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New Materials and Process Development for Energy-Efficient Carbon
Capture in the Presence of Water Vapor
Investigators All investigators are at Northwestern University. Note that the experimental part of the
project is described in a separate document, although experiment and modeling are
tightly integrated in the project.
Randall Q. Snurr, Professor, Chemical & Biological Engineering
Fengqi You, Assistant Professor, Chemical & Biological Engineering
Hanyu Gao, Graduate Researcher, Chemical & Biological Engineering
Emmanouil Tyllianakis, Post-doctoral Researcher, Chemical & Biological Engineering
Abstract
Using quantum chemical methods, we have screened a variety of functional groups
for their ability to bind CO2 and water. Most functional groups bind water more strongly
than CO2, making them ineffective for incorporation into materials for removing CO2
from humid flue gas. Preliminary calculations suggest that adding perfluorinated
functional groups strongly suppresses water binding, while having little effect on CO2
binding. Preliminary process-level modeling has shown that if materials are not available
for capturing CO2 from humid flue gas, it may be economically feasible to remove much
of the water from the flue gas prior to CO2 removal. This opens up a wider range of
material and process combinations for cost-effective CO2 capture.
Introduction
Adsorption processes based on porous solids are a promising technology for
removing CO2 from power plant flue gas. The premise of this proposal is that game-
changing improvement of adsorption separation processes for carbon capture and storage
(CCS) will require simultaneous development of new materials and specially designed
processes that take advantage of these new materials. Competitive adsorption of water is
regarded as the single greatest technical hurdle to adsorption-based CCS, but there is very
little research on new water-tolerant CCS adsorbents. One goal of this project is to
develop new metal-organic framework (MOF) materials with extraordinarily high
selectivity for CO2 over nitrogen and water, together with suitably high absolute capacity
for CO2. Several related strategies are being explored, and molecular modeling is being
used to guide the synthetic effort. In addition, we are using state-of-the-art process-level
modeling to optimize adsorption processes around the new class of sorbents and explore
the real efficiency limits of MOF-based adsorption processes that meet desired CCS
technical and economic criteria, while minimizing the life-cycle environmental impact.
Adsorption processes are already used in large-scale applications, such as air separation,
with high reliability. Discovery of new, water-stable and water-tolerant adsorbents for
CO2 capture and new, optimal process configurations for these sorbents would be a step-
out development in CCS.
Background
Research on MOFs continues to explode. Many research groups are investigating
MOFs for separation of CO2/N2 mixtures, motivated by carbon capture. However, very
few papers report results that take water into account. A small number of papers have
appeared recently on the stability of MOFs, including their stability in water or humid gas
streams.
Results
Molecular-level Modeling
We are using molecular-level modeling to 1) screen new candidate materials and 2)
obtain insights into the structures that provide the best performance. One focus this year
was to screen functional groups that could be incorporated into existing MOF materials
for selective adsorption of CO2 over N2 in the presence of water vapor. ZIF-8 was chosen
as a candidate MOF for functionalization due to its stability in the presence of water
(even under boiling water conditions). In addition, this material has been shown to be
very hydrophobic and to adsorb almost no water. This has been demonstrated
experimentally [1-2] and by simulations from our group [3].
A variety of different functional groups were tested for their ability to enhance the
target properties of ZIF-8. The binding energies for water and CO2 were calculated as an
initial measure of the ability to adsorb CO2 in the presence of water. The goal was to find
functional groups that would increase the adsorption of CO2 compared to the
unfunctionalized material but that would not adsorb too much water. Quantum
mechanical calculations were performed to obtain the binding energies. Calculations
were performed on a small and a large cluster extracted from the ZIF-8 structure, as
shown in Figures 1. For the small clusters, we used a high level of theory, namely second
order Møller–Plesset perturbation theory (MP2) with large basis sets such as 6-
311++G(2d,p). For the large clusters, we used less expensive density functional methods
using the wB97xD functional and a 6-31G(d,p) basis set.
Figure 1. Small and large clusters of ZIF-8 used for the quantum chemical
calculations.
For the large cluster, the different functional groups were added not only on the
central ring of the cluster but on all of the six peripheral rings as well. This was done to
observe any possible synergetic effect between the functional groups of adjacent rings,
and indeed we did observe such effects for some functional groups, where the interaction
of guest molecules with the cluster was significantly enhanced when groups were present
on every ring of the cluster rather than only on the central ring.
