CO2 absorption in aqueous solutions of hindered amines

Chakraborty, Amit; Astarita, Gianni; Bischoff, Kenneth B.

doi:10.1016/0009-2509(86)87185-8

Cited by 210 publications

(155 citation statements)

References 8 publications

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“…The classical zwitterion mechanism for the reaction of CO, with primary or secondary amines was not taken into account by Chakraborty et al (1986), because the carbamate of AMP is very unstable. The mechanism suggested by Chakraborty et al (1986) cannot explain the deviations from pseudo-first-order behavior observed in this study, however, while the present mechanism can. The present experimental results would lead to a pseudo-first-order reaction rate constant of about 0.4 m3 mol-' s-', which is of the magnitude suggested by Chakraborty et al (1986).…”

Section: Resultscontrasting

confidence: 94%

“…The relevant equilibrium constants for 298 K were presented in Bosch et al (1989). Because only an upper limit of the equilibrium constant describing the stability the carbamate of AMP (K,) is available (Chakraborty et al, 1986), this parameter also has to be obtained from the experiments. 2895 K log k,, = 10.635 -T.…”

Section: Resultsmentioning

confidence: 99%

“…This causes reactions (1) and (2) to proceed slightly in the reverse direction. Chakraborty et al (1986) studied absorption rates of CO, into AMP solutions in a pressure decrease cell. From the observed first-order relation between the reaction rate and both the CO, and the AMP concentration they concluded that AMP acts as a catalyst for the hydration of CO,, and that the rate-determining step in this catalytic route is the formation of an intermediate by the reaction of CO, with the amine.…”

Section: Resultsmentioning

confidence: 99%

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Kinetics of the reaction of CO2 with the sterically hindered amine 2-Amino-2-methylpropanol at 298 K

Bosch

Versteeg

Swaaij

1990

Chemical Engineering Science

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Abstract-Absorptionrates of CO, into aqueous solutions of the sterically hindered amine AMP (2-_amino-Zmethylpropanol), under reaction-controlled conditions were measured. The experiments were carried out in a stirkd vessel with a smooth horizontal interface. The results were interpreted in terms of the zwitterion mechanism for the reaction of CO, with primary or secondary amines as originally proposed by Caplow (1968, J. Am. &em. Sot. 90,[6795][6796][6797][6798][6799][6800][6801][6802][6803] and Danckwerts (1979, Ch em. Engng Sci. 34,443446). The reaction rate constants and the equilibrium constant describing the stability ofthe carbamate of AMP were determined by fitting numerically calculated absorption rates to the experimentally observed ones. These constants were compared with data reported for AMP and with those for not sterically hindered amines.The relative values of the reaction rate constants could by explained only partially.

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Section: Resultscontrasting

confidence: 94%

Section: Resultsmentioning

confidence: 99%

Section: Resultsmentioning

confidence: 99%

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Kinetics of the reaction of CO2 with the sterically hindered amine 2-Amino-2-methylpropanol at 298 K

Bosch

Versteeg

Swaaij

1990

Chemical Engineering Science

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“…Single alkanolamines systems, such as primary amines, monoethanolamine (MEA); secondary amines, diethanolamine (DEA), di-isopropanolamine (DIPA); sterically hindered amines, 2-amino-2-methyl-1-propanol (AMP) and tertiary amines, N-methyldiethanolamine (MDEA) have been widely used as chemical absorbents for the removal of acid gases (Astarita et al, 1983;Böttinger et al, 2008;Chakraborty et al, 1986;Kim et al, 2008;Kohl and Nilsen, 1997;Versteeg et al, 1996) . The major problem using this technology is relatively high operating costs, mainly due to the regeneration of absorbents.…”

Section: Introductionmentioning

confidence: 99%

Experimental study on phase change solvents in CO2 capture by NMR spectroscopy

Ciftja

Hartono

Svendsen

2013

Chemical Engineering Science

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Abstract2-(Diethylamino)ethanol (DEEA) and 3-(Methylamino) propylamine (MAPA) in combination may represent a promising absorbent system for CO 2 capture due to high CO 2 loading capacity, high equilibrium temperature sensitivity, low energy requirement for regeneration and relatively high reaction rate.Three different systems: DEEA-CO 2 -H 2 O; MAPA-CO 2 -H 2 O and DEEA-MAPA-CO 2 -H 2 O were studied quantitatively by NMR spectroscopy and the data are reported in the present work. The main products quantified for these systems are: carbonate-bicarbonate for the DEEA-CO 2 -H 2 O system; primary, secondary carbamate, dicarbamate for the MAPA-CO 2 -H 2 O system, and primary/ secondary carbamate, dicarbamate, carbonate/bicarbonate in blended DEEA-MAPA-CO 2 -H 2 O. The speciation data of the three systems were measured and reported in the present work. The blended system of 5M DEEA-2M MAPA can form two liquid phases after being loaded with CO 2 and both phases were analyzed quantitatively by NMR spectroscopy. The experimental data shows that the lower phase is rich in CO 2 and MAPA while the upper phase was lean in CO 2 and rich in DEEA. The ratio DEEA-MAPA in the lower phase increases with increasing partial pressure whereas for the upper phase the opposite is true.

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“…According to Chakraborty et al (1986) the introduction of substituents at the a-carbon creates a carbamate instability, which causes the hydrolysis to go faster, thus increasing the amount of bicarbonate, allowing for higher CO 2 loadings. Sartori and Savage (1983) suggested this instability was due to the steric hindrance created by these a-substituents.…”

mentioning

confidence: 99%