“…A quantitative prediction of the VLE is not possible for the selected systems with the PSRK model, but the calculated results can be used as rough estimates, and they describe the correct phenomenology. 5 Experimental [this work at 419.15 K (○,◊) and at 457.65 K (·,⧫)] and calculated [PSRK ()] P − x − y data for the system propane (1) + dodecane (2). 6 Experimental [this work at 408.15 K (○,◊) and at 448.15 K (·,⧫)] and calculated [PSRK ()] P − x − y data for the system propane (1) + 1-decanol (2). 7 Experimental [this work at 448.15 K (○,◊)] and calculated [PSRK ()] P − x − y data for the system ethane (1) + 1-decanol (2). 8 Experimental [this work at 308.15 K (○,◊) and at 318.15 K (·,⧫)] and calculated [PSRK ()] P − x − y data for the system ethylene (1) + 1-decanol (2). 9 Experimental [this work at 318.15 K (○,◊)] and calculated [PSRK ()] P − x − y data for the system carbon dioxide (1) + dodecane (2). 10 Experimental [literature data for ethane in decane (·), , propane in dodecane (⧫), − and carbon dioxide in dodecane (▴) 11,14-16 ] and calculated [PSRK ()] Henry coefficients.…”
Section: Resultsmentioning
confidence: 99%
“…The static, analytic apparatus for VLE determination presented in this work was shown to be applicable for 8,9 propane in dodecane ((), [11][12][13] and carbon dioxide in dodecane (2) 11,[14][15][16] asymmetric systems and under conditions of elevated pressure. Ten data sets were measured for six binary systems, and the results for the test system ethane + decane agree well with literature data.…”
Section: Discussionmentioning
confidence: 99%
“…Although a large amount of VLE (vapor−liquid equilibrium) and gas solubility data are available for the selected systems ethane + decane, − propane + dodecane, − carbon dioxide + dodecane, ,− and ethylene + 1-decanol, only a limited number of them provide the important information about the vapor phase composition. , The system ethane + decane was selected as a test system to verify the results obtained with our equipment by comparing them with those of Reamer and Sage . Only heat of mixing data and LLE (liquid−liquid equilibrium) data − are available for the system ethane + 1-decanol.…”
Isothermal vapor-liquid equilibrium data for the six following asymmetric binary systems were measured: ethane + decane at 411 and 444 K, propane + dodecane at 419 and 458 K, propane + 1-decanol at 408 and 448 K, ethane + 1-decanol at 448 K, ethylene + 1-decanol at 308 and 318 K, and carbon dioxide + dodecane at 318 K. A static apparatus equipped with rapid on-line sampler-injectors (ROLSIs) was used. With this device, very small samples can be withdrawn from the vapor and liquid phases in the equilibrium cell and transferred directly into the carrier gas stream for gas chromatographic analysis. The experimental data are compared to literature data and to the results predicted with the PSRK group contribution equation of state.
“…A quantitative prediction of the VLE is not possible for the selected systems with the PSRK model, but the calculated results can be used as rough estimates, and they describe the correct phenomenology. 5 Experimental [this work at 419.15 K (○,◊) and at 457.65 K (·,⧫)] and calculated [PSRK ()] P − x − y data for the system propane (1) + dodecane (2). 6 Experimental [this work at 408.15 K (○,◊) and at 448.15 K (·,⧫)] and calculated [PSRK ()] P − x − y data for the system propane (1) + 1-decanol (2). 7 Experimental [this work at 448.15 K (○,◊)] and calculated [PSRK ()] P − x − y data for the system ethane (1) + 1-decanol (2). 8 Experimental [this work at 308.15 K (○,◊) and at 318.15 K (·,⧫)] and calculated [PSRK ()] P − x − y data for the system ethylene (1) + 1-decanol (2). 9 Experimental [this work at 318.15 K (○,◊)] and calculated [PSRK ()] P − x − y data for the system carbon dioxide (1) + dodecane (2). 10 Experimental [literature data for ethane in decane (·), , propane in dodecane (⧫), − and carbon dioxide in dodecane (▴) 11,14-16 ] and calculated [PSRK ()] Henry coefficients.…”
Section: Resultsmentioning
confidence: 99%
“…The static, analytic apparatus for VLE determination presented in this work was shown to be applicable for 8,9 propane in dodecane ((), [11][12][13] and carbon dioxide in dodecane (2) 11,[14][15][16] asymmetric systems and under conditions of elevated pressure. Ten data sets were measured for six binary systems, and the results for the test system ethane + decane agree well with literature data.…”
Section: Discussionmentioning
confidence: 99%
“…Although a large amount of VLE (vapor−liquid equilibrium) and gas solubility data are available for the selected systems ethane + decane, − propane + dodecane, − carbon dioxide + dodecane, ,− and ethylene + 1-decanol, only a limited number of them provide the important information about the vapor phase composition. , The system ethane + decane was selected as a test system to verify the results obtained with our equipment by comparing them with those of Reamer and Sage . Only heat of mixing data and LLE (liquid−liquid equilibrium) data − are available for the system ethane + 1-decanol.…”
Isothermal vapor-liquid equilibrium data for the six following asymmetric binary systems were measured: ethane + decane at 411 and 444 K, propane + dodecane at 419 and 458 K, propane + 1-decanol at 408 and 448 K, ethane + 1-decanol at 448 K, ethylene + 1-decanol at 308 and 318 K, and carbon dioxide + dodecane at 318 K. A static apparatus equipped with rapid on-line sampler-injectors (ROLSIs) was used. With this device, very small samples can be withdrawn from the vapor and liquid phases in the equilibrium cell and transferred directly into the carrier gas stream for gas chromatographic analysis. The experimental data are compared to literature data and to the results predicted with the PSRK group contribution equation of state.
“…The solubility or mole fraction of the solute in the liquid phase was derived through material balances and equations of equilibrium as discussed previously (4,6). Thus the precision of the results is ±2% for the mole fraction at a given partial pressure of C02.…”
“…These quantities were calculated with the virial equation of state, truncated to the second coefficient, using experimental readings for the initial and final pressure in the gas cylinder, its temperature, and volume [12][13][14][15].…”
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