to form carbonated aggregates that are utilized in the concrete mixture. In some embodiments, the concentrated vapor containing CO₂ contacts aggregate to form carbonated aggregates. In certain embodiments, the carbonated aggregates are utilized in a concrete mixture.

In some embodiments, the gas source is an effluent from an industrial source, an atmospheric source, a commercially available CO₂ source, or liquefied CO₂. In some embodiments, the gas source is an atmospheric source.

In some embodiments, including any of the foregoing, the steps of the method are performed in the order recited.

In some embodiments, including any of the foregoing, the concentrated vapor containing CO₂ has a temperature that ranges from 20° C. to 80° C.

In some embodiments, including any of the foregoing, the concentrated vapor containing CO₂ has a temperature that ranges from 50° C. to 70° C.

In some embodiments, including any of the foregoing, the method includes collecting the concentrated vapor containing CO₂ comprises fractionally enriching the concentration of CO₂ in the concentrated vapor containing CO₂.

In some embodiments, including any of the foregoing, the concrete mixture comprises portland cement and the concrete component comprises virgin portlandite or portlandite residues.

In some embodiments, including any of the foregoing, the concrete mixture comprises at least one of coal combustion residues, aggregates, recycled concrete aggregates, slag, portland cement, lime, portlandite residues, or natural alkaline rocks.

In some embodiments, including any of the foregoing, the gas source is an effluent from an industrial source, an atmospheric source, a commercially-available CO₂ source, or liquefied CO₂.

In some embodiments, including any of the foregoing, the gas source is an atmospheric source.

In some embodiments, including any of the foregoing, the method includes adjusting the pH of the absorption solution occurs at ambient temperature.

In some embodiments, including any of the foregoing, the concentrated vapor containing CO₂ contacts aggregate wherein adjusting the pH of the absorption solution electrochemically to less than about 7 to release the CO₂ as a concentrated vapor containing CO₂ comprises using a pH swing induced by water electrolysis in a cell that incorporates at least one ion exchange membrane.

In some embodiments, including any of the foregoing, the method includes collecting the regenerated solvent and/or solute.

In some embodiments, including any of the foregoing, the concrete component comprises aggregates.

In some embodiments, including any of the foregoing, the concrete component is a green body.

In another embodiment, set forth herein is a concrete product formed by a method herein.

In another embodiments, set forth herein is a system for implementing a method herein.

In another embodiment, set forth herein is a system comprising a direct-air capture CO₂ system coupled to a carbonation chamber.

BRIEF DESCRIPTION OF THE DRAWINGS

FIG. 1 is a schematic illustration of a manufacturing process including a direct air capture system, a gas processing unit, and a reaction chamber, in accordance with various embodiments.

FIG. 2A is a plot of conversion-time profiles of portlandite particles exposed to gas streams with varying CO₂ concentrations (% v/v). FIG. 2A is a reproduction of FIG. 3(a) from Falzone, G., Mehdipour, I., Neithalath, N., Bauchy, M., Simonetti, D., & Sant, G. (2021). New insights into the mechanisms of carbon dioxide mineralization by portlandite. AIChE Journal, 67(5), e17160.

FIG. 2B is a plot of linearized conversion curves of carbonation rates of portlandite particles. FIG. 2B is a reproduction of FIG. 3(b) from Falzone, G., Mehdipour, I., Neithalath, N., Bauchy, M., Simonetti, D., & Sant, G. (2021). New insights into the mechanisms of carbon dioxide mineralization by portlandite. AIChE Journal, 67(5), e17160.

FIG. 3A is a plot of batch-wise trends for the CO₂ uptake and CO₂ utilization efficiency of producing concrete blocks at a first facility using coal-fired flue gas stream.

FIG. 3B is a plot of batch-wise trends for the CO₂ uptake and CO₂ utilization efficiency of producing concrete blocks at a second facility using both coal and natural gas fired flue gas streams.

FIG. 4 shows the effect of T and RH on the X (conversion) at 4 v./v.% using the developed regression model for the solid phase conversion.

FIG. 5 shows the effect of T and RH on the X (conversion) at 9 v./v.% using the developed regression model for the solid phase conversion.

FIG. 6 shows porosity reduction of carbonated concrete compared to non-carbonated as a function of CO₂ uptake.

FIG. 7 shows strength of nine concrete mixtures at 28 days comparing the carbonated and non-carbonated samples.

FIG. 8 shows an apparatus for mixing compressed air and CO₂ to achieve specific CO₂ concentrations at specific relative humidities and specific temperatures.

DETAILED DESCRIPTION

Embodiments of the present disclosure are directed to integrating direct air capture systems into the CO₂ mineralization process of forming cementitious materials and concrete products. The CO₂ uptake (quantified as a mass of CO₂ incorporated into solid products per mass of initial solid material) describes the material's efficiency in sequestering gaseous CO₂ in stable solids. Enhancing CO₂ uptake reduces a material's embodied CO₂ emissions footprint and allows impactful removal of gaseous CO₂ from industrial emissions sources. Such processes include, but are not limited to, those disclosed in PCT International Publication No. WO2016/061251 A1, U.S. Patent Application Publication No. 2019/0177220, which published on Jul. 13, 2019, U.S. Patent Application Publication No. 2020/0299203, which published on Sep. 24, 2022, US Patent Application Publication No. 2022-0227677-A1, which published on Jul. 21, 2022, International PCT Patent Application No. PCT/US22/35289, filed on Jun. 28, 2022, and U.S. patent application Ser. No. 17/722,036, filed Apr. 15, 2022, the entireties of which are hereby incorporated by reference herein for all purposes.

In some cases, there is low accessibility to point-source CO₂ emitters for the CO₂ mineralization process at masonry/precast concrete plants. When CO₂ emitters and masonry/precast concrete plants are not co-located, gas piping is required from the CO₂ emitter to the concrete plant. Depending on the piping distance and pipeline logistics, this process may not be technically or economically viable. In present embodiments, an on-site direct air capture system can be integrated into a CO₂ mineralization system to source CO₂ from ambient air and eliminate the need for piping from point-source CO₂ emitters.

In some embodiments, including any of the foregoing, the methods herein comprise flowing the concentrated vapor containing CO₂ through a gas processing unit to adjust at least one of a temperature, a relative humidity, or a flow rate of the concentrated vapor containing CO₂; and contacting the concentrated vapor containing CO₂ with a concrete component.

In some embodiments, the concentrated vapor containing CO₂ is piped to the concrete component from an on-site location from where the concrete component is carbonated.

In some embodiments, the concentrated vapor containing CO₂ flowing through a gas processing unit does not travel through piping that is longer than 1 kilometer before contacting the concentrated vapor containing CO₂ with a concrete component. In some of these embodiments, the concentrated vapor containing CO₂ flowing through a gas processing unit does not travel through piping that is longer than 0.5 kilometers before contacting the concentrated vapor containing CO₂ with a concrete component. In some of these embodiments, the concentrated vapor containing CO₂ flowing through a gas processing unit does not travel through piping that is longer than 10 meters before contacting the concentrated vapor containing CO₂ with a concrete component. In some of these embodiments, the concentrated vapor containing CO₂ flowing through a gas processing unit does not travel through piping that is longer than 5 meters before contacting the concentrated vapor containing CO₂ with a concrete component.

In some of these embodiments, the concentrated vapor containing CO₂ is sourced from the atmosphere and not from a point-source CO₂ emitter, such as a pressurized tank of CO₂.

