ABSTRACT

The solubilities of carbon dioxide in different alcohols, methanol, ethanol, and 1-propanol, were measured at two different temperatures (303.2 and 323.2) K and pressures up to 6 MPa. The experimental data of saturated alcohol density and viscosity were also reported at each temperature and pressure. The solubility data shows that the solubility of carbon dioxide in alcohol increases with pressure and decreases with temperatures in the studied pressure and temperature ranges. The higher dissolution of carbon dioxide in alcohols resulted in increase in the saturated liquid densities and decrease in saturated liquid viscosities. The experimental solubility as well as saturated liquid density data were predicted with two cubic equations of state (EOS), Peng Robinson (PR) and Soave Redlich Kwong (SRK). The modeling results demonstrated that both equations of state correlated the solubility data well over the studied pressure and temperature ranges. However, the saturated liquid densities calculated with the SRK EOS were much better than those of PR EOS.

Compounds

#	Formula	Name
1	CO2	carbon dioxide
2	CH4O	methanol
3	C2H6O	ethanol
4	C3H8O	propan-1-ol

Datasets

The table above is generated from the ThermoML associated json file (link above). POMD and RXND refer to PureOrMixture and Reaction Datasets. The compound numbers are included in properties, variables, and phases, if specificied; the numbers refer to the table of compounds on the left.
Type	Compound-#	Property	Variable	Phase	Method	#Points
POMD	2	Mass density, kg/m3 ; Liquid	Pressure, kPa; Liquid Temperature, K; Liquid	Liquid	ISOCHOR	20
POMD	3	Mass density, kg/m3 ; Liquid	Temperature, K; Liquid Pressure, kPa; Liquid	Liquid	ISOCHOR	20
POMD	4	Mass density, kg/m3 ; Liquid	Temperature, K; Liquid Pressure, kPa; Liquid	Liquid	ISOCHOR	20
POMD	2 1	Mole fraction - 1 ; Liquid	Temperature, K; Liquid Pressure, kPa; Liquid	Liquid Gas	Samples were flashed at atmospheric pressure. The volume of the evolved gas was measured by the Chandler Engineering Gasometer. Solubility was then calculated from density.	11
POMD	2 1	Mass density, kg/m3 ; Liquid	Temperature, K; Liquid Pressure, kPa; Liquid Mole fraction - 1; Liquid	Liquid	ISOCHOR	11
POMD	2 1	Viscosity, Pa*s ; Liquid	Temperature, K; Liquid Pressure, kPa; Liquid Mole fraction - 1; Liquid	Liquid	Moving piston method	11
POMD	3 1	Mole fraction - 1 ; Liquid	Temperature, K; Liquid Pressure, kPa; Liquid	Liquid Gas	Samples were flashed at atmospheric pressure. The volume of the evolved gas was measured by the Chandler Engineering Gasometer. Solubility was then calculated from density.	12
POMD	3 1	Mass density, kg/m3 ; Liquid	Temperature, K; Liquid Pressure, kPa; Liquid Mole fraction - 1; Liquid	Liquid	ISOCHOR	12
POMD	3 1	Viscosity, Pa*s ; Liquid	Temperature, K; Liquid Pressure, kPa; Liquid Mole fraction - 1; Liquid	Liquid	Moving piston method	12
POMD	4 1	Mole fraction - 1 ; Liquid	Temperature, K; Liquid Pressure, kPa; Liquid	Liquid Gas	Samples were flashed at atmospheric pressure. The volume of the evolved gas was measured by the Chandler Engineering Gasometer. Solubility was then calculated from density.	11
POMD	4 1	Mass density, kg/m3 ; Liquid	Temperature, K; Liquid Pressure, kPa; Liquid Mole fraction - 1; Liquid	Liquid	ISOCHOR	11
POMD	4 1	Viscosity, Pa*s ; Liquid	Temperature, K; Liquid Pressure, kPa; Liquid Mole fraction - 1; Liquid	Liquid	Moving piston method	11

Thermodynamics Research Center / ThermoML | Journal of Chemical Thermodynamics

Experimental measurements and predictions of density, viscosity, and carbon dioxide solubility in methanol, ethanol, and 1-propanol

Kariznovi, M.[Mohammad], Nourozieh, H.[Hossein], Abedi, J.[Jalal]

ABSTRACT