As expected from our choice of functional groups, we observed an increase in the
interaction energy between the ZIF cluster and the CO2 molecules upon functionalization
with all of the functional groups tested. In some cases, the enhancement was quite
pronounced, for example an increase in the magnitude of the binding energy from -13
kJ/mol to -94 kJ/mol. At the same time, when these groups were tested for their ability to
interact with water, the same trend was observed: in every case, the functional group
increased the binding of water as well. There was no functional group among the ones
tested that could bind CO2more strongly than H2O, supporting our initial idea that simple
functionalization was unlikely to be a successful strategy.
Functionalization with perfluoro group was given special attention. In a similar set of
calculations, the ZIF-8 methyl groups on the imidazole ring (Figure 1) were replaced by
perfluorinated methyl groups. The perfluorination of the methyl groups resulted in a
significant decrease in the interaction with water (from -36 kJ/mol to -24 kJ/mol), making
the material more hydrophobic. At the same time, this change had almost no effect on the
interaction with CO2, with binding energies of-13 kJ/mol for the original cluster and -12
kJ/mol for the cluster with the perfluorinated methyl groups.1 Thus, the material with
perfluoromethyl groups is predicted to be significantly more hydrophobic than the parent
material but to adsorb essentially the same amount of CO2. While the parent ZIF-8
material is not particularly good for CO2 capture, this finding may allow us to find other
materials that can be made hydrophobic while retaining their ability to adsorb CO2.
Process-level Modeling
There are two main objectives of the process-level modeling in this project: first, to
design a system that utilizes materials discovered in the project and, second, to provide
feedback to the materials discovery effort on the desired material properties. While our
primary focus is the development of materials that can adsorb CO2 in the presence of
water, we thought it worthwhile to first investigate how much it would cost to remove
water vapor from the flue gas prior to the CO2/N2 separation. A new graduate student
was recruited for this effort, and during the past several months, we designed several
different processes for water removal and determined the corresponding cost under
different requirements and operating conditions.
The total cost of the water removal system was estimated using a framework
proposed by Hasan et al. [4]. The total annualized cost (TAC) was divided into the
annualized investment cost (AIC) and the annual operating cost (AOC). The detailed
scheme for calculating the AIC is shown in Table 1. The AOC was determined by the
usage of utilities including process utilities (cooling water, steam, refrigerant) and
electricity. All equipment costs and utility costs were estimated using the Aspen Process
Economic Analyzer.
1It should be noted that with the simple cluster models, these energies are not expected to reflect the
adsorption enthalpies measured in the real materials. Rather, we are seeking trends with these calculations.
Table 1. Parameters for the economic analysis
parameter Value
Equipment (mover) installation cost (EIC) 80% of equipment
purchase cost(EPC)
Equipment (column, exchanger, etc.) installation cost (EIC) 4% of EPC
Total installed cost (TIC) All EPCs and EICs
Indirect cost (IDC) 32% of TIC
Balance of plant cost (BPC) 20% of TIC
Total plant cost (TPC) TIC+IDC+BPC
Annual maintenance cost (AMC) 5% of TPC
Capital recovery factor 15.4%
There are many different technologies for water removal. We mainly focused on two
of them, absorption with triethylene glycol (TEG) and cooling & condensation. Other
technologies include compression and condensation, cryogenic separation, membranes,
and solid adsorption. Compression and condensation was not considered because of the
high installation cost and electricity consumption for compressing the entire flue gas
stream. Cryogenic separation requires extensive use of coolant. Membrane technology is
also reported to cost more than TEG absorption by Hasan et al. [4] and was not
considered here. Solid adsorption needs further evaluation.
TEG absorption and cooling & condensation processes were simulated using Aspen
Plus. We assumed feed flue gas available at 1 bar and 55℃ with 15% H2O, 69.5% N2,
5.5% O2 and 10% CO2 (volumetric fractions). The flue gas then goes through a direct
contact cooler where it is saturated with water at 35℃ (corresponding to 5.5% H2O). The
flow rate of this stream was taken to be 1kmol/s (which is about the CO2 emission of a 30
MW power plant) for simplicity.
The process flow diagram for cooling & condensation is shown in Figure 2. Wet flue
gas is cooled down, and the liquid phase is separated from the vapor phase in a flash tank
operating at 1 atm. The temperature of the cooled mixture exiting the heat exchanger
depends on the requirement set for the water content in the dry gas. For example, if we
require less than 1% water in the dry gas, the cooling temperature is 75˚F. If the
requirement is 0.1%, the cooling temperature has to be 41˚F.
Figure 2. Cooling and condensation process flow diagram.
