- Email: [email protected]
Modeling and Simulation of Catalyst-aided Low Temperature CO2 Desorption from Blended Monoethanolamine (MEA) – N-Methyl-diethanolamine (MDEA) Solution
Available online at www.sciencedirect.com
ScienceDirect Energy Procedia 114 (2017) 1488 – 1494
13th International Conference on Greenhouse Gas Control Technologies, GHGT-13, 14-18 November 2016, Lausanne, Switzerland
Modeling and simulation of catalyst-aided low temperature CO2 desorption from blended Monoethanolamine (MEA) – N-Methyldiethanolamine (MDEA) solution Benjamin Decardi-Nelson, Ananda Akachuku, Priscilla Osei, Wayuta Srisang, Fatemeh Pouryousefi, Raphael Idem* Clean Energy Technologies Research Institute, University of Regina, 3737 Wascana Parkway, Regina, SK, Canada, S4N 1G9
Abstract A mathematical model for low temperature catalyst-aided CO2 desorption from loaded amines has been developed and validated against experimental data obtained from an integrated pilot plant utilizing blended 5M/2M MEA-MDEA using two industrial catalysts, namely, HZSM- DQGȖ-Al2O3. The rigorous model considers the presence of electrolytes and both the physical and chemical contribution of the catalyst in the desorption process. The simulation results agreed well with the experimental desorber CO2 production rate data with an AAD of 7.7 %. The validated model opens up a range of capabilities for further studies into the potential of the catalytic CO2 desorption process. © 2017 The Authors. Published by Elsevier Ltd. This is an open access article under the CC BY-NC-ND license © 2017 The Authors. Published by Elsevier Ltd. (http://creativecommons.org/licenses/by-nc-nd/4.0/). Peer-review under responsibility of the organizing committee of GHGT-13. Peer-review under responsibility of the organizing committee of GHGT-13. Keywords: Catalyst-aided CO2 desorption; Experimental validation; Integrated Pilot plant; Solid acid catalyst; Blended amines
* Corresponding author. Tel.: 1-306-585-4470; fax: 1-306-585-4855. E-mail address: [email protected]
1876-6102 © 2017 The Authors. Published by Elsevier Ltd. This is an open access article under the CC BY-NC-ND license (http://creativecommons.org/licenses/by-nc-nd/4.0/). Peer-review under responsibility of the organizing committee of GHGT-13. doi:10.1016/j.egypro.2017.03.1273
Benjamin Decardi-Nelson et al. / Energy Procedia 114 (2017) 1488 – 1494
Nomenclature AAD CO2 MDEA MEA
Absolute Average Deviation Carbon dioxide N-Methyldiethanolamine Monoethanolamine
1. Introduction The parasitic heat requirements for desorption of CO2 from loaded amines in a post combustion capture plant attached to a power plant has over the years been tackled by either solvent improvement and/or process improvement. This has led to the development of new solvents or blends of different solvents to harness the abilities of the individual solvents blended. Also, process improvements include absorber inter-cooling, stripper inter-heating, multi-pressure stripping etc. However, these solvent and process improvements are not expected to do better than 0.2 MWh/ton CO2 [1]. A recent development with a potential to address the high energy requirements is the application of a solid acid catalyst to aid in the desorption process by allowing the process to occur at temperatures below 100 °C [2-4]. In order to evaluate the potential of this technology to achieve heat requirement reduction, modeling and simulation is key. A mathematical model for the catalyst-aided desorption process has been developed and validated for the case where state-of-the-art MEA was used as solvent for CO2 in an integrated pilot plant [5]. However, most often, MEA is used as baseline to evaluate new developments or technologies for capturing CO2. It is therefore necessary to evaluate the performance of the catalyst in a mixed amine solution as well as validate the previously developed model to determine its capabilities in predicting the performance of the catalyst with blended amine solvent. This work thus presents the validation of a 1-dimensional rate-based model for catalyst-aided regeneration of CO2 in blended solution of MEA and MDEA with experimental data obtained from an integrated CO2 capture pilot plant. The simulations were conducted in Aspen Custom Modeler.