In one embodiment, as shown in FIG. 1, a manufacturing process of a low-carbon concrete product includes: (1) a direct air capture (DAC) system to derive CO₂ from the atmosphere (101), (2) a gas processing unit which conditions the temperature, relative humidity, and flow rate of the incoming CO₂ gas stream (102), and (3) a reaction chamber where the CO₂ gas stream reacts with green concrete components (103). In such embodiments, integrating optimal direct air capture (DAC) into carbonation processes enables the utilization of fractional enrichment of atmospheric CO₂ for producing low-carbon concrete products and carbonation of aggregates. This process may further utilize a smaller scale design and a more energy-efficient DAC system to supply low-cost and fractional CO₂ gas streams (>5 vol. % for CO₂) for the CO₂ mineralization process of concrete and aggregates such as portlandite, coal combustion residues, recycled concrete aggregates, slag, and natural alkaline rocks. In some embodiments, the process herein may further utilize a smaller scale design and a more energy-efficient DAC system to supply low-cost and fractional CO₂ gas streams (>4 vol. % for CO₂) for the CO₂ mineralization process of concrete and aggregates such as portlandite, coal combustion residues, recycled concrete aggregates, slag, and natural alkaline rocks. The carbonated aggregates can then be utilized in concrete.

In such embodiments, including any of the foregoing, the methods herein include fractionally enriching atmospheric CO₂ for producing low-carbon concrete products and carbonation of aggregates. In certain embodiments, the methods herein include increasing the concentration of CO₂ in the concentrated vapor containing CO₂. Fractionally enriching the concentrated vapor containing CO₂ includes sequentially increasing the concentration of CO₂. This may occur, for example, by collecting and combining low, relative concentration CO₂ into a container that increases the total CO₂ concentration. For example, in some embodiments, including any of the foregoing, the concentrated vapor containing CO₂ includes about 0.04% by volume (v/v) CO₂. For example, in some embodiments, including any of the foregoing, after one step of fractional enrichment, the concentrated vapor containing CO₂ may increase to 0.5% v/v CO₂. For example, in some embodiments, including any of the foregoing, after a second step of fractional enrichment, the concentrated vapor containing CO₂ may increase to 0.5% v/v CO₂. For example, in some embodiments, including any of the foregoing, after a second step of fractional enrichment, the concentrated vapor containing CO₂ may increase to 1% v/v CO₂. This process of fractional enrichment may continue to increase gradually to a final and predetermined value. For example, the process of fractional enrichment may continue to increase gradually to a final and predetermined value at 0.5% v/v CO₂ per step. In other embodiments, the process of fractional enrichment may continue to increase non-gradually to a final and predetermined value.

Further, atmospheric CO₂ may be readily utilized, and this process may eliminate the need for accessibility to point-source CO₂ emitters. Thus, the requirement that CO₂ emitters and precast concrete plants are not co-located is eliminated. Such an embodiment may also be advantageous when piping from CO₂ emitters to precast plants is not economically viable. It is understood that, in some embodiments, the amount of carbon dioxide in the CO₂ waste stream (e.g., post-combustion or post-calcination flue gas stream) is greater than concentration of carbon dioxide typically in the atmosphere (about 0.04% (v/v) CO₂).

In some embodiments, herein, the methods include in-situ acid/base generation that leads to amine regeneration within a single electrochemical cell.

In some embodiments, a mineralization process directly mineralizes CO₂ in dilute flue gas streams into a specially designed concrete mixture formulation in which ordinary portland cement (OPC) is largely replaced by portlandite (also known as hydrated lime produced via hydration of calcium oxide (Ca(OH₂)) and supplementary cementitious materials. Following concrete batching, mixing, and forming, precast concrete components are placed into a carbonation chamber where dilute CO₂ may contact the portlandite at ambient pressure and sub-boiling temperatures (e.g., 25° C., 30° C., 35° C., 40° C., 45° C., 50° C., 55° C., 60° C., 65° C., 70° C., 75° C., 80° C., 85° C., 90° C., and 95° C.). Portlandite may react rapidly and readily upon contact with dilute CO₂ stream resulting in calcium carbonate formation within the concrete. Calcium carbonate (limestone) may serve as a cementation agent that binds aggregate in concrete. Early-age carbonation curing may result in an increase in volume of reaction products by about 10% which reduces the porosity and enhances the mechanical properties and durability of the concrete.

In some examples, including any of the foregoing, the concentrated vapor comprises about 2-99% (v/v) CO₂. In certain examples, the relative humidity (RH) of the concentrated vapor comprising CO₂ is value between or equal to 5 to 30%. For example, the RH may be 5.0, 5.5, 6.0, 6.5, 7.0, 7.5, 8.0, 8.5, 9.0, 9.5, 10.0, 10.5, 11.0, 11.5, 12.0, 12.5, 13.0, 13.5, 14.0, 14.5, 15.0, 15.5, 16.0, 16.5, 17.0, 17.5, 18.0, 18.5, 19.0, 19.5, 20.0, 20.5, 21.0, 21.5, 22.0, 22.5, 23.0, 23.5, 24.0, 24.5, 25.0, 25.5, 26.0, 26.5, 27.0, 27.5, 28.0, 28.5, 29.0, 29.5, or 30.0. In some of these embodiments, the CO₂ concentration in the concentrated vapor is greater than or equal to 2% (v/v) CO₂. In some other of these embodiments, the CO₂ concentration in the concentrated vapor is less than or equal to 5% (v/v) CO₂. In some other of these embodiments, the CO₂ concentration in the concentrated vapor is less than or equal to 5% to less than or equal to 35 (v/v) CO₂. In some of these embodiments, the CO₂ concentration in the concentrated vapor is 2.0, 2.5, 3.0, 3.5, 4.0, 4.5, or 5.0% (v/v) CO₂. In some of these embodiments, the CO₂ concentration in the concentrated vapor has relative humidity that ranges from 5 to 35%. In some of these embodiments, the CO₂ concentration in the concentrated vapor has a relative humidity that ranges from 10-30%. In some of these embodiments, the CO₂ concentration in the concentrated vapor has a relative humidity that ranges from 5-30%.

In some examples, including any of the foregoing, the concentrated vapor comprises 2.0% to 5.0% (v/v) CO₂.

In some examples, including any of the foregoing, the concentrated vapor containing CO₂ has a temperature ranging from 20° C. to 80° C. In certain embodiments, the temperature ranges from 50° C. to 70° C. For example, the temperature may be 20° C., 21° C., 22° C., 23° C., 24° C., 25° C., 26° C., 27° C., 28° C., 29° C., 30° C., 30° C., 31° C., 32° C., 33° C., 34° C., 35° C., 36° C., 37° C., 38° C., 39° C., 40° C., 40° C., 41° C., 42° C., 43° C., 44° C., 45° C., 46° C., 47° C., 48° C., 49° C., 50° C., 50° C., 51° C., 52° C., 53° C., 54° C., 55° C., 56° C., 57° C., 58° C., 59° C., 60° C., 60° C., 61° C., 62° C., 63° C., 64° C., 65° C., 66° C., 67° C., 68° C., 69° C., 70° C., 70° C., 71° C., 72° C., 73° C., 74° C., 75° C., 76° C., 77° C., 78° C., 79° C., or 80° C. In certain embodiments, the temperature ranges from 45° C. to 75° C.

Definitions

As used herein, the singular terms “a,” “an,” and “the” include plural referents unless the context clearly dictates otherwise. Thus, for example, reference to an object can include multiple objects unless the context clearly dictates otherwise.

As used herein, the term “set” refers to a collection of one or more objects. Thus, for example, a set of objects can include a single object or multiple objects.

As used herein, the terms “substantially” and “about” are used to describe and account for small variations. When used in conjunction with an event or circumstance, the terms can refer to instances in which the event or circumstance occurs precisely as well as instances in which the event or circumstance occurs to a close approximation. For example, when used in conjunction with a numerical value, the terms can encompass a range of variation of less than or equal to ±10% of that numerical value, such as less than or equal to ±5%, less than or equal to ±4%, less than or equal to ±3%, less than or equal to ±2%, less than or equal to ±1%, less than or equal to ±0.5%, less than or equal to ±0.1%, or less than or equal to ±0.05%.

