Solubilities of gases in aqueous solutions of amine

Sada, Eizô; Kumazawa, H.; Butt, Muhammad Arif

doi:10.1021/je60074a011

Cited by 76 publications

(57 citation statements)

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“…Table 7 together with the data of Sada et al (1977Sada et al ( , 1978. (d) The diffusivity was determined from absorption measurements in a laminar film reactor.…”

Section: Physico-chemicalmentioning

confidence: 99%

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The effect of diffusivity on gas-liquid mass transfer in stirred vessels. Experiments at atmospheric and elevated pressures

Versteeg

Blauwhoff

Swaaij

1987

Chemical Engineering Science

121

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Abstract-Mass transfer has been studied in gas-liquid stirred vessels with horizontal interfaces which appeared to the eye to be completely smooth. Special attention has been paid to the influence of the coefficient of molecular diffusion. The results are compared with those published before. The simplifying assumptions of identical hydrodynamical conditions at the same stirrer speed in one particular geometry, which have been made in some previous investigations, is shown to be wrong and may-lead to incorrect conclusions on the influence of the diffusion coefficient. For the gas phase the mass transfer can be described by the penetration theory (Higbie, R.

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“…Table 7 together with the data of Sada et al (1977Sada et al ( , 1978. (d) The diffusivity was determined from absorption measurements in a laminar film reactor.…”

Section: Physico-chemicalmentioning

confidence: 99%

“…(d) The diffusivity was determined from absorption measurements in a laminar film reactor. The results are presented in Table 8 together with the data of Sada et al (1977Sada et al ( , 1978. The term Hea of the experimental solutions was also determined graphically.…”

Section: Physico-chemicalmentioning

confidence: 99%

The effect of diffusivity on gas-liquid mass transfer in stirred vessels. Experiments at atmospheric and elevated pressures

Versteeg

Blauwhoff

Swaaij

1987

Chemical Engineering Science

121

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“…[5] Sharma, Sada et al, Hikita et al, and Li et al obtained similar rate constants for CO 2 absorption into EDA solutions with different experimental methods. [6][7][8][9] At low amine concentrations (< 2 m) with low CO 2 loadings (< 0.1), EDA has a faster rate of reaction with CO 2 than MEA. At 298 K, the second-order rate constant is 15.1 m 3 mol À1 s À1 for EDA and 7.6 m 3 mol À1 s À1 for MEA.…”

Section: Introductionmentioning

confidence: 99%

Aqueous Ethylenediamine for CO₂ Capture

et al. 2010

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Aqueous ethylenediamine (EDA) has been investigated as a solvent for CO(2) capture from flue gas. EDA can be used at 12 M (mol kg(-1) H(2)O) with an acceptable viscosity of 16 cP (1 cP=10(-3) Pa s) with 0.48 mol CO(2) per equivalent of EDA. Similar to monoethanolamine (MEA), EDA can be used up to 120 degrees C in a stripper without significant thermal degradation. Inhibitor A will effectively eliminate oxidative degradation. Above 120 degrees C, loaded EDA degrades with the production of its cyclic urea and other related compounds. Unlike piperazine, when exposed to oxidative degradation, EDA does not result in excessive foaming. Over much of the loading range, the CO(2) absorption rate with 12 M EDA is comparable to 7 M MEA. However, at typical rich loading, 12 M EDA absorbs CO(2) 2 times slower than 7 M MEA. The capacity of 12 M EDA is 0.72 mol CO(2)/(kg H(2)O+EDA) (for P(CO(2) )=0.5 to 5 kPa at 40 degrees C), which is about double that of MEA. The apparent heat of CO(2) desorption in EDA solution is 84 kJ mol(-1) CO(2); greater than most other amine systems.

