The heat, equilibrium, and kinetics of adsorption of 1-ethoxy-2-propanol vapours on granulated activated carbon were determined simultaneously by a reaction calorimeter SETARAM C80 D at T=298.15 K at various relative vapour pressures (0.1< p/ps<0.8). The adsorption isotherm was correlated by the Freundlich equation. It was observed that the enthalpies of adsorption decrease slightly with increasing of the relative vapour pressure of the adsorptive. The rate of adsorption were calculated from analysis of the heat flux signals and it was found that the mass-transfer coefficient for 1-ethoxy-2-propanol vapours in granulated activated carbon increased with increasing relative vapour pressure of the adsorptive.
In this paper, examples are given of how calorimetric values can give greater certainty to phase equilibria calculated from
thermodynamic data. Errors that may arise when phase diagram evaluations are carried out largely from the basis of Gibbs energy
information only are illustrated by reference to recent evaluations of the Ti−Si system and the resulting calculated oxidation
behaviour of titanium silicides. The importance of calorimetric values for calculation of metastable phase equilibria is demonstrated
by results of work on the AlN−TiN hard-metal coating system. Finally, suggestions are made with regard to areas of work where
calorimetric data are urgently needed.
According to thermodynamic theories, the state of alloys can be divided into equilibrium and non-equilibrium. Non-equilibrium alloys generally exhibit some special mechanical and physical properties which are not
coefficients for gaseous products) an important problem is description of thermodynamic conditions under which experiments are carried out. Classic ‘single kinetic triplet’ f(α) or g(α)-E-A applies to thermokinetic conditions, not necessarily equilibrium. In