Results 211 to 220 of about 46,633 (264)
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Enthalpy of combustion of adenine
The Journal of Chemical Thermodynamics, 1983Abstract The enthalpy of combustion for a commercial adenine sample of 99.9 moles per cent purity was measured in an aneroid adiabatic bomb calorimeter. The molar enthalpy of combustion at 298.15 K for the reaction: C 5 H 5 N 5 ( c )+6.25 O 2 ( g ) = 5 CO 2 (g)+2.5 H 2 O (1)+2.5 N 2 ( g ),
Duane R Kirklin, Eugene S Domalski
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Enthalpy of combustion of purine
The Journal of Chemical Thermodynamics, 1984Abstract The enthalpy of combustion of a commercial purine sample of 99.8 moles per cent purity was measured in an aneroid adiabatic bomb calorimeter. The molar enthalpy of combustion at 298.15 K for the reaction: C 5 H 4 N 4 (cr)+6O 2 (g)=5CO 2 (g)+2H 2 O(1)+2N 2 (g) is Δ c H m o = −(2708.62 ...
Duane R Kirklin, Eugene S Domalski
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Enthalpy of combustion of diphenyl diselenide
The Journal of Chemical Thermodynamics, 1980Abstract The standard enthalpy of the combustion reaction ( C 6 H 5 ) 2 Se 2( c )+16.5 O 2 ( g )+2263 H 2 O(l) =12 CO 2 ( g )+2{ SeO 2 +1134 H 2 O }( l ) has been measured in a rotating-bomb combustion calorimeter to be ΔHco = − (615.3 ± 2.8) kJ mol−1. This leads to a standard
C.T Mortimer, Janette Waterhouse
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Enthalpy of combustion of triphenylarsine oxide
Thermochimica Acta, 1988Abstract The standard enthalpy of combustion of triphenylarsine oxide has been measured by use of a rotating-bomb combustion calorimeter. The enthalpy of formation, Δ H XXX f (Ph 3 AsO, c) = 18.8 ± 3.5 kcal mol − has been calculated, from which the bond dissociation energy D (Ph 3 As O) =102.6 ± 7.3 kcal mol − has been obtained.
D.S. Barnes +2 more
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Enthalpy of combustion of 4-diethylaminonitrosobenzene
The Journal of Chemical Thermodynamics, 1998The enthalpies of combustion and sublimation of 4-diethylaminonitrosobenzene are reported and the thermochemical results show to be consistent with this green compound being monomeric in the solid ...
Maria D.M.C. Ribeiro da Silva +3 more
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Enthalpies of combustion of the three aminophenols
The Journal of Chemical Thermodynamics, 1986Abstract The standard (po = 101.325 kPa) molar enthalpies of combustion in oxygen at 298.15 K were measured by static-bomb calorimetry and the standard molar enthalpies of sublimation at 298.15 K were measured by microcalorimetry for the three aminophenols. −Δ c H m o (cr)/(kJ · mol −1 ) Δ sub H m
L Nuñez +3 more
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Enthalpies of combustion and formation of acetonitrile
The Journal of Chemical Thermodynamics, 1983Abstract The enthalpy of combustion at 298.15 K has been determined and the standard enthalpy of formation for the compound in the liquid state derived as ΔH f o (l) = (40.56±0.40) kJ·mol −1 . The results of recent work on acetonitrile by Barnes and Pilcher are summarized.
Xu-Wu An, Margret Månsson
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Enthalpy of combustion, vapour pressures, and enthalpy of sublimation of 3-nitrophenol
The Journal of Chemical Thermodynamics, 1992Using a static-bomb combustion calorimeter, the standard ( p ° = 0.1 MPa) molar enthalpy of combustion at the temperature 298.15 K of 3-nitrophenol was determined: − Δ c H ° m (cr)/(kJ·mol −1 ) = 2870.0±1.5. The vapour pressure of the crystals was measured, as a function of the temperature T , by the Knudsen-effusion technique and the standard molar ...
Manuel A.V. Ribeiro da Silva +4 more
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Enthalpy of combustion of 1,4-dimethylcubane dicarboxylate
The Journal of Chemical Thermodynamics, 1989Abstract The energy of combustion of crystalline 1,4-dimethylcubane dicarboxylate was measured in the NIST aneroid adiabatic rotating calorimeter. The standard molar enthalpy of combustion at 298.15 K and p rmo = 1 × 10 5 Pa for the reaction: C 12 H 12 O 4 (cr) + 13O 2 (g) = 12CO 2 (g) + 6H 2 O(l) is Δ c H m o = −(6518.09±1.42) kJ·mol −1 .
Duane R. Kirklin +2 more
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Formation Enthalpy of Corannulene: Microbomb Combustion Calorimetry.
Journal of the American Chemical Society, 1995Herein we report our results from microbomb combustion calorimetry on corannulene and the first experimentally-based enthalpy of formation for this key compound. In order to obtain the formation enthalpy in the gaseous state, we must determine the sublimation enthalpy.
Tetsu Kiyobayashi +5 more
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