2. Model description Desorption is typically a two-phase heterogeneous system in which heat and mass transfer occurs simultaneously across the phases. The presence of the solid acid catalyst extends the system to a three phase system. In this work, the rate-based approach which is physically more consistent was used to develop the model with an assumption of a pseudohomogeneous liquid-solid phase. Fig. 1 shows a stage in a rate-based model. Loaded amine transports through the liquid film to the catalyst surface and into the catalyst pore where it reacts to form CO2 and free amine. Transport to the catalyst is handled by the activity and effectiveness factor of the catalyst hence detailed modeling of the transport phenomena is not required. The model as well as its underlying equations is presented in [5].
3. Experimental Section The experiments were conducted in an integrated pilot plant utilizing 5 M MEA and 2 M MDEA with 2 industrial catalysts, namely, Ȗ-Al2O3 and HZSM-5. The experimental data consist of 27 runs at 3 average catalyst bed temperature conditions for different catalyst weights and types. The experimental setup as well as the conditions are described in the thesis of Decardi-Nelson [5].
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Fig. 1. A rate-based stage in the catalytic CO2 desorption column, based on the 2–film theory
4. Model Validation The simulation flowsheet in ACM is shown below. The rich solvent exiting the absorber is heated in the heater before it enters the desorber. The heater is merged with the top section of the column without packing since the flow entering the column in the actual plant is most likely to be two phase after heating to the desired temperature. The gas exiting the top of the column combines with the gas from the heater to form the product gas. The lean solvent then leaves the desorber at the bottom.
Gas
ProductGas GasOut
RichSol
Mixer
Liquid Heater
Desorber
LeanSol Fig 1: Fig. 2.Simulation Simulationflowsheet flowsheet of ofmodel model in in ACM ACM
Validation is the key to determining the usefulness of the model. The kinetics of CO2 in MEA-MDEA system consist of equilibrium and kinetically controlled reactions. The equilibrium reaction constants were determined from
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the standard Gibbs free energy available in Aspen Plus databank. The kinetically controlled reaction rate constants were taken from various sources as shown in Tables 2 and 3. [6-8] Instantaneous reversible reactions
HCO3 H 2O ֖ CO32 H 3O
(R1)
MEA H 2O ֖ MEA H 2O H 2O ֖ OH H 3O
(R2)
(R3)
MDEA H 2 O ֖ MDEA H 3 O
(R4)
Kinetically controlled reversible reactions
MEACOO H 3O ֖ MEA H 2O CO2 3 ֖
HCO
(R5)
OH CO2
(R6)
MEACOO H 3O ֖ MEA H 2O CO2
(R7)
R4, R5 and R6 are assumed to be kinetically controlled and not instantaneous; hence they are approximated with fast forward and fast reverse reactions. Table 1. Kinetic parameters for kinetically controlled reactions occurring in MEA-CO2-H2O system
Reaction R5, Reverse R5, Forward R6, Reverse R6, Forward
K 9.77 x 1010 3.23 x 1019 4.20 x 1013 2.38 x 1017
E, cal/mol 9855.8 15655 13249 29451
R7, Reverse R7, Forward
2.21 x 108 8.89 x 1011
7432 15334
Comment Taken from [6] Taken from [7] Calculated using kinetic parameters of R5 reverse reaction and equilibrium constant of the reversible reaction. Taken from [8] Calculated using kinetic parameters of R7 reverse reaction and equilibrium constant of the reversible reaction.
Since the model was developed in Aspen Custom Modeler, the physical and chemical properties were taken from Aspen Properties. The model uses the Electrolyte Non-Random Two Liquids thermodynamic model to describe the non-ideal liquid phase behaviour of the system. As seen in Fig. 3, the model validates well with the experimental CO2 production rates with an absolute average deviation (AAD) of 7.7 %. Again, it can be seen that the model over-predicts the CO2 production rates at 95 °C and under-predicts at 75 °C with 85 °C being on either sides indicating a well-balanced prediction. This may be due to the fact that the model tuning parameters were fined tuned with 85 °C results hence a balanced result is seen while at other temperatures, the deviations are skewed to one side. Again, this could have been affected by several parameters and physical properties which are required in rate-based modelling and are affected differently at different temperatures.
