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Gerd Maurer - One of the best experts on this subject based on the ideXlab platform.
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simultaneous solubility of so2 and nh3 in salt h2o and Enthalpy change upon Dilution of so2 nh3 salt h2o in salt h2o salt nh4 2so4 or na2so4 experimental results and model predictions
Fluid Phase Equilibria, 2006Co-Authors: Eckehard Meyer, Viktor Ermatchkov, Alvaro Perezsalado Kamps, Gerd MaurerAbstract:Abstract The simultaneous solubility of sulfur dioxide and ammonia in aqueous solutions of (ammonium sulfate or sodium sulfate) was measured by a synthetic method in the temperature range from 313.6 to 373.2 K and at pressures up to 2.5 MPa. Furthermore, the Enthalpy change upon diluting aqueous solutions of sulfur dioxide, ammonia and (ammonium sulfate or sodium sulfate) in aqueous solutions of the same salt was measured in a batch calorimeter at about 313 and 352 K. The experimental results are used for comparison with predictions from a thermodynamic model for the vapor–liquid equilibrium and the Enthalpy of Dilution of those chemical reacting systems. In that model, activity coefficients are calculated from Pitzer's molality-scale-based Gibbs excess energy model, where all interaction parameters are either adopted from previous investigations on the properties of the binary and ternary sub-systems (if available) or they are neglected (if they are not available).
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Enthalpy of Dilution of so2 salt h2o in salt h2o salt nh4 2so4 or na2so4 experimental results and modeling
Thermochimica Acta, 2005Co-Authors: Alvaro Perezsalado Kamps, Viktor Ermatchkov, Eckehard Meyer, Gerd MaurerAbstract:Abstract New experimental results are presented for the Enthalpy change upon diluting aqueous solutions of sulfur dioxide containing a salt (either ammonium sulfate or sodium sulfate) in aqueous solutions of that salt at about 313 and 352 K. A previously developed thermodynamic model for the vapor–liquid equilibrium of the chemical reacting systems {SO 2 + (NH 4 ) 2 SO 4 + H 2 O} and (SO 2 + Na 2 SO 4 + H 2 O) is extended allowing for the formation of pyrosulfite and for the description of the new experimental results for the Enthalpy change upon Dilution.
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Enthalpy of Dilution of so2 h2o and so2 nh3 h2o in pure water experimental results and modeling
Fluid Phase Equilibria, 2005Co-Authors: Alvaro Perezsalado Kamps, Viktor Ermatchkov, Eckehard Meyer, Gerd MaurerAbstract:Abstract New experimental results for the Enthalpy change upon diluting aqueous solutions of sulfur dioxide as well as aqueous solutions of sulfur dioxide and ammonia in pure water at about 313 and 352 K are presented. The experimental results are used to modify a previously developed thermodynamic model for the vapor–liquid equilibrium of the chemical reacting system (SO2 + NH3 + H2O). That model is extended allowing on the one side for the formation of pyrosulfite, and on the other side for the description of experimental results for the Enthalpy change upon Dilution (in pure water) of (NH3 + H2O) (taken from the literature), as well as (SO2 + H2O) and (SO2 + NH3 + H2O) (from the present work).
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Enthalpy of Dilution in aqueous systems of single solutes ammonia, sodium sulfate and ammonium sulfate: Experimental results and modeling
Thermochimica Acta, 1997Co-Authors: Bernd Rumpf, Frank Weyrich, Gerd MaurerAbstract:Abstract The Enthalpy of Dilution in the sodium sulfate-water, ammonium sulfate-water and ammonia-water systems was measured at temperatures from 313 to 373 K with a Calvet-type batch calorimeter using specially designed mixing cells. The mixing cells allow to pressurize the solutions. The formation of a gas phase during the experiments is thus avoided. Experimental results for the Enthalpy of Dilution are reported and compared to literature data and correlations.
Alvaro Perezsalado Kamps - One of the best experts on this subject based on the ideXlab platform.
