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Paitoon Tontiwachwuthikul - One of the best experts on this subject based on the ideXlab platform.
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analysis of co2 solubility and absorption heat into 1 dimethylamino 2 propanol solution
Chemical Engineering Science, 2017Co-Authors: Raphael Idem, Helei Liu, Hongxia Gao, Paitoon Tontiwachwuthikul, Zhiwu LiangAbstract:Abstract In this work, the CO2 equilibrium solubility in 1-dimethylamino-2-propanol (1DMA2P) solution was determined as a function of 1DMA2P concentration (over the range of 1–5 M), temperature (in the range of 298–333 K), and CO2 partial pressure (in the range of 8–101 kPa), and the data used to fit the correlations for K2 using Kent-Eisenberg, Austgen, Li-Sheng and Hu-Chakma models. A new K2 correlation model was also developed to predict the CO2 equilibrium solubility in 1DMA2P solution. It was found that all of the models could fit the CO2 equilibrium solubility in 1DMA2P solution data with absolute average deviations (ADDs) for the models by Kent-Eisenberg, Austgen, Li-Sheng, Hu-Chakma and Liu et al. of 14, 15, 12, 6.3 and 10%, respectively. In addition, the heat of CO2 absorption in 1DMA2P solution estimated using Gibbs-Helmholtz Equation was found to be −31.67 kJ/mol. Information or guidelines about effective utilization of data of screened solvents is provided based on three absorption parameters, namely, CO2 equilibrium solubility, second order reaction constant, and CO2 absorption heat.
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solubility absorption heat and mass transfer studies of co2 absorption into aqueous solution of 1 dimethylamino 2 propanol
Fuel, 2015Co-Authors: Yujiao Liang, Raphael Idem, Helei Liu, Paitoon Tontiwachwuthikul, Zhiwu Liang, Wichitpan RongwongAbstract:Abstract In this work, the CO 2 absorption performance of aqueous 1-dimethylamino-2-propanol (1DMA2P) was comprehensively investigated in terms of CO 2 equilibrium solubility, CO 2 absorption rate, CO 2 absorption heat, and mass transfer efficiency. The CO 2 equilibrium solubility in 2 M 1DMA2P was measured over the temperature range of 298–333 K and CO 2 partial pressure range of 8–101 kPa. The results showed that the CO 2 equilibrium solubility of 1DAM2P was higher than those of conventional amines, MEA and MDEA. The CO 2 absorption heat of 1DMA2P based on the Gibbs–Helmholtz Equation was found to be −30.5 kJ/mol, which suggests that 1DMA2P needs a lower regeneration energy as compared with MEA and MDEA. Ion speciation (including 1DMA2P, 1DMA2PH + , HCO 3 − , CO 3 2 − ) plots obtained from the pH method were also generated at the temperatures of 298 K and 313 K. In addition, the overall mass transfer coefficient ( K G a v ) of 1DMA2P in a packed column was also experimentally obtained and compared with those of MEA and MDEA. The ranking was: MEA > 1DMA2P > MDEA.
Raphael Idem - One of the best experts on this subject based on the ideXlab platform.
