Experimental study on carbamate formation in the AMP–CO2–H2O system at different temperatures

Carbon dioxide capture characteristics from flue gas using aqueous 2-amino-2-methyl-1-propanol (AMP) and monoethanolamine (MEA) solutions in packed bed absorption and regeneration columns

“…It is suggested that due to instability of the carbamate formed, these readily undergo hydrolysis to form bicarbonate, releasing free amine that again reacts with CO 2 (Chakraborty et al, 1986;Hu and Chakma., 1990). However, recent studies of Ciftja et al (2014) and Jackson (2014) found the existence of carbamate, though small in quantity, in AMP-CO 2 -H 2 O absorption system throughout the run. It implies that carbamate formation reaction may play some role in absorption of CO 2 .…”

“…Recent work of Giuffrida et al (2013) on amine based post combustion CO 2 capture in air-blown IGCC (integrated gasification combined cycle) systems with cold and hot gas clean-up reported that combined cycle efficiency increases as high as 41.5% if hot coal derived gas clean up is realized before the syngas fuels the combustion turbine. Ciftja et al (2014) worked on AMP-CO 2 -H 2 O system at different temperatures and found consistent carbamate formation all through the run. This is in contradiction to earlier observation where most of the authors predicted very unstable carbamate due to steric hindrance effect of AMP.…”

Carbamation of Starch with Amine Using Dimethyl Carbonate as Coupling Agent

“…52 The signal of the carbonyl carbon could not be observed, most likely due to its long relaxation time. 55…”

Understanding the corrosion of CO2-loaded 2-amino-2-methyl-1-propanol solutions assisted by thermodynamic modeling

“…These different reaction pathways lead to different characteristics for primary and secondary amines to tertiary amines (Arcis et al, 2014). Sterically hindered amines, defined as either a primary amine in which the amino group is attached to a tertiary carbon or a secondary amine in which the amino group is attached to at least one secondary or tertiary carbon (Zhao and Winston Ho, 2012), present advantages in terms of a faster CO 2 absorption rate with respect to the tertiary amines, a higher solvent capacity, and a lower desorption energy when compared to their unhindered counterparts because of the instability of their carbamate but favorable bicarbonate pathway (Afkhamipour and Mofarahi, 2013;Arcis et al, 2014;Ciftja et al, 2011;Ciftja et al, 2014;Dash et al, 2011;Hamborg and Versteeg, 2009;Hartono et al, 2013;Kundu and Bandyopadhyay, 2006;Li et al, 2014;Mehdizadeh et al, 2013;Pahlavanzadeh et al, 2010;Park et al, 2002;Richner and Puxty, 2012;Sartori and Savage, 1983;Seo and Hong, 1996;Silkenbäumer et al, 1998;Tong et al, 2012;Wu et al, 2013;Yih and Shen, 1988). Furthermore, sterically hindered amines generally have low volatilities and lower degradation rates as a consequence of the bicarbonate reaction pathway (Ciftja et al, 2011;Hartono et al, 2013;Yih and Shen, 1988).…”

“…Thus, a reliable thermodynamic model for the CO 2 :AMP:H 2 O system is crucial in estimating the solution speciation for understanding the corrosion mechanism. Some work has been done on solubility measurements and thermodynamic modeling of CO 2 in aqueous solutions of various alkanolamine systems including AMP (Arcis et al, 2014;Ciftja et al, 2014;Hamborg and Versteeg, 2009;Hartono et al, 2013;Kundu and Bandyopadhyay, 2006;Li et al, 2014;Liang et al, 2015;Mehdizadeh et al, 2013;Pahlavanzadeh et al, 2010;Park et al, 2002;Rebolledo-Morales et al, 2011;Richner and Puxty, 2012;Silkenbäumer et al, 1998;Tong et al, 2012;Wu et al, 2013). The Kent-Eisenberg thermodynamics model (Pahlavanzadeh et al, 2010;Park et al, 2002;Rebolledo-Morales et al, 2011) or various equations for Gibbs energy and activity coefficients, such as NRTL (Hartono et al, 2013), Pitzer (Arcis et al, 2014;Silkenbäumer et al, 1998), e-UNIQUAC (Mehdizadeh et al, 2013) n xt n y − k l qu tion (Ciftja et al, 2014;Richner and Puxty, 2012;Tong et al, 2012), have been applied to AMP-based solutions.…”