Interactions between lanthanide cations and nitrate anions in water. Part 1.—Effect of the ionic strength on the Gibbs energy, enthalpy and entropy of complexation of the neodymium cation

1996 ◽  
Vol 92 (24) ◽  
pp. 4957-4963 ◽  
Author(s):  
Christine Bonal ◽  
Jean-Pierre Morel ◽  
Nicole Morel-Desrosiers
Keyword(s):  
Ionic Strength ◽  
Gibbs Energy ◽  
Lanthanide Cations ◽  
Entropy Of Complexation ◽  
Enthalpy And Entropy ◽  
Nitrate Anions

Phosphorylated Calixarenes as Receptors of L-Amino Acids and Dipeptides: Calorimetric Determination of Gibbs Energy, Enthalpy and Entropy of Complexation

2006 ◽  
Vol 18 (3) ◽  
pp. 167-176 ◽  
Author(s):  
Wojciech Zielenkiewicz ◽  
Agniaszka Marcinowicz ◽  
Sergey Cherenok ◽  
Vitaly I. Kalchenko ◽  
Jaroslaw Poznański
Keyword(s):  
Amino Acids ◽  
Gibbs Energy ◽  
Entropy Of Complexation ◽  
Enthalpy And Entropy ◽  
Calorimetric Determination

scholarly journals Temperature dependence of the specific heat and thermodynamic functions AК1М2 alloy, doped strontium

2019 ◽  
Vol 21 (1) ◽  
pp. 35-42 ◽  
Author(s):  
I. N. Ganiev ◽  
S. E. Otajonov ◽  
N. F. Ibrohimov ◽  
M. Mahmudov
Keyword(s):  
Heat Capacity ◽  
Gibbs Energy ◽  
Specific Heat ◽  
Temperature Dependence ◽  
Specific Heat Capacity ◽  
Thermodynamic Functions ◽  
Inverse Relationship ◽  
Alloying Element ◽  
Enthalpy And Entropy ◽  
Increasing Temperature

In the heat «cooling» investigated the temperature dependence of the specific heat capacity and thermodynamic functions doped strontium alloy AK1М2 in the range 298,15—900 K. Mathematical models are obtained that describe the change in these properties of alloys in the temperature range 298.15—900 K, as well as on the concentration of the doping component. It was found that with increasing temperature, specific heat capacity, enthalpy and entropy alloys increase, and the concentration up to 0.5 wt.% of the alloying element decreases. Gibbs energy values have an inverse relationship, i.e., temperature — decreases the content of alloying component — is up to 0.5 wt.% growing.

scholarly journals Solubility of Butylated Hydroxytoluene (BHT) in Aqueous and Alcohol Solutions from 293.15 to 313.15 K

2014 ◽  
Vol 28 ◽  
pp. 48-58 ◽  
Author(s):  
Shipra Baluja ◽  
Kapil Bhesaniya ◽  
Rahul Bhalodia ◽  
Sumitra Chanda
Keyword(s):  
Gibbs Energy ◽  
Thermodynamic Functions ◽  
Butylated Hydroxytoluene ◽  
Solubility Data ◽  
Different Temperatures ◽  
Enthalpy And Entropy

The solubility of Butylated hydroxyl toluene in aqueous and alcohol solutions were determined at different temperatures (293.15 to 313.15) K. Using Van’t Hoff and Gibb’s equations, some thermodynamic functions such as Gibbs energy, enthalpy and entropy of dissolution, and of mixing of Butylated hydroxyl toluene in aqueous and alcohol solutions, were evaluated from solubility data. The solubility was greater in butanol and minimum in water. The enthalpies, entropy and Gibb’s energy of dissolution were positive for all solvents.

scholarly journals Thermodynamic Study of the Solubility of Naproxen in Some 2-Propanol + Water Mixtures

2016 ◽  
Vol 12 (1) ◽  
pp. 48-55 ◽  
Author(s):  
Diego Iván Caviedes Rubio ◽  
Gerson Andrés Rodríguez Rodríguez ◽  
Daniel Ricardo Delgado
Keyword(s):  
Gibbs Energy ◽  
Volume Fraction ◽  
Pure Water ◽  
Water Structure ◽  
Negative Slope ◽  
Driving Mechanism ◽  
Linear Plot ◽  
Enthalpy And Entropy ◽  
The Mean ◽  
Rich Mixtures

