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through the proposed model. The cation/basic center interactions at the solid/liquid interface were also followed calorimetrically, and the set of thermodynamic data involved in these interactive processes was determined. Experimental
spectroscopical reports on these compounds, to our knowledge, no reports about their morphology control and little or no thermodynamic data are available. Properties of a compound are closely related to its particle morphology, which will affect on
Thermodynamics of the coordination compound Zn(Met)(NO3)2·1/2H2O(s) (Met = l-α-methionine)
Low temperature heat capacities and the standard molar enthalpy of formation
other thermodynamic data. If “s” = calorimetric solvent, 2 mol dm −3 HCl (aq), the dissolution process of the mixture of reactants in reaction ( 5 ) is expressed as {ZnSO 4 ·7H 2 O(s) + 2NaNO 3 (s) + l -Met(s)} + “s” to give solution A. The
NH 3 ) 2 ZnCl 4 (s) is given in Table 5 . The experimental values of the dissolution enthalpies of the reactants and product of the reaction 8 were combined with some auxiliary thermodynamic data, and [ 22 ], and the standard molar enthalpy of
Abstract
The distribution of La(III), Ce(III) and Y(III) from potassium thiocyanate solutions by tributyl phosphate is described. The dependence of extraction on pH, thiocyanate concentration, metal and extractant concentration, diluent type and temperature, was thoroughly investigated. Solvation numbers and thermodynamic data were calculated and discussed. A method has been suggested for the separation of Th(IV) from such elements.
, there is an urgent need for relevant thermodynamic data of sodium isophthalic acid derivatives. In this article, we synthesized sodium 5-methylisophthalic acid monohydrate (C 9 H 6 O 4 Na 2 ·H 2 O, s) and sodium isophthalic acid hemihydrate (C 8
Abstract
To study the coherence of thermodynamic data of the AgNO3-LiNO3 -RbNO3 ternary system, phase diagram of the binary system AgNO3 -LiNO3 has been obtained between 303 and 550 K by direct and differential thermal analysis technique. This system is characterized by an eutectic point (25% mol. LiNO3 , 445±1 K) and a plateau due to the solid-solid transition in AgNO3 at 434±1 K. In the solid state the solubility of each component in the other seems to be nil or negligible (no more than a few percents). Using other thermodynamic data, the excess properties of the binary liquid (AgNO3 - LiNO3 ) were calculated at 623 K.
The fluoride dilemma
Thermodynamics of anion recognition by calixpyrroles
Abstract
The implications of environmental contamination by fluoride on human health call upon the need for the development of monitoring systems for the ‘in situ’ detection of fluoride in contaminated sources and new technologies approaches for their removal. This paper reports recent work on the design of calixpyrrole receptors selective for the fluoride anion. The various steps undertaken for the thermodynamic characterization of these receptors and their anionic complexes are discussed. Thus based on thermodynamic data, the medium and ligand effects on selectivity are quantitatively assessed using representative calixpyrrole derivatives.
Abstract
Starting from tabulated thermodynamic data of stable compounds in the Mo−O−Cl system, phase diagrams for the Mo−O−Cl system were developed on the basis of GIBBS' phase law by means of thermodynamic calculations. The behaviour of molybdenum trioxide in a temperature gradient tube was investigated experimentally under chlorinating conditions, using99Mo as indicator. The thermochromatografically separated compounds were characterized by their deposition temperature in the temperature gradient tube and by an activation analytical determination of their Mo/Cl ratio. The experimental results were compared with the calculated phase diagram.
Abstract
Heat capacity of methacetin (N-(4-methoxyphenyl)-acetamide) has been measured in the temperature range 5.8–300 K. No anomalies in the C p(T) dependence were observed. Thermodynamic functions were calculated. At 298.15 K, the values of entropy and enthalpy are equal to 243.1 J K−1 mol−1 and 36360 J mol−1, respectively. The heat capacity of methacetin in the temperature range 6–10 K is well fitted by Debye equation C p = AT 3. The thermodynamic data obtained for methacetin are compared with those for the monoclinic and orthorhombic polymorphs of paracetamol.
