PROCESS FOR SYNTHESIZING ZWITTERIONIC BASES, ZWITTERIONIC BASES, PROCESS FOR CAPTURING CO2 AND USE

Abstract

The present invention relates to a process for capturing CO2 on a large scale using aqueous solutions of zwitterionic bases by contacting a gas stream containing one or more acid gases with said solutions. The internal salts obtained in the present invention have the advantage of not being volatile, being less susceptible to chemical and thermal decomposition, and also have lower absorption enthalpy. The present invention can be used in various industry sectors, such as in the energy sector, for capturing CO2 from exhaust gases, in the chemical sector, for removing CO2 from the gas streams of catalytic processes in which the CO2 can poison the catalysts, and, in particular, in the oil and gas sector, for purifying natural gas.

Description

FIELD OF THE INVENTION

The present invention addresses to cyclic sorption/desorption processes for the capture or purification of gaseous streams containing acidic gases using solutions of organic salts, herein called zwitterionic bases, with application in the energy, chemical and oil and gas fields in order to minimize the main intrinsic drawbacks in large-scale CO₂ and H₂S capture processes.

DESCRIPTION OF THE STATE OF THE ART

The processes for capturing acidic gases, such as carbon dioxide (CO₂) and hydrogen sulfide (H₂S) are used in various industrial segments both for environmental reasons and for economic reasons, as they are used, for example, to obtain products with a higher added value or to purify the gaseous feed streams of catalytic reactors. These processes are especially important in the oil and gas industry, where they are used to remove CO₂ and H₂S from natural gaseous streams from oil extraction plants.

One of the widely disseminated technologies for the separation of CO₂ and H₂S from natural gas is based on the reversible absorption of these gases using aqueous solutions of ethanolamines such as, for example, methyldiethanolamine (MDEA). The use of amines, although effective, presents some intrinsic problems, the main ones being related to the volatility of these compounds, which causes mass loss of the absorbent agent during the process, the relative high enthalpy of absorption and their gradual thermal and chemical decomposition for the formation, for example, of carbamates. These drawbacks motivated the search for new compounds to replace amines both in new plants and in existing plants for capturing CO₂ and H₂S.

The main strategy studied to increase chemical and thermal stability, eliminate the mass loss by evaporation and reduce the enthalpy of absorption of the acidic gas capture processes has been the use of ionic compounds and their solutions. There is a growing number of publications reporting the use of ionic liquids (ILs), ionic liquid solutions or organic salt solutions in CO₂ absorption processes.

In one of the first studies that demonstrated the solubility of CO₂ in ionic liquids, BLANCHARD, L. A. et al. “Processing using ionic liquids and CO₂”, Nature, v. 399, p. 28-29, 1999 reported molar fractions of up to 0.72 moles of CO₂ for each mole of 1-butyl-3-methyl-imidazolium hexafluorophosphate (BMIm·PF6) under pressures of 83 bar (8.3 MPa). Since then, numerous publications have demonstrated that CO₂ is remarkably soluble in ILs based on imidazolium cations, as described in the references of ANTHONY, J. L.; MAGINN, E. J.; BRENNECKE, J. F. “Gas solubilities in 1-n-butyl-3-methylimidazolium hexafluorophosphate”, Ionic liquids, p. 260-269, 2002; Cadena, C., et al. “Why is CO₂ so soluble in imidazolium-based ionic liquids?”, Journal of the American Chemical Society, v. 126, p. 5300-5308, 2004; BARA, J. E. et al. “Room-temperature ionic liquids and composite materials: platform technologies for CO₂ capture”, Accounts of Chemical Research, v. 43, p. 152-159, 2010; HASIB-UR-RAHMAN, M. et al. “Ionic liquids for CO₂ capture—Development and progress”, Chemical Engineering and Processing: Process Intensification, v. 49, p. 313-322, 2010; BRENNECKE, J. F.; GURKAN, B. E. “Ionic Liquids for CO₂ Capture and Emission Reduction”, The Journal of Physical Chemistry Letters, v. 1, p. 3459-3464, 2010; SHARMA, P. et al. “Effects of anions on absorption capacity of carbon dioxide in acid functionalized ionic liquids”, Fuel Processing Technology, v. 100, p. 55-62, 2012; ZHANG, X. et al. “Carbon capture with ionic liquids: overview and progress”, Energy & Environmental Science, v. 5, p. 6668-6681, 2012. The absorption of CO₂ in ionic liquids can occur either by physisorption or by chemisorption, or by a combination thereof. The physical absorption, or gas solubility, is influenced by a number of factors such as free volume, counterion size, strength of cation-anion interactions, pressure, temperature, and structural changes in the ionic pair. The chemisorption is normally influenced by the basicity of the salt and leads to the capture of CO₂ by the formation of species such as bicarbonate and carbamate. Therefore, when using ionic liquids or functionalized organic salts with basic groups, it is expected to combine the effects of physical and chemical absorption.

In a recent literature review, CUI, G. et al., “Active chemisorption sites in functionalized ionic liquids for carbon capture”, Chemical Society Reviews, v. 45, p. 4307-4339, 2016 report the existence of at least 77 different amino-functionalized ionic liquids, 102 ionic liquids free of the amine group (including those that use the phenolate anion) and 55 ionic liquids with multiple active sites that were used to capture CO₂. Although these ionic liquids have interesting properties, so far there is no proof of the industrial viability of these compounds, due to several factors such as, for example, high viscosity, complexity of synthesis processes, incompatibility with water.

In the specific case of amino-functionalized ionic liquids, the advantage over alkanolamines is related only to the low volatility of these compounds. This advantage is not enough to compensate the disadvantages related to its high viscosity and cost, mainly because, as they have the same functional group, they do not represent gains in thermal and chemical stability.

Ionic liquids with alternative functional groups, specifically the phenolate anion, draw attention because they eliminate decomposition via the formation of carbamates; however, in the presence of water or another source of protons, the phenolate is converted to phenol, a volatile and toxic compound, making its industrial use unfeasible.

The alternative to the use of phenolate groups without the formation of volatile products is the use of inner salts. In the study by Sakai, T. et al. “Bifunctional organocatalyst for Activation of carbon dioxide and epoxy to produce cyclic carbonate: betaine as a new catalytic Motif”, Organic Letters, v. 12, p. 5728-5731, inner salts containing the phenolate anion covalently associated with quaternary ammonium-type cations have been reported. Such a study is focused on the nucleophilicity of these compounds for the formation of adducts with CO₂ that are intermediates in coupling reactions of carbon dioxide with epoxides for the formation of cyclic carbonates, without investigating absorption of CO₂ under industrial conditions with such compounds.

A method for removing CO₂ from exhaust gases using ionic liquids associated with anions containing carboxylate groups was disclosed by U.S. Pat. No. 7,527,775B2. More recently, U.S. Pat. No. 8,721,770 describes the use of functionalized ionic liquids in CO₂ capture. Although promising, the use of ionic liquids for CO₂ absorption has the inconvenience of the high viscosity of these compounds, which, in practice, would make pumping and flow of these compounds difficult in industrial pipes and would impair mass transfer in the liquid.

An evolution of these methodologies is the use of solutions, including aqueous solutions, of ionic liquids and other organic salts that have lower viscosity than pure ionic liquids and similar or even greater capture capacity. One of the most important methods in the field of the present discovery was disclosed in the U.S. Pat. No. 8,536,371B2, which refers to the use of aqueous solutions of amino-functionalized organic salts for the capture of CO₂.

