Open Access

Thermal degradation of aqueous 2-aminoethylethanolamine in CO2 capture; identification of degradation products, reaction mechanisms and computational studies

  • Idris Mohamed Saeed1,
  • Vannajan Sanghiran Lee2,
  • Shaukat Ali Mazari3,
  • B. Si Ali1,
  • Wan Jeffrey Basirun2Email author,
  • Anam Asghar1,
  • Lubna Ghalib1 and
  • Badrul Mohamed Jan1
Chemistry Central Journal201711:10

DOI: 10.1186/s13065-016-0231-7

Received: 24 May 2016

Accepted: 7 December 2016

Published: 24 January 2017


Amine degradation is the main significant problems in amine-based post-combustion CO2 capture, causes foaming, increase in viscosity, corrosion, fouling as well as environmental issues. Therefore it is very important to develop the most efficient solvent with high thermal and chemical stability. This study investigated thermal degradation of aqueous 30% 2-aminoethylethanolamine (AEEA) using 316 stainless steel cylinders in the presence and absence of CO2 for 4 weeks. The degradation products were identified by gas chromatography mass spectrometry (GC/MS) and liquid chromatography-time-of-flight-mass spectrometry (LC-QTOF/MS). The results showed AEEA is stable in the absence of CO2, while in the presence of CO2 AEEA showed to be very unstable and numbers of degradation products were identified. 1-(2-Hydroxyethyl)-2-imidazolidinone (HEIA) was the most abundance degradation product. A possible mechanism for the thermal degradation of AEEA has been developed to explain the formation of degradation products. In addition, the reaction energy of formation of the most abundance degradation product HEIA was calculated using quantum mechanical calculation.


2-aminoethylethanolamine (AEEA) CO2 capture Thermal degradation Mechanism Computational study


Post-combustion CO2 capture is a topic of the environmental and climatic mitigation of carbon based energy system. Several studies have surveyed the environmental and climatic mitigation of carbon based energy system [1], and the impacts of lower-pollution energy system transition [2], including natural gas others [3, 4]. One of obvious conclusions is that without carbon capture and storage, carbon based energy system could not avoid the additional global warming. Post-combustion CO2 capture would reduce the pollutants and carbon emission, and increase environmental and climatic health. Post-combustion based on amine CO2 capture is the most dominant technology used for CO2 capture. This technique uses different aqueous alkanolamines to absorb CO2 gas from flue gas stream. This technology has several advantages such as good reactivity, high capacity and low cost. Moreover, the alkanolamines can be recovered after the completion of the whole process [5, 6].

However, alkanolamines also undergo irreversible reaction with acid gases to produce undesired compounds. Alkanolamines suffers from thermal and oxidative degradation. Thermal degradation occurs due to the high temperature in the stripper, and may also occur in the cross heat exchanger and the reclaimer, depending on the configuration [7, 8]. Degradation of amines is undesirable for amine-based CO2 capture as this causes growing economic burden and may cause operating problems like fouling, corrosion and foaming [911]. Amine degradation is one of the major issues associated with amine based post combustion carbon capture (PCC). The degradation products from the process causes foaming, increased viscosity, high corrosion of equipment and fouling [12, 13]. Furthermore, emissions and disposal of degradation products cause environmental and health issues. These contribute to economic glitches, which requires urgent panacea.

In recent years, new solvent such as 2-Aminoethylethanolamine (AEEA) has been utilized as an absorbent for CO2 from post-combustion exhaust gases [14, 15]. AEEA is a diamine, which contains two nitrogen atoms that can absorb CO2 and one OH group which increases the solubility in aqueous solution. AEEA exhibit better performance than other industrial amine such as N-methylethanolamine (MEA) [15], due to the higher solubility, lower vapor pressure, higher absorption capacity, greater heat absorption and lower desorption energy [1418].

There is a lack of data regarding to the thermal degradation investigation of AEEA-based CO2 scrubbing system, and the degradation product formation pathways and that require further research. In this article, the thermal degradation of 30% AEEA is presented in detail. Identification, reaction mechanism, computational chemistry studies of the degradation products are proposed and discussed.

