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Oct 1979

Volume 8, Issue 4, pp. 923-1298


Evaluated activity and osmotic coefficients for aqueous solutions: iron chloride and the bi‐univalent compounds of nickel and cobalt

R. N. Goldberg, R. L. Nuttall, and B. R. Staples

J. Phys. Chem. Ref. Data 8, 923 (1979); http://dx.doi.org/10.1063/1.555615 (82 pages)

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A critical evaluation of the mean activity and osmotic coefficients in aqueous solutions of iron chloride, nickel chloride, perchlorate, and nitrate and twenty‐nine bi‐univalent compounds of cobalt at 298.15 K is presented. Osmotic coefficients were calculated from direct vapor pressure measurements, from isopiestic measurements, from freezing point depression measurements, and from vapor pressure osmometry measurements. Given are empirical coefficients for three different correlating equations, obtained by a weighted least squares fit of the experimental data, and tables consisting of the activity coefficients of the compounds, the osmotic coefficients and activity of water, and the excess Gibbs energy of the solution as functions of the molality for each electrolyte system. The literature coverage is through the computerized version of Chemical Abstracts of April 1979.
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82.60.Lf Thermodynamics of solutions
82.60.Hc Chemical equilibria and equilibrium constants

Evaluated activity and osmotic coefficients for aqueous solutions: bi‐univalent compounds of lead, copper, manganese, and uranium

R. N. Goldberg

J. Phys. Chem. Ref. Data 8, 1005 (1979); http://dx.doi.org/10.1063/1.555611 (46 pages)

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A critical evaluation of the mean activity and osmotic coefficients in aqueous solutions of twelve bi‐univalent compounds of lead, copper, manganese and uranium at 298.15 K is presented. Osmotic coefficients were calculated from direct vapor pressure measurements, from isopiestic measurements and and from freezing point depression measurements. Activity coefficients were calculated from electromotive force measurements on galvanic cells without transference. Given are empirical coefficients for three different correlating equations, obtained by a weighted least squares fit of the experimental data, and tables consisting of the activity coefficients of the compounds, the osmotic coefficients and activity of water, and the excess Gibbs energy of the solution as functions of the molality for each electrolyte system. The literature coverage is through the computerized version of Chemical Abstracts of April 1979.
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82.60.Lf Thermodynamics of solutions
82.60.Hc Chemical equilibria and equilibrium constants

Microwave spectra of molecules of astrophysical interest. XVIII. Dimethyl ether

F. J. Lovus, H. Lutz, and H. Dreizler

J. Phys. Chem. Ref. Data 8, 1051 (1979); http://dx.doi.org/10.1063/1.555612 (58 pages) | Cited 4 times

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The microwave spectra of dimethyl ether (methoxymethane) is critically reviewed and supplemented through calculations which include the contributions of internal rotation and centrifugal distortion in the molecular Hamiltonian. The primary objective of this review is to provide microwave spectral transitions applicable to molecular radio astronomy for the ground vibrational state rotational spectrum of the most abundant isotopic form of dimethyl ether, 12CH316O12CH3. While all measured rotational transitions are included, the predicted transition frequencies were limited to J?15 in the range 1 GHz to 300 GHz. In order to provide a complete summary of the laboratory studies on dimethyl ether, the rotational constants of the less abundant isotopic species and excited torsional states are also tabulated and all reported rotational studies are referenced.
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33.20.Bx Radio-frequency and microwave spectra
33.15.Mt Rotation, vibration, and vibration-rotation constants
98.38.Bn Atomic, molecular, chemical, and grain processes
98.38.Er Interstellar masers
98.58.Bz Atomic, molecular, chemical, and grain processes
98.58.Ec Interstellar masers

Energy levels of potassium, K I through K XIX

Charles Corliss and Jack Sugar

J. Phys. Chem. Ref. Data 8, 1109 (1979); http://dx.doi.org/10.1063/1.555613 (38 pages) | Cited 7 times

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Data on the energy levels of the potassium atom in all of its stages of ionization, as derived from the analyses of atomic spectra, have been critically compiled. In cases where only line classifications are reported in the literature, level values have been derived. Electron configurations, term designations, J‐values, experimental g‐values, and ionization energies are included.
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32.30.Jc Visible and ultraviolet spectra
32.10.Hq Ionization potentials, electron affinities

Electrical resistivity of copper, gold, palladium, and silver

R. A. Matula

J. Phys. Chem. Ref. Data 8, 1147 (1979); http://dx.doi.org/10.1063/1.555614 (152 pages) | Cited 18 times

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In this work, recommended values for the electrical resistivity as a function of temperature from the cryogenic region to well beyond the melting point are given for bulk pure copper, gold, palladium, and silver. In addition to the total electrical resistivity values for the solid state, intrinsic electrical resistivity values are presented from cryogenic temperatures to the melting point. The values are corrected for the change in geometry due to thermal expansion. The recommendations are based on theoretical considerations and on the experimental data found in the open literature. That available experimental data together with information pertaining to the specimen characterization and measurement conditions are included in this work. The methods of data evaluation and other considerations used in arriving at the recommendations are described. For the solid state, an interpolation scheme is given to aid in the determination of values between those supplied in the tables; for the liquid state, equations are given.
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72.15.Eb Electrical and thermal conduction in crystalline metals and alloys
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