Additionally, amounts, ratios, and other numerical values are sometimes presented herein in a range format. It is to be understood that such range format is used for convenience and brevity and should be understood flexibly to include numerical values explicitly specified as limits of a range, but also to include all individual numerical values or sub-ranges encompassed within that range as if each numerical value and sub-range is explicitly specified. For example, a ratio in the range of about 1 to about 200 should be understood to include the explicitly recited limits of about 1 and about 200, but also to include individual ratios such as about 2, about 3, and about 4, and sub-ranges such as about 10 to about 50, about 20 to about 100, and so forth.

While the disclosure has been described with reference to the specific embodiments thereof, it should be understood by those skilled in the art that various changes may be made and equivalents may be substituted without departing from the true spirit and scope of the disclosure as defined by the appended claims. In addition, many modifications may be made to adapt a particular situation, material, composition of matter, method, operation or operations, to the objective, spirit and scope of the disclosure. All such modifications are intended to be within the scope of the claims appended hereto. In particular, while certain methods may have been described with reference to particular operations performed in a particular order, it will be understood that these operations may be combined, sub-divided, or re-ordered to form an equivalent method without departing from the teachings of the disclosure. Accordingly, unless specifically indicated herein, the order and grouping of the operations is not a limitation of the disclosure.

The embodiments, illustratively described herein may suitably be practiced in the absence of any element or elements, limitation or limitations, not specifically disclosed herein. Thus, for example, the terms “comprising,” “including,” “containing,” etc. shall be read expansively and without limitation. Additionally, the terms and expressions employed herein have been used as terms of description and not of limitation, and there is no intention in the use of such terms and expressions of excluding any equivalents of the features shown and described or portions thereof, but it is recognized that various modifications are possible within the scope of the claimed technology. Additionally, the phrase “consisting essentially of” will be understood to include those elements specifically recited and those additional elements that do not materially affect the basic and novel characteristics of the claimed technology. The phrase “consisting of” excludes any element not specified.

As used herein, the term “carbonatable concrete mixture” means a mixture comprising, consisting essentially of, or consisting of one or more materials that is capable of reacting with CO₂ to form a carbonate. A material capable of reacting with CO₂ to form a carbonate includes, but is not limited to, Ca(OH)₂, lime kiln dust, lime, hydrated lime, cement kiln dust, calcium-rich coal combustion residues, slag, off-spec fly ashes, biomass ashes, fluidized bed combustion ashes, circulating fluidized bed ashes, off-spec limes, mineral sorbent/scrubbing residues comprising anhydrous CaO and/or Ca(OH)₂, and combinations thereof. A material capable of reacting with CO₂ may further comprise at least one of oxides, hydroxides, carbonates, silicates, sulfites, sulfates, chlorides, nitrates, or nitrites of calcium and/or magnesium, or any combination thereof. Carbonates include, but are not limited to, CaCO₃, MgCO₃, and combinations thereof. Carbonates include, but are not limited to, calcium carbonate, calcite, vaterite, aragonite, or any combination thereof. Carbonated materials may include oxides, hydroxides, carbonates, silicates, sulfites, sulfates, chlorides, nitrates, or nitrites of calcium and/or magnesium and/or other uni-/multi-valent elements, or any combination thereof.

As used herein, the term “a carbonated concrete composite,” refers to a carbonated concrete object (e.g., a building material) made from early-age (e.g., fresh) concrete that is then contacted with a CO₂-containing curing gas having a suitable CO₂ concentration.

As used herein, “aluminosilicate mineral materials” refers to materials which include silica and/or alumina in the form of amorphous or crystalline or combination thereof. Alkaline-rich mineral materials include, but are not limited to, coal combustion residues, slag, off-spec fly ashes, biomass ashes, fluidized bed combustion ashes, circulating fluidized bed ashes, calcium rich fly ashes, calcium-poor fly ashes, ponded ashes, landfilled ashes, bottom ashes, flue gas ashes, and combinations thereof. The alkaline-rich mineral materials may further comprise at least one of oxides, hydroxides, carbonates, silicates, sulfites, sulfates, chlorides, nitrates, or nitrites of calcium and/or magnesium, or any combination thereof.

As used herein, the term “green body” refers to a concrete precursor.

As used herein, the term “rate of carbonation” refers to the rate which CO₂ is consumed. To quantify the carbonation kinetics, the time-CO₂ uptake profiles are fitted to an equation of the form

C(t)=C(t_u)(1−exp[(−k_carbt)/C(t_u)])  (Eq. 6)

where k_carb is the apparent carbonation rate constant and C(t_u) is the ultimate CO₂ uptake at the end of carbonation curing duration. For example, a carbonation at or above 0.005 per hour means that k_carb is a value 0.005 or greater. This would include, but is not limited to, k_carb of 0.05, or 0.5, or 1, or 2.

As used herein, a “concrete product,” refers to the product resulting from the carbonation, and optionally the hydration, of a concrete component.

As used herein, a “concrete component,” refers to concrete which may be shaped or pressed in a particular form, e.g., an I-beam, a masonry block, or a flat sheet. The fresh (i.e., unreacted) concrete may include portlandite (Ca(OH)₂) and is capable of reacting with CO₂ to form concrete.

As used herein, an “anionic compound,” refers to anions produced when CO₂ is absorbed into an amine solution. Anionic compounds include, but are not limited to, CO₃²⁻, HCO₃¹⁻, and compounds having negatively charged carboxylic acid groups (i.e., carbamate anions) such as RNHCO₂⁻ or RNCOO²⁻ wherein R is an organic substituent such as methyl, ethyl, or propyl.

As used herein, “regenerating,” refers to the process of reversibly removing absorbed CO₂ from an amine-containing solution.

As used herein, “virgin portlandite,” refers to portlandite (e.g., Ca(OH)₂)) which has not reacted with H₂O or CO₂.

As used herein, “portlandite residues” refers to portlandite (e.g., Ca(OH)₂)) which has reacted with H₂O and/or CO₂, but which could still react further with H₂O and/or CO₂, or other compounds that are partially carbonated.

As used herein, the term “active carbonation,” refers to a process which results in a carbonation reaction rate that is above a natural value. Herein, the natural value is the rate of carbonation if the material being carbonated is exposed to atmospheric levels of CO₂ (0.04% v/v) at room temperature and 1 atm. For example, a carbonation rate at or above 0.005 per hour is a non-limiting example of active carbonation.

As used herein, the term “concrete containing carbonated materials,” refers to a concrete object that is composed of carbonated materials in the form of slurry, aggregate, or dry powder, or any combinations thereof.

As used herein, the phrase “concentrated vapor containing CO₂,” refers to a gaseous stream that has a higher concentration of CO₂ than air does. The concentrated vapor containing CO₂ may include air, as well as the individual components of air, such as, but not limited to, N₂, O₂, water, and combinations thereof. In some examples, the concentrated vapor containing CO₂ is processed so it has a particular relative humidity, a particular temperature, a particular flow rate, or a combination thereof. In some examples, the concentrated vapor is processed so it has a particular CO₂ concentration. This may be accomplished using fractional enrichment processes that progressively increase the concentration of CO₂ in a gas that already has higher concentration of CO₂ than air does.