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simultaneous solubility of so2 and nh3 in salt h2o and Enthalpy change upon Dilution of so2 nh3 salt h2o in salt h2o salt nh4 2so4 or na2so4 experimental results and model predictions
Fluid Phase Equilibria, 2006Co-Authors: Eckehard Meyer, Viktor Ermatchkov, Alvaro Perezsalado Kamps, Gerd MaurerAbstract:Abstract The simultaneous solubility of sulfur dioxide and ammonia in aqueous solutions of (ammonium sulfate or sodium sulfate) was measured by a synthetic method in the temperature range from 313.6 to 373.2 K and at pressures up to 2.5 MPa. Furthermore, the Enthalpy change upon diluting aqueous solutions of sulfur dioxide, ammonia and (ammonium sulfate or sodium sulfate) in aqueous solutions of the same salt was measured in a batch calorimeter at about 313 and 352 K. The experimental results are used for comparison with predictions from a thermodynamic model for the vapor–liquid equilibrium and the Enthalpy of Dilution of those chemical reacting systems. In that model, activity coefficients are calculated from Pitzer's molality-scale-based Gibbs excess energy model, where all interaction parameters are either adopted from previous investigations on the properties of the binary and ternary sub-systems (if available) or they are neglected (if they are not available).
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Enthalpy of Dilution of so2 salt h2o in salt h2o salt nh4 2so4 or na2so4 experimental results and modeling
Thermochimica Acta, 2005Co-Authors: Alvaro Perezsalado Kamps, Viktor Ermatchkov, Eckehard Meyer, Gerd MaurerAbstract:Abstract New experimental results are presented for the Enthalpy change upon diluting aqueous solutions of sulfur dioxide containing a salt (either ammonium sulfate or sodium sulfate) in aqueous solutions of that salt at about 313 and 352 K. A previously developed thermodynamic model for the vapor–liquid equilibrium of the chemical reacting systems {SO 2 + (NH 4 ) 2 SO 4 + H 2 O} and (SO 2 + Na 2 SO 4 + H 2 O) is extended allowing for the formation of pyrosulfite and for the description of the new experimental results for the Enthalpy change upon Dilution.
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Enthalpy of Dilution of so2 h2o and so2 nh3 h2o in pure water experimental results and modeling
Fluid Phase Equilibria, 2005Co-Authors: Alvaro Perezsalado Kamps, Viktor Ermatchkov, Eckehard Meyer, Gerd MaurerAbstract:Abstract New experimental results for the Enthalpy change upon diluting aqueous solutions of sulfur dioxide as well as aqueous solutions of sulfur dioxide and ammonia in pure water at about 313 and 352 K are presented. The experimental results are used to modify a previously developed thermodynamic model for the vapor–liquid equilibrium of the chemical reacting system (SO2 + NH3 + H2O). That model is extended allowing on the one side for the formation of pyrosulfite, and on the other side for the description of experimental results for the Enthalpy change upon Dilution (in pure water) of (NH3 + H2O) (taken from the literature), as well as (SO2 + H2O) and (SO2 + NH3 + H2O) (from the present work).
Eckehard Meyer - One of the best experts on this subject based on the ideXlab platform.
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simultaneous solubility of so2 and nh3 in salt h2o and Enthalpy change upon Dilution of so2 nh3 salt h2o in salt h2o salt nh4 2so4 or na2so4 experimental results and model predictions
Fluid Phase Equilibria, 2006Co-Authors: Eckehard Meyer, Viktor Ermatchkov, Alvaro Perezsalado Kamps, Gerd MaurerAbstract:Abstract The simultaneous solubility of sulfur dioxide and ammonia in aqueous solutions of (ammonium sulfate or sodium sulfate) was measured by a synthetic method in the temperature range from 313.6 to 373.2 K and at pressures up to 2.5 MPa. Furthermore, the Enthalpy change upon diluting aqueous solutions of sulfur dioxide, ammonia and (ammonium sulfate or sodium sulfate) in aqueous solutions of the same salt was measured in a batch calorimeter at about 313 and 352 K. The experimental results are used for comparison with predictions from a thermodynamic model for the vapor–liquid equilibrium and the Enthalpy of Dilution of those chemical reacting systems. In that model, activity coefficients are calculated from Pitzer's molality-scale-based Gibbs excess energy model, where all interaction parameters are either adopted from previous investigations on the properties of the binary and ternary sub-systems (if available) or they are neglected (if they are not available).