Experimental methods


All chemicals such as 2-aminoethylethanolamine (AEEA) (≥98%), barium chloride (BaCl2) and standards solutions of hydrochloric acid (HCl), sodium hydroxide (NaOH) and sulfuric acid (H2SO4) were procured from Merck (Malaysia). Carbon dioxide (99%) and N2 (≥99.99%) gases were procured from a Linder (Malaysia). All chemicals were used as purchased without further purification.

Sample preparation and CO2 loading experiments

An aqueous AEEA solution was prepared in weight percent with concentrations of 30 wt% and diluted using di-ionized water. In the CO2 loading experiment, the reactor was equipped with a magnetic stirrer, and a pH meter linked to data acquisition system. A pH Probe linked to Metrohm was used to monitor the solution pH versus time. Figure 1 provides a description of the experimental setup. The reaction started by introducing a volume of 100 ml of 30% wt of aqueous AEEA into a double jacket reactor. The solution was then purged with nitrogen gas for 5 min to remove any possible dissolved oxygen. The CO2 gas was introduced into the reactor until it became saturated with CO2 with pH 7. Then samples were taken and transferred into the cylinders and CO2 loading was verified by titration [19]. In CO2 loading determination, two samples of nearly 0.5 g were withdrawn form reactor, and transferred into a mixture of 50 ml NaOH (0.1 M) and 25 ml of BaCl2 (0.5 M) in a 250 ml Erlenmeyer flask. The reaction of BaCl2 and NaOH with CO2 result in the formation of white precipitates of BaCO3. Samples were heated, then cooled and filtered using 0.45 µm pore size silicon filter paper. The white crystals were washed with 50 ml deionized water, and then 0.1 M HCl was added until all crystals dissolved. Acidified samples were then titrated with 0.1 M NaOH. All the titration tasks were performed using 785 DMP Titrino auto-titrator installed with Tiamo 1.3–45.
Fig. 1

Schematic diagram of CO2 loading setup for amine saturation method

Thermal degradation experiments

The thermal degradation experiment was performed in a metal cylinder (5 in. length and ½ in.outer diameter) made from 316 stainless steel and equipped with Swagelok end-caps. The method used was similar to Davis et al. [20]. 8 ml of sample with and without CO2 were introduced directly into the cylinder, placed in a Memmert 600 oven and heated at 135 °C, above the stripper temperature (to accelerate the reaction). Experiments were conducted at high temperature 135 °C as intention was to accelerate the thermal degradation to produce highly degraded samples within a reasonable timeframe.

The cylinders were periodically removed from the oven (once per week) during the whole 4 weeks. Any suspected leakage was checked by the weight differences of before and after the experiments. After the cylinders were cooled to room temperature, the samples were transferred to vials and kept refrigerated at 5 °C to quench the reaction and finally subjected to further analysis.

Analytical methods

Gas chromatography–mass spectrometry (GC–MS)

The GC–MS instrument (model 6890 N/5973 N) was from Shimadzu coupled with mass spectrometer (MS) using Shimadzu GCMS-QP2010, with Ultra autosampler AOC 20I+S. The separation of amines and degradation products were performed in RTX ®-5MS column using the conditions shown in Table 1. Each sample was diluted using methanol mixture in the ratio of 1:50 prior to the analysis to avoid contamination of the system and to provide a higher sensitivity. The analysis was performed for 30 min to ensure the elution of heavy degradation compounds.
Table 1

GC–MS parameters for identifications of degradation products



Length (m)


Internal diameter (µm)

0.25 mm

Thickness (µm)

0.25 µm

Initial temp. (°C)


Initial hold time (min)


Oven ramp (1) (°C min–1)


Oven ramp (2) (°C min–1)


Final temp. (°C)


Final hold time (min)


Injector temp. (°C)


Flow rate (constant) (ml min−1)


Carrier gas


Liquid chromatography-time-of-flight-mass spectrometry (LC-QTOF-MS)

