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- W2089313747 abstract "Heat capacities and phase-transition enthalpies have been measured for three ethanoate hydrates by adiabatic-shield calorimetry between 270 and 400 K. Enthalpies and entropies have been derived for the exact stoichiometries and tabulated for selected temperatures. The molar enthalpy of transition of CH3CO2Na·3H2O to (CH3CO2Na + aqueous solution) at 331.52 K is (37.86±0.25) kJ·mol−1. The molar enthalpy of transition of CH3CO2Na·3H2O to an aqueous solution is (38.7±0.3) kJ·mol−1, when the enthalpy of dissolution of remaining anhydrous enthanoate up to 358 K is included. The enthalpy of transition of CH3CO2Li·2H2O to (CH3CO2Li + aqueous solution) at 324.71 K is (24.25±0.20) kJ·mol−1. The enthalpy of transition of α-(CH3CO2)2Mg·4H2O to {aqueous solution + a less hydrated solid phase, presumably (CH3CO2)2Mg·H2O} at 336 K is (35.8±0.5) kJ·mol−1. Water-vapour saturation pressures above the samples have been measured at selected temperatures. Lattice constants determined from Guinier photographs at 300 K for CH3CO2Na·3H2O are: a = 1234.5 pm, b = 1045.1 pm, c = 1040.8 pm, β = 111.70°; for CH3CO2Li·2H2O: a = 682.1 pm, b = 1088.4 pm, c = 659.6 pm; for α-(CH3CO2)2Mg·4H2O: a = 480.5 pm, b = 1198.6 pm, c = 855.3 pm, β = 95.38°; and for (CH3CO2)2Mg·H2O: a = 1175.9 pm, b = 1753 pm, c = 666.3 pm. CH3CO2Na·3H2O might be of interest as an energy-storage material because of its high molar enthalpy of fusion, if supercooling and segregation of anhydrous ethanoate can be prevented." @default.
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- W2089313747 date "1984-06-01" @default.
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- W2089313747 title "Thermodynamic properties and phase transitions of salt hydrates between 270 and 400 K III. CH3CO2Na·3H2O, CH3CO2Li·2H2O, and (CH3CO2)2Mg·4H2O" @default.
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- W2089313747 doi "https://doi.org/10.1016/0021-9614(84)90003-x" @default.
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