Ionic Liquids IIIB - American Chemical Society

Downloaded by PENNSYLVANIA STATE UNIV on September 7, 2012 | http://pubs.acs.org Publication Date: March 15, 2005 | doi: 10.1021/bk-2005-0902.ch004

Chapter 4

Task-Specific Ionic Liquids for Separations of Petrochemical Relevance: Reactive Capture of C 0 Using Amine-Incorporating Ions

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James H. Davis, Jr. Department of Chemistry, University of South Alabama, Mobile, AL 36688 and The Center for Green Manufacturing, University of Alabama, Tuscaloosa, AL 35487

Introduction Natural gas, largely composed of CH4, is rarely removedfromthe earth in a state pure enough to trunk directly into pipeline systems for delivery to consumers (1). Depending upon the particular productionfield,the gas usually contains adulterants which run the gamutfromwater and heavier hydrocarbons to so-called acid gases. Perhaps more so than the removal of some species, the scrubbing of acid gases - C0 , H S and others -fromnatural gas streams is a process of vital importance. The former is non-combustable and its persistance in a gas stream lowers the fuel value of the entraining gas. In contrast, H S burns but is highly toxic and its combustion produces noxious and corrosive sulfur oxides. With supplies of relatively pure "sweet gas" dwindling in the face of increasing world demand, productionfieldsregarded heretofore as being of marginal value are being increasingly looked to as the production sources of the © 2005 American Chemical Society 49 2

2

2

In Ionic Liquids IIIB: Fundamentals, Progress, Challenges, and Opportunities; Rogers, R., et al.; ACS Symposium Series; American Chemical Society: Washington, DC, 2005.


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future. These "sour gas" fieldswill demand unprecedented scales of treatment for the removal of acid gases. The removal of acid gasesfromnatural gas - "scrubbing" or "sweetening" - is a process which has been practiced since die 1930's (2). A number of technologies have been used to accomplish this purification,some of them based upon the differing physical properties of the gases, but most relying upon chemical agents to effect acid gas capture. In turn, chemical agents are used in either of two ways, as physical solvents or reagents forreactivecapture. In either case, die established materials used in these processes themselves introduce complications into the gasremovalprocess. As both gas demand and pressures for increased sour gas utilization increase, so too will the demand for unproved scrubbing agents. Η

Figure /. Alkanolamines in common usefor CO2 scrubbing. Lefi to rig monoethanolamine (MEA); diethanolamine (DEA); methyldiethanola (MDEA). The most widely used technology for theremovalof acid gases is based upon scrubbing by aqueous alkanolanaiiies. Commonly used alkanolamines may be primary, seconday or tertiary amines. The structures of severalfrequentlyused materials are depicted in Figure 1. The means by which alkanolamiiie effect the capture of CO| is twofold [Scheme 1]. In the case of scrubbingreagentswith primary or secondary amines, the C0 canreactwith two equivalents of amine, forming ammonium carbamates. In the case of any of the amine groups, reaction of the amine with the water solvent produces equilibrium concentrations of ammonium hydroxides, whichreactwith CO3 to form bicarbonate ion. In the case of H S the principal operating mechanism appears to be the formation of hydrosulfide anion. Regardless of die gas beingremoved,die purging of die natural gas stream through die scrubbing solution creates problems. In diefirstplace, the exiting gas stream may berenderedacid gasfree,but it has been thoroughly charged with water vapor which has to beremovedin a subsequent, energy intensive condensation step. At the same, the alkanolamine - which is a neutral compound - may be taken up in some quantity into die ps stream White not posing problems in die sense that it is both combustable and not especially toxic, its lossrepresentssome economic drag on the scrubbing process. Finally, the extrusion of C0 fromthe loaded or spent scrubbingfluidmayrequirethe heating of die solution, which of course involves heating the solvating water along with thereagent,anodier undesireable energy cost 2

2

f

2



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la tenus of their potential utility in gas processing, ionic liquids can in a very real way be thought of as liquid solids. To the degree that solids have been considered or are utilized as soibents for gas processing in any arena, their chief advantage over liquids stemsfromtheir lack of vapor pressure. However, the limited surface area for solids - even materials like porous carbons - makes their capacity generally lower than ideal for many gas processing applications. When die solubility of a particular gas in a certain liquid is higher than its adsorption limit on a specific solid, die liquid would be preferred exceptforthe potential for cross-contamination created by the liquids' own vapor p Notably, one of die defining characteristics of ionic liquids is their lack of measurable vapor pressure up to their decomposition point Given die foregoing considerations, it seemed opportune to us to investigate ionic liquids for the capture of various acid gases.

2 R"NH

2

•

1

0=C=0

R-N

R-NHs

Ή

m

R-NHj

•

H

®

u

^cr

Θ Θ R-NHs H-0 +

•

R-NH3

Θ

H-0

©

0=C=0

•

R-NH3

®

Μ Η

VV H-0

5

o

Θ

Scheme 1. Mechanisms ofreactive acid gas capture operative in aqueo amine solutions.

