Heats of combustion of diamond and of graphite

Some experimental data on the heats of combustion of benzoic acid and carbon (graphite)

“…The value for the heat of combustion of graphite given here is slightly higher than that previously reported, and the data are being used in another report [9], in conjunction with a recalculation of the data previously reported [10,12,13], to obtain a selected "best" value for the heat of formation of carbon dioxide.…”

“…The samples of artificial graphite and Buckingham natural graphite were from the same source as those measured by Jessup [10]. The artificial graphite was of "spectrographic" grade 2 and was reported by the maker (National Carbon Co.) to contain less than 0.001 percent of ash.…”

“…The Buckingham natural graphite was purified by alternate treatments with hydrochloric acid and hydrofluoric acid by H. B. Knowles, of this Bureau. The effect of various purification treatments has been r eported by Jessup [10] .…”

Heat and free energy of formation of carbon dioxide, and of the transition between graphite and diamond

“…However, the experimental data recently obtained in a joint investigation by the Coal Research Laboratory, of the Carnegie Institute of Technology, and the National Bureau of Standards, and reported in the preceding papers by Dewey and Harper [5] and Jessup [6], throw an entirely new light upon the thermochemistry of carbon. These new data make necessary a reselection of the standard state for carbon, and a revision of the present accepted values for the heat and the free energy of formation of carbon dioxide (from oxygen and graphIte or diamond) and of the transition between graphite and diamond.…”

Heats of Formation of Metallic Borides by Fluorine Bomb Calorimetry

“…Although it has been demonstrated [7,8] that graphite can be burned successfully in an oxygen bomb to-give precise data, attempts to determine the heat of formation of carbon tetrafluoride by direct combination of the elements has not been as simple. Von Wartenburg and Schutte [77] calculated the heat of formation of CF4 to be -162 ±2 kcal mole-as a result of the direct combination of the elements.…”