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2 O 6 ·4H 2 O was interpreted by the Kissinger method [ 22 ]. The kinetic ( E a , ln A ) and thermodynamic functions (Δ H ≠ , Δ S ≠ , Δ G ≠ ) of the decomposition reaction of MnV 2 O 6 ·4H 2 O are discussed for the first time

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polynomial equation of heat capacities ( C p,m ) as a function of reduced temperature ( X ), [ X = f ( T )], by a least squares method so as to calculate smoothed heat capacities and various thermodynamic functions of the coordination compound

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Abstract  

Temperature dependences of solubility, saturated vapour pressure and crystal heat capacity of [4-(Benzyloxy)phenyl]acetic acid were determined. The solubility of this compound was investigated in n-hexane, buffered water solutions with pH 2.0 and 7.4 and n-octanol. The enthalpy of sublimation and vaporization as well as the fusion temperature were determined. Solvation and solubility processes have been analyzed. The thermodynamics of transfer processes from one buffer to another (protonation process), from buffers to 1-octanol (partitioning process), and from n-hexane to the applied solvents (specific interaction) have been calculated and compared to those of other NSAIDs. The relevant shares of specific and non-specific interactions in the process of solvation have been investigated and discussed.

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Journal of Thermal Analysis and Calorimetry
Authors: A. V. Markin, V. A. Ruchenin, N. N. Smirnova, G. V. Markin, S. Yu. Ketkov, V. A. Kuropatov, V. K. Cherkasov, G. A. Abakumov, and G. A. Domrachev

) thermodynamic functions heat capacity, enthalpy, entropy, and Gibbs function for fulleride dimer in the range from T → 0 to 175 K and for [(η 6 -( m -xylene)) 2 Mo] •+ [C 60 ] •− monomeric complex for the interval between 220 and 320 K; comparison the

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4 ) 6 Cl 2 and Ba 9.5 Cs 0.5 (PO 4 ) 6 Cl 2−δ were least squares fitted to obtain the following polynomials in temperature Table 2 Thermodynamic functions of Ba 10 (PO 4 ) 6 Cl 2 T /K C p ,m /J K −1 g −1 /J g −1 /J K −1 g −1  Measured Fit 298 0

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.99 The deviation from the ideal behavior can best be expressed in terms of excess thermodynamic functions, namely, excess free energy ( g E ), excess enthalpy ( h E ), and excess entropy ( s E ), which give a more quantitative idea about the nature of

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, respectively. Thermodynamic functions were calculated extrapolating the measured C p (T) curve down to 0 K. The smoothed values of the C p and the calculated thermodynamic parameters at selected temperatures are summarized in Table 2

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Thermal and kinetic analysis of uranium salts

Part 2. Uranium (VI) acetate hydrates

Journal of Thermal Analysis and Calorimetry
Authors: Gülbanu Koyundereli Çılgı, Halil Cetişli, and Ramazan Donat

with this selected equation. Using these optimized values, other thermodynamic functions (Δ H *, Δ S *, and Δ G *) were calculated. Theory There are different methods in the academic literature for the calculations of

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−1 , −69.88 J K −1 mol −1 and 93.27 kJ mol −1 for Δ H # , Δ S # and Δ G # , respectively) because the different methods and nature solid were applied. This indicates that the kinetic and thermodynamic functions of decomposition of each solid are

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Thermal and kinetic analysis of uranium salts

Part 1. Uranium (VI) oxalate hydrates

Journal of Thermal Analysis and Calorimetry
Authors: Halil Cetişli, Gülbanu Koyundereli Çılgı, and Ramazan Donat

energy value to those obtained from model-free equations. The optimized value of activation energy and Arrhenius factor were calculated with the best equation. Using these optimized values, other thermodynamic functions (Δ H *, Δ S *, and Δ G *) were

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