The equilibrium solubilities of the anti-inflammatory drug naproxen (NPX) in 2-propanol + water mixtures were determined at several temperatures from 298.15 to 313.15 K. The Gibbs energy, enthalpy, and entropy of solution and of mixing were obtained from these solubility data. The solubility was maximal in φ1 = 0.90 and very low in pure water at all the temperatures studied. A non-linear plot of ∆solnH° vs. ∆solnG° with negative slope from pure water up to 0.20 in volume fraction of 2-propanol and positive beyond this composition up pure 2-propanol was obtained at the mean temperature, 305.55 K. Accordingly, the driving mechanism for NPX solubility in the water-rich mixtures was the entropy, probably due to water-structure loss around non-polar moieties of the drug and for the 2-propanol-rich mixtures it was the enthalpy, probably due to its better solvation of the drug.

Evaluation of Thermodynamic Properties of Cerium in Liquid Cadmium Cathode Within LiCl-KCl Salt System

2016 ◽  
Author(s):  
Dalsung Yoon ◽  
Supathorn Phongikaroon
Keyword(s):  
Thermodynamic Properties ◽  
Gibbs Energy ◽  
Intermetallic Compounds ◽  
Linear Trend ◽  
Open Circuit ◽  
Salt System ◽  
Free Energies ◽  
Enthalpy And Entropy ◽  
Molten Salt System

Thermodynamic properties of Ce-Cd intermetallic compound were investigated in LiCl-KCl-CeCl3-CdCl2 molten salt system at various temperatures. Six Ce-Cd intermetallic compounds, CeCd, CeCd2, CeCd3, Ce13Cd58, CeCd6, and CeCd11 could be observed via cyclic voltammetry (CV) and the relative Gibbs free energies for the intermetallic formations were estimated by the analysis of the anodic peaks in the CV experiments. Furthermore, an open circuit chronopotentiometry which is known as a suitable method for measuring thermodynamic values of intermetallic compounds were performed. The linear trends of the relative Gibbs free energies were found by using potential difference from CV and CP methods. It can be noted that CV method can be easy and fast tool to estimate relative Gibbs energy for intermetallic compounds of Cd-Ms (metals). For the determination of standard Gibbs free energy, enthalpy, and entropy for the intermetallic formation, CP results were used. The linear trend of the Gibbs energy were obtained against temperature changing from 698 K to 823 K. From the linear relationship, the enthalpy and entropy of the formation were calculated.

Solubility of non-polar gases in cyclohexanone between 273.15 and 303.15 K at 101.32 kPa partial pressure of gas

1987 ◽  
Vol 65 (9) ◽  
pp. 2198-2202 ◽  
Author(s):  
María Asunción Gallardo ◽  
José María Melendo ◽  
José Santiago Urieta ◽  
Celso Gutierrez Losa
Keyword(s):  
Gibbs Energy ◽  
Partial Pressure ◽  
Temperature Dependence ◽  
Hard Sphere ◽  
Scaled Particle Theory ◽  
Sphere Diameter ◽  
Particle Theory ◽  
Enthalpy And Entropy

Solubility measurements of several non-polar gases (He, Ne, Ar, Kr, Xe, H2, D2, N2, O2, C2H4, C2H6, CF4, SF6, andCO2) in cyclohexanone at 273.15 to 303.15 K and a partial pressure of gas of 101.32 kPa, are reported. Gibbs energy, enthalpy, and entropy of solution at 298.15 K and 101.32 kPa partial pressure of gas were evaluated. Effective hard-sphere diameter temperature dependence has been studied and its effect on the calculated SPT (Scaled Particle Theory) solubilities, and enthalpies and entropies of solution was also examined.

scholarly journals Effect of alkaline earth metals on the heat capacity and change of thermodynamic function of AK1M2 alloy on the basis of specific aluminum

2020 ◽  
Vol 23 (3) ◽  
pp. 222-228
Author(s):  
I. N. Ganiev ◽  
S. E. Otajonov ◽  
M. Mahmudov ◽  
M. M. Mahmadizida ◽  
V. D. Abulkhaev
Keyword(s):  
Heat Capacity ◽  
Gibbs Energy ◽  
Temperature Dependence ◽  
Alkaline Earth ◽  
Reference Sample ◽  
Alkaline Earth Metals ◽  
Model Alloy ◽  
Cooling Mode ◽  
Cooling Rates ◽  
Enthalpy And Entropy