CO₂ Absorption by Electrochemically-Induced pH-Swing Process in DAC Systems

In some embodiments, including any of the foregoing, DAC systems use amine-based absorption to remove CO₂. As shown in a portion of FIG. 1, forming a low-carbon concrete product may first include integrating a DAC system into the CO₂ mineralization process. During a conventional amine scrubbing process, CO₂-containing gases, are contacted with a concentrated (20-50% v/v) aqueous amine solution. This solution is an aqueous solution with an amine solute. Under basic conditions (pH>10), absorption occurs via the reaction of CO₂ with the amine (e.g., MEA; RNH₂ where R═CH₂CH₂OH) to form carbamate anions (RNHCOO⁻, RNCOO²⁻), protonated amines (RNH₃+), and protons/hydronium ions (H⁺/H₃O⁺), according to Equations 1-3, while other gases, such as N₂ and O₂, escape in the effluent. CO₂ also forms carbonates at high pH (Equation 4).⁴

RNH₂+CO₂⇄H⁺+RNHCOO⁻  (1)

RNHCOO⁻+RNH₂⇄RNH₃⁺+RNCOO²⁻  (2)

RNHCOO⁻+H₂O⇄H₃O⁺+RNCOO²⁻  (3)

CO₂+H₂O⇄CO₃²⁻+2H⁺  (4)

The state-of-the art for releasing the CO₂ and regenerating the amine is a thermal process. In the thermal process, the solution is heated to elevated temperatures (>140° C.) where the carbamate decomposes to yield the original amine molecule and release CO₂ as a concentrated vapor.^{3, 5-6} However, large thermal duties (e.g., >5 MWh/tonne of CO₂ for a working capacity of 0.05 mol/mol for DAC applications)³ render the thermal process economically unattractive. Further, the high temperatures required for amine regeneration can result in solvent loss via chemical degradation and evaporation.³

An alternative to thermal amine regeneration is to shift the pH of the solution to acidic conditions (pH≤7), which favors the decomposition of the carbamate ions (via acid-hydrolysis) according to the reverse of Equations (1) and (3).

In some embodiments, the methods and systems set forth herein include methods for shifting the pH of the solution using a method other than the thermal amine regeneration method. For example, in some embodiments, including any of the foregoing, the methods and systems herein include a pH swing. The pH swing may include an electrolysis system. The pH swing may include at least one or ion exchange membranes [cation exchange membrane (CEM) and an anion exchange membrane (AEM)]. The pH swing may include an ion exchange resin (e.g., an anion exchange resin).

In some embodiments, including any of the foregoing, the pH-swing process can occur at ambient temperatures, and therefore offers the following advantages: (1) simpler process equipment requirements; (2) utilization of the maximum working capacity of the amine; and (3) reduced solvent loss. However, the requirement for acids and bases as stoichiometric reagents to shift the pH renders pH-swing processes unfeasible for widespread adoption. An alternative to mineral acids and bases is to use water electrolysis to generate the necessary protons for carbamate ion hydrolysis (e.g., to convert a rich amine solution to a lean solution) and to generate hydroxide ions needed to increase the pH of the lean solution for subsequent cycles of CO₂ absorption.

In some embodiments, including any of the foregoing, the methods herein include a step or a series of steps which comprise electrolysis and the use of at least one or more ion exchange membranes.

In some embodiments, including any of the foregoing, the methods herein include a step or a series of steps which comprise electrolysis and the use of two ion exchange membranes: a cation exchange membrane (CEM) and an anion exchange membrane (AEM). In some of these embodiments, the methods further include the use of a strong base anion exchange resin.

In the water electrolysis approach, protons are generated from aqueous solutions at the anode (with hydroxide ions generated at the cathode) in an electrochemical cell according to Equations (5) and (6) below:

2H₂O(l)→O₂(g)+4H⁺(aq)+4e⁻  (5)

4H₂O(l)+4e⁻→2H₂(g)+4OH⁻(aq)  (6)

The aqueous solution at the anode is referred as an anolyte. The protons diffuse into the rich amine solution across a cation exchange membrane (CEM) resulting in a decrease in the pH which leads to the decomposition of carbamate ions and release of CO₂. A CEM is included to prevent diffusion of carbamate anions into the anode and cathode cells, thereby preventing electro-oxidation of carbamates/MEA. To maintain electroneutrality, a concentrated salt solution (e.g., NaCl or NaNO₃) is used to provide counter anions to the amine solution and cations to the catholyte. An anion exchange membrane (AEM) prevents the diffusion of the salt solution cations into the aqueous amine solution (e.g., MEA compartment of a cell). After CO₂ is released, the lean amine solution is restored to high pH using a strong base anion exchange resin. This resin exchanges the counter ions (e.g., Cl⁻ or NO₃⁻) from the salt reservoir (e.g., that have accumulated in the amine solution) with hydroxide ions to increase the pH of the lean amine to its original basic value.

In some embodiments, including any of the foregoing, the anion exchange resin is regenerated using the hydroxide rich solution from the cathode compartment of the electrochemical cell, thereby recovering the anions used in the salt solution compartment. This regeneration process ensures efficient recycling of the necessary reagents, minimizing operating costs and preventing waste generation. This electrochemically-induced pH-swing process has the advantages of replacing hazardous, expensive, carbon-intensive reagents (e.g., mineral acids) with an abundant and benign source (e.g., water) while leveraging renewable energy to facilitate the process.

In some embodiments, the methods of the present disclosure include a method or step of directly capturing CO₂ from a gas source, comprising: contacting the gas source comprising CO₂ with an absorption solution comprising a solvent and a solute.

In some embodiments, including any of the foregoing, the methods of the present disclosure include a method or step of capturing CO₂ from a gas source, comprising: contacting the gas source comprising CO₂ with an absorption solution comprising a solvent and a solute. The solvent and a solute may be an aqueous amine solution as set forth in this disclosure. The solvent and/or the solute are capable of forming an anionic complex. The method of directly capturing CO₂ further includes adjusting the pH of the absorption solution electrochemically to less than about 7; collecting the CO₂ as a concentrated vapor that is released during or after the pH adjusting step; regenerating the solvent and/or solute; and optionally collecting the regenerated solvent and/or solute. In some embodiments, the pH is adjusted to less than 6. In some other embodiments, the pH is adjusted to less than 5. In other embodiments, the pH is adjusted to less than 4. In some embodiments, the pH is adjusted to less than 3. In some embodiments, the absorption solution comprise one or more amines. In some embodiments, the anionic complex comprises carbamate ions and/or a hydroxide (e.g., sodium hydroxide, potassium hydroxide). In some embodiments, the solvent is an amine. In some embodiments, the amine is R_xNH_3-x, wherein R is selected from an optionally substituted alkyl, ether, or alcohol; and wherein x is an integer from and including 0 to, and including, 3

In some embodiments, the pH adjusting step is performed via water electrolysis. In some embodiments, the CO₂ gas source is an effluent from an industrial source (e.g., flue gas emitted from a natural gas-fired power plant, a coal-fired power plant, an iron mill, a steel mill, a cement plant, an ethanol plant, or a chemical manufacturing plant). In some embodiments, the CO₂ source is an atmospheric source (e.g., ambient air). In some embodiments, the CO₂ source is a commercial product such as a commercially available CO₂. In some embodiments, the CO₂ source is liquefied CO₂. In some embodiments, the pH adjusting step is performed at a temperature of less than about 100° C. In some embodiments, the pH adjusting step occurs at ambient temperature (e.g., about 25° C.). In some embodiments, including any of the foregoing, the pH adjusting step occurs at a temperature of greater than, or equal to, 45° C., to less than, or equal to 75° C. In some embodiments, including any of the foregoing, the pH adjusting step occurs at a temperature of greater than, or equal to, 35° C., to less than, or equal to 65° C. In some embodiments, including any of the foregoing, the pH adjusting step occurs at a temperature of greater than, or equal to, 35° C., to less than, or equal to 75° C. In some embodiments, including any of the foregoing, the pH adjusting step occurs at a temperature of greater than, or equal to, 55° C., to less than, or equal to 75° C. In some embodiments, including any of the foregoing, the pH adjusting step occurs at a temperature of greater than, or equal to, 25° C., to less than, or equal to 55° C. In some embodiments, including any of the foregoing, the pH adjusting step occurs at a temperature of greater than, or equal to, 25° C., to less than, or equal to 35° C. In some embodiments, the pH adjusting step occurs at ambient temperature and pressure (e.g., about 1 atm). In some embodiments, the regenerated amine is collected and used for the same process again.

