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Standard molar entropy
About: Standard molar entropy is a research topic. Over the lifetime, 1586 publications have been published within this topic receiving 29886 citations.
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TL;DR: In this paper, five protic ionic liquids (PILs) have been synthesized through atom economic neutralization reaction between N-butyl hydroxyethyl amine and bronsted acid RCOOH, where R is H, CH 3, C 2 H 5, C 3 H 7, and C 4 H 9.
15 citations
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TL;DR: In this paper, a series of chiral dicationic ionic liquids (DILs) were successfully synthesized and characterized by IR and NMR, and the density of the whole family of ILs was measured and related physical properties including thermal expansion coefficient, molecular volume, standard molar entropy, and crystal energy were estimated by theoretical methods.
15 citations
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TL;DR: The osmotic coefficient measurements for binary aqueous solutions of 2,2,2-cryptand and 4,7,13,16,21,24-hexaoxa-1,10-diazabicyclo[8.8] hexacosane and the excess and mixing thermodynamic properties have been obtained using the activity data from this study and the heat data reported in the literature.
Abstract: The osmotic coefficient measurements for binary aqueous solutions of 2,2,2-cryptand (4,7,13,16,21,24-hexaoxa-1,10-diazabicyclo[8.8.8] hexacosane) in the concentration range of ~0.009 to ~0.24 mol·kg(-1) and in ternary aqueous solutions containing a fixed concentration of 2,2,2-cryptand of ~0.1 mol·kg(-1) with varying concentration of KBr (~0.06 to ~0.16 mol·kg(-1)) have been reported at 298.15 K. The diamine gets hydrolyzed in aqueous solutions and needs proper approach to obtain meaningful thermodynamic properties. The measured osmotic coefficient values are corrected for hydrolysis and are used to determine the solvent activity and mean ionic activity coefficients of solute as a function of concentration. Strong ion-pair formation is observed, and the ion-pair dissociation constant for the species [CrptH](+)[OH(-)] is reported. The excess and mixing thermodynamic properties (Gibbs free energy, enthalpy, and entropy changes) have been obtained using the activity data from this study and the heat data reported in the literature. Further, the data are utilized to compute the partial molal entropies of solvent and solute at finite as well as infinite dilution of 2,2,2-cryptand in water. The concentration dependent non-linear enthalpy-entropy compensation effect has been observed for the studied system, and the compensation temperature along with entropic parameter are reported. Using solute activity coefficient data in ternary solutions, the transfer Gibbs free energies for transfer of the cryptand from water to aqueous KBr as well as transfer of KBr from water to aqueous cryptand were obtained and utilized to obtain the salting constant (ks) and thermodynamic equilibrium constant (log K) values for the complex (2,2,2-cryptand:K(+)) at 298.15 K. The value of log K = 5.8 ± 0.1 obtained in this work is found to be in good agreement with that reported by Lehn and Sauvage. The standard molar entropy for complexation is also estimated for the 2,2,2-cryptand-KBr complex in aqueous medium.
15 citations
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TL;DR: In this paper, an experimental study of the equilibrium B2O3l + BCl3g = (BOCl)3g has been made by the method of transpiration in the temperature range of 536°-825°K.
Abstract: An experimental study of the equilibrium B2O3(l)+BCl3(g) = (BOCl)3(g) has been made by the method of transpiration in the temperature range of 536°—825°K. The enthalpy and entropy changes of the reaction in this temperature range were found to be 5.0±0.3 kcal/mole and 3.1±0.5 cal/deg/mole, respectively. The data have been interpreted to yield the heat of formation, ΔH°f695°K = 391.5±0.3 kcal/mole, and entropy, S°695°K = 124.2±0.5 cal/deg/mole, of gaseous (BOCl)3. Partial pressure studies indicate that the quantity of the monomer, BOCl, present in the temperature range under consideration is negligible.
15 citations
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TL;DR: In this article, the defect structure of complex oxides was described within the point defects approach by fitting the parameters of theoretical equations log (P O 2 ) = f ( δ ) to the set of experimental data.
15 citations