Equilibria in some secondary alcohol + hydrogen + ketone systems

Abstract

Equilibrium constants Kp for the systems containing propan-2-01 + propan-2-one, butan-2-01 + butan-2-one and pentm-3-01+ pentan-3-one were derived from measurements of the composition of mixtures obtained when the vapours were passed with hydrogen over a catalyst held at a measured temperature. Equations expressing the free-energy, enthalpy and entropy changes for the reactions over a range of temperature have been derived from observations by the use of published heatcapacity data. The results are compared with such published thermodynamic data as exist.Thermodynamic quantities for the ideal gas now recorded and not previously measured include the standard entropies of butan-2-01 (85.69 cal deg-1. mole-1) and pentan-3-01 (91.35 cal deg-1. mole-1) and the standard heat of formation of pentan-3-01 (-75.38 kcal mole-1).

Ideal gas thermodynamic properties of propanone and 2-butanone

“…67. 68, 69] and chemical equilibrium studies [41,43,45,66] as -57.02 ± 0.20kcal mol-I, which is in consistency with the value given in [83]. The reported enthalpies of reactions (AHrO) by ip-vestigators and the derived enthalpies of formation (flHr) for 2~butanone [56], the limiting values of (aCp/aPh at zero pressure at the above four temperatures were calculated.…”

Selective hydrodeoxygenation of bio-oil derived products: ketones to olefins

“…3. It can be seen that for both metals, acetone conversion increased with temperature until the thermodynamic limitation [59][60][61] is reached for the reaction conditions used in this study. The maximum conversion was obtained at 448 K for nickel and 473 K for copper.…”

Structure-reactivity relationships in the photoreduction of n,π*-excited ketones and azoalkanes: the effect of reaction thermodynamics, excited-state electrophilicity, and antibonding character in the transition state

“…(1) by using the known α C-H bond dissociation energy of propan-2-ol (∆H 1 = D 298 (C-H) = 374 kJ mol Ϫ1 ) 40 and its heat of formation (∆ f H 298 = Ϫ273 kJ mol Ϫ1 ). 41 The O-H bond dissociation energy for the ketyl radical (∆H 2 ) can then be determined according to eqn. (2) as ∆H 2 = D 298 (O-H) = 116 kJ mol Ϫ1 by using the reported ∆ f H 298 value of Ϫ219 kJ mol Ϫ1 for acetone.…”