Furthermore, in 2017, SIMON, N. M. et al. “Carbon dioxide capture by aqueous ionic liquid solutions”, ChemSusChem, v. 10, p. 4927-4933, 2017 reported, for example, the capture of CO₂ through aqueous solutions of ionic liquids containing imidazolium cations associated with acetate and imidazolate anions. Some other examples of CO₂ absorption methods by ionic compounds are reported in references US2005/0129598A1, U.S. Pat. No. 10,086,331B2, US2012/0063977A1, US2015/0314235A1, US2018/0179157A1 and WO2014/144523A3.

Document BR122012033196A2 refers to a method for absorbing CO₂ from a gaseous mixture, preferably a combustion exhaust gas containing from 1 to 60% by volume of CO₂, and also to the absorption medium and a device to perform the method, where absorption of CO₂ is carried out by contacting a gaseous mixture with an absorption medium comprising water and at least one amine. The method uses zwitterionic surfactants for CO₂ absorption, such as betaines, alkylglycines, sultaines, amphopropionates, amphoacetates, tertiary amine oxides and silicobetaines.

U.S. Pat. No. 8,741,246B2 discloses methods for preparing compositions in order to capture volatile compounds in industrial power generation and commercial natural gas production facilities. More specifically, systems for the reduction of volatile compounds, where the system comprises an N-functionalized imidazole and may optionally include an amine. The method uses the non-ionic N-functionalized imidazole under neutral conditions and about 20% to 80% by weight of the solvent system. In addition, this document discloses a process of absorption of CO₂ and other volatile compounds, such as H₂S, with the regeneration of N-functionalized imidazole through heating. However, the use of ethanolamine compounds, although effective, presents some intrinsic problems, the main ones being related to the volatility of these compounds, which causes mass loss of the absorbent agent during the process, the relative high enthalpy of absorption and its gradual thermal and chemistry decomposition for the formation.

Document U.S. Pat. No. 9,586,175B2 discloses a process for separating at least a portion of an acidic gas from a gaseous mixture, comprising contacting the gaseous mixture with an absorption medium and/or adsorption medium, being carried out in the presence of an acidic catalyst. The described absorption and regeneration method uses zwitterionic substances providing compositions, devices and apparatus for capturing acidic gases, such as carbon dioxide (CO₂), from flue gas flows, reform gas flows, natural gas flows or other industrial gas flows.

The study by YEBEDRI, S. et al. “Characterizations of crystalline structure and catalytic activity of zwitterionic imidazole derivatives”, Journal of Molecular Structure, v. 1193, p. 45-52, 2019 discloses the synthesis of a zwitterionic imidazole derivative and studies of catecholase activity by copper complexes in situ. Such a study focuses on the characterization of the crystalline structure and its catalytic activity, not being used on an industrial scale in the absorption of CO₂.

Thus, no document of the state of the art discloses a process for capturing CO₂ through solutions of zwitterionic bases such as that of the present invention.

In order to solve such problems, the present invention was developed, by obtaining a very specific family of organic salts, whose aqueous solutions have low viscosity and molar absorption capacity similar to conventional absorbents, such as MDEA, with the advantage of not being volatile, being less susceptible to chemical and thermal decomposition, as well as having a lower enthalpy of absorption. Such unique characteristics make them different from the aforementioned examples or from any other compound already used for the capture of acidic gases, especially carbon dioxide and hydrogen sulfide.

The present invention results in economic advantages when compared to traditional processes that use MDEA, such as, elimination of costs corresponding to the evaporation of the absorbent species, since the zwitterionic bases, as well as their conjugated acids, are not volatile; the reduction of about 20% of energy required for the desorption processes with zwitterionic solutions and the functional groups of the zwittwerions are extremely robust.

In addition, the invention has environmental and safety advantages that are related to the non-volatility of the inner salts, thus eliminating risks of possible human and environmental contaminations.

BRIEF DESCRIPTION OF THE INVENTION

The present invention addresses to the discovery of a family of inner salts with a basic character, whose solutions are used in cyclic processes of gas capture on a large scale, through the contact of a gaseous stream containing one or more acidic gases with such solutions in order to minimize the main intrinsic inconveniences in large-scale CO₂ and H₂S capture processes.

These inner salts, or zwitterionic bases, can be combined with different solvents, including water, to obtain low viscosity solutions that have molar absorption capacity similar to conventional absorbents, such as MDEA, with the advantage of not being volatile, being less susceptible to chemical and thermal decomposition, in addition to having a lower enthalpy of absorption.

The present invention can be applied in several industrial segments, such as in the energy sector for capturing CO₂ from exhaust gases, in the chemical sector for removing CO₂ from gaseous streams of catalytic processes in which CO₂ can poison the catalysts and, especially, in the oil and gas sector for the purification of natural gas.

BRIEF DESCRIPTION OF THE DRAWINGS

The present invention will be described in more detail below, with reference to the attached figures which, in a schematic way and not limiting the inventive scope, represent examples of its embodiment. In the drawings there are:

FIG. 1 illustrating developed inner salts: A) 1,3-dimethyl-2-(3-oxy-phenyl)-imidazolium and B) 1,3-dimethyl-2-(4-oxy-phenyl)-imidazolium;

FIG. 2 illustrating the first step of the synthesis of the 1,3-dimethyl-2-(3-oxy-phenyl)-imidazolium (synthesis of 1-methyl-2(3-hydroxy-phenyl)-imidazole) inner salt;

FIG. 3 illustrating the second step of the synthesis of the 1,3-dimethyl-2-(3-oxy-phenyl)-imidazolium inner salt (synthesis of 1,3-dimethyl-2(3-hydroxy-phenyl)-imidazolium iodide);

FIG. 4 illustrating the ESI(+)MS spectrum of the 1,3-dimethyl-2(3-hydroxy-phenyl)-imidazolium iodide precursor for the synthesis of the 1,3-dimethyl-2-(3-oxy-phenyl)-imidazolium inner salt, where there are represented the simulated spectrum at the top and below the experimentally obtained spectrum;

FIG. 5 illustrating the third step of the synthesis of the 1,3-dimethyl-2-(3-oxy-phenyl)-imidazolium inner salt (synthesis of the 1,3-dimethyl-2-(3-oxy-phenyl)-imidazolium inner salt);

FIG. 6 illustrating the NMR spectrum of ¹H NMR (400 MHz, D₂O) of 1,3-dimethyl-2-(3-oxy-phenyl)-imidazolium inner salt;

FIG. 7 illustrating the ¹³C NMR spectrum (100 MHz, D₂O) of 1,3-dimethyl-2-(3-oxy-phenyl)-imidazolium inner salt;

FIG. 8 illustrating the infrared spectrum of 1,3-dimethyl-2-(3-oxy-phenyl)-imidazolium inner salt;

FIG. 9 illustrating the first step of the synthesis of the 1,3-dimethyl-2-(4-oxy-phenyl)-imidazolium (synthesis of 1-methyl-2-(4-hydroxy-phenyl)-imidazole) inner salt;

FIG. 10 illustrating the second step of the synthesis of the 1,3-dimethyl-2-(4-oxy-phenyl)-imidazolium inner salt (synthesis of 1,3-dimethyl-2-(4-hydroxy-phenyl)-imidazolium iodide);

FIG. 11 illustrating the third step of the synthesis of the 1,3-dimethyl-2-(4-oxy-phenyl)-imidazolium inner salt (synthesis of the 1,3-dimethyl-2-(4-oxy-phenyl)-imidazolium inner salt);

FIG. 12 illustrating the NMR spectrum of ¹H NMR (400 MHz, DMSO-d₆) 1,3-dimethyl-2-(4-oxyphenyl)-imidazolium inner salt;

FIG. 13 illustrating the ¹³C NMR spectrum (100 MHz, DMSO-d₆) 1,3-dimethyl-2-(4-oxy-phenyl)-imidazolium inner salt;