The cost of this process was estimated for different requirements set on the water
content. Refrigerant at 10˚F was assumed to be available at $1.70 per ton-day [5]. With a
1% water requirement, the AIC and AOC are $39,504 and $296,154, respectively. The
total plant cost (TPC) is then $335,658, and the water removal costs $2.4 per ton of CO2
captured. With a 0.5% water requirement, the cost per ton of CO2 captured is $4.2. The
cost of cooling and condensation is low, because it is a simple process. The only utility
requirement is refrigeration, and the cooling temperature is not very low. However, this
simple process leads to significant loss of CO2, especially when requiring low water
content in the dry gas. For example, when a 0.1% water requirement is set, more than
25% of the CO2 is lost from the bottom of the flash tank. Our goal is to capture at least
90% of the CO2. If we instead require no more than 10% loss of CO2, the water content
can only go down to as low as 0.5%, which places significant restriction on this
technology.
The other technology studied for dehydration was TEG absorption. The process flow
diagram is given in Figure 3. Wet flue gas is contacted with 99.5% TEG in the absorption
column and dry gas is obtained from the top. TEG absorbed with water is then
regenerated using a flash tank operating at high temperature and low pressure.
Figure3. TEG absorption process flow diagram.
The cost of TEG absorption is generally higher than cooling & condensation under
the same requirement on water content. Figure 4 shows the cost per ton of CO2 captured
for the TEG absorption process under different requirements when the flash tank is
operating at 120℃ and 0.04 bar and the cooler outlet temperature is 65℃. The general
range is between $10 and $20 per ton of CO2 captured, while the cost goes to $73/ton
CO2 captured when the water requirement is 0.1%. This is because the operating
condition is far from optimal for this case.
Figure 4. Dependence of cost on water requirement in the outlet stream for TEG
absorption.
TEG absorption can achieve good separation of H2O from flue gas without sacrificing
CO2 recovery. The loss of CO2 is less than 3% even when the water percentage in the dry
gas is set to 0.1%. Unlike cooling & condensation, the operating conditions of TEG
absorption are adjustable even when the requirement on water removal is fixed. Changing
the temperature and pressure of the flash tank and the temperature of cooler outlet can
significantly influence the cost of the process, so the operating conditions need to be
optimized in order to achieve lower costs. The three main process variables are the flash
temperature (ranging from 100-140℃), the flash pressure (0.04-0.2 bar), and the cooler
0
20
40
60
80
0.0% 0.2% 0.4% 0.6% 0.8% 1.0% 1.2%
cost
pe
r to
n C
O2
cap
ture
d
(in
$)
water persentage required
outlet temperature (45-65℃). For the 1% water requirement case, 30 sampling points
were taken within these ranges using the Latin Hypercube Sampling method in
MATLAB. The cost was estimated for each sampling point. Among these sampling
points, the cost of CO2 capture ranges from $5.8 to $18.1 per ton of CO2 captured, with
the lowest cost found when the flash temperature is 108℃, flash pressure is 0.09 bar and
cooler outlet temperature is 61℃. For the 0.1% water requirement case, the lowest cost is
found at $10.9 per ton of CO2 captured when the flash temperature, flash pressure and
cooler outlet temperature are 140℃, 0.04 bar, and 40℃, respectively.
Progress
Our preliminary process-level modeling indicates that removing water prior to
capturing CO2 from flue gas may be economically and technically feasible. The question
of how much of the water to remove requires an integration of the process modeling and
the materials development and will be one focus in the coming year.
Development of fluorinated MOFs may provide a solution to the difficult problem of
selectively adsorbing CO2 over N2 in the presence of water vapor.
Future Plans
Computational screening of MOFs will continue in close association with the
experimental effort, as described in the original proposal. One new direction is suggested
by the process-level modeling, namely, an assessment of how MOFs perform in the
presence of a small amount of water vapor (as opposed to a stream that is essentially
saturated with water vapor).
We will finish our assessment of the cost of water removal. We have made good
progress in writing a MATLAB code for modeling adsorption units and will soon begin
modeling carbon capture processes based on MOF materials.
Publications and Patents There are no publications or patents yet.
References 1. V. Colombo, S. Galli, H.-J. Choi, G.-D. Han, A. Maspero, G. Palmisano, N. Masciocchi, J. R.
Long, Chem. Sci., 2, 1311 (2009).
2. P. Küsgens, M. Rose, I. Senkovska, H. Fröde, A. Henschel, S.Siegle, S. Kaskel, Micropor.
Mesopor. Mater.,120, 325 (2009).
3. P. Ghosh, K.C. Kim, R.Q. Snurr, manuscript in preparation.
4. M.M.F. Hasan, R.C. Baliban, J.A. Elia, C.A. Floudas, C. A., Ind. Eng. Chem. Res., 51, 15665
(2012).
