The standard molar enthalpies of combustion and formation of 2-methylbenzothiazole, 2-methylbenzoxazole, and 2-methyl-2-thiazoline

A static-bomb combustion calorimeter and a rotating-bomb combustion calorimeter were used to determine the energies of combustion of 2-methylbenzothiazole, 2-methylbenzoxazole, and 2-methyl-2-thiazoline. The static- and rotating-bomb calorimeters were recently calibrated by the standard benzoic acid combustion runs and they were tested with adequate secondary combustion standards. The rotating-bomb calorimeter was tested using thianthrene and, in the present work, 1,2,4-triazole was used to test the static-bomb calorimeter. From the energies of combustion of the compounds under study, the liquid-phase standard molar enthalpies of formation were derived, at T = 298.15 K, as: (72.5 ± 1.5), (?50.7 ± 2.1), and (?88.5 ± 2.8) kJ mol^?1, respectively.     

Measurement of enthalpies of vaporization of volatile heterocyclic compounds by DSC

An experimental procedure is proposed for direct measurement of the heat involved in the vaporization of volatile heterocyclic compounds. This technique consists on the vaporization of the liquid substance by a sudden decrease of the pressure then, the direct register of heat flow as function of time by differential scanning calorimetry. This procedure allows quantifying the enthalpy of vaporization of compounds such as tetrahydropyran, 2-methoxy-tetrahydropyran, N-morpholine and N-methyl-morpholine. Enthalpies of vaporization were measured in isothermal mode at T=298.15 K and then compared with results from the literature, which currently are obtained by vapour pressure measurements.     

Enthalpies of combustion and formation of 2-acetylpyrrole, 2-acetylfuran and 2-acetylthiophene

The combustion energies for 2-acetylpyrrole (cr) and 2-acetylfuran (cr) were determined using a static bomb calorimeter, whereas the combustion energy of 2-acetylthiophene (l) was determined with a rotating bomb calorimeter; both calorimeters have been recently described. The molar combustion energies obtained were: −(3196.1 ± 0.6) kJ mol⁻¹ for 2-acetylpyrrole, −(2933.8 ± 0.7) kJ mol⁻¹ for 2-acetylfuran, and −(3690.4 ± 0.8) kJ mol⁻¹ for 2-acetylthiophene. From these combustion energy values, the standard molar enthalpies of formation in the condensate phase were obtained as: −(163.51 ± 0.97) kJ mol⁻¹, −(283.50 ± 1.06) kJ mol⁻¹ and −(123.93 ± 1.15) kJ mol⁻¹, respectively. The obtained values of combustion and formation enthalpies of 2-acetylthiophene are in concordance with the reported previously. For the two last compounds, polyethene bags were used as an auxiliary material in the combustion experiments. The heat capacities and purities of the compounds were determined using a differential scanning calorimeter.     

Determination of the energies of combustion and enthalpies of formation of nitrobenzenesulfonamides by rotating-bomb combustion calorimetry

The energies of combustion for 2-nitrobenzenesulfonamide (cr), 3-nitrobenzenesulfonamide (cr), and 4-nitrobenzenesulfonamide (cr) were determined using a recently described rotating-bomb combustion calorimeter. The condensed phase molar energies of combustion obtained were ?(3479.2 ± 1.0) kJ · mol^?1 for 2-nitrobenzenesulfonamide (cr), ?(3454.2 ± 1.1) kJ · mol^-1 for 3-nitrobenzenesulfonamide (cr), and ?(3450.1 ± 1.9) kJ · mol^-1 for 4-nitrobenzenesulfonamide (cr). From these combustion energy values, the standard molar enthalpies of formation in the condensed phase were obtained as: ?(341.3 ± 1.3) kJ · mol^?1, ?(366.3 ± 1.3) kJ · mol^?1, and ?(370.4 ± 2.1) kJ · mol^?1, respectively. Polyethene bags were used as an auxiliary material in the combustion experiments. The heat capacities and purities of the compounds were determined using a differential scanning calorimeter.     

