Redetermination of the Heat of Combustion of Diphenylmethane

The energetics of the isomeric anthrols

“…However, combining another value of the experimental enthalpy of formation in the liquid phase of diphenylmethane [15] with the vaporization enthalpy for this compound taken from [12] we can obtain another calculated value for the enthalpy of formation in the gas phase of anthrone, 34.6 kJ mol À1 , closer to the experimental value.…”

Energetic effects of ether and ketone functional groups in 9,10-dihydroanthracene compound

“…As reported below, the calculated enthalpy of formation in the gaseous phase by Notario et al and the experimental value derived in the present work for anthrone are in very good agreement with G3(MP2)//B3LYP results after consideration of several working reactions. Therefore, after analysis of the data above, one may also conclude that the enthalpy of formation in the liquid phase of diphenylmethane due to Parks and Mosley [42] seems to be more accurate than that determined by Steele et al [43], both values considered in the computational work of Notario and collaborators [10]. …”

The standard enthalpies of formation of 2-methylbiphenyl and diphenylmethane,

“…Concurrently, Parks et al (10) reported D c H°m(l, 298.15 K) = −(6921.4 2 2.8) kJ·mol −1 . In 1950 Parks and Mosley (11) noted the ambiguity with respect to the phase of the diphenylmethane in their earlier combustion measurements (10) and reported values for both the crystalline and liquid phases; from three measurements: Parks and Mosley (11) {referring to the material used in the earlier study (reference 10)} noted ''that their material had probably deteriorated with time in the manner described by De Vries and Strow''. De Vries and Strow (31) found that the melting temperature of their samples of diphenylmethane decreased over a period of time.…”

“…Three studies of the energy of combustion of C 6 H 5 ·CH 2 ·C 6 H 5 are reported in the literature. (10,11,30) In the discussion which follows all values reported in each of the earlier thermochemical studies have been converted to modern units. In 1946 Coops et al (30) reported D c H°m(cr, 298.15 K) = −(6929.5 2 0.8) kJ·mol −1 .…”

“…On reading the early literature on the measurement of the energy of combustion of diphenylmethane, (10,11) it was noted that a problem arose as to the state (solid or liquid) of the sample within the bomb calorimeter under 3.04 MPa pressure of oxygen at T=296 K or 297 K. In order to circumvent such a problem in the study reported here, it was decided to increase the laboratory temperature, endure the uncomfortable conditions, and burn the diphenylmethane sample at T=303 K.…”