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Table 2. Pre-exponential constants and activation energy for catalytically controlled reactions for MEA-MDEA system developed by Akachuku (2016) [9].
MEACOO MEA MDEA 2HCO3 ֖ 2 MEA 3CO 2 MDEA H 2 O OH Catalyst Ȗ-Al2O3
Rate Equation r
ko
Ea e RT
Constants
§ [ MDEA ][ MEACOO ] · ¸ u¨ ¨ 1 k [ MDEA ] k [ MDEA] ¸ 1 2 © ¹
ko
Ea
L mol.s.gcat J 6.4 u 104 , mol
1.88 u 10 9 ,
k1 =81500 k2 =7037.911 HZSM-5 r
koe
Ea RT
§ [ MDEA ][ MEACOO ] u¨ ¨ (1 k [ MDEA ] k [ MDEA] 2 ) 2 1 2 ©
· ¸ ¸ ¹
ko
Ea
1.02 u 1010 ,
L mol.s.gcat
6.630 u 10 3 ,
J mol
k1 = 371.0 k2 = 159.8
Simulated CO2 production, kg/hr
0.16 95 °C
0.14 0.12 85 °C
0.1 0.08 0.06 75 °C
0.04
AAD = 7.7 %
0.02 0 0
0.05 0.1 0.15 Experimental CO2 production, kg/hr Gamma-Alumina
HZSM 5
Fig. 3. Experimental vs. simulated CO2 production rates in the desorber for MEA-MDEA
0.2
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8
Stage(Bottom to Top)
7 6 5 4 3 2 1 0 75
80
85 Temperature, °C
Experimental
90
95
Simulation
Fig. 4. Experimental and simulated desorber temperature profile for MEA-0'($5XQ JȖ-Al2O3 catalyst at 85 °C)
CO2 desorption is always accompanied by decrease in temperature as the process is endothermic. This is seen in the decrease in the temperature as CO2 is desorbed. The shape of the temperature profiles both simulated and experimental are similar even though the model under-predicted the experimental temperature profile. However, the simulation shows a sharp drop from the top of the column and then gradual drop to the bottom while the experimental profile shows a gradual drop in temperature from the top of the column to the bottom. In an ideal system, one would expect the rate of desorption at the top to be higher than at the bottom since solvent is hotter at the top. The rate of desorption should therefore translate into sharper drop in temperature at the top of the column and then gradual drop. The model predicts this trend very well just as the experimental temperature profile. 4. Conclusions Modelling is simulation is key in the advancement of new technologies especially the area of CO2 capture as issues pertaining to design, scale up, control and optimization need to be addressed. In this work, a rate-based catalyst-aided CO2 model has been presented and validated for a case where the solvent utilized is blended MEAMDEA solution. The model considers both the physical and chemical contribution of the catalyst in the desorption process. Experimental data was obtained from an integrated pilot plant with 2 different catalysts in the desorber. The model agreed well with the experimental CO2 production rate with an AAD of 7.7 %. Again, the model predicts the shape of the temperature profile well even though the profile was under-predicted. The developed model will provide a range of capabilities for design/scale up, optimization and control of the catalytic process.