FIG. 14 illustrating the infrared spectrum of 1,3-dimethyl-2-(4-oxy-phenyl)-imidazolium inner salt;

FIG. 15 illustrating the experimental apparatus for sorption tests, where there are represented the following items: 401—CO₂ cylinder; 402—CO₂ reservoir with monitored pressure; 403—valve for pressure control in the sorption vessel; 404—jacketed sorption vessel; 405—purge valve; 406—purge gas; 407—thermostatic bath to control the temperature of the process; 408—magnetic stirrer; 409—Field Logger pressure recorder; and 410—computer for data storage and processing;

FIG. 16 illustrating the UV-VIS spectra of the aqueous solution of the 1,3-dimethyl-2-(3-oxy-phenyl)-imidazolium inner salt, solution after absorption and after desorption;

FIG. 17 illustrating the recyclability of the aqueous solution of 1,3-dimethyl-2-(3-oxy-phenyl)-imidazolium, where the reaction conditions are: 5 mL of solution with a concentration of 1 M, absorption temperature of 40° C. and pressure of 1.3 bar absolute (130 kPa); desorption temperature of 100° C. and atmospheric pressure; absorption values determined through the pressure drop in the reservoir and expressed in moles CO₂ per moles of absorbent; mean represents mean absorption value from cycles 2 to 27±standard deviation.

FIG. 18 illustrating the recyclability of the aqueous solution of 1,3-dimethyl-2-(4-oxy-phenyl)-imidazolium, where the reaction conditions are: 5 mL of solution with a concentration of 1 M, absorption temperature of 40° C. and pressure of 1.3 bar absolute (130 kPa); desorption temperature of 100° C. and atmospheric pressure; absorption values determined through the pressure drop in the reservoir and expressed in moles CO₂ per moles of absorbent; mean represents mean absorption value from cycles 2 to 17±standard deviation;

FIG. 19 illustrating the recyclability of the commercial MDEA/Piperazine aqueous solution, where the reaction conditions are: 5 mL of MDEA/piperazine/water 40%:10%:50% solution, absorption temperature of 40° C. and pressure of 1.3 bar absolute (130 kPa); desorption temperature of 100° C. and atmospheric pressure; absorption values determined through the pressure drop in the reservoir and expressed in moles CO₂ per moles of absorbent; mean represents mean absorption value from cycles 1 to 26±standard deviation;

FIG. 20 illustrating the experimental apparatus for estimating the enthalpy of absorption, where there are represented the following items: 301—O₂ cylinder; 302—CO₂ reservoir with monitored pressure; 303—CO₂ admission valve in the sorption vessel; 304—sorption vessel; 305—pressure transducer to monitor the pressure in the CO₂ reservoir; 306—pressure transducer to monitor the pressure of the sorption vessel; 307—Field Logger pressure data recorder; 308—computer for storing and processing data; 309—thermostatic bath to control the temperature of the system; 310—isochoric balance chamber; 311—vacuum pump; and 312—syringe for adding the sorbent solution;

FIG. 21 illustrating the process of absorption of acidic gases using zwitterionic bases, where there are represented the following items: 101—gaseous feeding; 102—absorption unit operating at T₁, P₁; 103—purified gaseous stream; 104—zwitterionic solution rich in absorbed acidic gases; 105—desorption unit operating at T₂, P₂; 106—gaseous stream rich in CO₂ and/or other acidic gases; and 107—regenerated zwitterionic solution;

FIG. 22 illustrating the family of inner salts of the present invention with predictable effect for acidic gas capture processes from the mere direct extrapolation of the state of the art;

FIG. 23 illustrating the process of synthesis of zwitterionic bases of the present invention;

FIG. 24 illustrating the family of inner salts obtained by the process of synthesis of zwitterionic bases of the present invention;

FIG. 25 illustrating the ionic liquids used as a solvent of general formula A⁺Z⁻ for preparing the solutions of zwitterionic bases of the present invention;

FIG. 26 illustrating an embodiment of acidic gas absorption process using zwitterionic bases for the purification of natural gas, where there are represented the following items: 201—gas feed; 202—absorption unit at T₁, P₁; 203—purified gaseous stream; 204—zwitterionic solution rich in absorbed acidic gases; 205—desorption unit operating at T₂, P₂; 206—gaseous stream rich in CO₂ and/or other acidic gases; 207—regenerated zwitterionic solution; 208—reboiler; and 209—heat exchanger.

DETAILED DESCRIPTION OF THE INVENTION

The process of synthesizing zwitterionic salts according to the present invention is characterized by comprising three very simple steps that occur successively promoting reactions between its components in the liquid phase, in the presence of solvent, under mechanical stifling, under pressure atmospheric and at temperatures between −10° C. and 100° C., typically between 0° C. to 70° C.

a) First Step

The first step is characterized by promoting the reaction between a compound of the hydroxy-benzaldehyde type with a primary amine of general formula R1-NH₂ for the formation of the corresponding imine, followed by the cyclization reaction of this imine, in the presence of a salt of ammonium and a vicinal dialdehyde, to obtain a compound of the 2-(hydroxy-phenyl)-imidazole type, according to Step 1—FIG. 23.

The first step is characterized by occurring at temperatures that can vary between −10° C. and 80° C., typically 0° C. to 40° C. and reaction times between 10 minutes and 24 hours, typically 24 hours.

The first step is characterized by the reaction product of the 2-(hydroxy-phenyl)-imidazole type being purified by simple techniques of precipitation, crystallization and/or filtration followed, or not, by washing and/or evaporation of the solvent.

The compound of the hydroxy-benzaldehyde type is characterized by containing, in its aromatic ring, at least one hydroxyl group and the other substituents of the benzene ring being hydrogen, alkoxy groups containing between 1 and 10 carbons, halides, phenyl or alkyl group or containing between 1 and 10 carbons, with 3-hydroxy-benzaldehyde and 4-hydroxy-benzaldehyde being typically used.

The primary amine of general formula R1-NH₂ is characterized in that the radical R1 comprises an alkyl, aryl, alkylether or alkylalcohol group containing between 1 and 10 carbons, typically methylamine, and in that being used in the proportion of 0.5 to 2 equivalents to benzaldehyde, typically 1.05 equivalents.

The ammonium salt is characterized by having the general formula (NH₄)_nY, where Y comprises the bromide, chloride, sulfate, acetate, carbonate and bicarbonate anions; n has a value of 1 or 2 and, because this salt is used in a proportion of 0.3 to 2 equivalents relative to the benzaldehyde, typically 0.75 equivalents.

Dialdehyde is characterized by being typically glyoxal and can also be analogues of glyoxal with alkyl, aryl, alkylether or alkylalcohol substituents containing 1 to 10 carbons and for being used in the proportion of 0.5 to 2 equivalents in relation to benzaldehyde, typically 1 equivalent.

The solvent used in the first step comprises water, acetonitrile, ethyl acetate, aliphatic alcohols containing from 1 to 10 carbons in the alkyl chain or a mixture of these in any proportion in the amount of 1 time to 100 times the mass of benzaldehyde, typically 10 times.

The purification of the reaction products of the first step is characterized by using water, acetonitrile, ethyl acetate, aliphatic alcohols containing from 1 to 10 carbons in the alkyl chain or a mixture of these in proportions suitable for, under temperatures of −10° C. to 30° C., typically 0° C., the precipitation or crystallization of compounds of the 2-(hydroxy-phenyl)-imidazole type is carried out followed by removal of the solvent by filtration or simple decantation, being recommended to wash the product with the same solvent and evaporating the residual solvent under reduced pressure.

b) Second Step

The second step is characterized by promoting the N-alkylation reaction between the compound of the 2-(hydroxy-phenyl)-imidazole type obtained in the previous step and an alkylating agent of general formula R9-X to form a salt of 2-(hydroxy-phenyl)-imidazolium, in the presence of solvent, according to Step 2—FIG. 23.

