Abstract
The thermodynamic equilibrium of the liquid-phase bimolecular dehydration of 1-pentanol to di-n-pentyl ether (DNPE) and water was studied in the temperature range of 423−463 K over Amberlyst 70. Furthermore, the equilibrium position of two side reactions could be followed, DNPE decomposition to 1-pentanol and 1-pentene and isomerization of 1-pentene to 2-pentene. The etherification reaction proved to be slightly exothermic, with an enthalpy change of reaction at 298.15 K of −(3.8 ± 0.6) kJ mol-1. From this value, the standard formation enthalpy and molar entropy of DNPE were computed to be −(421.1 ± 1.2) kJ mol-1 and 473.71 J (K·mol)-1, respectively. The enthalpy changes of the reaction of DNPE decomposition to 1-pentene and 1-pentanol and 1-pentene isomerization to 2-pentene were 63.4 ± 0.9 and −19.7 ± 2.1 kJ mol-1, respectively.
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