Solubilities of hydrogen, nitrogen, and carbon dioxide in diphenylmethane

Abstract

Hydrogen (H2), nitrogen (N2) and carbon dioxide (CO2) 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 N2 in dodecane and CO2 in decane at 344 K. The experimental data were fitted by empirical correlation x=(aT2+bT+c)(dp2+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 CO2 > N2 ≈ H2. Krichevsky- Kasarnovsky (K-K) equation was used to fit the experimental data. The absolute average relative deviation (AAD) between the experimental data of H2+DPM, N2+DPM and CO2+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. H2 and N2 solubilities showed to be endothermic, while CO2 showed the opposite trend.