5. W.D. Seider, J.D. Seader, D.R. Lewin, S. Widagdo,Product and Process Design Principles:
Synthesis, Analysis, and Evaluation, 3rd ed.; John Wiley: Hoboken, NJ, 2009.
Contacts
Randall Q. Snurr, [email protected]
Fengqi You, [email protected]
New Materials and Process Development for Energy-Efficient
Carbon Capture in the Presence of Water Vapor Investigators All investigators are at Northwestern University. Note that the modeling part of the project is described in a separate document, although experiment and modeling are tightly integrated in the project. Omar K. Farha, Research Associate Professor, Chemistry Joseph T. Hupp, Professor, Chemistry Pravas Deria, Post-doctoral Researcher, Chemistry Zachary Brown, Graduate Student, Chemistry Olga Karagiaridi, Graduate Student, Chemistry Marianne Lalonde, Graduate Student, Chemistry Abstract The experimental portion of the project is currently focused on designing, synthesizing, characterizing, and functionally evaluating nanoporous materials that feature the following properties: a) excellent stability under conditions encountered in flue-gas environments, b) high capacity for gas uptake, c) ability to capture CO2 at pressures found in flue gas, and d) ability to inhibit competitive adsorption of water. Our initial strategy has focused on metal-organic framework (MOF) materials that present high surface areas and large total pore volumes. We have explored two approaches to incorporation of perfluorinated functional groups that can render MOF interior surfaces both hydrophobic and strongly attractive for carbon dioxide. 1. Decorating the Mesopores of the Zr-Based Metal-Organic Framework Material NU-1000 with Perfluoroalkyl Functional groups for Carbon Capture Under Humid Conditions. Among the requirements for effective sorption-based carbon capture are that the sorbent material: (a) have high capacity for CO2, (b) possess high selectivity for CO2 over N2, (c) be stable, and perform well, under humid condition of flue gas, and (d) display fast adsorption and desorption kinetics. It appears that isosteric heats of adsorption of ~50 kJ/mol (at 0.15 bar) would be required in order for a sorbent material to interact strongly enough with CO2 to capture 90% of the carbon present in flue gas while still allowing easy regeneration. For a sorbent material to function successfully under humid (~5% H2O in flue gas) conditions, it additionally must have a strongly preferential interaction with CO2 over H2O. MOFs that possess open metal coordination sites and exposed primary or secondary alkyl-amines often show high heats of adsorption. But, they are either water intolerant or exhibit excessive large isosteric heats of adsorption. The latter imply excessive energy consumption for subsequent carbon release and sorbent regeneration. To achieve these targeted physical properties within sorbent materials, we sought to functionalize a mesoporous MOF with fluorinated alkanes of various lengths. Notably, perfluoroalkanes are widely used as surfactants in processes involving
supercritical CO2. The strengths of interaction of C-F sites with carbon dioxide are believed to be 10 to 20 kJ/mol greater than strengths of interaction C-H sites with carbon dioxide. Additionally, perfluorinated materials typically are strongly hydrophobic, i.e. they typically exhibit little interaction with water.
We used the recently developed material, NU-1000 (Figure 1A), as a chemically robust and highly porous as a platform for grafting flexible fluoroalkane moieties onto the walls of a MOF. We identified conditions for quantitatively flexible, linear fluoroalkanes of various lengths (CnF2n+1COOH; n=1, 3, 5, 7, 9) to the MOF interior surface (Figure 1B), while keeping the overall structure intact (as evidenced in part by unchanged powder X-ray diffraction pattern data).
N2-gas adsorption results show a systematic decrease of (a) surface area, (b) pore diameter and volume, and (c) total gas uptake with increasing the decorated perfluoroalkane chain length (e.g. comparing CF3- to C7F15- functionalized NU-1000 MOF; the surface area, pore volume and total gas uptake reduced by ~1/2, whereas the pore width reduced by only ~2 Å). Preliminary CO2 adsorption studies suggest that going from CF3- to C7F15- functionalized NU-1000 MOF the isosteric heats of adsorption increase by ~6 kJ/mol while the water uptake is reduced by half. The latter changes are nicely correlated with the pore volumes measured for these two NU-1000 MOF derivatives (Figure 2A, B). Ongoing work is aimed at completing the adsorption study as a function of chain length, this novel perfluoroalkane decorated mesoporous MOF system will be further modified, next, to fine tune the physical adsorption parameters for CO2 and H2O uptake. These modifications would involve incorporation of bi-functional system, e.g. via installing CO2-philic and hydrophobic functionalities in the same Zr6 node.
A
B
Figure 1. (A) Structural units of NU-1000; (B) Cartoon depicting perfluoroalkyl functionalized NU-1000.