The analyses of the degraded samples were carried out using an Agilent 1260 infinity liquid chromatography coupled with 6224 time-of-flight (TOF) MS. The molecules were converted to ions by an electrospray ionization source (ESI). The column used was Zorbax Eclipse Plus (2.1 × 100 mm) and the amount of injected volume was 20 µl. The eluent was 0.10% formic acid in water (1) and methanol (2). A gradient profile is described in Table 2. The flow rate was set at 0.200 ml/min. The method developed by Huang et al. [21] was used for the detection of the degradation products.
Table 2

Gradient profile for the mobile phase ratio in this experiment

Time (min)

Mobile phase ratio

Formic acid (0.10%)

Methanol (99.9%)










Computational details

All the transition state structures and reactants were fully optimized, in the gas phase at 298.15K at B3LYP/6-311++G(d, p) level of theory using the Gaussian09 [22] and GaussView visualization program [23]. The transition state calculations of the proposed mechanisms were carried out. Synchronous transition methods were used to find a transition state (TS) under D mol3 module in Material Studio 4.4 for the structure optimization and reaction path calculations. All calculations were performed using the density functional theory (DFT) with local density approximation (LDA) of local functional PWC [24], with effective core potential treatment with the DN basis set. The reaction paths were obtained using the linear synchronous transit (LST) and optimization calculation performs a single interpolation to a maximum energy, followed by the quadratic synchronous transit (QST) method, for an energy maximum with constrained minimizations in order to refine the transition state to a high degree [25]. Another conjugate gradient minimization was performed at each point. The cycle was repeated until a stationary point was located or the number of allowed QST steps was exhausted. After the initial paths were converged, the highest energy points were optimized to the closest transition state (TS). Following the TS optimization, the minimum energy path (MEP) between the critical points were calculated with the nudged elastic band (NEB), to ensure continuity of the path and projection of the force, so that the system converges to the MEP. The TS were checked at the B3LYP/6-311++G (d, p) level by evaluating the vibrational frequencies. The optimized geometries obtained were characterized as stationary points on the potential energy surface (PES) and the transition states were characterized by only one imaginary frequency, which is confirmed to represent the most accurate reaction coordinate. The computational method used in this study is similar to Lee et al. [26].

Results and discussions

The investigation of formation of thermal degradation products in AEEA system was conducted in three different conditions; thermal degradation in the absence of CO2 (AEEA/H2O), thermal degradation in the presence of CO2 (AEEA/H2O/CO2) and quantum mechanical calculations of the formation of the main degradation product (HEIA). In the AEEA/H2O system, the aqueous amine solution was heated at 135 °C for 4 weeks. In the AEEA/H2O/CO2 system, the amine solution was first loaded with CO2 (α = 0.80 mol CO2/mol of amine) and then heated to 135 °C for 4 weeks. At the end of each experiment, the liquid phase analysis was carried out by using GC–MS and LC-QTOF-MS to identify the degradation products.

Identification of degradation products

The identification of amine degradation products were performed by GC–MS and LC-MS-QTOF techniques which are listed in Table 2. No degradation products were identified during the thermal degradation of AEEA in the absence of CO2. However, 27 degradation products were detected during the thermal degradation of AEEA in the presence of CO2. 1-(2-Hydroxyethyl)-2-imidazolidinone (HEIA) was the most abundant degradation product in the system, Fig. 2 represents the GC chromatogram of a sample of the thermal degradation of AEEA and mass spectrum of HEIA after 4 weeks. Low molecular weight volatile compounds such as ammonia are other degradation products which were likely to be formed in the process. However, the analytical methods employed in this work could not facilitate the detection. In this study, heat stable salts (HSS) such as formate, acetate were identified in this study in agreement with literature [27, 28]. However, the presence of HSS due to presence of oxygen in head space inside the cylinder as by-products of CO2 reduction that formed during degradation [28]. However, those products couldn’t be identified due to the limitations of our analytical techniques (Table 3).
Fig. 2

Gas chromatogram (a) and mass spectrum of HEIA (b) of aqueous AEEA solution After 4 weeks of the experiment using 30 wt% AEEA at temperature 135 °C with 0.80 moleCO2/mol of amine

