A general-purpose reaction-solution rotating-bomb calorimeter for measurements up to about 400 K and 800 kPa

Olofsson, Gerd; Sunner, Stig; Efimov, M.E.; Laynez, José

doi:10.1016/s0021-9614(73)80079-5

Cited by 24 publications

(4 citation statements)

References 5 publications

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“…For determination of H m,2 ∞ values at various temperatures, the apparent molar enthalpies given by Kilday 28 can also be used. In addition to wide heat-of-solution data reported in her study at 298.15 K (see Figure 1A), she also determined one ΔH app value ∞ at various temperatures, was also based here on the apparent molar enthalpies determined by Olofsson et al 50 for the KCl solution where the molality of KCl was 0.123 mol•kg −1 . This group reports the enthalpy values of this solution at 298.…”

Section: Of Ref 20 Together With the Values Of H M2mentioning

confidence: 85%

“…This means, for example, in the determination of H m,2 ∞ for 298.54 K, the PI parameters for 298.15 K in Table were used. The determination of H m,2 ∞ at various temperatures, was also based here on the apparent molar enthalpies determined by Olofsson et al for the KCl solution where the molality of KCl was 0.123 mol·kg –1 . This group reports the enthalpy values of this solution at 298.15, 313.15, 328.15, 333.15, and 360.15 K. We determined using parametrization PI from these enthalpies the H m,2 ∞ values that are presented in Table .…”

Section: Resultsmentioning

confidence: 99%

“…Partial Molar Enthalpies of Potassium Chloride (Symbol 2) at Infinite Dilution Obtained Using Parameterization PI from the KCl Data of Kilday,28 Vasilj'ev and Lobanov,49 and Olofsson et al50 …”

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Thermodynamically Traceable Calorimetric Results for Dilute Aqueous Potassium Chloride Solutions at Temperatures from (273.15 to 373.15) K. Part 1. The Quantities Associated with the Partial Molar Enthalpy

Partanen

Partanen²,

Vahteristo

2019

J. Chem. Eng. Data

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In our previous study (Partanen, J. I.; Partanen, L. J.; Vahteristo, K. P., J. Chem. Eng. Data 2019, 64, 16–33), we presented a fully traceable two-parameter Hückel equation with parameters B and b 1 for activity and osmotic coefficients in dilute KCl(aq) in the temperature range of (273.15 to 383.15) K. This equation applies within experimental error to almost all thermodynamic data in the literature at least up to a molality of 0.2 mol·kg–1. In our Hückel model, parameter B is treated as a constant, whereas parameter b 1 depends quadratically on the temperature. In the present study, the same model is applied to the molar enthalpies of the components in KCl solutions. No new parameter estimations are necessary for the treatment of these calorimetric data. We also extend now the previous enthalpy results for dilute NaCl solutions (see Partanen, J. I.; Partanen, L. J.; Vahteristo, K. P., J. Chem. Eng. Data 2017, 62, 2717–2632) up to 373 K because in that study the treatment of calorimetric data was limited only up to 353 K. In a future publication (Part 2 of this study), it will be shown that this Hückel model applies additionally well to the heat-capacity literature available for dilute KCl solutions. Here, we also consider a second parametrization of the Hückel equation for KCl solutions obtained in a previous work (Partanen, J. I., J. Chem. Eng. Data 2016, 59, 286–306). This is seen to apply better to enthalpy data in less dilute KCl solutions up to the saturated solutions in the range of (298 to 303) K. However, the alternative parametrization is not fully traceable and not as accurate as our primary one. Following the success of these Hückel models, we supplement the thermodynamic tables for KCl solutions with the relative apparent and partial molar enthalpies of KCl in these solutions from (273.15 to 373.15) K. We also give here the values of these quantities for NaCl in dilute aqueous NaCl solutions at 373.15 K. We have good reason to believe that the new tables contain the most reliable values available for the enthalpy quantities of dilute NaCl and KCl solutions.

