THERMODYNAMIC PARAMETERS OF IRON-CYANIDE ADSORPTION ONTO GAMMA-AL2O3

In this study, we describe the adsorption of ferricyanide (Fe(CN)(6)(3 -)) on gamma-Al2O3 by a modified Langmuir adsorption isotherm. The mod ified Langmuir isotherm developed herein can accurately predict the ap parent equilibrium constant (K-app) at different pH values and tempera tures. In the experimental pH range of 5-6.5, adsorption capacity and apparent equilibrium constants decrease as the temperature increases. Because surface protonation increases as pH decrease, a more positivel y charged site on the surface increases the attraction force that exis ts between gamma-Al2O3 and the adsorbate. According to the Gibbs-Hehmh oltz equation, these apparent equilibrium constants at various tempera tures and pH conditions can be applied to determine enthalpy changes ( Delta H-0) for the adsorption at different pH conditions. The result i ndicates that enthalpy change at different pH values is near -5 kcal/m ol which indicates that the enthalpy change is in the order of hydroge n bonding and confirms the exothermic nature of the adsorption process . The results also indicate that other thermodynamic parameters change of ferricyanide adsorption. The positive entropy change (Delta S-0) h as been explained from the viewpoint of exchange reaction in this stud y. The negative free energy change (Delta G(ads)(0)) for ferricyanide adsorption shows the spontaneous nature of the adsorption process. (C) 1997 Academic Press.