In some embodiments, the amine comprises: one or more primary amines (e.g., monoethanolamine (MEA), 2-ethylaminoethanol, 2-methylaminoethanol, ethylenediamine, benzylamine); one or more secondary amines (e.g., diethanolamine (DEA), pyrrolidine, morpholine, 2,6-dimethylmorpholine, monoisopropanolamine, piperazine (PZ)); one or more tertiary amines (e.g., 2-(dimethylamino)ethanol (DMAE), N-tert-butyldiethanolamine (tBDEA), 3-dimethylamino-1-propanol (DMA-1P), 3-(dimethylamino)-1,2-propanediol (DMA-1,2-PD), 2-diethylaminoethanol (DEAE), 3-diethylamino-1,2-propanediol (DEA-1,2-PD), 3-diethylamino-1-propanol (DEA-1P), triethanolamine (TEA), 1-dimethylamino-2-propanol (DMA-2P), 1-(2-hydroxyethyl)pyrrolidine [1-(2HE)PRLD], 1-diethylamino-2-propanol (DEA-2P), 3-pyrrolidino-1,2-propanediol (PRLD-1,2-PD), 2-(diisopropylamino)ethanol (DIPAE), 1-(2-hydroxyethyl)piperidine [1-(2HE)PP], 2-(dimethylamino)-2-methyl-1-propanol (DMA-2M-1P), 3-piperidino-1,2-propanediol (3PP-1,2-PD), 3-dimethylamino-2,2-dimethyl-1-propanol (DMA-2,2-DM-1P), 3-hydroxy-1-methylpiperidine (3H-1MPP), N-ethyldiethanolamine, 1-ethyl-3-hydroxypiperidine); and mixtures thereof.

In some embodiments, the amine is monoethanolamine (MEA). In other embodiments, the amine is a combination of monoethanolamine (MEA) and one or more other amines.

In some embodiments, the amine is piperazine. In other embodiments, the amine is a combination of piperazine and one or more additional amines.

In some embodiments, the amine is a combination of monoethanolamine (MEA) and piperazine. In other embodiments, the amine is a combination of monoethanolamine (MEA), piperazine, and one or more additional amines.

In some embodiments, the solution absorbing CO₂ has a basic pH (e.g., >7). In some embodiments, the pH of the solution absorbing CO₂ is greater than about 7, greater than about 7.5, greater than about 8, greater than about 8.5, greater than about 9, greater than about 9.5, greater than about 10, greater than about 10.5, greater than about 11, greater than about 11.5, or greater than about 12, or any range or value therein between. In some embodiments, the solution absorbing CO₂ has a pH of about 7, about 7.5, about 8, about 8.5, about 9, about 9.5, about 10, about 10.5, about 11, about 11.5, about 12, about 12.5, about 13, about 13.5, or about 14, or any range or value therein between.

In some embodiments, the CO₂ absorption step is performed at a temperature of less than about 100° C., less than about 95° C., less than about 90° C., less than about 85° C., less than about 80° C., less than about 75° C., less than about 70° C., less than about 65° C., less than about 60° C., less than about 55° C., less than about 50° C., less than about 45° C., less than about 40° C., less than about 30° C., or less than about 25° C., or any range or value therein between. In some embodiments, the CO₂ absorption step is performed at a temperature of about 100° C., about 95° C., about 90° C., about 85° C., about 80° C., about 75° C., about 70° C., about 65° C., about 60° C., about 55° C., about 50° C., about 45° C., about 40° C., about 30° C., or about 25° C., or any range or value therein between. In some embodiments, the CO₂ absorption step is performed under ambient conditions (e.g., room temperature and pressure).

In some embodiments, the pH of the solution is adjusted electrochemically to release the CO₂ as a concentrated vapor. In some embodiments, the pH of the solution is adjusted to less than about 7.5, less than about 7, less than about 6.5, less than about 6, less than about 5.5, less than about 5, less than about 4.5, less than about 4, less than about 3.5, less than about 3, less than about 2.5, less than about 2, less than about 1.5, or less than about 1, or any range or value therein between. In some embodiments, the pH of the solution is adjusted about 7.5, about 7, about 6.5, about 6, about 5.5, about 5, about 4.5, about 4, about 3.5, about 3, about 2.5, about 2, about 1.5, or about 1, or any range or value therein between. Herein, electrochemical adjustment includes the use of water electrolysis.

In some embodiments, the pH adjusting step is performed at a temperature of less than about 100° C., less than about 95° C., less than about 90° C., less than about 85° C., less than about 80° C., less than about 75° C., less than about 70° C., less than about 65° C., less than about 60° C., less than about 55° C., less than about 50° C., less than about 45° C., less than about 40° C., less than about 30° C., or less than about 25° C., or any range or value therein between. In some embodiments, the pH adjusting step is performed at a temperature of about 100° C., about 95° C., about 90° C., about 85° C., about 80° C., about 75° C., about 70° C., about 65° C., about 60° C., about 55° C., about 50° C., about 45° C., about 40° C., about 30° C., or about 25° C., or any range or value therein between. In some embodiments, the pH adjusting step is performed under ambient conditions (e.g., room temperature and pressure). In such embodiments, the pH adjusting step requires simpler process equipment, allows for complete amine regeneration, thus maximizing working capacity, and exhibits reduced solvent loss.

In some embodiments, the pH adjusting step is performed at a temperature of 45° C. to 75° C.

In some embodiments, the pH adjusting step is performed at a temperature of 55° C. to 75° C.

In some embodiments, the pH adjusting step is performed at a temperature of 65° C. to 75° C.

In some embodiments, the pH adjusting step is performed at a temperature of 45° C. to 65° C.

In some embodiments, the pH adjusting step is performed at a temperature of 55° C. to 65° C.

In some embodiments, the pH adjusting step is performed at a temperature of 44° C. to 55° C.

In some embodiments, the pH adjusting step is performed at an ambient pressure. In some embodiments, the pressure is at a pressure in a range of about 0.5 to about 10 atm (e.g., 0.5 atm, 1 atm, 2 atm, 3 atm, 4 atm, 5 atm, 6 atm, 7 atm, 8 atm, 9 atm, or 10 atm).

In some embodiments, the concentrated vapor comprises (v/v) about 2% to about 99% CO₂, about 2% to about 95% CO₂, about 2% to about 90% CO₂, about 2% to about 85% CO₂, about 2% to about 80% CO₂, about 2% to about 75% CO₂, about 2% to about 70% CO₂, about 2% to about 65% CO₂, about 2% to about 60% CO₂, about 2% to about 55% CO₂, about 2% to about 50% CO₂, about 2% to about 45% CO₂, about 2% to about 40% CO₂, about 2% to about 35% CO₂, about 2% to about 30% CO₂, about 2% to about 25% CO₂, about 2% to about 20% CO₂, about 2% to about 15% CO₂, about 2% to about 10% CO₂, about 2% to about 5% CO₂, or any range or value therein. In some embodiments, the concentrated vapor comprises (v/v) about 2% CO₂, about 5% CO₂, % CO₂, about 10% CO₂, about 15% CO₂, about 20% CO₂, about 25% CO₂, about 30% CO₂, about 35% CO₂, about 40% CO₂, about 45% CO₂, about 50% CO₂, about 55% CO₂, about 60% CO₂, about 65% CO₂, about 70% CO₂, about 75% CO₂, about 80% CO₂, about 85% CO₂, about 90% CO₂, about 95% CO₂, about 96% CO₂, about 97% CO₂, about 98% CO₂, about 99% CO₂, or greater, or any range or value therein between. In some embodiments, the concentrated vapor comprises (v/v) greater than or equal to about 4% CO₂. In some embodiments, the concentrated vapor comprises (v/v) greater than or equal to about 5% CO₂. In some embodiments, the concentrated vapor comprises (v/v) greater than or equal to about 10% CO₂. In some embodiments, the concentrated vapor comprises (v/v) greater than or equal to about 15% CO₂.

