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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, the Gibbs energy of formation of Tm2Ru2O7(s) has been determined employing a solid-state electrochemical cell incorporating an oxide ion conducting electrolyte.

2 citations

Journal ArticleDOI
TL;DR: In this paper, the molar volume and the partial molar entropy of the adsorbed monolayer were determined as a function of the temperature, and it was shown that the volume of the monolayers is practically constant under the present experimental conditions.
Abstract: With the use of high-precision gas-chromatography, the multilayer adsorption of methane on fused silica beads was precisely measured between 145.0 K and 213.6 K. The molar volume and the partial molar entropy of the adsorbed methane were determined as a function of the temperature. The molar volume in the monolayer region depends much less on the temperature than that of the bulk liquid. However, the molar volume of multilayer adsorbed methane shows a dependence on the temperature similar to that of bulk liquid, which is at a lower temperature. The volume of the monolayer is practically constant under the present experimental conditions. The apparent thickness of the adsorbed monolayer was interpreted in terms of a simple collision model. The partial molar entropy of the adsorbed phase is much lower than that of the saturated bulk liquid. The lower dependence of the molar volume on the temperature and the lower entropy suggest that the freedom of motion of the adsorbed molecules is restricted as compared ...

2 citations

Journal ArticleDOI
TL;DR: In this paper , the thermal properties of aqueous electric double layer capacitors with KOH electrolytes were measured using the in situ and operando 3ω hot-wire method.

2 citations

Journal Article
TL;DR: The standard entropy of K 3 Na[UO 2 (CO 3 ) 3 ] at 298.15 K (-4001.0 ′ 8.5 kJ/mol) was determined by reaction calorimetry as mentioned in this paper.
Abstract: The standard enthalpy of formation of crystalline K 3 Na[UO 2 (CO 3 ) 3 ] at 298.15 K (-4001.0 ′ 8.5 kJ/mol) was determined by reaction calorimetry. The heat capacity of the compound was measured by adiabatic calorimetry overthe temperature range 8-560 K, and its thermodynamic functions were calculated. The standard entropy (-955.5 ′ 2.1 J/(mol K)) and Gibbs function of formation at 298.15 K (-3716.0 ′ 9.0 kJ/mol) were determined.

2 citations

Journal ArticleDOI
TL;DR: In this article, the crystal growth kinetics of CHZ-ethanol for different degrees of supersaturation (SS) has been studied, and the particle size control in batch crystallization can be achieved by optimizing the operating conditions to get the desired size crystals.
Abstract: Background: Chlorzoxazone (CHZ) is a water-insoluble drug having bioavailability problems. The absorption rate of such drugs can be improved by reducing their particle size. In this work, the crystal growth kinetics of CHZ–ethanol for different degrees of supersaturation (SS) has been studied. Method: The equilibrium solubility data of CHZ in ethanol is determined by the shake-flask method within the 283.15–313.15 K temperature range. The mole fraction solubility of CHZ is calculated and correlated with the modified Apelblat equation, λh equation, van’t Hoff equation, Wilson, and non-random two liquid (NRTL) equation. Batch crystallization experiments are performed on three different degrees of SS-1.16, 1.18, and 1.20 at 293.15 K as a function of time. Results: The maximum root mean square difference (RMSD) and relative average deviation (RAD) values of 169.24 x10-6 and 0.699 x10-2, respectively, are observed in the NRTL equation model. The dissolution properties such as standard enthalpy, standard entropy, and Gibbs free energy are predicted using van’t Hoff equation. Using a simple integral technique, the average crystal growth rate constant KG is calculated as 1.58 (μm/min) (mg/ml)-1 and the order n=1 for CHZ–ethanol at 293.15 K. Conclusion: The obtained result concludes that the crystals growth size is found to be varied at different SS ratio in batch crystallization. The particle size control in batch crystallization can be achieved by optimizing the operating conditions to get the desired size crystals.

2 citations


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Performance
Metrics
No. of papers in the topic in previous years
YearPapers
202316
202229
202141
202055
201949
201857