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selection of components for formulation of amine blends for post combustion co2 capture based on the side chain structure of primary secondary and tertiary amines
Chemical Engineering Science, 2017Co-Authors: Jessica Narkutetteh, Pailin Muchan, Chintana Saiwan, Teeradet Supap, Raphael IdemAbstract:Abstract The effect of the side chain structure and the number of hydroxyl groups in primary, secondary and tertiary amines on CO 2 absorption and desorption kinetics, equilibrium loading, heat duty, cyclic capacity, heat of absorption and pKa were studied and used to develop rational criteria for selecting components to formulate an optimum amine blend. Based on the criteria, amines that had a combination of high absorption parameter and high desorption parameter were selected. Their mixing ratios and concentrations were varied to obtain the best overall performance. The results of this study showed that, in comparison with their straight-chain analogues, steric hindrance present in branched-chain alkanolamines resulted in much faster desorption rate, higher solubility CO 2 and cyclic capacity, and much lower heat duty for solvent regeneration, but just a slight decrease in CO 2 absorption rate. The developed criteria resulted in formulating an excellent bi-solvent aqueous amine blend (comprising 2 M BEA + 2 M AMP), which was shown to have an outstanding desorption characteristics/heat duty as well as very good absorption characteristics. In addition, this work developed a new non-trial-and-error procedure to determine the heat of CO 2 absorption based on Gibbs-Helmholtz Equation. Furthermore, this work showed that the CO 2 absorption rate and the heat of CO 2 absorption may not necessarily be proportional to the heat of absorption and heat duty, respectively. Both these relations were shown to be strong functions of the amine structure.
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analysis of co2 solubility and absorption heat into 1 dimethylamino 2 propanol solution
Chemical Engineering Science, 2017Co-Authors: Raphael Idem, Helei Liu, Hongxia Gao, Paitoon Tontiwachwuthikul, Zhiwu LiangAbstract:Abstract In this work, the CO2 equilibrium solubility in 1-dimethylamino-2-propanol (1DMA2P) solution was determined as a function of 1DMA2P concentration (over the range of 1–5 M), temperature (in the range of 298–333 K), and CO2 partial pressure (in the range of 8–101 kPa), and the data used to fit the correlations for K2 using Kent-Eisenberg, Austgen, Li-Sheng and Hu-Chakma models. A new K2 correlation model was also developed to predict the CO2 equilibrium solubility in 1DMA2P solution. It was found that all of the models could fit the CO2 equilibrium solubility in 1DMA2P solution data with absolute average deviations (ADDs) for the models by Kent-Eisenberg, Austgen, Li-Sheng, Hu-Chakma and Liu et al. of 14, 15, 12, 6.3 and 10%, respectively. In addition, the heat of CO2 absorption in 1DMA2P solution estimated using Gibbs-Helmholtz Equation was found to be −31.67 kJ/mol. Information or guidelines about effective utilization of data of screened solvents is provided based on three absorption parameters, namely, CO2 equilibrium solubility, second order reaction constant, and CO2 absorption heat.
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solubility absorption heat and mass transfer studies of co2 absorption into aqueous solution of 1 dimethylamino 2 propanol
Fuel, 2015Co-Authors: Yujiao Liang, Raphael Idem, Helei Liu, Paitoon Tontiwachwuthikul, Zhiwu Liang, Wichitpan RongwongAbstract:Abstract In this work, the CO 2 absorption performance of aqueous 1-dimethylamino-2-propanol (1DMA2P) was comprehensively investigated in terms of CO 2 equilibrium solubility, CO 2 absorption rate, CO 2 absorption heat, and mass transfer efficiency. The CO 2 equilibrium solubility in 2 M 1DMA2P was measured over the temperature range of 298–333 K and CO 2 partial pressure range of 8–101 kPa. The results showed that the CO 2 equilibrium solubility of 1DAM2P was higher than those of conventional amines, MEA and MDEA. The CO 2 absorption heat of 1DMA2P based on the Gibbs–Helmholtz Equation was found to be −30.5 kJ/mol, which suggests that 1DMA2P needs a lower regeneration energy as compared with MEA and MDEA. Ion speciation (including 1DMA2P, 1DMA2PH + , HCO 3 − , CO 3 2 − ) plots obtained from the pH method were also generated at the temperatures of 298 K and 313 K. In addition, the overall mass transfer coefficient ( K G a v ) of 1DMA2P in a packed column was also experimentally obtained and compared with those of MEA and MDEA. The ranking was: MEA > 1DMA2P > MDEA.
James K Baird - One of the best experts on this subject based on the ideXlab platform.
