Solvent losses in gas absorption. Solubility of methanol in compressed natural and synthetic gases

Abstract

Experimental results are reported for the solubility of methanol in compressed nitrogen, methane, ethane and carbon dioxide in the region −45° to +10°C and 17 to 62 bars. New and previously published experimental data are used to obtain (or estimate) second virial coefficients for all binary pairs in mixtures containing hydrogen, nitrogen, carbon monoxide, methane, ethane, propane, carbon dioxide, hydrogen sulfide and methanol. These coefficients, combined with experimental data for the vapor pressure of methanol and with Henry's constants, partial molar volumes and Margules coefficients for dissolved gases in methanol, yield a correlation for calculating solvent losses as a function of temperature, pressure and gas composition. For a large‐scale natural‐gas absorption process, these losses may represent a significant economic factor in plant design.

Correlating Mass Transfer Coefficients of O2 and N2 in Methanol in a Stirred‐Tank Reactor

“…Fig. 3 also shows that K H of N 2 in methanol is universally greater than that of O 2 in the range of testing, which is consistent with the previous reports on the solubility of O 2 and N 2 in methanol systems 29, 30.…”

John M. Prausnitz: Bridging abstractions and realities

“…The subjects ranged from the fundamentally rigorous to the fully applied. Some examples include statistical mechanical partition functions to obtain equations of state, intermolecular force models and molecular simulation, acid‐gas absorption, complex mixtures, and distillation . In other directions, there were 17 articles on adsorption (one of which has been cited 959 times) and seven on weak electrolytes, including one cited 316 times.…”

Simulation of continuous-contact separation processes: unsteady-state, multicomponent, adiabatic absorption

“…The above equations must be solved simultaneously to determine values of the dependent variables, listed in Table I, as functions of time and position within the column. In this study, equilibrium distribution coefficients, K¡, were calculated either from solubility data presented by Lazalde-Crabtree et al (1980) and Landolt-Bórnstein (1976) or by using equations of state for both the liquid and vapor phase. The equations of state used in this work were the Soave-Redlich-Kwong (SRK) equation and the Peng-Robinson (PR) equation; binary interaction parameters were obtained from Chang (1984).…”