Table 3

Compounds identified by the present study by using GC-MS and LC-MS-QTOF in AEEA/CO2/H2O system at 135 °C



MW (g/mol)


Analytical technique

































































N-(2-hydroxyethyl)-N -methylpiperazine
























1-(2-(2-Hydroxyethoxy)ethyl) piperazine













Amine lose and the concentration of the degradation products

The concentration profiles of initial amine (AEEA) and the degradation products of 2-hydroxyethyl-2-oxazolidone (HEIA), (3-(2-Hydroxyethyl)-2-oxazolidinone (HEOD) and 1,4-Bis(2-hydroxyethyl)piperazine (BHEP) concentrations in the samples degraded at 135 °C were obtained as a function of time, as shown in Fig. 3. Concentration of HEIA increased with time and then a little decreased, representing that it is stable product and it plays a role as intermediate after 3 weeks undergoing further reaction rather than a final product. In addition, it is observed that the DEA and BHEP concentrations were very small during the experimental run, which suggests that it may be a key intermediate compound.
Fig. 3

Percentage of AEEA loss and formation of degradation products

Possible reaction pathway of identified degradation products

An overall reaction pathway has been developed to explain the formation of the major products during the thermal degradation. The objective is to understand the most probable reactions which occur during the thermal degradation process and offer solutions for the elimination of a particular degradation product. The reaction mechanism of the thermal degradation of AEEA was proposed based on the reaction of AEEA with CO2 in aqueous solution.

Nevertheless, the proposed reaction mechanism of main degradation products based on this study and literature is debated in this manuscript. Products like HEIA, HEOD, BHEP are the abundant degradation products as per this study. So mechanism postulated in this study is based on the main products. Most of the reaction mechanisms were proposed based on the influence of the ionic species (carbamate and dicarbmate) in the solution.

1-(2-Hydroxyethyl)-2-imidazolidinone (HEIA) and 2-hydroxyethyl-2-oxazolidone (HEOD)

AEEA is a type of diamine compound which contains two nitrogen atoms and reacts with CO2 to form several ionic species. It is also known that any ethylenediamine type of structure with two amino groups separated by an ethylene molecule, should form a cyclic urea when exposed to CO2 [28]. Cyclic urea, such as 1-(2-Hydroxyethyl)-2 imidazolidinone (HEIA), were observed in MEA degradation and the reaction mechanism in this work is similar to the literature [20, 29]. HEIA is the most abundance degradation products in thermal degradation of AEEA. The formation of HEIA postulated through two different pathways. In Scheme 1, at the presence of CO2 HEIA (5) formed at high temperature via the carbamate formation, by dehydration and internal cyclization of the secondary AEEA Carbamate (4). Also There is other possibility of internal cyclization of AEEA secondary carbamate and released of Ammonia to form 2-hydroxyethyl-2-oxazolidone (HEOD) (6). This is analogous to the oxazolidone formation in the presence of ethanolamine and CO2, which was described in detail in the thermal degradation of MEA and DEA [20, 28, 3032]. The other possibility of thermal degradation of carbonated AEEA is generation of HEIA which occurred through internal cyclization of AEEA primary carbamate (7) to generate HEIA (8).
Scheme 1

Proposed mechanisms for the formation of HEIA and HEOD

2-Imidazolidinone (HEI)

Scheme 2 showed the formation of another type of cyclic urea (HEI) which generated during the thermal degradation of AEEA by the protonation of HEIA (1), followed by the elimination of ethyl alcohol of protonated (HEIA) (2) to produce 2-Imidazolidinone (3) and released ethylene oxide molecule (4).
Scheme 2

Proposed mechanisms for the formation of HEI

1,4-Diformylpiperazine (DFP)

Also at high temperature, the ring closure of dicarbamate-AEEA (1) will result in the formation of di-carbamate piperazine (2), followed by the protonation of the carbonyl in both amides (3) which further breaks the O–C bond and forms the π bond to produce the 1,4-Diformylpiperazine (4), according to Scheme 3.
Scheme 3