A proof-of-concept of an electrochemical pH-swing system is disclosed in U.S. patent application Ser. No. 17/722,036, filed Apr. 15, 2022, which is hereby incorporated by reference in its entirety, including pages 7-10 and FIG. 4.

Flowing the Concentrated Vapor Through a Gas Processing Unit

In some embodiments, methods according to the present disclosure include a method or step of flowing the concentrated vapor produced in the CO₂ absorption step discussed above through a gas processing unit, also shown in FIG. 1. In some embodiments, the method or step of flowing the concentrated vapor through the gas processing unit includes adjusting the temperature, relative humidity, and flow rate of the concentrated vapor. In some embodiments, the temperature of the concentrated vapor may be adjusted to be in a range of about 15° C. to about 100° C. (e.g., 15° C., 25° C., 35° C., 45° C., 55° C., 65° C., 75° C., 85° C., 95° C., or 100° C., inclusive). In some embodiments, the relative humidity of the concentrated vapor may be adjusted to be in a range of about 0% to about 95% (e.g., 0%, 10%, 20%, 30%, 40%, 50%, 60%, 70%, 80%, 90%, or 95%, inclusive). In some embodiments, the flow rate of the concentrated vapor may be adjusted to be in a range of about 50 SCFM to about 5000 SCFM (e.g., 50 SCFM, 100 SCFM, 500 SCFM, 1000 SCFM, 2500 SCM, or 5000 SCFM, inclusive).

Contacting the Concentrated Vapor in a Reaction Chamber

In some embodiments, methods according to the present disclosure include a method or step of contacting the concentrated vapor in a reaction chamber with a concrete component so as to form a low-carbon concrete product, as also shown in FIG. 1. In some embodiments, a carbonatable concrete mixture is provided in the reaction chamber. In some embodiments, the concrete mixture may be ordinary portland cement (OPC). In some embodiments, the concrete mixture may comprise at least one of portlandite (e.g., commercially-available “virgin” portlandite or portlandite residues), coal combustion residues, recycled concrete aggregates, slag, portland cement, lime, or natural alkaline rocks. In some embodiments, the concrete mixture may be processed by any suitable processing step, such as, but not limited to, concrete batching, mixing, and forming.

In some embodiments, the concrete mixture may then be hydrated so as to form a concrete component. In some embodiments, a cementitious slurry is formed. In some embodiments, the cementitious slurry contains a concrete component. In some embodiments where the concrete mixture is portland cement, the concrete component comprises virgin portlandite or portlandite residues. The cementitious slurry may formed by combining water and a binder including the concrete component, and optionally cement and coal combustion residues (e.g., fly ash) at a water-to-binder mass ratio (w/b) of about 0.5 or less, about 0.45 or less, about 0.4 or less, about 0.35 or less, about 0.3 or less, about 0.25 or less, about 0.2 or less, about 0.15 or less, about 0.1 or less, or any range or value therein between. In some embodiments, forming the cementitious slurry includes combining water and a binder including a cement, virgin portlandite or portlandite residues, and coal combustion residuals.

Coal combustion residues may include coal ash and can include components such as those residuals produced when coal is burned by power plants. Coal ash may comprise at least one of fly ash, bottom ash, and boiler slag. Fly ash may generally comprise silica and can be made from the burning of finely ground coal.

In some embodiments, forming the cementitious slurry may include drying the cementitious slurry. In some embodiments, the cementitious slurry may then be shaped by any suitable method, such as dry-casting, wet-casting, any combination thereof, or any other suitable method. Drying and/or shaping the cementitious slurry may reduce a fraction of pore volume that is saturated with liquid water (Sw) to less than 1, such as about 0.9 or less, about 0.8 or less, about 0.7 or less, about 0.6 or less, about 0.5 or less, about 0.4 or less, about 0.3 or less, 0.2 or less, and down to about 0.1, or any range or value therein between.

Systems

Also set forth herein are systems for implementing the methods disclosed herein.

In some embodiments, including any of the foregoing, set forth herein is a system for implementing a method or process disclosed herein. In some examples, the system includes a direct-air capture CO₂ system coupled to a carbonation chamber.

In some embodiments, including any of the foregoing, the system further comprises a pH swing.

In some embodiments, including any of the foregoing, the system further includes a gas processing unit configured to adjust at least one of a temperature, a relative humidity, or a flow rate of a concentrated vapor containing CO₂.

In some embodiments, including any of the foregoing, the system includes concrete components inside the carbonation chamber.

In some embodiments, including any of the foregoing, the system includes concrete components are arranged in a periodic manner.

In some embodiments, including any of the foregoing, the system includes concrete components are arranged to minimize turbulent air flow.

In some embodiments, including any of the foregoing, the system includes concrete components are arranged to maximize carbonation rates.

In some embodiments, including any of the foregoing, the system includes a device for fractionally enriching the concentration of CO₂ in the concentrated vapor containing CO₂.

In some embodiments, including any of the foregoing, the system includes at least one ion exchange membrane.

EXAMPLES

Example 1

In some embodiments, the concentrated vapor obtained by DAC systems and adjusted through the gas processing unit may then contact the concrete component. In some embodiments, the concrete component comprises portlandite which readily carbonates in dilute CO₂ streams with greater than 2% CO₂ (v/v) at ambient pressure and ambient temperature, forming calcium carbonate. As shown in FIGS. 2A and 2B, reaction kinetics of portlandite is largely independent of CO₂ concentration when CO₂ concentration is greater than or equal to 2% (v/v) which allows for integrating a simple and cost-effective DAC system for the CO₂ mineralization process in concrete to supply dilute CO₂ streams when CO₂ emitters and precast concrete plants are not co-located. FIG. 2b also shows a larger increase in reactant conversion between 2% CO₂ and 5% CO₂. The difference in reactant conversion above 5% is less than the difference between 2% CO₂ and 5% CO₂ for exposure times less than about 7 hours. At longer exposure time periods, e.g., at 25 hours, FIG. 2A shows that 2% CO₂ and 5% CO₂ have about the same reactant conversion fraction as does 65% CO₂. FIG. 2B demonstrates that low concentration CO₂ (e.g., 2% to 5% CO₂) from DAC is suitable for achieving high reactant conversion fractions. FIGS. 2A and 2B were previously published in Falzone, G., Mehdipour, I., Neithalath, N., Bauchy, M., Simonetti, D., & Sant, G. (2021). New insights into the mechanisms of carbon dioxide mineralization by portlandite. AIChE Journal, 67(5), e17160, the entire contents of which are herein incorporated by reference in its entirety for all purposes.

FIG. 2A shows a conversion-time profile plot of portlandite particles exposed to gas streams conditioned to varying CO₂ concentrations [CO₂] (% v/v) at a temperature of 65° C., relative humidity of 80%, and a 2 slpm flow rate. The data in the plot in FIG. 2A is fitted to Equation (7) below:

$\begin{array}{cc}X\left(t\right)=X_f\frac{\mathrm{kt}}{X_f+\mathrm{kt}}& \left(7\right)\end{array}$

Equation 7 is used to estimate the final conversion fraction X_f and the apparent first-order rate constant of carbonation k [s⁻¹]. The conversion reaction kinetics of the portlandite is largely independent of CO₂ concentration when CO₂ concentration is greater than or equal to 5% (v/v).