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a chemical test of critical point isomorphism reactive dissolution of ionic solids in isobutyric acid water near the consolute point
Journal of Physical Chemistry B, 2015Co-Authors: James K Baird, Baichuan Hu, Jonathan D Baker, Joshua R Lang, Alison K Sides, Karen E Joyce, Randi D RicheyAbstract:Binary liquid mixtures having a consolute point can be used as solvents for chemical reactions. When excess cerium(IV) oxide is brought into equilibrium with a mixture of isobutyric acid + water, and the concentration of cerium in the liquid phase is plotted in van’t Hoff form, a straight line results for temperatures sufficiently in excess of the critical solution temperature. Within 1 K of the critical temperature, however, the concentration becomes substantially suppressed, and the van’t Hoff slope diverges toward negative infinity. According to the phase rule, one mole fraction can be fixed. Given this restriction, the temperature behavior of the data is in exact agreement with the predictions of both the principle of critical point isomorphism and the Gibbs–Helmholtz Equation. In addition, we have determined the concentration of lead in the liquid phase when crystalline lead(II) sulfate reacts with potassium iodide in isobutyric acid + water. When plotted in van’t Hoff form, the data lie on a straigh...
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A Chemical Test of Critical Point Isomorphism: Reactive Dissolution of Ionic Solids in Isobutyric Acid + Water near the Consolute Point
2015Co-Authors: James K Baird, Jonathan D Baker, Alison K Sides, Karen E Joyce, Joshua R. Lang, Randi D RicheyAbstract:Binary liquid mixtures having a consolute point can be used as solvents for chemical reactions. When excess cerium(IV) oxide is brought into equilibrium with a mixture of isobutyric acid + water, and the concentration of cerium in the liquid phase is plotted in van’t Hoff form, a straight line results for temperatures sufficiently in excess of the critical solution temperature. Within 1 K of the critical temperature, however, the concentration becomes substantially suppressed, and the van’t Hoff slope diverges toward negative infinity. According to the phase rule, one mole fraction can be fixed. Given this restriction, the temperature behavior of the data is in exact agreement with the predictions of both the principle of critical point isomorphism and the Gibbs–Helmholtz Equation. In addition, we have determined the concentration of lead in the liquid phase when crystalline lead(II) sulfate reacts with potassium iodide in isobutyric acid + water. When plotted in van’t Hoff form, the data lie on a straight line for all temperatures including the critical region. The phase rule indicates that two mole fractions can be fixed. With this restriction, the data are in exact agreement with the principle of critical point isomorphism
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chemical equilibrium and critical phenomena the solubilities of iron iii oxide and cobalt ii iii oxide in isobutyric acid water near the consolute point
International Journal of Thermophysics, 2010Co-Authors: Baichuan Hu, James K BairdAbstract:The solubilities of iron(III) oxide, formula Fe2O3, and cobalt(II,III) oxide, formula Co3O4, have been determined in the liquid mixture, isobutyric acid + water, along the critical isopleth at temperatures above the upper critical solution temperature near 299 K. When plotted in van’t Hoff form with ln s versus 1/T, the measurements of solubility, s, lie on a straight line for values of the temperature, T, in kelvin, which are sufficiently in excess of the critical solution temperature, Tc. The sign of the slope, (∂ ln s/∂(1/T)), indicates that in the case of both oxides, the dissolution reaction is endothermic. When the temperature is within 1K of Tc, however, the slope departs from its constant value and appears to diverge toward negative infinity. The principle of critical-point universality predicts that a divergence in (∂ ln s/∂(1/T)) is to be expected for T near Tc in those cases where the stoichiometry of the dissolution reaction involves both components of the solvent; moreover, the Gibbs–Helmholtz Equation predicts that, if the heat of solution is endothermic, the sign of the divergence should be negative. Both of these predictions are confirmed by the solubilities of Fe2O3 and Co3O4 measured as a function of temperature along the critical isopleth of isobutyric acid + water.