2. MOF channel functionalization for carbon capture via solvent assisted linker exchange (SALE). Linker exchange offers a second means of incorporating desired flouroalkane functional groups into porous MOFs (Figure 3). Although MOFs are often regarded as rigid, almost inert materials, we have shown that SALE can be applied to some of the most robust members of the MOF family, such as zeolitic imidazolate frameworks (ZIFs). We have synthesized ZIFs with unprecedented linker-topology combinations by replacing the 2-ethylimidazolate linkers in CdIF-4 (rho topology) with 2-methylimidazolate and the 2-methylimidazolate linkers in ZIF-8 (sod topology) with unsubstituted imidazolate. The latter case led to an increase in the aperture size of the sodalite cage, and a resulting uptake of solvents of larger kinetic diameter, which was confirmed with thermogravimetric analysis experiments.
We were able to further use the SALE strategy to create a series of hydrophobic zeolitic imidazolate frameworks (ZIFs.) ZIF-69 is a gme topology ZIF composed of a 1:1 ratio of 2-nitroimidazole and 5-chlorobenzimidazole.1 Upon soaking in a 2 M solution of 5-trifluoromethyl benzimidazole at 100 °C for 3 days, the 5-trifluoromethyl benzimidazole selectively replaces only the 5-chlorobenzimidazole up to 95%. The resulting material is SALEM-10, the first ZIF
A
B
Figure 2. Plot of (A) isosteric heat of adsorption of CO2 and (B) water adsorption isotherm in CF3- (black) to C7F15- (red) functionalized NU-1000 MOF. Water adsorption isotherm for a Cr3-cluster based mesoporous MIL-101(light purple triangle) and ZIF-8 (light cyan square) MOFs are presented for comparison purpose.
synthesized using selective SALE. (Figure 4.) SALEM-10 contains 14 Å trifluoromethyl-decorated channels, allowing for maximum interaction of potential sorbates with trifluoromethyl functional groups.
Figure 3. Schematic representation of SALE
Figure 4. 2-nitroimidazole is retained, while 5-chlorobenzimidazole is substituted for 5-trifluoromethyl benzimidazole, in the first example of selective SALE in ZIFs.
The procedure was repeated for ZIF-76 (lta, 1:1 imidazole and 5-chlorobenzimidazole), ZIF-78 (gme, 1:1 2-nitroimidazole and 5-nitrobenzimidazole) and ZIF-95 (poz, 5-chlorobenzimidazole.) In the ZIF-76 and ZIF-78 cases, the 5-trifluoromethyl benzimidazole replaces the 5-chlorobenzimidazole selectively, up to 90% and 92% respectively, resulting in SALEM-11 and SALEM-10-B. In the ZIF-95 case, 5-chlorobenzimidazole is the sole linker, and it is replaced up to 81% to form SALEM-12. (Table 1.)
Table 1: Parent ZIFs and Product SALEMs. Percent exchange represents the percentage of each benzimidazole component exchanged for 5-trifluoromethyl benzimidazole.
While fluorinated moieties are considered attractive for CO2 sorption,2 there were no increases in CO2 uptake from the ZIFs to their SALEM analogues. However, there was a significant increase in hydrophobicity from the SALEM to the analogous ZIF as based on contact angle measurements. Likewise, SALEM-10 showed a decreased water vapor uptake from ZIF-69. (Figures 5-7.) As water is a non-negligible component of flue gas, hydrophobicity is a desired trait of potential CO2 sorbents, especially as many MOFs are either unstable in water,3 or competitively adsorb water over carbon dioxide. Further studies are focusing on introducing other functional groups that may simultaneously enhance carbon dioxide sorption and inhibit competitive water sorption.
Figure 5. A summary of contact angle measurements for parent ZIFs (blue) and product SALEMs (green) averaged over 15 trials.
Figure 6. Representative contact angle measurements for ZIF-69 and SALEM-10.
Figure 7. Water vapor sorption measurements for SALEM-10 and ZIF-69.
References 1. Banerjee, R., Hiroyasu, F., Britt, D., Knobler, C., O’Keeffe, M., Yaghi, O. M. J. Am. Chem. Soc., 2009, 131, 3875. 2. Almantariotis, D., Gefflaut, T., Padua, A. A. H., Coxam, J.-Y., Costa Gomes, M. F., J. Phys. Chem. B., 2010, 114, 3608. 3. Küsgens, P., Rose, M., Senkovska, I., Fröde, H., Henschel, A., Siegle, S., Kaskel, S. Microporous Mesoporous Mater., 2009, 120, 325.