Proposed mechanism for the formation of DFP

1,4-Bis(2-hydroxyethyl)piperazine (BHEP)

BHEP is a cyclic triamine which is formed by the nucleophilic attack of the HEOD (1) by AEEA (2), where the ring opening promotes the formation of 2-((2-Aminoethyl)-(2-(2-aminoethylamino)-(ethylamino)ethanol (AAEEA) (3). This is followed by the internal cyclization of the AAEEA (3) which releases ammonia (4) and produces the BHEP (5), as shown in Scheme 4.
Scheme 4

Proposed mechanism for the formation of BHEP

N,N’-Dimethyl-2-imidazolidinone (DMDZ)

The generation of N,N’-Dimethyl-2-imidazolidinone (DMDZ) happen by the attack of formic acid, formaldehyde through a reaction called Eschweiler-Clarke reaction. The reaction began by methylation of amine with protonated formaldehyde to form an iminium ion intermediate, which further react formic acid to form methylated ammonium ion and released CO2 as by product. The deprotonation of the ammonium ion affords the final methylated amine product. These steps are repeated twice to give the final tertiary amine product, according to Scheme 5.
Scheme 5

Proposed mechanisms for the formation of DMDZ

Computational results

In this work, the different pathways of formation of HEIA are investigated theoretically using quantum mechanical calculations. In Figs. 4 and 5, the schematic details of the reaction mechanism, including the transition states, for the formation of HEIA is presented.
Fig. 4

Reaction energy profile for the formation of HEIA (path 1) based on B3LYP/6-311++g(d, p) calculation

Fig. 5

Reaction energy profile for the formation of HEIA (path 2) based on B3LYP/6-311++g(d, p) calculation

The first possibility pathway (path 1) involves the addition of CO2 to the secondary amine in AEEA, with simultaneous dehydration to form HEIA and water molecule with an energy barrier of −2.15 kcal/mol. The second mechanism (path 2) involves the addition of CO2 to the primary amine in AEEA, with simultaneous dehydration and intermolecular cyclization to form the HEIA and water molecule with an energy barrier of −6.97 kcal/mol. Path 1 has higher activation energy than path 2. The optimized bond lengths in (Å) at the B3LYP/6-31+G(d, p) level of theory are given for the bonds involved in the transition state (Table 4).
Table 4

The computed energy and activation barriers for TS1, TS2 obtained at B3LYP/6-311++g(d, p) level of theory for the formation of product according to Figs. 4 and 5


Energy (Ha)

Relative energy (Ha)

Relative energy (kcal/mol)

Reactant 1








Product 1




Reactant 2








Product 2





Thermal degradation of 30% AEEA was performed in the presence and absence of CO2 loading at 135 °C. AEEA showed high stability in the absence of CO2, and no degradation products were identified. However, AEEA degraded significantly in the presence of CO2 and twenty-seven degradation products were identified by GC–MS based on the (NIST) library search, and based on LC-QTOF-MS search. 2-hydroxyethyl imidazolidone (HEIA) was the most abundant degradation product, which contributed to the loss of the AEEA concentration. The reaction energy of HEIA formation were calculated for the both pathways of its formations and found to be −2.15 kcal/mol and −6.97 kcal/mol. Degradation rates of AEEA show that it may not be a choice of commercialization or large CO2. However, under lab scale more investigation may be conducted by using degradation inhibitors. Or another way may be modification of AEEA by addition of an alkyl group to the amines groups could be a possible way to prevent the carbamate formation.


Authors’ contributions

WJB initiate the idea of this work, IMS prepare the solutions and conduct the degradation experiments, VSL carried out the quantum mechanical calculations, BSA and BHMJ assested to write and revised the final manuscript. AA and LG developed the CO2 loading setup. SAM carried out the sample analysis using chromatographic techniques. All authors read and approved the final manuscript.


We are thankful to University of Malaya Research Grant (UMRG): RP038C 15HTM, RP020C-14AFR, RP031B-15AFR and IPPP (PG209-2014B) University of Malaya, Kuala Lumpur, Malaysia 50603 for financial assistance.