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chemical equilibrium and critical phenomena solubility of indium oxide in isobutyric acid water near the consolute point
Journal of Chemical & Engineering Data, 2009Co-Authors: Baichuan Hu, Randi D Richey, James K BairdAbstract:We have determined the solubility, s, of indium oxide in the liquid mixture isobutyric acid + water along the critical isopleth at temperatures above the upper critical solution temperature near 299 K. When plotted in van’t Hoff form with ln s vs 1/T, the measurements of solubility lie on a straight line for values of the absolute temperature, T, which are sufficiently in excess of the critical solution temperature, Tc. The sign of the slope, (∂ ln s/∂(1/T)), indicates that the enthalpy of dissolution is endothermic. When the temperature is within 1 K of Tc, however, the slope departs from its constant value and appears to diverge toward negative infinity. The principle of critical point universality predicts that a divergence in (∂ ln s/∂(1/T)) is to be expected for T near Tc in those cases where the stoichiometry of the dissolution reaction involves both components of the solvent; moreover, the Gibbs−Helmholtz Equation predicts that if the enthalpy of solution is endothermic, the sign of the divergence ...
Randi D Richey - One of the best experts on this subject based on the ideXlab platform.
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a chemical test of critical point isomorphism reactive dissolution of ionic solids in isobutyric acid water near the consolute point
Journal of Physical Chemistry B, 2015Co-Authors: James K Baird, Baichuan Hu, Jonathan D Baker, Joshua R Lang, Alison K Sides, Karen E Joyce, Randi D RicheyAbstract:Binary liquid mixtures having a consolute point can be used as solvents for chemical reactions. When excess cerium(IV) oxide is brought into equilibrium with a mixture of isobutyric acid + water, and the concentration of cerium in the liquid phase is plotted in van’t Hoff form, a straight line results for temperatures sufficiently in excess of the critical solution temperature. Within 1 K of the critical temperature, however, the concentration becomes substantially suppressed, and the van’t Hoff slope diverges toward negative infinity. According to the phase rule, one mole fraction can be fixed. Given this restriction, the temperature behavior of the data is in exact agreement with the predictions of both the principle of critical point isomorphism and the Gibbs–Helmholtz Equation. In addition, we have determined the concentration of lead in the liquid phase when crystalline lead(II) sulfate reacts with potassium iodide in isobutyric acid + water. When plotted in van’t Hoff form, the data lie on a straigh...
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A Chemical Test of Critical Point Isomorphism: Reactive Dissolution of Ionic Solids in Isobutyric Acid + Water near the Consolute Point
2015Co-Authors: James K Baird, Jonathan D Baker, Alison K Sides, Karen E Joyce, Joshua R. Lang, Randi D RicheyAbstract:Binary liquid mixtures having a consolute point can be used as solvents for chemical reactions. When excess cerium(IV) oxide is brought into equilibrium with a mixture of isobutyric acid + water, and the concentration of cerium in the liquid phase is plotted in van’t Hoff form, a straight line results for temperatures sufficiently in excess of the critical solution temperature. Within 1 K of the critical temperature, however, the concentration becomes substantially suppressed, and the van’t Hoff slope diverges toward negative infinity. According to the phase rule, one mole fraction can be fixed. Given this restriction, the temperature behavior of the data is in exact agreement with the predictions of both the principle of critical point isomorphism and the Gibbs–Helmholtz Equation. In addition, we have determined the concentration of lead in the liquid phase when crystalline lead(II) sulfate reacts with potassium iodide in isobutyric acid + water. When plotted in van’t Hoff form, the data lie on a straight line for all temperatures including the critical region. The phase rule indicates that two mole fractions can be fixed. With this restriction, the data are in exact agreement with the principle of critical point isomorphism
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chemical equilibrium and critical phenomena solubility of indium oxide in isobutyric acid water near the consolute point
Journal of Chemical & Engineering Data, 2009Co-Authors: Baichuan Hu, Randi D Richey, James K BairdAbstract:We have determined the solubility, s, of indium oxide in the liquid mixture isobutyric acid + water along the critical isopleth at temperatures above the upper critical solution temperature near 299 K. When plotted in van’t Hoff form with ln s vs 1/T, the measurements of solubility lie on a straight line for values of the absolute temperature, T, which are sufficiently in excess of the critical solution temperature, Tc. The sign of the slope, (∂ ln s/∂(1/T)), indicates that the enthalpy of dissolution is endothermic. When the temperature is within 1 K of Tc, however, the slope departs from its constant value and appears to diverge toward negative infinity. The principle of critical point universality predicts that a divergence in (∂ ln s/∂(1/T)) is to be expected for T near Tc in those cases where the stoichiometry of the dissolution reaction involves both components of the solvent; moreover, the Gibbs−Helmholtz Equation predicts that if the enthalpy of solution is endothermic, the sign of the divergence ...
