Solubility of nonpolar gases in 2,6-dimethylcyclohexanone

Abstract

URIETA, and CELSO GUTIERREZ LOSA. Can. J. Chem. 68, 435 (1990).Solubility measurements of He, Ne, Ar, Kr, Xe, Hz, DZ, N2, CH4, C2H4, C2H6, CF4, SF6, and C 0 2 in 2,6-dimethylcyclohexanone at temperatures 273.15 to 303.15 K and at a gas partial pressure of 101.33 kPa are reported. Standard changes in Gibbs energy, enthalpy, and entropy for the dissolution process at 298.15 K are also presented. Results for both solubility and thermodynamic functions are compared with those for cyclohexanone and 2-methylcyclohexanone. The scaled particle theory is used to obtain the effective Lennard-Jones (6,12) pair potential parameters for 2,6-dimethylcyclohexanone and, from these, the values it predicts for the solubility of the studied gases in the solvent are obtained.

Solubilities of gases in cycloethers. The solubility of 13 nonpolar gases in 2,5-dimethyltetrahydrofuran at 273.15 to 303.15 K and 101.32 kPa

“…are. The same pattern has been observed for the similar cycloketone series cyclohexanone, 2-methylcyclohexanone, and 2,6-dimethylcyclohexanone [33][34][35].…”

Solubility Measurement and Thermodynamic Properties Calculation for Several CO2 + Ether Absorbent Systems

“…Two parameters, Henry’s constant ( H x ) and mass solubility ( S ), were used to assess the absorption ability for per mole and gram absorbent, respectively. Thus, the parameters at 273.15 K for the ether absorbents, ionic liquids, , common solvents, − and absorbents studied in previous work were compared and are shown in Table . The absorption ability of per gram absorbent may be dominated by H x and the molecular weight of the absorbent, which can be verified by Table .…”

Study of Molecular Interactions in Binary Mixtures at Various Temperatures Containing 2,6-Dimethylcyclohexanone and Aliphatic Primary Alcohols: Thermodynamics and FT-IR Spectroscopic Studies

“…The purity of the solvents was assessed by comparing the experimental density, speed of sound, and viscosity with available literature values ,− at different temperatures; see Table . However, the excess volume ( V E ) was calculated from the following relation: V normalE = ∑ i = 1 n x i M i ρ m − prefix∑ i = 1 n x i M i ρ i Here, ρ represents the density of the mixture; M i­ and ρ i are the molar mass and density of component i , and x i is its mole fraction.…”