The solid−liquid equilibrium (SLE) has been measured above 280 K for eight mixtures of n-alkanes
(octadecane, eicosane, docosane, tetracosane, pentacosane, hexacosane, heptacosane, octacosane) with
methyl 1,1-dimethylethyl ether (MTBE). Experimental results of solubility are compared with values
calculated by means of the Wilson, UNIQUAC, and NRTL equations utilizing parameters taken from
the SLE. The existence of a solid−solid first-order phase transition in hydrocarbons has been taken into
consideration in the solubility calculations. The solubility of hydrocarbons in branched chain ethers is
lower than that in n-alkanes but higher than that in cycloalkanes, branched alkanes, 1-alcohols, and
tert-alcohols. The best correlation of the solubility data has been obtained by the NRTL equation, where
the average root-mean-square deviation of the solubility temperatures is 0.46 K. The liquid−liquid
equilibrium (LLE) has been measured between 300 and 360 K for binary mixtures of water with ethyl
1,1-dimethylethyl ether, methyl 1,1-dimethylpropyl ether, and ethyl 1,1-dimethylpropyl ether. The
solubility of water in branched chain ether increases with increasing temperature, whereas the solubility
of ether in water is decreasing up to 330 K and at the higher temperatures is slightly increasing. The
excess molar volumes
have been measured at the temperatures 298.15 K and 308.15 K for binary
mixtures of hexane, octane, decane, dodecane, tetradecane, hexadecane, cyclohexane, and 1-heptyne with
ethyl 1,1-dimethylpropyl ether. The excess molar volumes of all mixtures except for 1-heptyne are positive
over the whole composition range. The experimental results have been correlated with the Redlich−Kister polynomial and compared with the results predicted from Prigogine−Flory−Patterson theory. The
interchange parameter X
12, which minimized
experimental data, was adjusted and then used to
predict the heat of mixing.