FIG. 2B shows a conversion curve plot between inverse time and inverse conversion. FIG. 2B shows stronger bi-linearity as the CO₂ concentration is reduced. Data at atmospheric CO₂ concentration (about 0.04% (v/v)) is not shown. A steeper slope of the curve fits indicates a smaller carbonation rate constant. Therefore, conversion reaction kinetics of the portlandite is largely independent of CO₂ concentration when CO₂ concentration is greater than or equal to 5% (v/v). When CO₂ concentration is less than 5% (v/v), the conversion reaction kinetics (such as the rate constant k) is largely dependent on the CO₂ concentration.

Example 2

FIG. 3A shows the batch-wise trends for CO₂ uptake and CO₂ utilization efficiency of produced concrete masonry blocks at a first facility from the CO₂ mineralization process discussed above. In FIG. 3A, all of the batches used a coal-fired flue gas stream with an average CO₂ concentration of about 12% (v/v). Twelve production runs were demonstrated at the first facility. The system's performance fulfilled all design specifications including: (i) CO₂ utilization efficiency greater than 75% (mass basis); (ii) CO₂ uptake greater than 0.25 tonnes per batch; and (iii) product compliance with industry construction standards.

Concrete blocks were composed of cement, fly ash, portlandite and aggregates.

Portlandite was the primary reactant in concrete block to absorb CO₂. Each batch included substantially the same starting materials.

FIG. 3B shows the batch-wise trends for CO₂ uptake and CO₂ utilization efficiency of produced concrete masonry blocks at a second facility from the CO₂ mineralization process discussed above. In FIG. 3B, the ITC batch represents the first facility with an average CO₂ concentration of about 12% (v/v). Batches N1, N2, N3, and N6 used coal flue gas with an average CO₂ concentration of about 12% (v/v). Batches N4 and N5 used natural gas flue gas with an average CO₂ concentration of about 4% (v/v). As shown, batches N4 and N5 demonstrate a lower CO₂ uptake and a lower CO₂ utilization efficiency in comparison to most of the other batches, with the exception of batch N1. A similar CO₂ utilization efficiency was achieved in the second facility as was achieved in the first facility. Further, both facilities demonstrated fulfilled performance metrics using a “direct CO₂ utilization” process without any carbon capture and clean-up steps at ambient pressure which confirms the viability of the CO₂ mineralization process disclosed above using very dilute CO₂ streams such as natural gas flue gas streams.

Concrete blocks were composed of cement, fly ash, portlandite and aggregates. Portlandite was the primary reactant in concrete block to absorb CO₂. Batches N1, N2, N3, and N6 used coal flue gas with an average CO₂ concentration of about 12% (v/v). Batches N4 and N5 used natural gas flue gas with an average CO₂ concentration of about 4% (v/v).

Example 3

A model was developed to calculate the conversion of the solid phase (Ca(OH)₂ to CaCO₃ after 24 hours of carbonation. Ca(OH)₂ is an equivalent material for modeling concrete formation. The relationship between processing conditions ([CO₂ concentration, Relative Humidity, Temperature) is shown in FIG. 4, for [CO₂]=4% v/v; and FIG. 5, for [CO₂]=9% v/v. The results show the improved conversion of the solid material and therefore greater CO₂ uptake by increasing the CO₂ concentration in the reactor. The model is valid for 2-to-16% v/v CO₂.

A parametric approach was followed to systematically evaluate the influence of processing conditions on the conversion of the solid phase of the dry-cast concrete from available Ca(OH)₂ to CaCO₃. An experimental matrix covering a combination of operating conditions within the ranges of 20° C.<temperature<65° C., 10%<relative humidity<80% and 4%<CO₂<14% (v/v) was developed to produce a model. The model determines the total conversion to CaCO₃ based on the operating conditions. The maximum theoretical CaCO₃ formation was calculated based on the mixture design of the concrete and the stoichiometric maximum CaCO₃.

Dry-cast concrete was mixed at a low water to cement (w/c) ratio (i.e., zero slump) then consolidated by mechanical compaction. The concrete mixture was placed in a metal mold and a 15 MPa compaction stress was applied at a loading rate of 0.9 kN/s followed by holding the stress for 15 seconds before removing the compaction stress. After that, the compacted concrete sample was removed from the mold to undergo curing. USP grade CO₂ (purity >99.5%) and compressed air were mixed and regulated using mass flow controllers to achieve a specific CO₂ concentration in the gas stream for the bench-scale carbonation reactor. The relative humidity was controlled by bubbling the gas through two wash bottles placed in series (within oven #1) as shown in FIG. 8. The temperature of oven #1 was adjusted to reach the desired gas relative humidity. The humidified flue gas was then streamed to a reactor that contained the concrete samples and placed in oven #2 to control the temperature.

To quantify the carbonation in the concrete, a powder was extracted from the concrete at 24 hours of carbonation. The powder collected was analyzed by thermogravimetric analysis (TGA) using an STA 6000 (Perkin Elmer). A temperature range of 35 to 950° C. using a heating rate of 15° C./min with ultra-high purity N2 gas (purity >99.99%) purge at a 20 mL/min flow rate was used. The CO₂ content (mass % of total solids) in the sample was quantified by using the following equation to calculate the difference in the residual mass at a temperature range between 600 to 900° C. at which mineral carbonates (such as CaCO₃) decompose. See, as background, S. Maheswaran, A. Ramachandra Murthy, V. Ramesh Kumar, A. Karunanithi, Characterisation studies on the particle size effect of calcium carbonate in high-strength concrete, Magazine of Concrete Research. 73 (2021) 661-673. https://doi.org/10.1680/jmacr.19.00375; N. Vogler, P. Drabetzki, M. Lindemann, H.-C. Kane, Description of the concrete carbonation process with adjusted depth-resolved thermogravimetric analysis, J Therm Anal calorim. 147 (2022) 6167-6180. https://doi.org/10.1007/s10973-021-10966-1:

$\begin{array}{cc}{m}_{CO2}=\frac{m_{\left(600-900°C.\right)}}{m_{\mathrm{solid}}}\times 100& \mathrm{Eq}.3\end{array}$

where m_CO2 is the mass percentage of CO₂ determined from TGA (mass %), m_{(600-900 ° C.)} is the mass loss between 600 to 900° C. (mg), and m_solid is the mass of the solid sample (mg). The initial content of CO₂ in the pre-carbonated samples was subtracted from the post-carbonation samples to account for CO₂ that was formed during the carbonation process. The total CaCO₃ formed from the carbonation process was divided by the maximum possible CaCO₃ formation to determine the total conversion of the solid material.

Example 4

The Example shows that early age carbonation curing results in an increase in volume of reaction products by about 10% which reduces the porosity and enhances the mechanical properties and durability of the concrete.

Porosity reduction of carbonated versus non-carbonated concrete samples dependent on CO₂ uptake is shown in FIG. 6. There is clear increased volume reduction with increased CO₂ uptake by at least 13.2%. The samples tested had varied mixture designs of portlandite, class C fly ash and Portland cement. The samples were carbonated at 50° C., 14 v/v % CO₂ and 10% RH for 24 hours. The samples included portlandite, cement, fly ash and aggregates. The strength improvements from carbonation increased from 6.8-to-37.9% depending on the mixture design. See FIG. 7.

Example 5

Rate constants of portlandite carbonation as particulates as a function of CO₂ concentration after 24 hours of carbonation are shown below in Table 1. See, for example, G. Falzone, I. Mehdipour, N. Neithalath, M. Bauchy, D. Simonetti, G. Sant, New insights into the mechanisms of carbon dioxide mineralization by portlandite, AIChE J. 67 (2021). https://doi.org/10.1002/aic.17160), which is incorporated by reference in its entirety for all purposes.

