Volumetric Behavior of Decane + Carbon Dioxide at High Pressures. Measurement and Calculation

Abstract

The volumetric behavior of carbon dioxide (1) + decane (2) mixtures has been investigated under the high pressures 20, 30, and 40 MPa in the temperature range [308.15 K to 368.15 K]. Densities have been measured for pure decane and for x 1 ) 0.15, 0.30, 0.51, 0.66, 0.78, and 0.84. Density variations show a peculiar behavior: a crossover phenomenon with the composition at a given pressure and temperature is observed. The measured fluid densities have been compared with values predicted by equations of state with various mixing rules. This comparative study has revealed models well adapted to these density estimations.

High pressure solubility data of carbon dioxide in (tri-iso-butyl(methyl)phosphonium tosylate+water) systems

“…The apparatus and the measurement procedure followed have been previously described in detail [35][36][37]. The variable volume high pressure cell sketched in figure 1 consists in a horizontal hollow stainless steel cylinder closed at one end by a movable piston and one sapphire window at the other end allowing for visual observation of the fluid.…”

Fractionation technologies for liquid mixtures using dense carbon dioxide

“…Few studies reporting experimental data of binary mixtures of alcohols or acetone with CO 2 are reported in the literature [231][232][233][234]. Indeed, most studies reporting experimental values of the volumetric behaviour of mixtures with CO 2 or other gases at high pressures relate to hydrocarbons [235][236][237][238][239][240][241][242]. Fluid densities can also be obtained from phase equilibrium modelling by use of an appropriate EoS.…”

Compressed liquid densities and excess molar volumes for (CO2+1-pentanol) binary system at temperatures from 313 to 363K and pressures up to 25MPa

“…Even though the concept of excess property cannot be thermodynamically correct apply, because the pure components of the mixture are not in the same phase due to the ranges of temperature and pressures measured in this work [22], the calculated ''excess'' property can be used to establish a deviation from the ideal sum of properties of the mixture. Therefore, the V E m is a mixing excess value and not an excess value from a thermodynamic point of view [23].…”