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Enthalpy of Dilution of so2 salt h2o in salt h2o salt nh4 2so4 or na2so4 experimental results and modeling
Thermochimica Acta, 2005Co-Authors: Alvaro Perezsalado Kamps, Viktor Ermatchkov, Eckehard Meyer, Gerd MaurerAbstract:Abstract New experimental results are presented for the Enthalpy change upon diluting aqueous solutions of sulfur dioxide containing a salt (either ammonium sulfate or sodium sulfate) in aqueous solutions of that salt at about 313 and 352 K. A previously developed thermodynamic model for the vapor–liquid equilibrium of the chemical reacting systems {SO 2 + (NH 4 ) 2 SO 4 + H 2 O} and (SO 2 + Na 2 SO 4 + H 2 O) is extended allowing for the formation of pyrosulfite and for the description of the new experimental results for the Enthalpy change upon Dilution.
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Enthalpy of Dilution of so2 h2o and so2 nh3 h2o in pure water experimental results and modeling
Fluid Phase Equilibria, 2005Co-Authors: Alvaro Perezsalado Kamps, Viktor Ermatchkov, Eckehard Meyer, Gerd MaurerAbstract:Abstract New experimental results for the Enthalpy change upon diluting aqueous solutions of sulfur dioxide as well as aqueous solutions of sulfur dioxide and ammonia in pure water at about 313 and 352 K are presented. The experimental results are used to modify a previously developed thermodynamic model for the vapor–liquid equilibrium of the chemical reacting system (SO2 + NH3 + H2O). That model is extended allowing on the one side for the formation of pyrosulfite, and on the other side for the description of experimental results for the Enthalpy change upon Dilution (in pure water) of (NH3 + H2O) (taken from the literature), as well as (SO2 + H2O) and (SO2 + NH3 + H2O) (from the present work).
Mercedes Cáceres - One of the best experts on this subject based on the ideXlab platform.
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aqueous solutions of tris 1 2 diaminoethane cobalt iii chloride and tris 1 3 diaminopropane cobalt iii chloride att 278 15 k Enthalpy of Dilution
The Journal of Chemical Thermodynamics, 2001Co-Authors: Jesús M. Arsuaga, Mercedes Taravillo, F Fernandezmartin, Mercedes CáceresAbstract:Abstract The enthalpies of Dilution of aqueous solutions of {Co(en) 3 }Cl 3 and {Co(tn) 3 }Cl 3 (where en = 1,2-diaminoethane and tn = 1,3-diaminopropane) have been measured up to m = 1 mol · kg − 1 at T = 278.15 K and atmospheric pressure with an isoperibol calorimeter by the long-jump method. Relative apparent molar enthalpies L φ,m have been extracted from an empirical polynomial of the molality square root. Previously reported data at T = 298.15 K are compared with the new experimental Dilution results. A noticeable decrease in L φ,m was observed at every experimental concentration when temperature diminished from 298.15 K to 278.15 K. An inversion in the relative layout for the L φ,m curves of aqueous {Co(en) 3 }Cl 3 and {Co(tn) 3 }Cl 3 was also found.
