A new calculation method was presented using surface area data for the thermal analysis of adsorbents. Five parts from a silica gel (Hypersil) were heated at the temperatures of 500, 640, 700, 770, and 850 °C, respectively, for 16 h. The maximum adsorption capacity as liquid nitrogen volume (0.930 cm3 g−1), monolayer capacity (0.093 cm3 g−1), surface area (AH = 245 m2 g−1), number of monolayer (10) in the multimolecular adsorption, and heat of the first layer (3300 J mol−1) were evaluated from the nitrogen adsorption data obtained at − 196 °C. Surface area (A) of the preheated samples was determined similarly. The assumed parameters $$k = - (\partial A/\partial T)_{\text{p}} / A$$ and $$K = \left( {1 - a} \right)/ a$$ were calculated for each preheating temperature, where $$a = A/A_{\text{H}}$$ is the relative decrease in the surface area by the thermal deactivation, because the k and K supplying Arrhenius equations and van’t Hoff equation behave as reaction rate constant and equilibrium constant, respectively. The activation energy for the thermal deactivation of the silica gel was calculated as $$E^{\# } = 27330$$ J mol−1 from the slope of a straight line which is plotted according to the Arrhenius equation. The enthalpy change $$(\Delta H^{0} = 28936$$ J mol−1) and entropy change ( $$\Delta S^{0} = 47.42$$ J mol−1 K−1) for the same case were, respectively, evaluated from the slope and intercept of a straight line which is plotted according to the van’t Hoff equation. Accordingly, temperature dependence of the Gibbs energy is written as $$\Delta G^{0} = \Delta H^{0} - T\Delta S^{0} = 28936 - 47.42 T$$ by the SI units. The spontaneous nature of the deactivation was discussed using the last relationship.
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