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Section: Of Ref 20 Together With the Values Of H M2mentioning

confidence: 85%

Section: Resultsmentioning

confidence: 99%

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Thermodynamically Traceable Calorimetric Results for Dilute Aqueous Potassium Chloride Solutions at Temperatures from (273.15 to 373.15) K. Part 1. The Quantities Associated with the Partial Molar Enthalpy

Partanen

Partanen²,

Vahteristo

2019

J. Chem. Eng. Data

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“…We have also made calorimetric ineasurements of the enthalpy of oxidation of monomeric Cr3+(aq) with Ce(IV) in 0.5 M HC104 solution as represented by [3] Cr3+(aq) + 3Ce(IV) = Cr(V1) + 3Ce(III)…”

Section: Results and Calculationsmentioning

confidence: 99%

Enthalpies of formation of Cr³⁺(aq) and the inner sphere complexes CrF²⁺(aq), CrCl²⁺(aq), CrBr²⁺(aq), and CrSO₄⁺(aq)

Dellien¹,

Hepler²

1976

Can. J. Chem.

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INGEMAR DELLIEN and LOREN G. HEPLER. Can. J. Chem. 54, 1383Chem. 54, (1976. We have carried out calorimetric measurements leading to AHfO = -60 kcal mol-1 for Cr3+(aq). Further calorimetric measurements have led to enthalpies of reaction of Cr3+(aq) with HF(aq), C1-(aq), Br-(aq), and SO4'-(aq) to form the 'inner sphere' complexes CrF2+(aq), CrCI2+(aq), CrBr2+(aq), and CrS04+(aq). values ranging from -5 1 to -62 kcal mol-I for Cr3+(aq). We (2) selected AH; = -57 kcal mol-' for Cr3+(aq) and the corresponding

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Calorimetry as an Analytical Tool in Biochemistry and Biology

Spink

Wadsö

1976

Methods of Biochemical Analysis

136

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A general-purpose reaction-solution rotating-bomb calorimeter for measurements up to about 400 K and 800 kPa

Cited by 24 publications

References 5 publications

Thermodynamically Traceable Calorimetric Results for Dilute Aqueous Potassium Chloride Solutions at Temperatures from (273.15 to 373.15) K. Part 1. The Quantities Associated with the Partial Molar Enthalpy

Thermodynamically Traceable Calorimetric Results for Dilute Aqueous Potassium Chloride Solutions at Temperatures from (273.15 to 373.15) K. Part 1. The Quantities Associated with the Partial Molar Enthalpy

Enthalpies of formation of Cr³⁺(aq) and the inner sphere complexes CrF²⁺(aq), CrCl²⁺(aq), CrBr²⁺(aq), and CrSO₄⁺(aq)

Calorimetry as an Analytical Tool in Biochemistry and Biology

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A general-purpose reaction-solution rotating-bomb calorimeter for measurements up to about 400 K and 800 kPa

Cited by 24 publications

References 5 publications

Thermodynamically Traceable Calorimetric Results for Dilute Aqueous Potassium Chloride Solutions at Temperatures from (273.15 to 373.15) K. Part 1. The Quantities Associated with the Partial Molar Enthalpy

Thermodynamically Traceable Calorimetric Results for Dilute Aqueous Potassium Chloride Solutions at Temperatures from (273.15 to 373.15) K. Part 1. The Quantities Associated with the Partial Molar Enthalpy

Enthalpies of formation of Cr3+(aq) and the inner sphere complexes CrF2+(aq), CrCl2+(aq), CrBr2+(aq), and CrSO4+(aq)

Calorimetry as an Analytical Tool in Biochemistry and Biology

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Enthalpies of formation of Cr³⁺(aq) and the inner sphere complexes CrF²⁺(aq), CrCl²⁺(aq), CrBr²⁺(aq), and CrSO₄⁺(aq)