Chloroform liquid temperature range

One incinerator that has been evaluated rather extensively and for which test results have been reported is the liquid chemical waste incinerator facility owned by the Metropolitan Sewer District (MSD) of Greater Cincinnati, Ohio (1 ). The MSD facility uses a rotary kiln and liquid injection cyclone furnace to incinerate a wide variety of liquid industrial chemical wastes. The total design heat release rate is 120 million kJ/h (114 million Btu/h). Tests conducted over a wide temperature range ( 900°C to 1300°C) for six Appendix VIII chemicals (carbon tetrachloride, chloroform, hexachlorobenzene, hexachlorocyclo-pentadiene, and hexachloroethane) have shown DREs equal to or very near 99.99%. 

One of the most classic examples of chiral expression in thermotropic liquid crystals is that of the stereospecific formation of helical fibres by di-astereomers of tartaric acid derivatised either with uracil or 2,6-diacylamino pyridine (Fig. 9) [88]. Upon mixing the complementary components, which are not liquid crystals in their pure state, mesophases form which exist over very broad temperature ranges, whose magnitude depend on whether the tartaric acid core is either d, l or meso [89]. Electron microscopy studies of samples deposited from chloroform solutions showed that aggregates formed by combination of the meso compounds gave no discernable texture, while those formed by combinations of the d or l components produced fibres of a determined handedness [90]. The observation of these fibres and their dimensions makes it possible that the structural hypothesis drawn schematically in Fig. 9 is valid. This example shows elegantly the transfer of chirality from the molecular to the supramolecular level in the nanometer to micrometer regime. 

Huggins, Pimentel, and Shoolery measured NMR shifts of chloroform in acetone and in triethylamine (982). This study furnishes corroborative evidence that the chloroform-base interaction can be classified as a H bond. More important, however, it serves as a prototype of the use of NMR chemical shifts in the study of complex formation. Huggins et al, based their analysis on an expression analogous to equation (7). They show that two data—the experimental values of 5 in pure chloroform and at infinite dilution, combined with the equilibrium constant for association—permit csdculation of the entire concentration dependence of 5. This implies that the measurement of 5 over the range from pure liquid to infinite dilution gives an estimate of the equilibrium constant. Of course the temperature dependence of the constant gives the heat of association. The appropriate equations are given in reference 982 where they are used to obtain K and A// for the association of chloroform with the bases acetone and triethylamine. 

Ge(CH3)4 is a colorless liquid at room temperature and has a sweetish odor somewhat resembling that of chloroform [1]. Experimental values of the density in the 0 to 25 C range [20, 28, 39, 48] are represented graphically in Fig. 1. The data can be expressed by the equations... 

Several polymer systems have been successfully analysed by equation (2) and meaningful rate and energetic parameters determined (from the temperature dependence). Liquid-induced crystallization, with acetone and chloroform, of polycarbonate s develops as spherulites for which n = 3.0 over the temperature of crystallization range 561—586 K. Cellulosealso crystallizes from solution but with a rod-like morphology, for which = 1.0 these differences may reflect differences in chain flexibility. 

There are numerous examples of polar liquids at room temperature at least which exhibit Debye or nearly so behavior (in the sense of conformity to equation (35) over most of the frequency range of dispersion. Only a few of these are mentioned here others can be found for example in Bottcher-Bordewijk (48) and in the tables compiled by Buckley and Maryott (49). This is true of substituted methanes (50) (including methanol ) such as chloroform CHCl with = 5.7ps at 25 C. Even for these and other simple molecules there are small residual effects as indicated schematically in Figure 3(a). These seen as millimeter far infrared absorption are a resultant of inertial effects and Foley absorption variously attributed to librations coupling to translational modes and the subject of ot er contributions to these proceedings. 

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