Calorimetric studies and thermodynamic properties of liquid Ag–Ca alloys

Dębski, A.; Gąsior, W.

doi:10.1016/j.jct.2014.05.021

Cited by 4 publications

(4 citation statements)

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“…references Table 5. Calculated formation enthalpy of the CaLi 2 phase compared with the experimental data [1,5].…”

Section: Discussionmentioning

confidence: 99%

“…Dedicated to the memory of Professor Dragana Živković calibration coefficient with the increasing amount of melt were considered in the calculations. The voltage signal from the thermopile was registered in a digital form and next the heat effects and the enthalpies were calculated according to the procedure presented in [5].…”

Section: J Min Metall Sect B-metall 53 (3) B (2017) 203 -208mentioning

confidence: 99%

“…3, in a comparison with the experimental data from this study. The calculated enthalpy of formation of CaLi 2 phase in comparison with experimental data [1,5] is shown in table 5.…”

Section: The Calculation Of the Phase Diagram (Calphad)mentioning

confidence: 99%

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Calorimetric measurements of the Ca-Li liquid alloys

Dębski

Garzeł

Zakulski

et al. 2017

J min metall B Metall

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An isothermal high-temperature mixing calorimeter was used for the determination of the enthalpy of mixing Δ mix H for liquid Ca-Li solutions, for 63 alloys of different compositions at the four following temperatures: 588 K, 648 K, 820 K and 1159 K. The studies were performed by way of dropping solid metal samples at ambient temperature into liquid alloys, starting from pure elements. In three series, calcium was dropped into liquid lithium, whereas solid Li samples were added into liquid Ca in the fourth series. Because of the high reactivity of the alloy components, all the steps of the experiment were conducted in a high purity argon atmosphere. It was found that the Ca-Li system is characterized by small negative Δ mix H values and its minimal value is lower than-1.5 kJ/mol. Additionally, the differential thermal analysis was used to determine the phase transformation temperature for 11 Ca-Li alloys. Finally, the Calphad method was used to assess the phase diagram, applying the data of these studies as well as all the experimental results available in the literature.

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“…references Table 5. Calculated formation enthalpy of the CaLi 2 phase compared with the experimental data [1,5].…”

Section: Discussionmentioning

confidence: 99%

Section: J Min Metall Sect B-metall 53 (3) B (2017) 203 -208mentioning

confidence: 99%

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Calorimetric measurements of the Ca-Li liquid alloys

Dębski

Garzeł

Zakulski

et al. 2017

J min metall B Metall

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“…When we calculate the enthalpy differential for the components of a mixture, as a solution or an alloy [7], variations in the thermodynamic property are expressed by mol in the mixture; however in the case of a mixture as that described in this work which determines the change in the experimental enthalpy for the mixture of carbonaceous solids, water, and ion Ni(II), the contribution cannot be calculated by mol but per gram of each system component.…”

Section: Differential Enthalpy Of the Mixture Componentsmentioning

confidence: 99%

Enthalpic Contribution of Ni(II) in the Interaction between Carbonaceous Material and Aqueous Solution

Giraldo

Moreno–Piraján

2017

Journal of Chemistry

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Solid adsorbents were prepared from corn cob that was modified with a solution of HNO 3 6 M at different contact times. The solids are characterized by physical N 2 adsorption at 77 K to know their surface area by applying the BET model and surface chemistry is determined using the Bohem method. Once we have prepared the adsorbents we determine the immersion enthalpy, Δ im , of the solids in Ni(II) aqueous solutions of different concentrations between 20 and 800 mg⋅L −1 , with values for Δ im between 10.0 and 35.3 J⋅g −1 . From the results obtained for the immersion enthalpy in function of the ion Ni(II) concentration we calculate the contribution to the immersion enthalpy that corresponds to the ion when it is treated with the system adsorbent-solution as a mixture in which the solid, the solvent, and the adsorbate are involved. The solution thermodynamics allows for establishing the enthalpic changes that bring the ion in function of the concentration and the intensity of the interaction of solid-metal ion that is favored by the presence of acid groups in the solid.

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