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Abstract
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In this work, solubility of hydrogen in some alkenes was investigated at diferent temperatures and pressures. Solubility values were calculated using the Peng–Robinson equation of state. Binary interaction parameters were calculated using ftting
the equation of state on experimental data, Group contribution method and Moysan correlations and total average absolute
deviation for these methods was 3.90, 17.60 and 13.62, respectively. Because hydrogen solubility in Alkenes is low, Henry’s
law for these solutions were investigated, too. Results of calculation showed with increasing temperature, Henry’s constant
was decreased. The temperature dependency of Henry’s constants of hydrogen in ethylene and propylene was higher than to
other alkenes. In addition, using Van’t Hof equation, the thermodynamic parameters for dissolution of hydrogen in various
alkenes were calculated. Results indicated that the dissolution of hydrogen was spontaneous and endothermic. The total
average of dissolution enthalpy (ΔH◦) and Gibbs free energy (ΔG◦) for these systems was 3.867 kJ/mol and 6.361 kJ/mol,
respectively. But dissolution of hydrogen in almost of alkenes was not an entropy-driven process.
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