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Acknowledgements The financial support provided by the Natural Science and Engineering Research Council of Canada (NSERC), Canada Foundation for Innovation (CFI), the Clean Energy Technologies Research Institute (CETRI), and Faculty of Graduate Studies and Research (FGSR), University of Regina is gratefully acknowledged. References [1] G.T. Rochelle, '"Amine scrubbing for CO2 capture," Science, vol. 325, no. 5948, Sep 25, pp. 1652-1654. [2] R. Idem, H. Shi, D. Gelowitz and P. Tontiwachwuthikul, '"Catalytic method and apparatus for separating a gas component from an incoming gas stream," WO patent, vol. 12013821, pp. 2011. [3] Z. Liang, R. Idem, P. Tontiwachwuthikul, F. Yu, H. Liu and W. Rongwong, '"Experimental study on the solvent regeneration of a CO2䇲㼘㼛㼍㼐㼑㼐㻌㻹 㻱㻭㻌㼟㼛㼘㼡㼠㼕㼛㼚㻌㼡㼟㼕㼚㼓㻌㼟㼕㼚㼓㼘㼑㻌㼍㼚㼐㻌㼔㼥㼎㼞㼕㼐㻌㼟㼛㼘㼕㼐㻌㼍㼏㼕㼐㻌㼏㼍㼠㼍㼘㼥㼟㼠㼟㻘㻎 AIChE J., vol. 62, no. 3, pp. 753-765. [4] H. Shi, A. Naami, R. Idem and P. Tontiwachwuthikul, '"Catalytic and non catalytic solvent regeneration during absorption-based CO2 capture with single and blended reactive amine solvents," International Journal of Greenhouse Gas Control, vol. 26, pp. 39-50. [5] B. Decardi-Nelson, '"Modeling, simulation and experimental validation of a new rigorous desorber model for low temperature catalytic desorption of CO2 from CO2-loaded amine solvents over solid acid catalysts (Master's thesis),". [6] H. Hikita, S. Asai, H. Ishikawa and M. Honda, '"The kinetics of reactions of carbon dioxide with monoethanolamine, diethanolamine and triethanolamine by a rapid mixing method," the chemical Engineering Journal, vol. 13, no. 1, pp. 7-12. [7] B. Pinsent, L. Pearson and F. Roughton, '"The kinetics of combination of carbon dioxide with hydroxide ions," Transactions of the Faraday Society, vol. 52, pp. 1512-1520. [8] N. Ramachandran, A. Aboudheir, R. Idem and P. Tontiwachwuthikul, '"Kinetics of the absorption of CO2 into mixed aqueous loaded solutions of monoethanolamine and methyldiethanolamine," Ind Eng Chem Res, vol. 45, no. 8, pp. 2608-2616. [9] A. Akachuku, '"Kinetic study of the catalytic desorption of carbon dioxide (CO2) from CO2-loaded Monoethanolamine (MEA) and blended Monoethanolamine-Methyldiethanolamine (MEA-MDEA) during post comubustion CO2 capture from industrial flue gases (Master's thesis),".
ScienceDirect Energy Procedia 114 (2017) 1488 – 1494
13th International Conference on Greenhouse Gas Control Technologies, GHGT-13, 14-18 November 2016, Lausanne, Switzerland
Modeling and simulation of catalyst-aided low temperature CO2 desorption from blended Monoethanolamine (MEA) – N-Methyldiethanolamine (MDEA) solution Benjamin Decardi-Nelson, Ananda Akachuku, Priscilla Osei, Wayuta Srisang, Fatemeh Pouryousefi, Raphael Idem* Clean Energy Technologies Research Institute, University of Regina, 3737 Wascana Parkway, Regina, SK, Canada, S4N 1G9
Abstract A mathematical model for low temperature catalyst-aided CO2 desorption from loaded amines has been developed and validated against experimental data obtained from an integrated pilot plant utilizing blended 5M/2M MEA-MDEA using two industrial catalysts, namely, HZSM- DQGȖ-Al2O3. The rigorous model considers the presence of electrolytes and both the physical and chemical contribution of the catalyst in the desorption process. The simulation results agreed well with the experimental desorber CO2 production rate data with an AAD of 7.7 %. The validated model opens up a range of capabilities for further studies into the potential of the catalytic CO2 desorption process. © 2017 The Authors. Published by Elsevier Ltd. This is an open access article under the CC BY-NC-ND license © 2017 The Authors. Published by Elsevier Ltd. (http://creativecommons.org/licenses/by-nc-nd/4.0/). Peer-review under responsibility of the organizing committee of GHGT-13. Peer-review under responsibility of the organizing committee of GHGT-13. Keywords: Catalyst-aided CO2 desorption; Experimental validation; Integrated Pilot plant; Solid acid catalyst; Blended amines
* Corresponding author. Tel.: 1-306-585-4470; fax: 1-306-585-4855. E-mail address: [email protected]
