Abstract:The corrosion of molten carbonate fuel cell (MCFC) NiO cathodes during cell operation has ,been brought to attention recently (1-5) and is considered one of the major technical difficulties facing MCFC development at the present time. NiO, solubilized in the molten Li]K carbonate (62/38 mole ratio) at the cathode/carbonate interface, is diffusionally transported through the carbonate reservoir towards the.anode. At some location intermediate between the two electrodes, the local cell environment's oxygen parti… Show more
“…Combining Eq. [4]- [7], the following can be obtained Li/K: log x = y log {Kai~(K)/Kdis(Li)} + log {Kse" Kd~ (K) -1" Pcoz} [8] LENa: log x = y log {Kdi~(Na)/Kdi~(Li)} + log {Ksp" Kdis (Na) -1 9 Pco2} [9] Since K~s and Ksp are constant at a fixed temperature, a linear relationship between log x and y should be obtained at a fixed CO2 pressure if the assumption is correct.…”
Cathode dissolution is a major problem for the development of the molten carbonate fuel cell. In order to evaluate the stability of the cathode, the solubility of
normalNiO
has been measured for several compositions of molten alkaline carbonates in the
CO2
pressure range from 10−5 to 1 atm and the temperature range from 873 to 1023 K. The solubility depended on the
CO2
pressure, although the solubility of
normalNiO
was independent of either
O2
or
H2O
pressure. In any composition of the Li/K and Li/Na carbonate melts, the acid dissolution has been observed at higher
CO2
pressure and the basic dissolution has been observed at low
CO2
pressure.
normalNiO
was found to be more stable in Li rich or Li/Na melts than in the Li/K eutectic melt.
“…Combining Eq. [4]- [7], the following can be obtained Li/K: log x = y log {Kai~(K)/Kdis(Li)} + log {Kse" Kd~ (K) -1" Pcoz} [8] LENa: log x = y log {Kdi~(Na)/Kdi~(Li)} + log {Ksp" Kdis (Na) -1 9 Pco2} [9] Since K~s and Ksp are constant at a fixed temperature, a linear relationship between log x and y should be obtained at a fixed CO2 pressure if the assumption is correct.…”
Cathode dissolution is a major problem for the development of the molten carbonate fuel cell. In order to evaluate the stability of the cathode, the solubility of
normalNiO
has been measured for several compositions of molten alkaline carbonates in the
CO2
pressure range from 10−5 to 1 atm and the temperature range from 873 to 1023 K. The solubility depended on the
CO2
pressure, although the solubility of
normalNiO
was independent of either
O2
or
H2O
pressure. In any composition of the Li/K and Li/Na carbonate melts, the acid dissolution has been observed at higher
CO2
pressure and the basic dissolution has been observed at low
CO2
pressure.
normalNiO
was found to be more stable in Li rich or Li/Na melts than in the Li/K eutectic melt.
“…lution in a mixture of Na2CO3 and K2CO3 may be complicated by the presence of several different dissolution products. If only NiO22 and NiO2'-compounds are considered as dissolution products, the following equations describe the dissolution NiO + Na20 = 2Na + + NiO22- [2] 2NiO + Na20 + 1/2 02 = 2Na § + 2NIO2-…”
Section: Theoretical Backgroundmentioning
confidence: 99%
“…lution in a mixture of Na2CO3 and K2CO3 may be complicated by the presence of several different dissolution products. If only NiO22 and NiO2'-compounds are considered as dissolution products, the following equations describe the dissolution NiO + Na20 = 2Na + + NiO22- [2] 2NiO + Na20 + 1/2 02 = 2Na § + 2NIO2- [3] NiO + K20 = 2K § + NiO22- [4] 2NiO + K20 + 1/2 02 = 2K § + 2NIO2 [5] If the data from dissolution in K2CO3 (1) are considered, reactions involving nickel in a lower oxidation state must be added to this list to explain the dependence of solubility on pO2. With this number of reactions to consider, and little known about the free energies of any of them, the solubilities in mixtures cannot be easily related to those in single salts.…”