It is known that high purity aluminum with a minimum content of impurities is widely used in electronic technology for the manufacture of conductive paths in integrated circuits. Hence the development of new compositions of alloys based on such a metal is a very urgent task. One of the promising alloys based on such a metal is alloy AK1M2 (Al + 1 % Si + 2 % Cu). This alloy was accepted by us as a model alloy and subjected to modification by alkaline earth metals.Heat capacity is the most important characteristic of substances and by its variation with temperature one can determine the type of phase transformation, the Debye temperature, the energy of formation of vacancies, the coefficient of electronic heat capacity, and other properties. In the present work, the heat capacity of the AK1M2 alloy with alkaline earth metals was determined in the “cooling” mode from the known heat capacity of a reference sample from copper. For which, by processing the curves of the cooling rate of samples from the alloy AK1M2 with alkaline earth metals and the standard, polynomials were obtained which describe their cooling rates. Further, by experimentally found values of the cooling rates of the standard and samples from alloys, knowing their masses, the polynomials of the temperature dependence of the heat capacity of the alloys and the standard were established, which are described by a four-term equation. Using the integrals of the specific heat, the models of temperature dependence of the change in enthalpy, entropy and Gibbs energy were established.The dependences obtained show that with an increase in temperature, the heat capacity, enthalpy, and entropy of alloys increase, and the values of Gibbs energy decrease. At the same time, additives of alkaline earth metals do not significantly reduce the heat capacity, enthalpy and entropy of the original alloy AK1M2 and increase the value of Gibbs energy. During the transition from alloys with calcium with barium, the heat capacity of the alloys decreases, which correlates with the heat capacity of pure alkaline earth metals within the subgroup.

scholarly journals Thermodynamic study of the solubility of ibuprofen in acetone and dichloromethane

2010 ◽  
Vol 46 (2) ◽  
pp. 227-235 ◽  
Author(s):  
Diana Marcela Aragón ◽  
Jaiver Eduardo Rosas ◽  
Fleming Martínez
Keyword(s):  
Hydrogen Bonds ◽  
Gibbs Energy ◽  
Transfer Process ◽  
Thermodynamic Functions ◽  
Thermodynamic Quantities ◽  
Dipolar Interactions ◽  
Solvent Interactions ◽  
Solution Processes ◽  
Enthalpy And Entropy ◽  
Solvation Processes

Thermodynamic functions, Gibbs energy, enthalpy and entropy for the solution processes of ibuprofen (IBP) in acetone and dichloromethane (DCM) were calculated from solubility values obtained at temperatures ranging from 293.15 K to 313.15 K. The respective thermodynamic functions for mixing and solvation processes as well as the activity coefficients for the solute were calculated. IBP solubility was high and proved similar in both solvents but was greater in DCM than acetone. In addition, the thermodynamic quantities for the transfer process of this drug from cyclohexane to the organic solvents were also calculated in order to estimate the contributions of hydrogen-bonds or of other dipolar interactions. The results were discussed in terms of solute-solvent interactions.

scholarly journals Temperature dependence of the heat capacity and change in the thermodynamic functions of strontium-alloyed AK1M2 alloy

2018 ◽  
Vol 4 (3) ◽  
pp. 119-124
Author(s):  
Izatullo N. Ganiev ◽  
Suhrob E. Otajonov ◽  
Nasim F. Ibrohimov ◽  
M. Mahmudov
Keyword(s):  
Heat Capacity ◽  
Gibbs Energy ◽  
Mathematical Models ◽  
Specific Heat ◽  
Temperature Dependence ◽  
Thermodynamic Functions ◽  
Temperature Decrease ◽  
Cooling Mode ◽  
Enthalpy And Entropy ◽  
Aluminum Base

The temperature dependence of the specific heat capacity and change in the thermodynamic functions of strontium-alloyed ultrahigh-purity aluminum base AK1M2 alloy have been studied in “cooling” mode over the 298.15–900 K range. Mathematical models describing the evolution of these properties of the alloys in the abovementioned temperature range with change in alloying addition concentration have been obtained. The heat capacity, enthalpy and entropy of the alloys increase with temperature, decrease with an increase in the alloying addition concentration to 0.5 wt.% and grow with a further increase in the alloying addition concentration. The Gibbs energy of the alloys has an inverse dependence: it decreases with an increase in temperature and grows with an increase in the alloying addition concentration to 0.5 wt.%.

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