1876-6102 © 2017 The Authors. Published by Elsevier Ltd. This is an open access article under the CC BY-NC-ND license (http://creativecommons.org/licenses/by-nc-nd/4.0/). Peer-review under responsibility of the organizing committee of GHGT-13. doi:10.1016/j.egypro.2017.03.1273
Benjamin Decardi-Nelson et al. / Energy Procedia 114 (2017) 1488 – 1494
Nomenclature AAD CO2 MDEA MEA
Absolute Average Deviation Carbon dioxide N-Methyldiethanolamine Monoethanolamine
1. Introduction The parasitic heat requirements for desorption of CO2 from loaded amines in a post combustion capture plant attached to a power plant has over the years been tackled by either solvent improvement and/or process improvement. This has led to the development of new solvents or blends of different solvents to harness the abilities of the individual solvents blended. Also, process improvements include absorber inter-cooling, stripper inter-heating, multi-pressure stripping etc. However, these solvent and process improvements are not expected to do better than 0.2 MWh/ton CO2 [1]. A recent development with a potential to address the high energy requirements is the application of a solid acid catalyst to aid in the desorption process by allowing the process to occur at temperatures below 100 °C [2-4]. In order to evaluate the potential of this technology to achieve heat requirement reduction, modeling and simulation is key. A mathematical model for the catalyst-aided desorption process has been developed and validated for the case where state-of-the-art MEA was used as solvent for CO2 in an integrated pilot plant [5]. However, most often, MEA is used as baseline to evaluate new developments or technologies for capturing CO2. It is therefore necessary to evaluate the performance of the catalyst in a mixed amine solution as well as validate the previously developed model to determine its capabilities in predicting the performance of the catalyst with blended amine solvent. This work thus presents the validation of a 1-dimensional rate-based model for catalyst-aided regeneration of CO2 in blended solution of MEA and MDEA with experimental data obtained from an integrated CO2 capture pilot plant. The simulations were conducted in Aspen Custom Modeler.
2. Model description Desorption is typically a two-phase heterogeneous system in which heat and mass transfer occurs simultaneously across the phases. The presence of the solid acid catalyst extends the system to a three phase system. In this work, the rate-based approach which is physically more consistent was used to develop the model with an assumption of a pseudohomogeneous liquid-solid phase. Fig. 1 shows a stage in a rate-based model. Loaded amine transports through the liquid film to the catalyst surface and into the catalyst pore where it reacts to form CO2 and free amine. Transport to the catalyst is handled by the activity and effectiveness factor of the catalyst hence detailed modeling of the transport phenomena is not required. The model as well as its underlying equations is presented in [5].
3. Experimental Section The experiments were conducted in an integrated pilot plant utilizing 5 M MEA and 2 M MDEA with 2 industrial catalysts, namely, Ȗ-Al2O3 and HZSM-5. The experimental data consist of 27 runs at 3 average catalyst bed temperature conditions for different catalyst weights and types. The experimental setup as well as the conditions are described in the thesis of Decardi-Nelson [5].
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Fig. 1. A rate-based stage in the catalytic CO2 desorption column, based on the 2–film theory
4. Model Validation The simulation flowsheet in ACM is shown below. The rich solvent exiting the absorber is heated in the heater before it enters the desorber. The heater is merged with the top section of the column without packing since the flow entering the column in the actual plant is most likely to be two phase after heating to the desired temperature. The gas exiting the top of the column combines with the gas from the heater to form the product gas. The lean solvent then leaves the desorber at the bottom.
