Volume 20, Issue 3, May 1991
Index of content:
20(1991); http://dx.doi.org/10.1063/1.555887View Description Hide Description
A substantial data base concerning the rate constants for the gas‐phase reactions of the nitrate (NO3) radical with organic compounds is now available, with rate constants having been determined using both absolute and relative rate methods. To date, the majority of these kinetic date have been obtained at room temperature using relative rate techniques utilizing both the reactions of the NO3 radical with other organic compounds and the equilibrium constant for the NO3+NO2⇄N2O5 reactions as the reference reaction. In this article, the literature kinetic and mechanistic data for the gas‐phase reactions of the NO3 radical with organic compounds (through late 1990) have been tabulated, reviewed and evaluated. While this available data base exhibits generally good agreement and self‐consistency, further absolute rate data are needed, preferably as a function of temperature. Most importantly, mechanistic and product data for the reactions of the NO3 radical with organic compounds need to be obtained.
20(1991); http://dx.doi.org/10.1063/1.555888View Description Hide Description
Equations that described the thermodynamic properties of the NaBr+H2O system were obtained from a fit to experimental results for this system. The experimental results included in the fit spanned the range of temperature of approximately 260 to 623 K and the range of pressure from the vapor pressure of the solution to 150 MPa. New equations and/or values for the following properties are given in the present work: 1) the change in chemical potential with respect to temperature and pressure for NaBr(cr), valid from 200 to 900 K, 2) Δ f G 0 m and Δ f H 0 m for formation from the elements for NaBr(cr) for 298.15 K and 0.1 MPa, 3) Δ f G 0 m and Δ f H 0 m from the elements, as well as S 0 m and C 0 p,m , all for 298.15 K, 0.1 MPa for NaBr⋅2H2O(cr), 4) the change in chemical potential for both NaBr and H2O in NaBr(aq) as a function of temperature, pressure, and molality, valid from 260 to 600 K and from the vapor pressure of the solution to 150 MPa.
Cross Sections and Swarm Coefficients for Nitrogen Ions and Neutrals in N2 and Argon Ions and Neutrals in Ar for Energies from 0.1 eV to 10 keV20(1991); http://dx.doi.org/10.1063/1.555889View Description Hide Description
Graphical and tabulated data and the associated bibliography are presented for cross sections for elastic, excitation, and ionization collisions of N+, N+ 2, N, and N2 with N2 and for Ar+ and Ar with Ar for laboratory energies from 0.1 eV to 10 keV. Where appropriate, drift velocities and reaction or excitation coefficients are calculated from the cross sections and recommended for use in analyses of swarm experiments and electrical discharges. In the case of N+ in N2, cross sections for momentum transfer, charge transfer, electronic excitation, and electron production are recommended. Drift velocity calculations predict runaway for N+ in N2 for electric field to gas density ratios E/n greater than 4.3×103 Td, where 1 Td (townsend)=10− 2 1 V m2. For N+ 2 in N2, the cross sections include those for N+ and N+ 3 formation, electronic excitation, and electron production. Drift velocities and average cross sections are calculated for E/n≥500 Td. In the case of N in N2, only cross sections for momentum transfer are recommended. For N2 in N2, cross sections for momentum transfer, electronic excitation, and electron production are recommended. Collisions of electronically excited states with N2 are not included. For Ar+ in Ar, cross sections for charge transfer, electronic excitation, and electron production are recommended. For Ar in Ar, cross sections for momentum transfer, electronic excitation, and electron production are recommended.
20(1991); http://dx.doi.org/10.1063/1.555905View Description Hide Description
This critical review covers the existing literature on the solubility of CO2 in water from 273 K to the critical temperature of the solvent (647 K). Results of the evaluation are expressed in the form of fitting equations for the infinite dilution Henry’s constant, k 0, as a function of the density of the solvent, and also as an explicit function of the temperature. The pressure effect on the solubility is considered in the formulation. Different equations of state were used for the description of the CO2–H2O vapor phase and the effects on the calculated Henry’s constant values are analyzed. The ‘‘best’’ solubility estimates are presented in smoothed tabular form.