Thermochemical Study of 1-Methylhydantoin

Using static bomb combustion calorimetry, the combustion energy of 1-methylhydantoin was obtained, from which the standard molar enthalpy of formation of the crystalline phase at T = 298.15 K of the compound studied was calculated. Through thermogravimetry, mass loss rates were measured as a function of temperature, from which the enthalpy of vaporization was calculated. Additionally, some properties of fusion were determined by differential scanning calorimetry, such as enthalpy and temperature. Adding the enthalpy of fusion to the enthalpy of vaporization, the enthalpy of sublimation of the compound was obtained at T = 298.15 K. By combining the enthalpy of formation of the compound in crystalline phase with its enthalpy of sublimation, the respective standard molar enthalpy of formation in the gas phase was calculated. On the other hand, the results obtained in the present work were compared with those of other derivatives of hydantoin, with which the effect of the change of some substituents in the base heterocyclic ring was evaluated.     

Enthalpies of formation of primary, secondary, and tertiary amineborane adducts in tetrahydrofuran solution

The enthalpies of solution of primary, secondary, and tertiary amines in THF were determined from calorimetric experiments for five primary, five secondary, and three tertiary amines. The enthalpies of formation of amineborane adducts from borane and the corresponding amines in THF solution were also determined. The differences in adduct formation enthalpies from borane and the corresponding amines can be explained by taking into account steric effects and the chain length of the substituents on the amine. In general, as the alkyl chain length, branching, or the number of chains increases, the formation enthalpy of amineborane adducts is less exothermic. That is to say, the steric effect is more important in tertiary and secondary amines than in primary ones. The enthalpy of solution of linear primary amines in THF was more endothermic as the alkyl chain increased and a similar behavior was observed with linear secondary and tertiary ones. An analysis is made of the amine structural factors which affect the amineborane adduct formation.     

Thermochemistry of amineborane adduct formation of pyridine and picoline isomers

The enthalpy of reaction of pyridine, 2-, 3-, and 4-picoline with BH₃·THF and the enthalpy of solution of the same amines in THF were determined by reaction-solution calorimetry. From these data, the enthalpies of formation of the corresponding amineborane adducts in solution of THF were also determined. The results can be explained by considering the steric and inductive effects of the methyl group on the pyridine ring and the basicity of amines. The enthalpy of formation of the adducts in solution of THF correlates well with the available literature values of pK _a of amines also determined in THF, and the influence of the solvent on the basicity features of studied amines is verified.     

The effect of a double n(O) → π∗(C = O) intramolecular interaction on the stability of 3-nitrophthalic acid

Structural Chemistry - It is not frequent that weak non-covalent interactions counteract moderate hydrogen bonds. And it is also very uncommon to observe two concurrent n → π∗...     

The reaction of biphenyl radical anion and dianion with alkyl fluorides. From ET to SN2 reaction pathways and synthetic applications

The reaction of dilithium biphenyl (Li₂C₁₂H₁₀) with alkyl fluorides has been studied from the point of view of the distribution of products. Two main reaction pathways, the nucleophilic substitution (S_N2) and the electron transfer (ET), can compete to yield the same alkylation products in what is known as the S_N2-ET dichotomy. S_N2 seems to be the main mechanism operating with primary alkyl fluorides (n-RF). Alkylation proceeds in good yields, and the resulting alkylated dihydrobiphenyl anion (n-RC₁₂H₁₀Li) can be trapped with a second conventional electrophile (E⁺) affording synthetically interesting dearomatized biphenyl derivatives (n-RC₁₂H₁₀E). The reaction gives a higher amount of ET products as we move to secondary (s-RF) and to tertiary alkyl fluorides (t-RF), in which case the mechanism seems to be dominated by ET. In this case, alkylation by radical coupling is still feasible, giving access to the synthesis of t-RC₁₂H₁₀E, although in lower yields. A rational interpretation of this S_N2-ET dichotomy is given on the basis of the full distribution of products observed when 5-hexenyl fluoride and 1,1-dimethyl-5-hexenyl fluoride were are used as radical probes in their reaction with Li₂C₁₂H₁₀ and LiC₁₂H₁₀.