Abstract:The energy of reaction of liquid trinitrofluoromethane with diethyl oxalate as fuel was determined in a rotating bomb calorimeter. The standard heat of formation, which is -51.99 ± 0.48 kcál. per mole (±0.48 is estimated standard deviation of the mean), at °C. was calculated using a computer program which has been developed for compounds containing C, H, O, N( F, Cl, Br). The effect of temperature on density, vapor pressure, and surface tension of the compound was determined for a given temperature range. The … Show more
“…For comparison purposes, some properties of the halogen compounds of the trinitromethane series as determined in this laboratory are listed in Table III. "Through oversight densities of trinitrofluoromethane are reported incorrectly in (11). The first digits (.7 and .6) in the density series should read 5 and 4-i.e., 1.595 instead of 1.795; 1.489 instead of 1.689.…”
“…For comparison purposes, some properties of the halogen compounds of the trinitromethane series as determined in this laboratory are listed in Table III. "Through oversight densities of trinitrofluoromethane are reported incorrectly in (11). The first digits (.7 and .6) in the density series should read 5 and 4-i.e., 1.595 instead of 1.795; 1.489 instead of 1.689.…”
“…per mole and the dissociation energy values reported by Wilkins (10) were used in the calculations. The value for C-F was calculated from the measured heat of formation of fluorotrinitromethane (12) assuming that the C-F bond in the two molecules, fluorotrinitromethane and FDE, are the same. The calculated heat of formation of TDP is -59.37 kcal.…”
Section: Resultsmentioning
confidence: 99%
“…The average deviations from the mean in these measurements were 0.044 and 0.095% for TDP and FDE, respectively. The procedure was essentially the same as that reported previously (12).…”
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