Competing interests

The authors declare that they have no competing interests.

Open AccessThis article is distributed under the terms of the Creative Commons Attribution 4.0 International License (, which permits unrestricted use, distribution, and reproduction in any medium, provided you give appropriate credit to the original author(s) and the source, provide a link to the Creative Commons license, and indicate if changes were made. The Creative Commons Public Domain Dedication waiver ( applies to the data made available in this article, unless otherwise stated.

Authors’ Affiliations

Department of Chemical Engineering, Faculty of Engineering, University of Malaya
Department of Chemistry, Faculty of Science, University of Malaya
Department of Chemical Engineering, Dawood University of Engineering and Technology


  1. Zhan SF, Zhang XC, Ma C (2009) Coal classification based on environmental protection and burning quality. J China Coal Soc. 34:1535–1539Google Scholar
  2. Zhang X, Chen W, Ma C, Zhan S (2013) Modeling particulate matter emissions during mineral loading process under weak wind simulation. Sci Total Environ 449:168–173View ArticleGoogle Scholar
  3. Zhang X, Myhrvold NP, Caldeira K (2014) Key factors for assessing climate benefits of natural gas versus coal electricity generation. Environ Res Let 9(11):114022View ArticleGoogle Scholar
  4. Zhang X, Chen W, Ma C, Zhang G, Ju M (2012) Assessment method for regional environmental risk based on pressure-state-response model. China Environ Sci. 32:84–87Google Scholar
  5. Zhao Z, Dong H, Huang Y, Cao L, Gao J, Zhang X et al (2015) Ionic degradation inhibitors and kinetic models for CO2 capture with aqueous monoethanolamine. Int J Greenhouse Gas Control 39:119–128View ArticleGoogle Scholar
  6. Gouedard C, Picq D, Launay F, Carrette P-L (2012) Amine degradation in CO2 capture. I. A review. Int J Greenhouse Gas Control 10:244–270View ArticleGoogle Scholar
  7. Rochelle GT (2012) Thermal degradation of amines for CO2 capture. Curr Opin Chem Eng. 1(2):183–190View ArticleGoogle Scholar
  8. Mazari SA, Ali BS, Jan BM, Saeed IM, Nizamuddin S (2015) An overview of solvent management and emissions of amine-based CO2 capture technology. Int J Greenhouse Gas Control 34:129–140View ArticleGoogle Scholar
  9. Mazari SA, Ali BS, Jan BM, Saeed IM (2014) Degradation study of piperazine, its blends and structural analogs for CO2 capture: a review. Int J Greenhouse Gas Control 31:214–228View ArticleGoogle Scholar
  10. Vevelstad SJ, Grimstvedt A, Knuutila H, da Silva EF, Svendsen HF (2014) Influence of experimental setup on amine degradation. Int J Greenhouse Gas Control 28:156–167View ArticleGoogle Scholar
  11. Fytianos G, Ucar S, Grimstvedt A, Hyldbakk A, Svendsen HF, Knuutila HK (2016) Corrosion and degradation in MEA based post-combustion CO2 capture. Int J Greenhouse Gas Control 46:48–56View ArticleGoogle Scholar
  12. Zoannou K-S, Sapsford DJ, Griffiths AJ (2013) Thermal degradation of monoethanolamine and its effect on CO2 capture capacity. Int J Greenhouse Gas Control 17:423–430View ArticleGoogle Scholar
  13. Rey A, Gouedard C, Ledirac N, Cohen M, Dugay J, Vial J et al (2013) Amine degradation in CO2 capture. 2. New degradation products of MEA. Pyrazine and alkylpyrazines: analysis, mechanism of formation and toxicity. Int J Greenhouse Gas Control 19:576–583View ArticleGoogle Scholar