Gas
ProductGas GasOut
RichSol
Mixer
Liquid Heater
Desorber
LeanSol Fig 1: Fig. 2.Simulation Simulationflowsheet flowsheet of ofmodel model in in ACM ACM
Validation is the key to determining the usefulness of the model. The kinetics of CO2 in MEA-MDEA system consist of equilibrium and kinetically controlled reactions. The equilibrium reaction constants were determined from
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Benjamin Decardi-Nelson et al. / Energy Procedia 114 (2017) 1488 – 1494
the standard Gibbs free energy available in Aspen Plus databank. The kinetically controlled reaction rate constants were taken from various sources as shown in Tables 2 and 3. [6-8] Instantaneous reversible reactions
HCO3 H 2O ֖ CO32 H 3O
(R1)
MEA H 2O ֖ MEA H 2O H 2O ֖ OH H 3O
(R2)
(R3)
MDEA H 2 O ֖ MDEA H 3 O
(R4)
Kinetically controlled reversible reactions
MEACOO H 3O ֖ MEA H 2O CO2 3 ֖
HCO
(R5)
OH CO2
(R6)
MEACOO H 3O ֖ MEA H 2O CO2
(R7)
R4, R5 and R6 are assumed to be kinetically controlled and not instantaneous; hence they are approximated with fast forward and fast reverse reactions. Table 1. Kinetic parameters for kinetically controlled reactions occurring in MEA-CO2-H2O system
Reaction R5, Reverse R5, Forward R6, Reverse R6, Forward
K 9.77 x 1010 3.23 x 1019 4.20 x 1013 2.38 x 1017
E, cal/mol 9855.8 15655 13249 29451
R7, Reverse R7, Forward
2.21 x 108 8.89 x 1011
7432 15334
Comment Taken from [6] Taken from [7] Calculated using kinetic parameters of R5 reverse reaction and equilibrium constant of the reversible reaction. Taken from [8] Calculated using kinetic parameters of R7 reverse reaction and equilibrium constant of the reversible reaction.
Since the model was developed in Aspen Custom Modeler, the physical and chemical properties were taken from Aspen Properties. The model uses the Electrolyte Non-Random Two Liquids thermodynamic model to describe the non-ideal liquid phase behaviour of the system. As seen in Fig. 3, the model validates well with the experimental CO2 production rates with an absolute average deviation (AAD) of 7.7 %. Again, it can be seen that the model over-predicts the CO2 production rates at 95 °C and under-predicts at 75 °C with 85 °C being on either sides indicating a well-balanced prediction. This may be due to the fact that the model tuning parameters were fined tuned with 85 °C results hence a balanced result is seen while at other temperatures, the deviations are skewed to one side. Again, this could have been affected by several parameters and physical properties which are required in rate-based modelling and are affected differently at different temperatures.
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Table 2. Pre-exponential constants and activation energy for catalytically controlled reactions for MEA-MDEA system developed by Akachuku (2016) [9].
MEACOO MEA MDEA 2HCO3 ֖ 2 MEA 3CO 2 MDEA H 2 O OH Catalyst Ȗ-Al2O3
Rate Equation r
ko
Ea e RT
Constants
§ [ MDEA ][ MEACOO ] · ¸ u¨ ¨ 1 k [ MDEA ] k [ MDEA] ¸ 1 2 © ¹
ko
Ea
L mol.s.gcat J 6.4 u 104 , mol
1.88 u 10 9 ,
k1 =81500 k2 =7037.911 HZSM-5 r
koe
Ea RT
§ [ MDEA ][ MEACOO ] u¨ ¨ (1 k [ MDEA ] k [ MDEA] 2 ) 2 1 2 ©
· ¸ ¸ ¹
ko
Ea
1.02 u 1010 ,
L mol.s.gcat
6.630 u 10 3 ,
J mol
k1 = 371.0 k2 = 159.8
Simulated CO2 production, kg/hr
0.16 95 °C
0.14 0.12 85 °C
0.1 0.08 0.06 75 °C
0.04
AAD = 7.7 %
0.02 0 0
0.05 0.1 0.15 Experimental CO2 production, kg/hr Gamma-Alumina
HZSM 5
Fig. 3. Experimental vs. simulated CO2 production rates in the desorber for MEA-MDEA
0.2
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8
Stage(Bottom to Top)
7 6 5 4 3 2 1 0 75
80
85 Temperature, °C
Experimental
90
95
Simulation
Fig. 4. Experimental and simulated desorber temperature profile for MEA-0'($5XQ JȖ-Al2O3 catalyst at 85 °C)
CO2 desorption is always accompanied by decrease in temperature as the process is endothermic. This is seen in the decrease in the temperature as CO2 is desorbed. The shape of the temperature profiles both simulated and experimental are similar even though the model under-predicted the experimental temperature profile. However, the simulation shows a sharp drop from the top of the column and then gradual drop to the bottom while the experimental profile shows a gradual drop in temperature from the top of the column to the bottom. In an ideal system, one would expect the rate of desorption at the top to be higher than at the bottom since solvent is hotter at the top. The rate of desorption should therefore translate into sharper drop in temperature at the top of the column and then gradual drop. The model predicts this trend very well just as the experimental temperature profile. 4. Conclusions Modelling is simulation is key in the advancement of new technologies especially the area of CO2 capture as issues pertaining to design, scale up, control and optimization need to be addressed. In this work, a rate-based catalyst-aided CO2 model has been presented and validated for a case where the solvent utilized is blended MEAMDEA solution. The model considers both the physical and chemical contribution of the catalyst in the desorption process. Experimental data was obtained from an integrated pilot plant with 2 different catalysts in the desorber. The model agreed well with the experimental CO2 production rate with an AAD of 7.7 %. Again, the model predicts the shape of the temperature profile well even though the profile was under-predicted. The developed model will provide a range of capabilities for design/scale up, optimization and control of the catalytic process.