The second step is characterized by occurring at temperatures that can vary between 40° C. and 100° C., typically 70° C., and reaction times between 10 minutes and 24 hours, typically 1 hour.

The second step is characterized in that the reaction product of the 2-(hydroxy-phenyl)-imidazolium salt type precipitates as it is formed and is removed from the reaction mixture by filtration or decantation followed by washing and evaporation of the residual solvent under reduced pressure.

The alkylating agent of general formula R9-X is characterized in that R9 comprises an alkyl, arylalkyl, alkylether or alkylalcohol group containing between 1 and 10 carbons, and the X group comprises the halide, alkylsulfonate and alkylsulfate group, in which the alkyl group has between 1 and 5 carbons, typically iodomethane or methanesulfonyl chloride.

The solvent used in the second step comprises water, acetonitrile, ethyl acetate, aliphatic alcohols containing from 1 to 10 carbons in the alkyl chain or the mixture of these in appropriate proportions in the amount of 1 time to 20 times the mass of the compound of 2-(hydroxy-phenyl)-imidazole type, typically 5 times.

c) Third Step

The third step is characterized by promoting the deprotonation of the phenolic OH group of the 2-(hydroxy-phenyl)-imidazolium salt, obtained in the previous step, through the reaction of an aqueous solution of this component with a strongly basic ion exchange resin, which results in the formation of the inner or zwitterionic salt of the 2-(oxy-phenyl)-imidazolium type, as shown in Step 3—FIG. 23.

The third step is also characterized in that the reaction between the 2-(hydroxy-phenyl)-imidazolium salt and the ion exchange resin occurs by simply mixing and stifling these components for periods of up to 60 minutes, typically 10 minutes, or by passing a solution of the 2-(hydroxy-phenyl)-imidazolium salt through a fixed or fluidized bed column of resin at temperatures between 10° C. and 80° C., typically 30° C.

Furthermore, the third step is characterized in that the aqueous solution containing the product is separated from the ionic resin by filtration or simple decantation and the reaction product, inner salt of the 2-(oxy-phenyl)-imidazolium type, is isolated by simple evaporation of the solvent under reduced pressure and temperatures between 10° C. and 80° C., typically 40° C.

The zwitterionic bases obtained in the synthesis process disclosed herein have as their main structural characteristic the presence of an imidazolium cation covalently linked, through carbon C-2, to an oxy-phenyl group, having as possible substituents of the imidazolium ring, R₇ and R₈, hydrogen or alkyl, aryl, alkylether or alkylalcohol groups containing 1 to 10 carbons; and as substituents on the benzene ring, necessarily an O⁻ group, the others being hydrogen, hydroxyl, alkoxy groups containing between 1 and 10 carbons, halide, phenyl or alkyl group containing between 1 and 10 carbons, as shown in FIG. 24.

The zwitterionic bases obtained in the synthesis processes are neutral compounds that have opposite charges in different regions of their structure and can also be called inner salts or hybrid salts.

The zwitterionic bases obtained in the synthesis processes are solids soluble in water and polar organic solvents, such as alcohols, polyalcohols, acetonitrile and acetone.

Unlike most traditional zwitterions, which are amphoteric amino acids, the main property of zwitterionic bases is precisely the fact that they are basic inner salts, and have relatively high basicity, typical of the phenolate group, and may vary depending on the substituents of the benzene ring.

The zwitterionic bases have a unique characteristic for the process of capturing acidic gases, the fact that both they and their acid-conjugates are organic salts, therefore, non-volatile.

The key aspect of the zwitterionic bases disclosed herein is the presence of a phenolate group covalently linked to an imidazolium cation to form a basic salt with good solubility in water and polar solvents.

The process for capturing acidic gases through zwitterionic base solutions comprises contacting, under sorption conditions, a gaseous stream containing one or more acidic gases with a zwitterionic base sorbent solution for the removal of at least part of the acidic gases, and obtaining a purified gaseous stream and a solution with sorbed acidic gases; and the regeneration of the sorbent solution, under desorption conditions, to obtain a zwitterionic base solution and a stream of acidic gases.

FIG. 21 illustrates in a simplified way the continuous cyclic process of purification of a gaseous stream using solutions of zwitterionic bases. The feed stream 101 enters the sorption unit 102, which contains the zwitterionic base solution and whose temperature is controlled by heat extraction. In the sorption unit, the gaseous stream comes into contact with the zwitterionic base solution under temperature and pressure conditions (T1 and P1) so that at least part of the acidic gases contained in the feed stream is absorbed by the zwitterionic base solution, generating a purified gaseous stream 103 and a solution rich in sorbed acidic gases 104, which is conducted to the desorption unit 105. In the desorption unit, acidic gases are desorbed from the solution through appropriate temperature and pressure conditions (T2 and P2) generating a gaseous stream rich in acidic gases 106 and the regenerated zwitterionic base solution 107.

Conventional equipment can be used for the various functions necessary for the process of capturing acidic gases by solutions of zwitterionic bases, such as, for example, to control the gaseous flow, to promote contact between the gas and the sorbent solutions, for pumping the solutions between the sorption and desorption units, to promote heat exchanges between the process streams in such a way as to obtain an efficient cyclic process of capturing acidic gases.

FIG. 26 shows an embodiment of the cyclic capture process of acidic gases by solutions of zwitterionic bases in which heat exchangers are used between the sorption tower (scrubbing) and the desorption tower (stripping). This process is particularly suitable for the purification of natural gas. The stream of natural gas 201 containing acidic gases, especially CO₂ or H₂S, comes into contact with the zwitterionic base solution in a sorption tower 202, under temperature and pressure conditions (T₁ and P₁) typical for sorption, giving rise to the gaseous stream of purified natural gas 203 and a stream of saturated solution of acidic gases 204. The saturated solution of acidic gases is pumped to the regeneration (or desorption) tower, in which it is subjected to a temperature and pressure condition (T₂ and P₂), which favors the desorption of acidic gases generating a gaseous stream rich in acidic gases 206 and the regenerated zwitterionic base solution. The temperature in the regeneration tower is maintained by reboiler 208, which heats the regenerated zwitterionic base solution. A part of the regenerated solution 207 that passes through the reboiler is sent back to the sorption tower and another part returns to the desorption tower to maintain the temperature. The regenerated solution stream 207 exchanges heat by heating the solution stream saturated in acidic gases through heat exchanger 209.

The absorption step of the process promotes the direct or indirect contact, by means of contact membranes, of the gaseous feed stream, with zwitterionic solutions without concentration between 0.5 M and 7 M, temperatures (T₁) between 0° C. to 60° C. and pressures (P₁) between 1 and 150 bar absolute (100 kPa and 15 MPa), typically 40° C. and 1.3 bar to 3 bar absolute (130 kPa to 300 kPa).

The desorption step of the process promotes the regeneration of zwitterionic solutions by heating the solution rich in acidic gases at temperatures (T₂) greater than the absorption temperature (T₁) and/or through the use of pressures (P₂) lower than the absorption pressure (P₁), the desorption temperatures (T₂) being between 60° C. and 150° C. and the desorption pressures between 0 and 10 bar absolute (1 MPa), typically 100° C. and 1 bar absolute (100 kPa).

