Thermodynamic Properties of the NaCl+H2O System l. Thermodynamic Properties of NaCl(cr)

Archer, Donald G.

doi:10.1063/1.555913

Cited by 79 publications

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“…To describe temperature dependence of heat capacity in a wide temperature range (including literature heat capacities obtained using adiabatic calorimetry and data obtained by Quantum Design PPMS), the following equation proposed by Archer [21] was used:…”

Section: Heat Capacity Measurementsmentioning

confidence: 99%

Heat Capacities of l-Arginine, l-Aspartic Acid, l-Glutamic Acid, l-Glutamine, and l-Asparagine

et al. 2021

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In an effort to establish reliable thermodynamic data for amino acids, heat capacity and phase behavior is reported for l-arginine (CAS RN: 74-79-3), l-aspartic acid (CAS RN: 56-84-8), l-glutamic acid (CAS RN: 56-86-0), l-glutamine (CAS RN: 56-85-9), and l-asparagine (CAS RN: 70-47-3). Prior to heat capacities measurement, thermogravimetric analysis was performed to determine decomposition temperatures. Crystal heat capacities of all five amino acids were measured by Tian-Calvet calorimetry in the temperature interval (262-358) K and by power compensation DSC in the temperature interval (215-451) K. Experimental values of this work were combined with the literature data obtained with adiabatic calorimetry. Low temperature heat capacities of l-arginine and l-asparagine, for which no or limited literature data were available, were measured using the relaxation (heat pulse) calorimetry. As a result, reference heat capacities and thermodynamic functions for crystalline phase from near 0 K to 450 K were developed. Keywords Crystalline phase • Heat capacity •This article is part of the Special Issue in Memory of Professor Talgat Khasanshin.

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Section: Heat Capacity Measurementsmentioning

confidence: 99%

Heat Capacities of l-Arginine, l-Aspartic Acid, l-Glutamic Acid, l-Glutamine, and l-Asparagine

et al. 2021

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“…The bulk densities and salinities between 300C and 800C used in the lookup tables come from tables presented by Anderko and Pitzer [1993]. For bulk density values from 0C to 300C, a program developed by Archer [1992] was used to construct the lookup tables. Specific enthalpies between 300C and 800C are calculated using the framework of Tanger and Pitzer [1989].…”

Section: Momentum Conservation Equationmentioning

confidence: 99%

The response of two-phase hydrothermal systems to changing magmatic heat input at mid-ocean ridges

Choi

Lowell

2015

Deep Sea Research Part II: Topical Studies in Oceanography

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Hydrothermal processes at oceanic spreading centers are largely influenced by changing magmatic heat input. I use the NaCl-H 2 O FISHES code to investigate the evolution of surface temperature and salinity as a function of time-varying heat flux at the base of a two-phase, vaporbrine hydrothermal system. I consider a two-dimensional rectangular box that is 1.5 km deep and 4 km long with homogeneous permeability of 10 -13 m 2 . Temperature and pressure at top boundary correspond to seafloor conditions of 10C, 25MPa respectively. Impermeable,

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“…All of the selected enthalpy increments and heat capacities were fitted simultaneously by means of a cubic-spline method described previously. 8 Briefly, a function f(T) was used, where…”

Section: K 2 So 4 (Cr)mentioning

confidence: 99%

Enthalpies of Solution of Sodium Chloride and Potassium Sulfate in Water. Thermodynamic Properties of the Potassium Sulfate + Water System

Archer

Kirklin

2001

J. Chem. Eng. Data

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An adiabatic calorimeter was used to measure enthalpies of solution into water of sodium chloride (∼0.13 mol‚kg -1 ) at nominal temperatures of 298.15 K, 303.15 K, and 308.15 K and of potassium sulfate (∼0.039 mol‚kg -1 ) at nominal temperatures of 298.15 K and 303.15 K. The results for sodium chloride were compared to a previous equation of state so as to validate the use of values from that equation of state for calibration of, or checks on the accuracy of, solution calorimeters. Thermodynamic properties from the literature for the potassium sulfate + water system and the present measurements were used to generate equations that represented the thermodynamic properties of this system from the freezing point of the aqueous solution to 500 K. The measured values included in the fitted equations spanned the range of temperature of approximately 271 K to 530 K for K 2 SO 4 (aq) and 13 K to 854 K for K 2 SO 4 (cr). New equations and/or values for the following properties are given in the present work: (1) thermal properties of K 2 SO 4 (cr) from 0 K to near the orthorhombic to hexagonal transition at 857 K, (2) the change in chemical potential for both K 2 SO 4 and H 2 O in K 2 SO 4 (aq) as a function of temperature and molality, valid from 271 K to 500 K, from 0 mol‚kg -1 to the saturation molality, and to pressures of 40 MPa, and (3) standard-state properties for the aqueous solution process.

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Thermodynamic Properties of the NaCl+H2O System l. Thermodynamic Properties of NaCl(cr)

Cited by 79 publications

References 0 publications

Heat Capacities of l-Arginine, l-Aspartic Acid, l-Glutamic Acid, l-Glutamine, and l-Asparagine

Heat Capacities of l-Arginine, l-Aspartic Acid, l-Glutamic Acid, l-Glutamine, and l-Asparagine

The response of two-phase hydrothermal systems to changing magmatic heat input at mid-ocean ridges

Enthalpies of Solution of Sodium Chloride and Potassium Sulfate in Water. Thermodynamic Properties of the Potassium Sulfate + Water System

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