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Aqueous solutions of tris(1,2-diaminoethane)cobalt(III) chloride and tris(1,3-diaminopropane)cobalt(III) chloride atT = 278.15 K. Enthalpy of Dilution
The Journal of Chemical Thermodynamics, 2001Co-Authors: Jesús M. Arsuaga, F. Fernández-martín, Mercedes Taravillo, Mercedes CáceresAbstract:Abstract The enthalpies of Dilution of aqueous solutions of {Co(en) 3 }Cl 3 and {Co(tn) 3 }Cl 3 (where en = 1,2-diaminoethane and tn = 1,3-diaminopropane) have been measured up to m = 1 mol · kg − 1 at T = 278.15 K and atmospheric pressure with an isoperibol calorimeter by the long-jump method. Relative apparent molar enthalpies L φ,m have been extracted from an empirical polynomial of the molality square root. Previously reported data at T = 298.15 K are compared with the new experimental Dilution results. A noticeable decrease in L φ,m was observed at every experimental concentration when temperature diminished from 298.15 K to 278.15 K. An inversion in the relative layout for the L φ,m curves of aqueous {Co(en) 3 }Cl 3 and {Co(tn) 3 }Cl 3 was also found.
Viktor Ermatchkov - One of the best experts on this subject based on the ideXlab platform.
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simultaneous solubility of so2 and nh3 in salt h2o and Enthalpy change upon Dilution of so2 nh3 salt h2o in salt h2o salt nh4 2so4 or na2so4 experimental results and model predictions
Fluid Phase Equilibria, 2006Co-Authors: Eckehard Meyer, Viktor Ermatchkov, Alvaro Perezsalado Kamps, Gerd MaurerAbstract:Abstract The simultaneous solubility of sulfur dioxide and ammonia in aqueous solutions of (ammonium sulfate or sodium sulfate) was measured by a synthetic method in the temperature range from 313.6 to 373.2 K and at pressures up to 2.5 MPa. Furthermore, the Enthalpy change upon diluting aqueous solutions of sulfur dioxide, ammonia and (ammonium sulfate or sodium sulfate) in aqueous solutions of the same salt was measured in a batch calorimeter at about 313 and 352 K. The experimental results are used for comparison with predictions from a thermodynamic model for the vapor–liquid equilibrium and the Enthalpy of Dilution of those chemical reacting systems. In that model, activity coefficients are calculated from Pitzer's molality-scale-based Gibbs excess energy model, where all interaction parameters are either adopted from previous investigations on the properties of the binary and ternary sub-systems (if available) or they are neglected (if they are not available).
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Enthalpy of Dilution of so2 salt h2o in salt h2o salt nh4 2so4 or na2so4 experimental results and modeling
Thermochimica Acta, 2005Co-Authors: Alvaro Perezsalado Kamps, Viktor Ermatchkov, Eckehard Meyer, Gerd MaurerAbstract:Abstract New experimental results are presented for the Enthalpy change upon diluting aqueous solutions of sulfur dioxide containing a salt (either ammonium sulfate or sodium sulfate) in aqueous solutions of that salt at about 313 and 352 K. A previously developed thermodynamic model for the vapor–liquid equilibrium of the chemical reacting systems {SO 2 + (NH 4 ) 2 SO 4 + H 2 O} and (SO 2 + Na 2 SO 4 + H 2 O) is extended allowing for the formation of pyrosulfite and for the description of the new experimental results for the Enthalpy change upon Dilution.
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Enthalpy of Dilution of so2 h2o and so2 nh3 h2o in pure water experimental results and modeling
Fluid Phase Equilibria, 2005Co-Authors: Alvaro Perezsalado Kamps, Viktor Ermatchkov, Eckehard Meyer, Gerd MaurerAbstract:Abstract New experimental results for the Enthalpy change upon diluting aqueous solutions of sulfur dioxide as well as aqueous solutions of sulfur dioxide and ammonia in pure water at about 313 and 352 K are presented. The experimental results are used to modify a previously developed thermodynamic model for the vapor–liquid equilibrium of the chemical reacting system (SO2 + NH3 + H2O). That model is extended allowing on the one side for the formation of pyrosulfite, and on the other side for the description of experimental results for the Enthalpy change upon Dilution (in pure water) of (NH3 + H2O) (taken from the literature), as well as (SO2 + H2O) and (SO2 + NH3 + H2O) (from the present work).