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“…The nitrous oxide data of Sada et al (1977Sada et al ( , 1968 were used assuming the ratios determined at 298 K are unchanged at 323 K. The concentration of physically dissolved COz in pure water at 323 K and Pco2 = 140 kN/m2 is determined to be 2.67 X mol/cm3, and the diffusivity of COz in pure water at 323 K was set at 3.8 x 10-5 cmz/s, which is the average of two values: 4.1 X by the It should be noted that in the DIPA case, both C* and D decrease precipitously with increasing concentration beyond the 1M level (Sada et al, 1978). Accordingly, the data for the 3M DIPA solution cannot be analyzed further in this study and a question remains unresolved as to whether the observed behavior of 3M DIPA in Figure 6 is due to diffusion limitation or to the Occurrence of third-order kinetics similar to that observed by Nunge and Gill (1963) for the pure DEA system.…”

Section: Resultsmentioning

confidence: 99%

Chemical kinetics of carbon dioxide reactions with diethanolamine and diisopropanolamine in aqueous solutions

Savage

Kim

1985

AIChE Journal

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(MEA), diethanolamine (DEA), and diisopropanolamine (DIPA) were measured over a wide range of carbonation ratios. Analysis of the chemical-reaction-ratecontrolled data showed that the chemical reaction rates for all three aminoalcohols are first order with respect to the free-amine concentration. Corporate Research TechnologyFeasibility Center Exxon Research and Engineering Co.Linden, NJ 07036 SCOPEDespite widespread use in gas treating of aqueous solutions of monoethanolamine (MEA), diethanolamine (DEA), and diisopropanolamine (DIPA) for regenerative COz removal from gases, the underlying chemical reaction kinetics are not fully understood. It is generally agreed that the reaction of MEA with dissolved COz proceeds by second-order kinetics, i.e., first order with respect to the free amine concentration. For the DEA reaction, however, serious discrepancies exist among results of recent studies. The reaction order with respect to the free DEA concentration was proposed to be unity, two, or intermediate between one and two. Danckwerts postulated that the change in kinetics from second order for MEA to third-order for DEA may originate from the increased steric requirements of DEA as compared with MEA. This postulate would thus predict that a n amine with further increased steric crowding would give third-order kinetics. Accordingly, we undertook to examine the reaction of DIPA, an amine which is sterically more crowded than DEA. For this purpose, COz absorption rates into 1-3 molar aqueous solutions of MEA, DEA, DIPA were measured at 325 K using a single-sphere absorber. The chemical-reaction-con,.trolled absorption rate data, obtained over a wide range of carbonation ratios, were then analyzed to determine the chemical kinetics. CONCLUSION AND SIGNIFICANCEThe rates of COZ absorption at 323 K into 2 and 3M DEA and 1M DIPA solutions were found to be chemical-reaction-ratecontrolled. A thermodynamic model was derived to estimate the free amine concentrations at various carbonation ratios. The absorption rate results were rigorously analyzed using Danckwerts' theoretical model. The resultant chemical reaction rates showed dependencies on the free aniine concentration to the power of 1.13 in the DEA system and 0.93 in the DIPA system. This result shows that the order of chemical reaction with respect to the free amine concentration is close to unity for both DEA and DIPA. Thus, the present study suggests that MEA, DEA, and DIPA all follow the same kinetics. No evidence for shifting to higher-order kinetics owing to increasing stcric crowding of the amine structure was observed.

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Solubilities of gases in aqueous solutions of amine

Cited by 76 publications

References 3 publications

The effect of diffusivity on gas-liquid mass transfer in stirred vessels. Experiments at atmospheric and elevated pressures

The effect of diffusivity on gas-liquid mass transfer in stirred vessels. Experiments at atmospheric and elevated pressures

Aqueous Ethylenediamine for CO₂ Capture

Chemical kinetics of carbon dioxide reactions with diethanolamine and diisopropanolamine in aqueous solutions

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Solubilities of gases in aqueous solutions of amine

Cited by 76 publications

References 3 publications

The effect of diffusivity on gas-liquid mass transfer in stirred vessels. Experiments at atmospheric and elevated pressures

The effect of diffusivity on gas-liquid mass transfer in stirred vessels. Experiments at atmospheric and elevated pressures

Aqueous Ethylenediamine for CO2 Capture

Chemical kinetics of carbon dioxide reactions with diethanolamine and diisopropanolamine in aqueous solutions

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Product

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Aqueous Ethylenediamine for CO₂ Capture