Solubilities of hydrogen, nitrogen, and carbon dioxide in diphenylmethane

Hydrogen (H 2 ), nitrogen (N 2 ) and carbon dioxide (CO 2 ) solubilities were measured at the temperature (313 to 363) K and the pressure (0.809 to 6.194) MPa. The reliability of the experimental system was verified by measuring the solubilities of N 2 in dodecane and CO 2 in decane at 344 K. The experimental data were fitted by empirical correlation x = ( a T 2 + b T + c ) ( d p 2 + e p + f ) $x=(a{T}^2+bT+c)(d{p}^2+ep+f)$ , and the relative deviations between the experimental value and the literature value for the solubilities at given pressure and temperature were less than ±5 %. Under the same temperature and pressure conditions, the solubilities of the three gases in DPM is CO 2 > N 2 ≈ H 2 . Krichevsky- Kasarnovsky (K-K) equation was used to fit the experimental data. The absolute average relative deviation (AAD) between the experimental data of H 2 +DPM, N 2 +DPM and CO 2 +DPM systems and the calculated values of K-K equation are 1.21 %, 1.86 % and 0.88 %, respectively. In addition, the Henry constants of three gases dissolved in DPM were calculated, and the solution enthalpy, solution entropy, solution Gibbs free energy and solution specific heat capacity were calculated. H 2 and N 2 solubilities showed to be endothermic, while CO 2 showed the opposite trend.