Task-Specific Ionic Liquids for Reactive Capture In a paper presented in 2000 at an AIChE symposium cm advances in solvent selection, we coined die term "task-specific* ionic liquids to describe a new, non-treditional type of IL under development by us in which the cation, anion, or both of the IL incorporated functional groups capable of imparting specific 9



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properties or reactivities to the resulting IL (3). Among the ILs under development were materials incorporating appended amine groups. These materials became the initial testbed for our continuing studies of the reactive capture of acid gases with ionic liquids. OurfirstTSIL with appended amine groups built upon the work of Herrmann, who had reported the synthesis of an amine-appended imidazolium cation which he used as a precursor to imidazoUdene caibene ligands (4). In that instance, the salt was not isolated as the aminefreebase, and the counterion was bromide, making the salt Tooth high melting and non-basic, impediments to their utilization as ILs for acid gas capture. After developing a protocol for both the generation of thefreeamine and an anion exchange, we isolated several structurally related amine-appended imidazolidene ILs in modest yields. Using these compounds, we were able to demonstrate their utility as C0 capture reagents (5). For example, using IL 1 [Figure 2], we were able to capture near the theoretical maximum of C0 for this salt (0.5 mol / mol). Given the water-free nature of both the IL and the model gas stream, we expected the capture mechanism to be formation of an ammonium carbamate derivative of the IL. The CMMRofthe product salt after treatment with C0 firmlyestablished this to be the case, the expected doubling of all imidazoliumringpeaks being observed as well as a signal for die carbamate carbon (5). 2

2

13

2

1

0

~Ph Ph

Figure 2. Amine appended TSILs with one (IL 1) and two (IL 2) a amine groups per ion pair. As mentioned, die incorporation of one amine group per ion pair coupled with die need for two amine groups to effect C0 capture by carbamate formation dictates that the maximum capture capacity for salts of type 1 is 0.5 mol C0 / mol IL. Consequendy we began to examine approaches to boost the C0 capture capacity by boosting die number of amine groups per ion pair. While there are several potential approaches for doing so, we began our effort by focusing on the anion as the carrier for the second amine group. There are several immediate possibilities in this regard, including the conjugate bases of 2

2

2


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amino acids, a concept suggested by Quinn and Pez in patents concerning die use of certain salt hydrates for CQ capture (6). However, since carboxylatcbased anions tend to be less than ideal in IL formulations, we decided to probe die use of the non-proteogenic amino acid taurine in combination with amineappended cations. At die same time, we decided to probe the use of a new amine appended cation, this species incorporating a phosphonium head group [Figure 2]. Our rationale for doing so stemmedfromboth a desire to identify less costly head groups as well as to avoid the potential for imidazolium C^-H deprotonation by the appended amine group. It should be noted that die isolated salt contained 3-6 molecules of water per ion pair which were tenaciously bound, making it formally a molten salt- or ionic liquid hydrate.


2

1

1

• monoamine TSIL -•-diamine TSIL

Figure J. Measured CO2 uptake capacity of TSIU containing one versus amine groups per ion pair.


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When exposed to a stream of dry CO* bis-amine IL 2 proved to be capable of absorbing twice as much C0 per mole of DL as did IL 1. [Figure 3] In addition, where die viscosity of 1 visibly increased with the uptake of CO* that of 2 appeared to decrease, a phenomenon we have yet to understand The C-NMR of the product exhibited two poorly resolved peaks for carbamate carbons (presumably one for taurine-bound carbamate and one for cation bound carbamate), but also exhibited a small third peak in die same vicinity, ascribed to bicarbonate. Observation of die latter was not surprising given die water content of die sequestering salt Like C0 loaded 1, decarboxylation is readily accomplished by heating the samples in vacuo overnight. Uptake experiments were repeated on the same sample of 2 for five runs with no observed diminution ofC0 uptake capacity. 2

13


2

2

Task-Specific Ionic Liquids for Increased CO) Physical Solubility

As mentioned, current technology for gas sweetening uses aqueous solutions of alkanolamines. Given that the sequestration mechanism turns on either the directreactionof the amine group with C0 or with water to generate hydroxide, the question arises as to what function is served by the alcohol group of these molecules. In short, the alcohol group increases the solubility of the amine in the water and aids in itsretentionby the scrubbing solution as the natural gas is purged through the system Unfortunately, the presence of the alcohol in the same molecule as the amine (especially on a β carbon) alsorendersthese molecules susceptible to (under certain pH conditions) the formation of fivemembcred cyclic carbamates, speciesfromwhich extrusion of C0 is not readily accomplished. Over time, this leads to a loss of capture capacity on die part of the scrubbing solution. With amine-appended TSILs, such problems are avoided since the molecules do not incorporate the complicating hydroxyl group. Still, as C0 is absorbed by the TSILs, each system becomes not just a mixture of ions but rather one of zwitterions. In this case, one can imagine die creation of an extensive network of ionic cross-links which could effect diffueivity of excess C0 through the system. Such a process appears to be operative, being evidenced in TSILs applied to membranes for C0 separation becoming rapidly impermeable to C02 transport (7). And, since the development of membrane based gas separation systems is being widely investigated, we have also begun to develop ionic liquids which we hope will prove to be better physical solvents for CO* in order to provide a complimentary technology. It is well known that a number of highly polar aprotic organic solvents have a high capacity for dissolving certain gases such as C0 . While most of these 2