Rate constants of portlandite carbonation within concrete mixtures as a function of CO₂ concentration after 24 hours of carbonation are shown below in Table 2.

Tables 1 and 2 shows the apparent rate constant in terms of the conversion of solid material. Tables 1 and 2 show the benefit of a high relative humidity (80%) for CO₂ concentrations of 2% or greater including 2%, 5%, 12%, 25%, and 65% v/v.

The data in this Example is for portlandite particles. Unlike concrete, higher RH results in a greater carbonation rate constant for particles. See FIG. 1(a) in Falzone, Gabriel, Iman Mehdipour, Narayanan Neithalath, Mathieu Bauchy, Dante Simonetti, and Gaurav Sant. “New insights into the mechanisms of carbon dioxide mineralization by portlandite.” AIChE Journal 67, no. 5 (2021): e17160; doi.org/10.1002/aic.17160, the entire contents of which are herein incorporated by reference in its entirety for all purposes, which demonstrates this.

Conversion of the portlandite particles and concrete at time t (s), was calculated using Eq. 2:

$\begin{array}{cc}X\left(t\right)=Xf\frac{kt}{Xf+kt}& \mathrm{Eq}.2\end{array}$

Where X(t) is the conversion at time t, Xf is the final conversion for given operating conditions, t is time (s) and k is the rate constant (s⁻¹).

TABLE 1
Carbonation rate constants for portlandite particles as a function of CO2
concentration for reactor conditions at 65° C. and 80% RH
CO2 concentration
(v/v %) Apparent rate constant (s−1)
0.04    1.31E−06
2       1.37E−04
5       1.57E−04
12      2.49E−04
25      3.13E−04
65      3.00E−04

TABLE 2
Carbonation rate constants for portlandite within concrete
mixtures at 65° C. and 10% RH.
CO2 concentration
(v/v %) Apparent rate constant (s−1)
4       5.98E−05
9       7.65E−05
14      9.00E−05

The following references may be relevant for background purposes. 1. Keith, D. W.; Holmes, G.; St. Angelo, D.; Heidel, K. A Process for Capturing CO₂ from the Atmosphere. Joule 2018, 2 (8), 1573-1594. 2. Keith, D. W.; Ha-Duong, M.; Stolaroff, J. K. Climate Strategy with CO₂ Capture from the Air. Clim. Change 2006, 74 (1), 17-45. 3. Sakwattanapong, R.; Aroonwilas, A.; Veawab, A., Behavior of Reboiler Heat Duty for CO₂ Capture Plants Using Regenerable Single and Blended Alkanolamines. Ind. Eng. Chem. Res. 2005, 44, 4465-4473. 4. Feng, B.; Du, M.; Dennis, T. J.; Anthony, K.; Perumal, M. J., Reduction of Energy Requirement of CO₂ Desorption by Adding Acid into CO₂-Loaded Solvent. Energy & Fuels 2010, 24 (1), 213-219. 5. Dutcher, B.; Fan, M.; Russell, A. G., Amine-Based CO₂ Capture Technology Development from the Beginning of 2013—A Review. ACS Appl. Mater. Interfaces 2015, (7), 2137-2148. 6. MacDowell, N.; Florin, N.; Buchard, A.; Hallett, J.; Galindo, A.; Jackson, G.; Adjiman, C. S.; Williams, C. K.; Shah, N.; Fennell, P., An Overview of CO₂ Capture Technologies. Energy Environ. Sci. 2010, 3, 1645-1669.

Other embodiments are set forth in the following claims.

The embodiments and examples described above are intended to be merely illustrative and non-limiting. Those skilled in the art will recognize or will be able to ascertain using no more than routine experimentation, numerous equivalents of specific compounds, materials and procedures. All such equivalents are considered to be within the scope and are encompassed by the appended claims. In particular, while certain methods may have been described with reference to particular operations performed in a particular order, it will be understood that these operations may be combined, sub-divided, or re-ordered to form an equivalent method without departing from the teachings of the disclosure. Accordingly, unless specifically indicated herein, the order and grouping of the operations is not a limitation of the disclosure. It should be understood by those skilled in the art that various changes may be made and equivalents may be substituted without departing from the true spirit and scope of the disclosure as defined by the appended claims. In addition, many modifications may be made to adapt a particular situation, material, composition of matter, method, operation or operations, to the objective, spirit and scope of the disclosure. All such modifications are intended to be within the scope of the claims appended hereto.

Claims

1. A method of forming a concrete product, the method comprising: capturing CO2 from a gas source, the capturing comprising: contacting the gas source with an absorption solution having a solvent and a solute, wherein the solvent and/or the solute are capable of reacting with CO2 to form an anionic compound;adjusting the pH of the absorption solution electrochemically to less than about 7 to release the CO2 as a concentrated vapor containing CO2;collecting the concentrated vapor containing CO2;regenerating the solvent and/or the solute; andflowing the concentrated vapor containing CO2 through a gas processing unit to adjust at least one of a temperature, a relative humidity, or a flow rate of the concentrated vapor containing CO2; andcontacting the concentrated vapor containing CO2 with a concrete component.

2. The method of claim 1, wherein the concentrated vapor comprises about 2-99% (v/v) CO2.

3. The method of claim 1, wherein the concentrated vapor comprises greater than or equal to 2% (v/v) CO2.

4. The method of claim 1, wherein the concentrated vapor comprises less than or equal to 5% (v/v) CO2.

5. The method of claim 1, wherein the concentrated vapor comprises 2.0% to 5.0% (v/v) CO2.

6. The method of claim 1, wherein the concentrated vapor comprises 2.0, 2.5, 3.0, 3.5, 4.0, 4.5, or 5.0% (v/v) CO2.

7. The method of claim 1, wherein the concentrated vapor containing CO2 has a relative humidity that ranges from 5% to 90%.

8. (canceled)

9. The method of claim 1, wherein the concentrated vapor containing CO2 has a temperature that ranges from 20° C. to 80° C.

10. (canceled)

11. The method of claim 1, wherein collecting the concentrated vapor containing CO2 comprises fractionally enriching the concentration of CO2 in the concentrated vapor containing CO2.

12. The method of claim 1, wherein the absorption solution comprises one or more amines.

13. (canceled)

14. The method of claim 1, wherein contacting the concentrated vapor containing CO2 with the concrete component further comprises: providing a carbonatable concrete mixture comprising the concrete component;hydrating the carbonatable concrete mixture, reacting the carbonatable concrete mixture, or both hydrating and reacting the carbonatable concrete mixture to form the concrete component; andcontacting the concrete component with the concentrated vapor containing CO2 to harden the concrete mixture via the formation of carbonate minerals to form a concrete product.

15.-16. (canceled)

17. The method of claim 1, wherein the gas source is an effluent from an industrial source, an atmospheric source, a commercially-available CO2 source, or liquefied CO2.

18. (canceled)

19. The method of claim 1, wherein adjusting the pH of the absorption solution occurs at ambient temperature.

20.-21. (canceled)

22. The method of claim 1, wherein the concentrated vapor containing CO2 is not stored.

23. The method of claim 1, wherein adjusting the pH of the absorption solution electrochemically to less than about 7 to release the CO2 as a concentrated vapor containing CO2 comprises using a pH swing induced by water electrolysis in a cell that incorporates at least one ion exchange membrane.

24. The method of claim 1, further comprising collecting the regenerated solvent and/or solute.

25.-26. (canceled)

27. A concrete product formed by the method of claim 1.

28. (canceled)

29. A system comprising a direct-air capture CO2 system coupled to a carbonation chamber.

30. The system of claim 29, wherein the system further comprises a pH swing.

31. The system of claim 29 or 30, further comprising a gas processing unit configured to adjust at least one of a temperature, a relative humidity, or a flow rate of a concentrated vapor containing CO2.

32.-37. (canceled)