The process feed gaseous stream can be composed of any gaseous stream or gaseous mixture containing one or more acidic gases, such as carbon dioxide and hydrogen sulfide, in concentrations of 5% to 90%, typically streams of natural gas containing from 1% to 20% CO₂.

The zwitterionic solutions used in the capture process are any of those in which the zwitterionic base is dissolved in water, methanol, ethanol, isopropanol or other hydrocarbon, aliphatic alcohol having from 1 to 18 carbons in the alkyl chain, diols having from 2 to 5 carbon atoms or polyols having from 3 to 6 carbon atoms, ethylene glycol monoalkylethers of the formula H(OCH₂CH₂)_nOR₂, where n varies from 1 to 4 and R₂ consists of an alkyl group containing from 1 to 12 carbons or ionic liquids functionalized with the hydroxyl group as well as mixing these solvents in appropriate proportions, typically water, ethylene glycol, glycerol and ionic liquids functionalized with the hydroxyl group.

Ionic liquids functionalized with the hydroxyl group are compounds with the general formula A⁺Z⁻, wherein A⁺ represents a quaternary ammonium cation, an imidazolium cation, a pyridinium cation, a pyrrolidinium cation or a phosphonium cation, and Z⁻ represents susceptible anions to form a liquid salt with these cations at the absorption temperature.

The cations of ionic liquids include derivatives of the imidazolium cation, the pyridinium cation, the pyrrolidinium cation, the quaternary phosphonium cation or the quaternary ammonium in which, as shown in FIG. 25, the R₂₁, R₂, R₂₃, R₂₄, R₂₅ and R₂₆ substituents are H, alkylalcohols, alkylether, aryl or alkyl containing between 1 and 10 carbons in each of these groups, typically 1,2-dimethyl-3-(3-hydroxypropyl)-2,3-imidazolium.

The anions of ionic liquids include chloride, bromide, iodide, perchlorate, nitrate, tetrafluoroborate, tetrachloroborate, hexafluorophosphate, trifluoromethanesulfonate, bis(trifluoromethanesulfonyl)imidate, typically NTf₂⁻ and PF₆⁻.

From the mere direct extrapolation of the results disclosed herein, in particular, the results of example 3, example 4, example 5 and example 6 and example 7, it can be concluded that the zwitterionic bases have a predictable effect for capturing acidic gases and that have in their structure an organic cation covalently linked to a phenolate anion; therefore, the process of capturing acidic gases described herein is characterized by the zwitterionic base being an organic compound formed by the covalent association of quaternary ammonium, quaternary phosphonium, and pyridinium cations, pyrrolidinium or imidazolium with substituents, independent of each other, comprising hydrogen and alkyl, aryl, alkylether or alkylalcohol groups containing between 1 and 10 carbons, with the phenolate anion with substituents, independent of each other, comprising hydrogen, halides, phenyl, alkoxy containing between 1 and 10 carbons or alkyl containing between 1 and 10 carbons, according to FIG. 22, typically the zwitterionic bases are 1,3-dimethyl-2-(4-oxy-phenyl)-imidazolium and 1,3-dimethyl-2-(3-oxy-phenyl)-imidazolium.

The use of solutions, especially aqueous solutions, of the inner salts called herein zwitterionic bases, object of the present invention, minimizes the main intrinsic inconveniences of large-scale CO₂ capture processes based on aqueous solutions of ethanolamines, as follows:

• • I) The problems resulting from the loss of mass of the absorbents during the process, such as the increase in costs related to their replacement and the greater operational complexity, are completely solved by the fact that both the absorbent agents and the absorption products are ionic species and, therefore, have negligible vapor pressure;
  • II) The problems related to thermal and mainly chemical decomposition are minimized by the innovative use of the phenolate functional group in substitution of the amino group, which completely eliminates the decomposition via the formation of carbamates;
  • III) The costs associated with the energy expenditure of the process are minimized, as estimates suggest that the enthalpy of absorption using aqueous solutions of the inner salts described herein are about 20% lower than the enthalpy of absorption of aqueous solutions of MDEA;
  • IV) The process embodiment in which ionic liquids are used as solvents also eliminates energy losses resulting from solvent evaporation in the desorption process.

The zwitterion solutions containing the phenolate group, especially aqueous solutions, can be used in gas washing or scrubbing equipment, that is, in conventional equipment intended for the absorption of acidic gases by liquids.

Therefore, in addition to the various technical advantages, this technology is easy to implement, as it allows already-existing CO₂ absorption plants that use aqueous alkanolamine solutions, in particular, in CO₂ and H₂S removal plants from natural gas, are converted into absorption plants by zwitterionic base solutions without all the equipment having to be replaced, requiring only small adaptations, for example, to adjust the energy demand of the process.

EXAMPLE

For this work, the following tests were carried out, which represent examples of embodiment of the present invention.

Example 1: Synthesis of 1,3-dimethyl-2-(3-oxy-phenyl)-imidazolium inner salt (FIG. 1-A)

The synthesis of 1,3-dimethyl-2-(3-oxy-phenyl)-imidazolium inner salt is carried out in three steps. In the first step, 1-methyl-2(3-hydroxy-phenyl)-imidazole is obtained, as shown in FIG. 2.

In a reaction flask, methylamine (40% aqueous solution, 3.3 g; 42 mmol) was added over a solution of 3-hydroxy-benzaldehyde (4.88 g; 40 mmol) in 20 mL of methanol at room temperature. The exothermic reaction causes a slight heating of the reaction mixture and, then, the precipitation of the corresponding imine is observed. The suspension was stirred for another 10 minutes and then ammonium carbonate (2.88 g, 30 mmol) was added. The resulting mixture was cooled to 0° C. using an external ice-water bath. Glyoxal (40% aqueous solution, 5.8 g; 40 mmol) dissolved in 15 mL of CH₃OH was added slowly and under stirring. The reaction mixture was stirred for another 30 minutes at 0° C., generating a gradual dissolution of the solids. The ice bath was removed and the reaction was stirred for another 24 hours at room temperature, observing the precipitation of the desired reaction product. At the end, 15 mL of water were added to the suspension, the solid was filtered in a Büchner funnel, icy washed with CH₃OH/H₂O 1:1 and dried under reduced pressure. 2.69 g of a slightly yellowish solid were obtained (38.6% yield).

In the second step of the synthesis, 1,3-dimethyl-2(3-hydroxy-phenyl)-imidazolium iodide is obtained, as shown in FIG. 3. In a Schlenk flask, 40 mL of acetonitrile, 1-methyl-2-(3-hydroxy-phenyl)-imidazole (6.20 g; 35.6 mmol) and iodomethane (7.60 g; 53.4 mmol). The flask was closed with a rubber septum and the suspension was heated to 70° C., under stirring with the aid of a magnetic bar, for 1 hour. The solvent in the resulting brownish solution was evaporated to give a solid which was washed with ethyl acetate and then dried under reduced pressure. 10 g of brownish solid were obtained (88.9% yield) according to the ESI(+)-MS spectrum, as illustrated in FIG. 4.

In the third step of the synthesis, the 1,3-dimethyl-2-(3-oxy-phenyl)-imidazolium inner salt is obtained, as shown in FIG. 5. In a test tube, there was measured the volume of 14 mL of the ion exchange resin Ambersep 900 OH. The resin was washed three times with distilled water. Next, the resin was added to a solution of 1,3-dimethyl-2-(3-hydroxy-phenyl)-imidazolium iodide (3.16 g, 10.0 mmol) in 10 mL of water. The reaction remained under stirring at room temperature in a beaker for 10 minutes. After this time the ion exchange resin was separated by filtration, and the water in the solution was evaporated under reduced pressure, resulting in 1.8 g of a hygroscopic brown solid (96% yield). The 1 H NMR, ¹³C NMR, infrared spectra are presented, respectively, in FIG. 6, FIG. 7, and FIG. 8.

