Heat capacities of aqueous solutions of nickelous chloride and nickel chloride-sodium chloride (NiCl2.2NaCl) from 0.12 to 3.0 mol kg-1 and 321 to 572 K at a pressure of 17.7 MPa

Abstract

parallels the Increase of the relative oxygen content of the ether molecules. We note that, in general, the excess enthalpy of cyclic ether + cyclohexene Is distinctly smaller than that of the corresponding system cyclic ether + cyclohexane (2, 24, 25)\ at x = 0.5, these Increments vary between ca. -400 and -700

Heat capacity of aqueous magnesium chloride from 349 to 598 K

“…The Cp¿ s presented in this paper, together with experimental standard Gibbs free energies and enthalpies at 298.15 K, allow calculations of the thermodynamic properties of MgCI2(aq) at temperatures to 600 K. Calculation of standard Gibbs free energies by this route allows the calculation of equilibrium constants for chemical reactions involving MgCI2(aq) under these conditions. The details of the calculations have been reported elsewhere (27,28).…”

Thermodynamic Properties of Aqueous HClO4 to 373 K and at Low Pressure: A Comprehensive Pitzer Ion-Interaction Model

“…The only values of (KClO 4 ) at T > 298 K are those from Mastroiani and Criss, which are based on andtheir enthalpy of solution measurements for NaClO 4 (solid). The only other non-actinide or -lanthanide chloride−perchlorate pairs for which relevant heat capacity data exist are those for Ni[ClO 4 ] 2 (aq) 37 and NiCl 2 (aq). − At other than 298 K the measurements for the latter two systems were made at substantially different pressures and thus were not used.…”

“…The only other non-actinide or -lanthanide chlorideperchlorate pairs for which relevant heat capacity data exist are those for Ni[ClO 4 ] 2 (aq) 37 and NiCl 2 (aq). [38][39][40] At other than 298 K the measurements for the latter two systems were made at substantially different pressures and thus were not used.…”

A new version of differential flow heat capacity calorimeter; tests of heat loss corrections and heat capacities of aqueous NaCl from T= 300 K to T= 623 K

“…The Berkeley calorimeter produced a limited number of data for Na 2 SO 4 (aq) (3) and MgSO 4 (aq) (5) at temperatures up to 473 K and for KCl(aq) (6) up to 573 K. The Delaware calorimeter was twice reconstructed (7,8) and has been continuously improved while yielding an important quantity of data for aqueous solutions over a period of 15 years. A series of measurements was performed in the 1980s for aqueous 1-1 and 2-1 electrolytes (LiCl, NaCl, KCl, NaBr, CaCl 2 , MgCl 2 , FeCl 2 , and NiCl 2 at temperatures typically between 300 K and 623 K (4,(9)(10)(11)(12)(13)(14)(15)(16) ) followed in the 1990s by investigations of solutions of HCl, NH 4 Cl, H 3 PO 4 , and SO 2 in the same temperature range, reported by Sharygin and collaborators. (17)(18)(19) A group of thirteen organic electrolytes and nonelectrolytes of different molecular structures was studied to T = 525 K by Inglese et al (20)(21)(22) The most important results from Delaware were, however, those obtained at T > 623 K, through the critical region of water, where the apparent molar heat capacity of a dilute solution exhibits a typical "S" like behaviour switching between deeply negative and highly positive values, or vice versa.…”