Apparent molar heat capacities of aqueous NaCl solutions from 0.05 to 3.0 mol·kg−1, 350 to 600 K, and 2 to 18 MPa

The system H2O–NaCl. Part II: Correlations for molar volume, enthalpy, and isobaric heat capacity from 0 to 1000°C, 1 to 5000bar, and 0 to 1 XNaCl

“…At 179 bar (Fig. 12a), the curves are compared to the experimental data of Gates et al (1987). There is generally a good agreement at low temperatures as well as for high temperatures and low to moderate concentrations.…”

“…Here, the most significant difficulty is that experimental enthalpies are mostly heats of dilution, which rather reflect This study Gates et al (1987) This study Bischoff & Rosenbauer (1985) This study White et al (1988) Fig. 13.…”

Standard state thermodynamic properties of aqueous cesium chloride using high dilution calorimetry up to 598.15K

“…The contribution to C p;2 from the molar volume, the third term in equation (20), indicates that a 10% uncertainty at temperature of 598.15 K in this term will introduce an error of less than 2% to the overall value of C p;2 . The standard state Gibbs free energies of solution of cesium chloride are calculated (table 6) from equation (21) together with equation (19), parameter values from table 3, (op/oT) sat from the steam tables [8] and the values of the standard state molar volume of solution, D sol V :…”

“…The standard state partial molar heat capacities of CsCl(aq) at p sat can now be calculated from equation (20) and the parameters from table 3 and are listed in table 5…”

“…in part be the result of extrapolation of their measured osmotic coefficients from the concentrated solutions (m > 0.7) to infinite dilution and that the only thermodynamic data for dilute solution available to them were the enthalpies of dilution of CsCl(aq) from temperatures of (373.15 to 473.15) K [19]. The difficulties involving the extrapolations of various thermodynamic functions from regions outside the validity of a simple limiting law (Debye-Hüc-kel) have been discussed in more detail elsewhere [20]. The C p;2 values from this study are compared with the published results in the literature in table 7, and compare well with those calculated from standard state enthalpy of solution reported by Holmes and Mesmer [18] from temperature of (298.15 to 473.15) K. The standard state partial molar heat capacities for CsCl(aq) from this study are also in good agreement with Saluja et al [21] up to T = 373.15 K.…”