Example 2: Synthesis of 1,3-dimethyl-2-(4-oxy-phenyl)-imidazolium (FIG. 1-B)

The synthesis of 1,3-dimethyl-2-(4-oxy-phenyl)-imidazolium inner salt is carried out in three steps. In the first step, 1-methyl-2-(4-hydroxy-phenyl)-imidazole is obtained, as shown in FIG. 9.

Into a reaction flask, there was added at room temperature methylamine (40% aqueous solution, 3.30 g; 42 mmol) over a solution of 4-hydroxy-benzaldehyde (4.88 g; 40 mmol) in 30 mL of methanol. The reaction mixture warms up a little and is stirred for another 10 minutes. After that time, ammonium carbonate (2.88 g; 30 mmol) was added and to the resulting suspension there was added glyoxal (40% aqueous solution, 5.80 g; 40 mmol) dissolved in 15 mL of CH₃OH, slowly and under stirring. After the addition, the reaction mixture was stirred for another 2 hours at room temperature and then 60 mL of water were added, observing the precipitation of the desired reaction product. The solid was filtered on a Büchner funnel, cold washed with CH₃OH/H₂O 1:1 and dried under reduced pressure. 1.57 g of a slightly yellowish solid were obtained (22.5% yield).

In the second step of the synthesis, 1,3-dimethyl-2-(4-hydroxy-phenyl)-imidazolium iodide was obtained, as shown in FIG. 10. In a Schlenk flask, 12 mL of acetonitrile, 1-methyl-2-(3-hydroxy-phenyl)-imidazole (1.04 g; 6.00 mmol) and iodomethane (1.28 g; 9.00 mmol). The flask was closed with a rubber septum and the suspension was heated at 70° C., under magnetic stirring, for 1 hour. After this period, 5 mL of ethyl acetate was added and the resulting solid was filtered, washed with ethyl acetate and dried under reduced pressure. 1.65 g of brownish crystals were thus obtained (87% yield).

In the third step of the synthesis, the 1,3-dimethyl-2-(4-oxy-phenyl)-imidazolium inner salt was obtained, as shown in FIG. 11. In a test tube, there was measured the volume of 14 mL of the ion exchange resin Ambersep 900 OH. The resin was washed three times with distilled water. Then, the resin was added to a solution of 1,3-dimethyl-2-(3-hydroxy-phenyl)-imidazolium iodide (3.16 g; 10 mmol) in 10 mL of water. The reaction remained under stirring at room temperature in a beaker for 10 minutes. After this time, the ion exchange resin was separated by filtration, and the water in the solution was evaporated under reduced pressure, resulting in 1.8 g of a highly hygroscopic brownish solid (96% yield). The ¹H NMR, ¹³C NMR and infrared spectra are presented respectively in FIG. 12, FIG. 13 and FIG. 14.

Example 3: CO₂ absorption by aqueous solutions of the 1,3-dimethyl-2-(3-oxy-phenyl)-imidazolium and 1,3-dimethyl-2-(4-oxy-phenyl)-imidazolium inner salts at low pressure determined through the pressure drop in the CO₂ reservoir

The laboratory tests of absorption and desorption of CO₂ of the solutions of the inner salts were carried out in an experimental apparatus that allows the temperature and pressure of the sorption vessel to be kept constant while the pressure drop in a CO₂ reservoir is monitored for determining the amount of gas absorbed, as shown in FIG. 15.

To carry out the test, the reservoir with calibrated volume 402 is previously filled with CO₂ contained in the cylinder 401. The pressure control valve 403 is adjusted to maintain the pressure of the sorption vessel at 1.3 bar absolute (130 kPa) during the absorption test. The temperature of the sorption vessel 404 is adjusted by circulating, in its jacketed wall, thermal fluid from the thermostatic bath 407 to the absorption temperature (T1), typically 40° C. Then, 5 mL of 1 M aqueous solution of 1,3-dimethyl-2-(3-oxyphenyl)-imidazolium or 1,3-dimethyl-2-(4-oxy-phenyl)-imidazolium inner salt is added to the reaction vessel. The system was purged with CO₂ for 5 seconds by opening purge valve 406, and the reservoir 402 was refilled with CO₂ at 4 bar absolute (400 kPa). The absorption process begins when the magnetic stirrer 408 is activated and, from then on, the pressure drop in the CO₂ reservoir is monitored to determine the number of moles of CO₂ consumed. The pressure is monitored through a transducer installed in the CO₂ reservoir coupled to a recorder 409 and a computer 410 for data processing. For the calculations, the ideal gas equation of state and the previously calibrated volume of the reservoir were considered. The end of absorption was considered when the reservoir pressure as a function of time remained at an unchanged level for at least 10 minutes.

At the end of the absorption step, the sorption vessel 404 was opened and the temperature of the thermostatic bath 407 adjusted to the desorption temperature (T2), typically 100° C. The system was kept under stifling for 30 minutes to regenerate the zwitterionic solution. With the aim of validating the method and obtaining a parameter for comparison, the absorption test was carried out with the commercial mixture MDEA/piperazine/water normally used in industrial CO₂ absorption processes (Input 1, Table 1). It is important to point out that the tested salts present absorption at wavelengths in the UV-VIS region typical of phenolic decompositions. The wavelengths before and after absorption differ, as shown in FIG. 16, suggesting that these systems can be monitored by UV-VIS spectroscopy.

TABLE 1
Sorption tests of aqueous solutions of inner salts. ª
		Pressure	Absorption
		drop	by 13C	HCO3− After
		absorption	NMR	desorption
		(molesCO2/	(molesCO2/	(Percentage of
Input	Absorbent	molessalt) b	molessalt) c	desorption) d
1	MDEA/piperazine/	0.66	0.64	<0.3 (>95%)
	water(40%/
	10%/50% by
	mass) e
2		0.88 ± 0.06	0.91	0.18 ± 0.3 (80%)
3		0.69 ± 0.09	0.81 ± 0.05	<0.3 (>95%)
a Reaction conditions: 5 mL of solution with a concentration of 1 mol/L, temperature of 40° C. and pressure. Mean of at least two analyses ± standard deviation.
b Absorption values expressed in moles CO2 per moles of absorbent obtained by pressure measurements of 1.3 bar (130 kPa).
c Absorption values expressed in moles CO2 per moles of absorbent obtained by quantitative 13C NMR.
d Desorption percentage = (1-(HCO3− equivalents after desorption at 100° C. for 30 minutes / 13C NMR absorption))*100.
e CO2 absorption in relation to the number of moles of MDEA + moles of piperazine.

Example 4: Recyclability of aqueous solutions of 1,3-dimethyl-2-(3-oxy-phenyl)-imidazolium and 1,3-dimethyl-2-(4-oxy-phenyl)-imidazolium inner salts

The recyclability of aqueous solutions of the new developed absorbents was tested in cyclic tests of absorption followed by desorption. These tests were carried out in the same experimental apparatus used in Example 1 and shown in FIG. 15. The results of these tests are shown in Table 2 and detailed in FIG. 17, FIG. 18 and FIG. 19.

TABLE 2
Recyclability tests. ª
			Mean Absorption
		Number of	Value b
Input	Absorbent	tested cycles	(molesCO2/molessalt)
1	MDEA/Piperazine/water	26	0.57 ± 0.04 c
	(40%/10%/50% by
	mass)
2		27	0.58 ± 0.04
3		17	0.58 ± 0.08
a Reaction conditions: 5 mL of solution with a concentration of 1 mol/L, absorption temperature 40° C., and pressure of 1.3 bar (130 kPa), desorption temperature 100° C., atmospheric pressure (30 min.).
b Absorption values determined through the pressure drop in reservoir and expressed in moles CO2 per moles of absorbent. Mean represents mean absorption value of the cycles ± standard deviation.
c moles of CO2 per total moles of amines (MDEA + piperazine) MDEA/piperazine/water 40%:10%:50% solution.

