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25 th European Symposium on Applied Thermodynamics, June 24 - 27, 2011, Saint Petersburg, Russia. Phase Equilibria for Carbon Dioxide + 1-Pentanol System at High Pressures. Politehnica University of Bucharest, Department of Applied Physical Chemistry & Electrochemistry - PowerPoint PPT Presentation
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Catinca Secuianu*, Viorel Feroiu, and Dan Geană
Phase Equilibria for Carbon Dioxide + 1-Pentanol System at High Pressures
25th European Symposium on Applied Thermodynamics, June 24 - 27, 2011, Saint Petersburg, Russia
Politehnica University of Bucharest, Department of Applied Physical Chemistry & Electrochemistry1-7 G-ral Gh. Polizu, S1, 011061 Bucharest, ROMANIA
Thermodynamic knowledge of the high-pressure phase behaviour of carbon dioxide + alcohols mixtures is essential for the design and implementation of many chemical and biotechnological processes. Very often a small amount of a polar modifier such as an alcohol is added to the supercritical carbon dioxide toenhance the extraction efficiency of polar compounds.
In this work the fluid phase behaviour of the binary system carbon dioxide + 1-pentanol has been measured. Measured and literature data were modelled with different equations of state coupled with classical van der Waals and GE-EOS (HVID, MHV1, MHV2) mixing rules.
Thermodynamic knowledge of the high-pressure phase behaviour of carbon dioxide + alcohols mixtures is essential for the design and implementation of many chemical and biotechnological processes. Very often a small amount of a polar modifier such as an alcohol is added to the supercritical carbon dioxide toenhance the extraction efficiency of polar compounds.
In this work the fluid phase behaviour of the binary system carbon dioxide + 1-pentanol has been measured. Measured and literature data were modelled with different equations of state coupled with classical van der Waals and GE-EOS (HVID, MHV1, MHV2) mixing rules.
Introduction
Phase behaviour measurements were made in a high-pressure visual cell with variable volume based on the static-analytical method [1,2].
Vapour-liquid and vapour-liquid-liquid equilibria data for the carbon dioxide + 1-pentanol system at 293.15, 303.15, 316.65, and 333.15 K up to 10.67 MPa were determined. The higher temperatures branch of the three-phase liquid-liquid-vapour line and the upper critical endpoint and the lower critical endpoint were measured.
Phase behaviour measurements were made in a high-pressure visual cell with variable volume based on the static-analytical method [1,2].
Vapour-liquid and vapour-liquid-liquid equilibria data for the carbon dioxide + 1-pentanol system at 293.15, 303.15, 316.65, and 333.15 K up to 10.67 MPa were determined. The higher temperatures branch of the three-phase liquid-liquid-vapour line and the upper critical endpoint and the lower critical endpoint were measured.
Experimental work
Results
AcknowledgementsThe authors are grateful to the National Council of Scientific
Research of Romania (CNCS) for financial support.
Pressure-composition data for carbon dioxide + 1-pentanol system
P-T projection of the LLV line (second branch)
P-T fluid phase diagram of carbon dioxide + 1-pentanol system
Comparison of measured and literature data at 313.15 K
Comparison of measured and literature VLE data at different temperatures with model results
Comparison of literature VLE data at 426.86 K with model results
[1] Secuianu, C., Feroiu, V., Geana, D., J. Chem. Eng. Data 48 (2003) 1384.[2] Secuianu, C., Feroiu, V., Geana, D., Rev. Chim. (Bucharest) 54 (2003) 874.[3] Staby, A., Mollerup, J., J. Supercrit. Fluids 4 (1991) 233.[4] Jennings, D.W., Chang, F., Bazaan, V., Teja, A.S., J. Chem. Eng. Data 37 (1992) 337.[5] Silva-Oliver, G., Galicia-Luna, L.A., Sandler, S.I., Fluid Phase Equilib. 200 (2002) 161.[6] Raeissi, S., Gauter, K., Peters, C., Fluid Phase Equilib. 147 (1998) 239.[7] Gutierrez, J.E., Bejarano, A., de la Fuente, J.C., J. Chem. Thermodyn. 42 (2010) 591.
[1] Secuianu, C., Feroiu, V., Geana, D., J. Chem. Eng. Data 48 (2003) 1384.[2] Secuianu, C., Feroiu, V., Geana, D., Rev. Chim. (Bucharest) 54 (2003) 874.[3] Staby, A., Mollerup, J., J. Supercrit. Fluids 4 (1991) 233.[4] Jennings, D.W., Chang, F., Bazaan, V., Teja, A.S., J. Chem. Eng. Data 37 (1992) 337.[5] Silva-Oliver, G., Galicia-Luna, L.A., Sandler, S.I., Fluid Phase Equilib. 200 (2002) 161.[6] Raeissi, S., Gauter, K., Peters, C., Fluid Phase Equilib. 147 (1998) 239.[7] Gutierrez, J.E., Bejarano, A., de la Fuente, J.C., J. Chem. Thermodyn. 42 (2010) 591.
References
0
2
4
6
8
10
12
0 0.2 0.4 0.6 0.8 1
p/M
Pa
Mole fractions of CO2
T = 293.15 K
T = 303.15 K
T = 316.65 K
T = 333.15 K
LLV line
8.7
8.75
8.8
8.85
8.9
8.95
9
315 315.5 316 316.5 317 317.5 318
p/M
Pa
T/K
LLV line this work
LCEP
UCEP
UCEP (Raeissi et al.)
LCEP (Raiessi et al.)
0
2
4
6
8
10
12
14
16
18
20
200 300 400 500 600
p/M
Pa
T/K
UCEP
LCEP
UCEP
SLLV
GEOS/2PCMR
PR/2PCMR
0
5
10
15
20
25
302 307 312 317
p/M
Pa
T/K
313.15 K
0
5
10
15
20
25
0 0.2 0.4 0.6 0.8 1
p/M
Pa
Mole fractions of CO2
T = 325.9 K
GEOS/2PCMR
T = 337.4 K
PR/2PCMR
T = 343.2 K
SRK/MHV2
T = 353.15 K
SRK/HVID
T = 373.2 K
SRK/2PCMR
T = 426.86 K
SRK/MHV1
0
5
10
15
20
0 0.2 0.4 0.6 0.8 1
p/M
Pa
Mole fractions of CO2
T = 426.86 K
GEOS/2PCMR
PR/2PCMR
SRK/2PCMR
SRK/HVID
SRK/MHV1
SRK/MHV2
0
1
2
3
4
5
6
7
8
9
0 0.2 0.4 0.6 0.8 1
p/M
Pa
Mole fractions of CO2
T = 313.15 K (this work)
T = 313.2 K (Staby & Mollerup, 1993)
T = 313 K (Gutierrez et al., 2010)
•Current address: Qatar Carbonates & Carbon Storage Research Centre, Department of Chemical Engineering Imperial College London, South Kensington Campus, Exhibition Road, London SW7 2AZ U.K. Tel.: +44 (0)20 7594 1341. Fax: +44 (0)20 7594 5692/5700 Email: [email protected] http://www3.imperial.ac.uk/people/c.secuianu
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