2

2

2

2

2


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solvents - compounds such as dimethylformamide (DMF), dimethylsulfoxide (DMSO) and N-methylpyrrolidinone (NMP) - have relatively low vapor pressures, those vapor pressures still pose a problem for gas processing. At die same time, elegent work by Brennecke has shown that CO& compared to several other gases, has a relatively high solubility in "conventional** ionic liquids, and at least one patent has been issued based upon their use in membrane systems (8). Consequently, it is our hope that task-specific ionic liquids in which one of the ions incorporates functionality similar to that in DMF, DMSO, NMP or other solvents might exhibit even higher capacities for die solvation of C0 . To this end, we have been working to prepare such compounds. Downloaded by PENNSYLVANIA STATE UNIV on September 7, 2012 | http://pubs.acs.org Publication Date: March 15, 2005 | doi: 10.1021/bk-2005-0902.ch004

2

CHaCfe

3

Figure 4. Synthesis ofan NMP-like TSILfromcommercially available sta materials. One of ourfirstsuccessful forays in this area centers on the synthesis of a pyridinium DL with an appended NMP-like group, 3 [Figure 4]. We believe our synthetic methodology for the assembly of this compound to be unique as an approach to IL synthesis. It is well established that pyrrylium salts will react direcdy with primary amines, cleanly substituting an R-N fragment for die ring oxygen with the concommitant loss of water. By combining die commercially available compounds 2,4,6-trimethylpynylium tetrafluoroborate with N-(3aminopropyl)-pyrrolydin-2-one we were able to isolate IL 3 as a viscous liquid in 58% yield. We note that IL 3 is not diefirstpyrrolidinone-based DL to have been proposed. A 2002 paper by Demberelnyamba reported the synthesis of a new IL by N-alkylation of N-vinyl pyrrolidinone with an alkyl iodide (9), However, we have been unable to repeat this work and note that the Nalkylation of amides is virtually unprecedented. Further, a 1984 paper by Smith specifically descrbes the O-alkylation of N-vinyl pyrrolidinone with oxonium salts (these more powerful alkylating reagents being required to accomplish t


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alkylation on my paît of aie molecule), and the subsequent decomposition of those species to amino acids upon contact with water (10). To date, we have not begun to measure die solubility of COa in 3. However, we have found die solubility of a number of polar molecules (e.g., sugars) to be higher in it than in conventional IL, pointing to the similarity of this molecule to that which it is intended to resemble, NMP. The complete results of our work to prepare new solvent-analog ILs as well as their gas solubility capacities will be reported in due course.


References 1. Understanding Natural Gas. Accessible on the web at: siepr.stanford.edu/about/Natural_Gas.pdf 2. Kohl, A. and Nielsen, & Gas Purification; Gulf: Houston, 1997. 3. Davis, J.H., Jr. and Wierzbicki, A. Proceedings of die Symposium on Advances in Solvent Selection and Substitution for Extraction; AIChE: New York, 2000; Paper 14F. 4. Hermann, W..A.; Kocher, C.; Goossen, L. J. and Artus, G. R. J. Chemistry: a European Journal, 1996, 2, 1625-1635. 5. (a) USP pending (filed April 2002). (b) Bates, E. D.; Mayton, R. D.; Ntai, I.; Davis, J. H., Jr.; J. Am. Chem. Soc., 2002; 124, 926-927 6. (a) Quinn, R.; Pez, G. P. and Appleby, J. B. USP 5,338,521 (August 16, 1994). (b) Quinn, R. and Pez, G. P. USP 4,973,456 (November 27,1990). 7. Scovazzo, P. and Davis, J. H., Jr. Unpublished results. 8. (a) Anthony, J. L.; Maginn, E. J. and Brennecke, J. J. Gas Solubilities in 1butyl-3-methyl imidazolium hexafluorophosphate. In Ionic Liquids; Rogers, R. D. and Seddon, K. R., Eds.; American Chemical Society: Washington, D. C ., 2002; ACS Symp. Ser. No. 818, pp 260-269. (b) Brennecke, J. F. and Maginn, E. J. USP 6,579,343 (June 17, 2003). 9. Demberelnyamba, D.; Shin, Β. K. and Lee, H. Chemical Commun., 2002, 1538-1539. 10. Smith, M. B. and Shroff; H. N. J. Org. Chem., 1984, 49, 2900-2906.


Ionic Liquids IIIB - American Chemical Society

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