Example 5: CO₂ absorption by aqueous solutions of the 1,3-dimethyl-2-(3-oxy-phenyl)-imidazolium inner salt determined using the ¹³C nuclear magnetic resonance spectroscopy technique

The capture of CO₂ by zwitterionic solutions of the 1,3-dimethyl-2-(3-oxy-phenyl)-imidazolium inner salt was also studied through quantitative analyses of ¹³C. This analysis methodology was described by SIMON, N. M. et al. “Carbon dioxide capture by aqueous ionic liquid solutions”, ChemSusChem, v. 10, p. 4927-4933, 2017 and allows to directly quantify both the chemisorption and the physisorption of CO₂ in the solutions.

To carry out this experiment, a syringe pump coupled to a zirconia NMR tube installed in an NMR spectrometer was used. The syringe pump allows CO₂ pressure control during experiments. The results were analyzed considering the proportion between the integrals of the signals corresponding to the dissolved CO₂ and the bicarbonate formed in relation to the integral of the methyl carbons of the zwitterion. The results are presented in Table 3.

TABLE 3
CO2 absorption determined using 13C NMR with pressure variation during
spectra acquisition. a
	Gauge	Physisorption	Chemisorption
	pressure	(molesCO2/	(molesCO2/
Absorbent	(bar - × 0.1 MPa)	molesSALT)	molesSALT)
	10 20 33 40	0.07 0.13 0.25 0.27	0.99 1.01 1.01 0.99
a Reaction conditions: 0.5 mL of solution with a concentration of 2.2 mol/L (1.1 mmol of the inner salt, dissolved in 0.5 mL of D20), absorption temperature 40° C. The NMR spectra were obtained in a Bruker-400-Avance-IIIHD NMR equipment operating at a frequency of 100 MHz for 13C equipped with a 5 mm probe with direct detection, with field gradient in z and thermostated via BCU-xtreme with constant temperature and spectral window from −15 ppm to 235 ppm. Used syringe pump: Xtreme-10 syringpump - deadalus innovation.

Example 6: CO₂ absorption by solutions of the 1,3-dimethyl-2-(3-oxy-phenyl)-imidazolium inner salt in protic solvents

One of the main advantages of the CO₂ capture process using zwitterionic solutions is that the zwitterionic bases are not volatile. On the other hand, a fraction of the solvent (usually water) can be lost by evaporation and during the desorption step, which represents energy losses in the process and the need of replacing this solvent. The cyclic CO₂ capture processes with the inner salts disclosed in the present discovery can also be carried out using non-aqueous solvents to minimize, or even eliminate, such mass losses in the desorption step. Alcohols, diols, polyols and ionic liquids functionalized with a hydroxyl group are solvents that, when combined with zwitterionic bases, are capable of reversibly absorbing CO₂ through the formation of the respective alkyl carbonates. In Table 4, some examples of absorption in non-aqueous systems are presented. n-propanol, n-butanol, ethylene glycol or glycerol are alternative solvents with boiling points of 97.0° C., 117.7° C., 197.6° C. and 290° C., respectively. On the other hand, the 1,2-dimethyl-3-(3-hydroxypropyl)-imidazolium bistrifluoromethylsulphonylimidate ionic liquid is a solvent with negligible vapor pressure and represents a totally ionic system for CO₂ capture in which there is certainly no loss of mass by evaporation.

TABLE 4
CO2 absorption through solutions of 1,3-dimethyl-2-(3-oxy-phenyl)-
imidazolium inner salt in different protic solvents. a
		Pressure drop	Absorption by	Percentage
		absorption (molCO2/	13C NMR	of
Absorbent	Solvent	molSALT) b	(molCO2/molSALT) c	desorption d
		0.74 0.67 0.68 −	0.86 0.66 0.73 0.83	>95% >95% >95% >95%
		0.64	−	−
a Reaction conditions: 5 mL of solution with a concentration of 1 mol/L, temperature of 40° C. and pressure. Mean of at least two analyses ± standard deviation.
b Absorption values expressed in moles CO2 per moles of absorbent obtained by pressure measurements of 1.3 bar (130 kPa).
c Absorption values expressed in moles CO2 per moles of absorbent obtained by quantitative 13C NMR.
d Desorption percentage = (1-(HCO3− equivalents after desorption at 100° C. for 30 minutes /13C NMR absorption))*100.

Example 7: Estimation of the enthalpy of absorption in aqueous solutions of the 1,3-dimethyl-2-(3-oxy-phenyl)-imidazolium inner salts

The experimental apparatus shown in FIG. 20 was used to determine the global equilibrium constants of the absorption process at temperatures of 10° C., 20° C., 30° C., 40° C., 50° C. and 60° C. The balance chamber 310 keeps all its components submerged in water with a temperature at the analysis temperature, controlled by the thermostatic bath 309. The reservoir 302 is filled with CO₂ from the cylinder 301 with the pressure measured by the pressure transducer 305. The sorption vessel 304 is then evacuated with the aid of a vacuum pump 311 and the zwitterionic-based sorbent solution is injected, through a septum located in the upper part of the sorption vessel, with the aid of a syringe 312. Then, the sorption vessel is pressurized with CO₂ through the brief opening of the valve 303. Finally, the pressure drop in the sorption vessel is monitored from the pressure transducer 306, which sends the data to the recorder 307 and the data is processed in the computer 308. Enthalpy of absorption of inner salts was determined using the same methodology reported by GABRIELSEN, J. et al. “Model for estimating CO₂ solubility in aqueous alkanolamines”, Industrial & Engineering Chemistry Research, v. 44, p. 3348-3354, 2005 to estimate the heat of absorption of CO₂ by aqueous solutions of alcoholamines. Table 5 shows the experimental results of the enthalpy of absorption of a commercial MDEA/piperazine/water mixture and for an aqueous solution of the 1,3-dimethyl-2-(3-oxy-phenyl)-imidazolium inner salt.

TABLE 5
Estimation of enthalpy of absorption.
		Estimated Enthalpy of
Input	Absorbent	Absorption (kJ/mol)
1	MDEA/Piperazine/water	−45.0
	(40%/10%/50% by mass)
2		−36 ± 0.8
a Reaction conditions: 0.5 mL of solution with a concentration of 1 Mol/L, absorption temperature between 10° C. and 60° C. Equilibrium pressure between 0.9 bar and 1.4 bar absolute (90 a 140 kPa).

It should be noted that, although the present invention has been described in relation to the attached drawings, it may undergo modifications and adaptations by technicians skilled on the subject, depending on the specific situation, but provided that within the inventive scope defined herein.

Claims

1- A process of synthesis of zwitterionic bases, characterized in that it comprises three steps: a) First step: promoting the reaction between a compound of the hydroxy-benzaldehyde type with a primary amine to form the corresponding imine, followed by the cyclization reaction of this imine, by adding an ammonium salt and a vicinal dialdehyde, for obtaining a compound of the 2-(hydroxy-phenyl)-imidazole type, in the presence of a solvent, at temperatures between −10° C. and 80° C. for times between 10 minutes and 24 hours;b) Second step: promoting the N-alkylation reaction between the compound of 2-(hydroxy-phenyl)-imidazole type obtained in the previous step and an alkylating agent to form a 2-(hydroxy-phenyl)-imidazolium salt, in the presence of solvent, at temperatures between 40° C. and 100° C. and in reaction times between 10 minutes and 24 hours;c) Third step: promoting the deprotonation of the phenolic OH group of the 2-(hydroxy-phenyl)-imidazolium salt, obtained in the second step, through the reaction of an aqueous solution of this component with a strongly basic ion exchange resin, which results in the formation of the inner or zwitterionic salt of the 2-(oxy-phenyl)-imidazolium type in a time of up to 60 minutes and temperatures between 10° C. and 80° C.