  14. Ma’mun S, Jakobsen JP, Svendsen HF, Juliussen O (2006) Experimental and modeling study of the solubility of carbon dioxide in aqueous 30 mass% 2-((2-aminoethyl) amino) ethanol solution. Ind Eng Chem Res 45(8):2505–2512View ArticleGoogle Scholar
  15. Mamun S, Svendsen HF, Hoff KA, Juliussen O (2007) Selection of new absorbents for carbon dioxide capture. Energy Convers Manag. 48(1):251–258View ArticleGoogle Scholar
  16. Bonenfant D, Mimeault M, Hausler R (2003) Determination of the structural features of distinct amines important for the absorption of CO2 and regeneration in aqueous solution. Ind Eng Chem Res 42(14):3179–3184View ArticleGoogle Scholar
  17. Kierzkowska-Pawlak H (2015) Kinetics of CO2 absorption in aqueous N, N-diethylethanolamine and its blend with N-(2-aminoethyl) ethanolamine using a stirred cell reactor. Int J Greenhouse Gas Control 37:76–84View ArticleGoogle Scholar
  18. Ma’mun S, Dindore VY, Svendsen HF (2007) Kinetics of the reaction of carbon dioxide with aqueous solutions of 2-((2-aminoethyl) amino) ethanol. Ind Eng Chem Res 46(2):385–394View ArticleGoogle Scholar
  19. Hilliard MD (2008) A predictive thermodynamic model for an aqueous blend of potassium carbonate, piperazine, and monoethanolamine for carbon dioxide capture from flue gas
  20. Davis JD (2009) Thermal degradation of aqueous amines used for carbon dioxide capture
  21. Huang Q, Bhatnagar S, Remias JE, Selegue JP, Liu K (2013) Thermal degradation of amino acid salts in CO2 capture. Int J Greenhouse Gas Control 19:243–250View ArticleGoogle Scholar
  22. Frisch MJ, Trucks GW, Schlegel HB, Scuseria GE, Robb MA, Cheeseman JR, Scalmani G, Barone V, Mennucci B, Petersson GA et al (2009) Gaussian09 RA.1. Gaussian Inc., WallingfordGoogle Scholar
  23. Dennington R, Keith T, Millam J (2009) GaussView, version 5. Semichem Inc, Shawnee MissionGoogle Scholar
  24. Perdew JP, Wang Y (1992) High-precision sampling for brillouin-zone integration in metals. Phys Rev B. 45(23):13View ArticleGoogle Scholar
  25. Halgren TA, Lipscomb WN (1977) The synchronous-transit method for determining reaction pathways and locating molecular transition states. Chem Phys Lett 49(2):225–232View ArticleGoogle Scholar
  26. Lee VS, Kodchakorn K, Jitonnom J, Nimmanpipug P, Kongtawelert P, Premanode B (2010) Influence of metal cofactors and water on the catalytic mechanism of creatininase-creatinine in aqueous solution from molecular dynamics simulation and quantum study. J Comput Aided Mol Des 24(10):879–886View ArticleGoogle Scholar
  27. Lawal O, Bello A, Idem R (2005) The role of methyl diethanolamine (MDEA) in preventing the oxidative degradation of CO2 loaded and concentrated aqueous monoethanolamine (MEA)-MDEA blends during CO2 absorption from flue gases. Ind Eng Chem Res 44(6):1874–1896View ArticleGoogle Scholar
  28. Freeman SA, Rochelle GT (2012) Thermal degradation of aqueous piperazine for CO2 capture: 2. Product types and generation rates. Ind Eng Chem Res 51(22):7726–7735View ArticleGoogle Scholar
  29. Lepaumier H (2008) Etude des mécanismes de dégradation des amines utilisées pour le captage du CO2 dans les fumées
  30. Lepaumier H, Picq D, Carrette P-L (2009) New amines for CO2 capture. I. Mechanisms of amine degradation in the presence of CO2. Ind Eng Chem Res 48(20):9061–9067View ArticleGoogle Scholar
  31. Willson CG, Lawler DF Oxidation and thermal degradation of methyldiethanolamine/piperazine in CO2 capture
  32. Kennard ML, Meisen A (1985) Mechanisms and kinetics of diethanolamine degradation. Ind Eng Chem Fundam 24(2):129–140View ArticleGoogle Scholar


© The Author(s) 2017