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Solid iron can be observed at environmental conditions and also as metallic component of quasicrystalline alloys. Its behavior in aqueous solution is analyzed from some particular thermochemical relationships. The model utilizes free Gibbs energy to obtain pH and pe parameters which are related to iron redox reactions. The solid iron system, defined as Fe (s) : Fe 2+ - Fe 3+ - Fe 2 O 3 (hematite) – Fe 3 O 4 (magnetite), was modelled by considering a low molar concentration and environmental temperature. In order to obtain pe values, equations relating Gibbs standard free energy and equilibrium constants were applied. A stability diagram such as pe x pH was chosen to depict these thermochemical relationships. Thus, straight line dpe/dpH slopes were obtained for each process step of the solid iron system. In systems relating solid iron to iron species Fe 2+ and Fe 3+ the slopes are equal to zero; i.e. horizontal line shows the iron species dominance in some specific pH (hydronium ions) range. The negative values obtained show the pH dependence of the iron species investigated. In natural water environment, it is possible to distinguish hematite formation from magnetite formation. However in quasicrystalline AlCuFe alloys the last iron species formed is hematite which ion pairs to copper. Due to the strong hydronium ions (pH) dependence, it is necessary to measure it both in environmental conditions and quasicrystalline phase’s formation. Considering that the temperature adopted was 25°C, the results are valid only for this temperature.

THERMODYNAMIC STUDY OF IRON IN ALLOYS OF QUASICRYSTALLINE AlCuFe