Abstract
The activation energy for thermal dehydroxylation in vacuum of alkaline-earth hydroxides has been calculated from thermogravimetric data. The experimental results of Mg(OH)2 Ca(OH)2 and Sr(OH)2 are in agreement with an unimolecular decay law and their activation energies are similar to the values of enthalpies of decomposition. In contrast, as the dehydroxylation process of Ba(OH)2 takes place in liquid phase and the BaO does not dissolve into the molten Ba(OH)2, a kinetic of zero order describes the reaction rate and the activation energy is lower than the enthalpy of decomposition.
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