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Acknowledgements The financial support provided by the Natural Science and Engineering Research Council of Canada (NSERC), Canada Foundation for Innovation (CFI), the Clean Energy Technologies Research Institute (CETRI), and Faculty of Graduate Studies and Research (FGSR), University of Regina is gratefully acknowledged. References [1] G.T. Rochelle, '"Amine scrubbing for CO2 capture," Science, vol. 325, no. 5948, Sep 25, pp. 1652-1654. [2] R. Idem, H. Shi, D. Gelowitz and P. Tontiwachwuthikul, '"Catalytic method and apparatus for separating a gas component from an incoming gas stream," WO patent, vol. 12013821, pp. 2011. [3] Z. Liang, R. Idem, P. Tontiwachwuthikul, F. Yu, H. Liu and W. Rongwong, '"Experimental study on the solvent regeneration of a CO2䇲㼘㼛㼍㼐㼑㼐㻌㻹 㻱㻭㻌㼟㼛㼘㼡㼠㼕㼛㼚㻌㼡㼟㼕㼚㼓㻌㼟㼕㼚㼓㼘㼑㻌㼍㼚㼐㻌㼔㼥㼎㼞㼕㼐㻌㼟㼛㼘㼕㼐㻌㼍㼏㼕㼐㻌㼏㼍㼠㼍㼘㼥㼟㼠㼟㻘㻎 AIChE J., vol. 62, no. 3, pp. 753-765. [4] H. Shi, A. Naami, R. Idem and P. Tontiwachwuthikul, '"Catalytic and non catalytic solvent regeneration during absorption-based CO2 capture with single and blended reactive amine solvents," International Journal of Greenhouse Gas Control, vol. 26, pp. 39-50. [5] B. Decardi-Nelson, '"Modeling, simulation and experimental validation of a new rigorous desorber model for low temperature catalytic desorption of CO2 from CO2-loaded amine solvents over solid acid catalysts (Master's thesis),". [6] H. Hikita, S. Asai, H. Ishikawa and M. Honda, '"The kinetics of reactions of carbon dioxide with monoethanolamine, diethanolamine and triethanolamine by a rapid mixing method," the chemical Engineering Journal, vol. 13, no. 1, pp. 7-12. [7] B. Pinsent, L. Pearson and F. Roughton, '"The kinetics of combination of carbon dioxide with hydroxide ions," Transactions of the Faraday Society, vol. 52, pp. 1512-1520. [8] N. Ramachandran, A. Aboudheir, R. Idem and P. Tontiwachwuthikul, '"Kinetics of the absorption of CO2 into mixed aqueous loaded solutions of monoethanolamine and methyldiethanolamine," Ind Eng Chem Res, vol. 45, no. 8, pp. 2608-2616. [9] A. Akachuku, '"Kinetic study of the catalytic desorption of carbon dioxide (CO2) from CO2-loaded Monoethanolamine (MEA) and blended Monoethanolamine-Methyldiethanolamine (MEA-MDEA) during post comubustion CO2 capture from industrial flue gases (Master's thesis),".