Excess Molar Volumes, Viscosities, and Heat Capacities for the Mixtures of Ethylene Glycol + Water from 273.15 K to 353.15 K

Abstract

Experimental densities, viscosities, and heat capacities at different temperatures were measured over the entire mole fraction range for the binary mixture of ethylene glycol + water. Density values were used in the determination of excess molar volumes, V E . The excess volumes, V E , are fitted as a function of the mole fraction to a polynomial. ∆η was fitted to the Redlich-Kister equation. The excess volumes are negative over the entire composition at the lower temperatures. They show a U-shaped concentration dependence and decrease in absolute value with increasing temperature. At high temperatures, the excess molar volume shows an S-shaped dependence. ∆η values are negative over the entire range of mole fraction and have a very similar trend to that for V E . The heat capacities of mixtures have the maximum values at x 1 ) 0.0312.

Specific heat of metal oxide nanofluids at high concentrations for heat transfer

“…All obtained deviations are well within the combined accuracy of both data sets. Unlike ethylene glycol, the ethylene glycol + water mixture exhibits a non-linear temperature behavior as it has been reported in literature [72,79]. This can be ascribed to the temperature behavior of excess molar heat capacity due to hydrogen bounds in the mixture.…”

“…It must also be pointed out that, only the data reported by Stephens et al [74] and Zábranský et al [76] cover the entire temperature range in which ethylene glycol was studied in this work. Percentage Average Absolute Deviations, AAD%, between both data sets are less or equal to 1.7% for ethylene glycol [71][72][73][74][75][76][77] and 2.5% for the ethylene glycol + water mixture at 50% in volume [59,72,78,79]. All obtained deviations are well within the combined accuracy of both data sets.…”

“…Firstly, the values obtained for base fluid were compared with those available in the literature [59,[71][72][73][74][75][76][77][78][79] with the aim of verifying whether reported heat capacity measurements are valuable. It must also be pointed out that, only the data reported by Stephens et al [74] and Zábranský et al [76] cover the entire temperature range in which ethylene glycol was studied in this work.…”

Viscosity Measurements and Correlation of the Squalane + CO2 Mixture

“…(2) and determined from the experiment with toluene. The experimental data for ethylene glycol and toluene were taken from Yang et al [8] and Assael et al [9], respectively. As shown in Tables I and II, fairly good agreement was obtained for both cases.…”

Non-ideal behaviour of imidazolium based room temperature ionic liquids in ethylene glycol at T= (298.15 to 318.15) K

“…EG is highly self-associated because of hydrogen bonding ability of its two hydroxyl groups. When mixed in water [21][22][23][24][25][26] or organic solvents [27,28] the self-associated structure of EG disrupts and give rise to the interesting thermodynamic properties as a consequence of specific interactions. However, the mixing behaviour of EG in the ILs is scarcely examined [29].…”