Kinetics of the Catalyzed Supercritical Water-Quinoline Reaction. (Reannouncementwith New Availability Information)

摘要

The kinetics of the catalyzed reaction between supercritical water and quinolinewas studied over the temperature range of 400-500 deg C. The reaction rate is first-order with respect to both quinoline and ZnCl2 (catalyst) and inversely proportional to water concentration. These observations are consistent with a Langmuir-Hinshelwood heterogeneous mechanism which involves competitive adsorption on the catalytic surface, with water much more strongly adsorbed. The Arrhenius parameters for the rate constant were an activation energy of 112 kJ/mol and preexponential factor of 1.7 x 105 mol/ (L-g-s). This activation energy is well below the C-C and C-N bond energies in aromatic heterocycles.