2- The process according to claim 1, characterized in that the compound of the hydroxy-benzaldehyde type contains at least one hydroxyl group in its aromatic ring and the other substituents of the benzene ring are hydrogen, alkoxy groups containing between 1 and 10 carbons, halides, phenyl or alkyl group or containing between 1 and 10 carbons.

3- The process according to claim 2, characterized in that the compound of the hydroxy-benzaldehyde type is 3-hydroxy-benzaldehyde or 4-hydroxy-benzaldehyde.

4- The process according to claim 1, characterized in that the primary amine has the general formula R1-NH2 in which the radical R1 comprises an alkyl, aryl, alkylether or alkylalcohol group containing between 1 and 10 carbons.

5- The process according to claim 4, characterized in that the primary amine is methylamine.

6- The process according to claim 1, characterized in that the primary amine is in a proportion of 0.5 to 2 equivalents in relation to the compound of the hydroxy-benzaldehyde type.

7- The process according to claim 1, characterized in that the ammonium salt has the general formula (NH4)nY, where Y comprises the bromide, chloride, sulfate, acetate, carbonate and bicarbonate anions; n has a value of 1 or 2.

8- The process according to claim 1, characterized in that the ammonium salt is in a proportion of 0.3 to 2 equivalents in relation to the compound of the hydroxy-benzaldehyde type.

9- The process according to claim 1, characterized in that the dialdehyde is glyoxal or its analogues with alkyl, aryl, alkylether or alkylalcohol substituents containing 1 to 10 carbons.

10- The process according to claim 1, characterized in that the dialdehyde is in a proportion of 0.5 to 2 equivalents in relation to the compound of the hydroxy-benzaldehyde type.

11- The process according to claim 1, characterized in that the solvent of the first step is water, acetonitrile, ethyl acetate, aliphatic alcohols containing from 1 to 10 carbons in the alkyl chain or a mixture of these in any proportion in the amount of 1 to 100 times the mass of the compound of the hydroxy-benzaldehyde type.

12- The process according to claim 11, characterized in that the solvent is an amount of 10 times the mass of the compound of the hydroxy-benzaldehyde type.

13- The process according to claim 1, characterized in that the alkylating agent has the general formula R9-X, in which R9 comprises an alkyl, arylalkyl, alkylether or alkylalcohol group containing between 1 and 10 carbons, and the X group comprises a halide, alkylsulfonate and alkylsulfate group, in which the alkyl group has between 1 and 5 carbons.

14- The process according to claim 13, characterized in that the alkylating agent is iodomethane or methanesulfonyl chloride.

15- The process according to claim 1, characterized in that the second step occurs at a temperature of 70° C., under stifling for 1 hour.

16- The process according to claim 1, characterized in that the solvent of the second step is water, acetonitrile, ethyl acetate, aliphatic alcohols containing from 1 to 10 carbons in the alkyl chain or a mixture of these in any proportion in the amount of 1 to 20 times the mass of the compound of the hydroxy-benzaldehyde type.

17- The process according to claim 16, characterized in that the solvent is an amount of 5 times the mass of the compound of the hydroxy-benzaldehyde type.

18- The process according to claim 1, characterized in that the third step occurs at a temperature of 30° C. and under stifling for 10 minutes.

19- Zwitterionic bases, as obtained in the process of claim 1, characterized in that they present in their structure an imidazolium cation covalently linked, through carbon C-2, to a phenolate anion, represented by the general formula:

20- The zwitterionic bases according to claim 19, characterized in that they are solids soluble in water and polar organic solvents, such as alcohols, polyalcohols, acetonitrile and acetone.

21- A CO2 capture process, using zwitterionic base solutions as defined in claim 19, characterized in that it promotes the contact, under sorption conditions, of a gaseous stream containing acidic gases with a zwitterionic base sorbent solution for the removal of, at least, part of these acidic gases, obtaining a purified gaseous stream and a solution with sorbed acidic gases; and, in parallel, it promotes the regeneration of the sorbent solution, under desorption conditions, to obtain a zwitterionic base solution and a stream of acidic gases.

22- The CO2 capture process according to claim 21, characterized in that the gaseous feed stream is composed of a gaseous mixture containing one or more acidic gases, such as carbon dioxide and hydrogen sulfide.

23- The CO2 capture process according to claim 21, characterized in that the zwitterionic base is an inner organic salt formed by the covalent association of a quaternary ammonium cation, quaternary phosphonium, pyridinium, pyrrolidinium or imidazolium, with the phenolate anion.

24- The CO2 capture process according to claims 21 to 23, characterized in that the zwitterionic base containing the quaternary ammonium cation has the formula:

25- The CO2 capture process according to claims 21 to 23, characterized in that the zwitterionic base containing the quaternary phosphonium cation has the formula:

26- The CO2 capture process according to claims 21 to 23, characterized in that the zwitterionic base containing pyridinium has the formula: wherein R1, R2, R3, R4 and R5 comprise hydrogen and alkyl, aryl, alkylether or

27- The CO2 capture process according to claims 21 to 23, characterized in that the zwitterionic base containing the pyrrolidinium cation has the formula:

28- The CO2 capture process according to claims 21 to 23, characterized in that the zwitterionic base containing the imidazolium cation has the formula:

29- The CO2 capture process according to claim 21, characterized in that the zwitterionic solution is a solution of 1,3-dimethyl-2-(3-oxyphenyl)-imidazolium or 1,3-dimethyl-2-(4-oxy-phenyl)-imidazolium inner salt.

30- The CO2 capture process according to claim 21, characterized in that the zwitterionic solution uses as solvent water, methanol, ethanol, isopropanol, aliphatic alcohol having from 1 to 18 carbons in the alkyl chain, diols having from 2 to 5 atoms of carbon or polyols having from 3 to 6 carbon atoms, ethylene glycolmonoalkylethers of the formula H(OCH2CH2)nOR2, where n varies from 1 to 4 and R2 consists of an alkyl group containing from 1 to 12 carbons, ionic liquids functionalized with the hydroxyl group or mixtures thereof.

31- The CO2 capture process according to claim 21, characterized in that the absorption condition is: concentration of the zwitterionic base solution between 0.5 M and 5 M, temperature between 0° C. and 60° C. and pressure between 1 and 150 bar absolute (100 kPa and 15 MPa).

32- The CO2 capture process according to claim 21, characterized in that the zwitterionic solution of the absorption step presenting a temperature of 40° C. and pressure between 1.3 and 3 bar absolute (130 and 300 kPa).

33- The CO2 capture process according to claim 21, characterized in that the desorption condition being: temperature between 60° C. and 150° C. and a pressure between 0 and 10 bar absolute (1 MPa).

34- The CO2 capture process according to claim 33, characterized in that the zwitterionic solution of the desorption step presents a temperature of 100° C. and a pressure of 1 absolute bar (100 kPa).

35- A use of the co t capture process, as defined in claim 21, characterized in that it is applied in industrial segments, such as in the energy sector to capture CO2 from exhaust gases, in the chemical sector to remove CO2 from process gaseous streams catalysts in which CO2 can poison the catalysts and especially in the oil and gas sector for the purification of natural gas.