Corrosion Behavior of Nickel‐Iron Alloys in Molten Carbonate

Abstract

Cyclic voltammetry experiments show that the corrosion behavior of binary nickel‐iron alloys shows a gradual change from iron‐like behavior to nickel‐like behavior. The behavior of the 50 and 75% iron alloy is similar to the behavior of pure iron, the behavior of the 10% iron alloy is similar to the behavior of pure nickel, but during a cathodic scan, some significant differences can be observed. At an iron content of approximately 25%, characteristics of iron‐rich and nickel‐rich behavior could be observed. At cathodic potentials of −1500 mV carbonate decomposition and, when scanning anodically, carbon reoxidation (−1500 mV) proceeds faster on the iron‐rich alloys than on nickel‐rich alloys. The first oxidation reaction of the metal is the oxidation of iron: a cubic solid solution of FeO and is formed. This reaction is followed by the oxidation of FeO to . At a more anodic potential a cubic solid solution of and NiO (ca. −700 mV) and (ca. −500 mV in cyclic voltammograms) are formed. On the surface of the 25, 50, and 75% iron alloys a dual layer is present on the surface. The outer layer is , the inner layer is a cubic solid solution of NiO and . On the 10% iron alloy two oxide layers are present: both cubic solid solutions of and NiO, with small amounts of . At very anodic potentials is formed. This compound is formed slowly on the iron‐rich alloys and its formation cannot be observed in a cyclic voltammogram. The corrosion products identified are roughly in agreement with the thermodynamic equilibrium diagram of Yokokawa et al. The first reduction reaction that proceeds is the reduction of trivalent nickel ions in the scale. This reaction is followed by the reduction of . In a later stage the NiO in the cubic solid solution is reduced. At potentials of approximately −1300 mV in the cubic solid solution also is reduced. At more cathodic potentials (until approximately −1500 mV) the reduction of bivalent and trivalent iron ions in the oxide proceeds until contact loss between the metal and the oxide occurs. Then, probably dissolved , and are reduced to the metallic state.