Zhiwu Liang - One of the best experts on this subject based on the ideXlab platform.
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analysis of co2 solubility and absorption heat into 1 dimethylamino 2 propanol solution
Chemical Engineering Science, 2017Co-Authors: Raphael Idem, Helei Liu, Hongxia Gao, Paitoon Tontiwachwuthikul, Zhiwu LiangAbstract:Abstract In this work, the CO2 equilibrium solubility in 1-dimethylamino-2-propanol (1DMA2P) solution was determined as a function of 1DMA2P concentration (over the range of 1–5 M), temperature (in the range of 298–333 K), and CO2 partial pressure (in the range of 8–101 kPa), and the data used to fit the correlations for K2 using Kent-Eisenberg, Austgen, Li-Sheng and Hu-Chakma models. A new K2 correlation model was also developed to predict the CO2 equilibrium solubility in 1DMA2P solution. It was found that all of the models could fit the CO2 equilibrium solubility in 1DMA2P solution data with absolute average deviations (ADDs) for the models by Kent-Eisenberg, Austgen, Li-Sheng, Hu-Chakma and Liu et al. of 14, 15, 12, 6.3 and 10%, respectively. In addition, the heat of CO2 absorption in 1DMA2P solution estimated using Gibbs-Helmholtz Equation was found to be −31.67 kJ/mol. Information or guidelines about effective utilization of data of screened solvents is provided based on three absorption parameters, namely, CO2 equilibrium solubility, second order reaction constant, and CO2 absorption heat.
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solubility absorption heat and mass transfer studies of co2 absorption into aqueous solution of 1 dimethylamino 2 propanol
Fuel, 2015Co-Authors: Yujiao Liang, Raphael Idem, Helei Liu, Paitoon Tontiwachwuthikul, Zhiwu Liang, Wichitpan RongwongAbstract:Abstract In this work, the CO 2 absorption performance of aqueous 1-dimethylamino-2-propanol (1DMA2P) was comprehensively investigated in terms of CO 2 equilibrium solubility, CO 2 absorption rate, CO 2 absorption heat, and mass transfer efficiency. The CO 2 equilibrium solubility in 2 M 1DMA2P was measured over the temperature range of 298–333 K and CO 2 partial pressure range of 8–101 kPa. The results showed that the CO 2 equilibrium solubility of 1DAM2P was higher than those of conventional amines, MEA and MDEA. The CO 2 absorption heat of 1DMA2P based on the Gibbs–Helmholtz Equation was found to be −30.5 kJ/mol, which suggests that 1DMA2P needs a lower regeneration energy as compared with MEA and MDEA. Ion speciation (including 1DMA2P, 1DMA2PH + , HCO 3 − , CO 3 2 − ) plots obtained from the pH method were also generated at the temperatures of 298 K and 313 K. In addition, the overall mass transfer coefficient ( K G a v ) of 1DMA2P in a packed column was also experimentally obtained and compared with those of MEA and MDEA. The ranking was: MEA > 1DMA2P > MDEA.