By G. R. Kinney (auth.), K. D. Timmerhaus (eds.)
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NI and N 2 are the actual mol fractions of the solvent and solute. E V is the energy required for infinite separation per unit volume. and so is a measure of the internal pressure. H is the heat of vaporization at the temperature for which the computation is made. E 1/2 (- ) V 1 • has been term~d the solubility parameter by Hildebrand. who introduced this relationship. It is related to an earlier treatment of the van der Waals equation by van Laar. thus is the volume fraction of the solvent. 10 J .
When the solubility of the hydrocarbon in liquid oxygen is low, Hildebrand's equation appears to predict the right order of magnitude, as illustrated by the solubility of acetylene and carbon dioxide in liquid oxygen. Even for n-hexane, in spite of extensive extrapolation in obtaining internal energy and molal volume data in order to compute the N values from equation (3), the computed and experimental solubilities are not far apart, considering the huge correction necessary for the difference in heat capacity between the liquid and solid nhexane extrapolated to low temperatures.
A detonation shown inFigure 6 is considered to be a visible flash or audible report or both. Odor of burning is sometimes used as an indication of detonation. Doubtful tests are repeated. In the course of testing several facts have been discovered about the specimens size and form. 5 cc. Specimens outside of this range give results, but those within the range give reliable reproducible results. Flat thin specimens are not as sensitive to impact as the same material in a lump specimen of the same volume.
Advances in Cryogenic Engineering: Proceedings of the 1958 Cryogenic Engineering Conference by G. R. Kinney (auth.), K. D. Timmerhaus (eds.)