The solubility of NiO in mixtures of Li2CO3-K2CO3 and Na2CO~-K2CO3 was measured as a function of the calculated basicity of the solvent mixture and as a function of the temperature. Acid and basic dissolution were found in all mixtures of the Na2CO3-K2CO3 system and in the K2CO3-rich mixtures of the Li2CO3-K2CO3 system. The slopes of the acid solubility lines were markedly different from those in the single salts. The solubilities in mixtures were not quantitatively related in a simple manner to the solubilities in the pure salts of which the mixtures were composed. However, useful qualitative trends may be discerned.Materials degradation owing to corrosion is an important issue for virtually all energy-producing systems, including the advanced molten carbonate fuel cells now under development. Current collectors and other metallic components of the fuel cell may be rapidly degraded at high temperatures if molten salt contacts the surface. This form of attack, known as hot corrosion, is thought to be due to "fluxing," wherein the normally protective oxide scale on an alloy is destroyed by a dissolution reprecipitation process. To help identify hot corrosion mechanisms and to evaluate fluxing quantitatively, data on the chemistry of oxide dissolution are needed.Although the solubility of transition metal oxides in pure molten carbonates has been previously reported (1), in practical terms the solubilities in mixtures are often more important. Baumgartner (2), Kaun (3), and Doyon et al. (4) have reported solubilities of I~iO in mixtures of K2CO3 and Li2CO3. The purpose of the present paper is to investigate the effects of basicity, composition, and temperature on the solubility of NiO in binary mixtures of Na2CO3-K2CO3 and Li2CO~-K2CO3.
Theoretical BackgroundWhen NiO dissolves in a single molten alkali metal carbonate the solubility is a function of the basicity of the solvent. This basicity is determined experimentally by the cation of the melt and the pCO2 in the gas phase above the melt (1). In a mixture of two or more salts the basicity of the melt is function of these same variables but since two or more cations are present the basicity is also a function of the mole fractions of the components. For example, in a binary mixture of Na2CO3 and K2CO~ the basicity will be a function of the pCO2 above the melt and of the mole fractions of Na2CO3 and K2CO3. If the pCO2 is varied for a mixture of fixed composition the basicity is directly proportional to log (pCO2), just as for the single salts. However, when the composition of the solvent is varied at a fixed pCO2, the basicity is a nonlinear function of composition, expressed as activities of the components. This relationship was explored in a Previous paper (5) and is summarized in Fig. 1 and 2 for mixtures of Li2CO3-K2CO3 and Na2CO3-K2CO3. The M20 described in these figures is the neutral counterpart of a common oxide ion activity calculated from the free energies of dissociation of both salts at the indicated pCO3, and the activity of each component in the mixtu...
“…25 In order to develop a better process, we require a basic understanding of the formation mechanism and the nature of thin oxides. Si surface cleaning using wet chemical solutions, such as an RCA clean, are most important.1 Cleaning removes oxides, carbon, or metallic impurities, reduces surface damage or roughness, and forms surfaces for protection from contaminants between processing stages.…”
We studied the uniformity of chemical oxides formed on Si surfaces during wet chemical cleaning. The uniformity was determined by the surface morphology during the initial stage of photoexcited F2 etching. Since photoexcited F2 etches silicon 40 times faster than it etches silicon oxide, it highlights chemical oxides on silicon surfaces making them observable by scanning tunnel microscopy or atomic force microscopy. We found that the chemical oxides were not uniform, whereas oxides formed in gas phase were uniform. Boiling in HC1-H202-H20 (1:1:4 volume) or NH4OH-H202-H20 (1:1.4:4 volume) solutions formed 30 to 70 nm oxide islands. The island density was in the order of iO'° cm2. Boiling in a HNO3 solution also resulted in a chemical oxide which was composed of 25 nm diam dense islands and had pinholes at a density of 5 >< iO cm2. The island density was between 1 X 1011 and 3 X 1011 cm2. The chemical oxide nonuniformities were independent of both crystallographic orientation and substrate resistivity for the most part. It is possible that the nonuniformities may negatively influence subsequent processing. ) unless CC License in place (see abstract). ecsdl.org/site/terms_use address. Redistribution subject to ECS terms of use (see 142.58.129.109 Downloaded on 2015-06-06 to IP
scite is a Brooklyn-based organization that helps researchers better discover and understand research articles through Smart Citations–citations that display the context of the citation and describe whether the article provides supporting or contrasting evidence. scite is used by students and researchers from around the world and is funded in part by the National Science Foundation and the National Institute on Drug Abuse of the National Institutes of Health.