New
phase equilibrium data of CO2 in n-hexadecane, n-heptadecane, n-octadecane, n-nonadecane, and n-eicosane were measured
at temperatures from 333.15 to 373.15 K up to 23.73 MPa by a constant-volume
method. Thermodynamic properties of Gibbs free energy (Δsol
G), enthalpy change (Δsol
H), entropy change (Δsol
S), and Henry’s coefficient (H)
were calculated and analyzed for elucidating the dissolution mechanism
of CO2 in alkanes. Results showed that the CO2 solubility increased with increasing pressure but decreased with
increasing temperature and carbon number. In addition, increasing
carbon number also led to an increase in the minimum miscibility pressure
(MMP) of alkanes with CO2 and thus limited CO2 solubility in alkanes.