skip to main content
OSTI.GOV title logo U.S. Department of Energy
Office of Scientific and Technical Information

Title: Alumina solubility in KF-AIF{sub 3}-based low-temperature electrolyte system.

Abstract

No abstract prepared.

Authors:
; ; ;
Publication Date:
Research Org.:
Argonne National Lab. (ANL), Argonne, IL (United States)
Sponsoring Org.:
EE
OSTI Identifier:
915006
Report Number(s):
ANL/ES/CP-59151
TRN: US200817%%57
DOE Contract Number:
DE-AC02-06CH11357
Resource Type:
Conference
Resource Relation:
Conference: TMS 2007 Annual Meeting and Exhibition; Feb 24 - Mar 1, 2007; Orlando, FL
Country of Publication:
United States
Language:
ENGLISH
Subject:
37 INORGANIC, ORGANIC, PHYSICAL AND ANALYTICAL CHEMISTRY; ELECTROLYTES; SOLUBILITY; ALUMINIUM OXIDES; SOLVENT PROPERTIES; POTASSIUM FLUORIDES; ALUMINIUM FLUORIDES

Citation Formats

Yang, J., Graczyk, D. G., Wunsch, C., and Hryn, J. N.. Alumina solubility in KF-AIF{sub 3}-based low-temperature electrolyte system.. United States: N. p., 2007. Web.
Yang, J., Graczyk, D. G., Wunsch, C., & Hryn, J. N.. Alumina solubility in KF-AIF{sub 3}-based low-temperature electrolyte system.. United States.
Yang, J., Graczyk, D. G., Wunsch, C., and Hryn, J. N.. Mon . "Alumina solubility in KF-AIF{sub 3}-based low-temperature electrolyte system.". United States. doi:.
@article{osti_915006,
title = {Alumina solubility in KF-AIF{sub 3}-based low-temperature electrolyte system.},
author = {Yang, J. and Graczyk, D. G. and Wunsch, C. and Hryn, J. N.},
abstractNote = {No abstract prepared.},
doi = {},
journal = {},
number = ,
volume = ,
place = {United States},
year = {Mon Jan 01 00:00:00 EST 2007},
month = {Mon Jan 01 00:00:00 EST 2007}
}

Conference:
Other availability
Please see Document Availability for additional information on obtaining the full-text document. Library patrons may search WorldCat to identify libraries that hold this conference proceeding.

Save / Share:
  • Molten salts in the LiNO/sub 3/-KNO/sub 3/ system can be used in lithium-based electrochemical cells. They are stable in the presence of elemental lithium and high lithium activity alloys due to the formation of a protective lithium oxide solid electrolyte layer. Their thermodynamic properties allow their use with reversible positive electrodes with potentials between 2.5 and 4.3 V with respect to lithium. This paper reports the possibility of reducing the melting point so that such systems by the introduction of a third component. A ternary eutectic has been found in the LiNO/sub 3/-KNO/sub 3/-CsNO/sub 3/ system that melts at 96more » + or - 2/sup 0/C. This composition, 35.2-39.8-25.0 m/o, is also stable in the presence of elemental lithium, indicating the formation of a lithium oxide layer. Experiments will be reported on the electrochemical stability range of this low temperature eutectic composition, as well as on the use of lithium cobalt oxides as reversible positive electrode materials in electrochemical cells employing it as an electrolyte.« less
  • This paper describes the low temperature operation of a solid oxide fuel cell using cubic stabilized zirconia in the ZrO[sub 2]-Sc[sub 2]O[sub 3]-Al[sub 2]O[sub 3] system as an electrolyte. The hydrogen-oxygen fuel cell was fabricated by using La[sub 0.8]Sr[sub 0.2]MnO[sub 3] as the cathode material and Ni-YSZ as the anode material. The maximum power density is 0.63 W/cm[sup 2] at 800 C and 1.0 W/cm[sup 2] at 880 C. The current-voltage performance of this fuel cell suggests that the present electrolyte is a good candidate for fuel cells operating in the temperature range between 800 and 900 C.
  • Oxygen sensors are important for combustion control, in particular, for vehicles. A perovskite-type oxide of LaGaO{sub 3} doped with Sr and Mg exhibits a high oxide ion conductivity over a wide range of oxygen partial pressures. In this study, the application of LaGaO{sub 3}-based oxide as the electrolyte of a potentiometric oxygen sensor was investigated. It became clear that silver is the most effective electrode for decreasing the operating temperature. Although a temperature higher than 800 K is required when a conventional Y{sub 2}O{sub 3}-stabilized ZrO{sub 2} electrolyte is used, an operating temperature as low as 600 K is adequatemore » when La{sub 1{minus}x}Sr{sub x}Ga{sub 0.8}Mg{sub 0.2}O{sub 3} at X = 0.1 and 0.2 is used. The open-circuit potential was slightly smaller than that estimated with the Nernst equation. There was agreement with the Nernst equation down to 673 K when Nd-doped LaGaO{sub 3}-based oxide was used. Moreover, 90% of the response was attained within 15 s at 673 K for the sensor with Nd-doped LaGaO{sub 3}-based oxide.« less
  • The concentrations of the various species present in 0.1, 0.5, and 1.0 M solutions of H/sub 2/SO/sub 4/ and of HNO/sub 3/ saturated with respect to Ag/sub 2/SO/sub 4/ are discussed as a function of temperature. The values of the solubility product, of the enthalpy and entropy of solution, and of the standard partial molal entropy of the solute Ag/sub 2/SO/sub 4/ are given vs. temperature to 200 deg C. (auth)
  • An aqueous thermodynamic model is developed, based on the equations of Pitzer, which accurately model the major binary electrolytes in the Na-NO{sub 3}-NO{sub 2}-SO{sub 4}-CO{sub 3}-F-PO{sub 4}-OH-Al(OH){sub 4}-H{sub 2}O chemical system. This model was developed both from existing data in the literature, and from new osmotic and solubility measurements made as part of this study. Some of the new experimental data developed as part of this study include measurements of osmotic coefficients for NaNO{sub 3}, NaNO{sub 2}, and Na{sub 3}PO{sub 4} at both 50 and 100{degrees}C as well as selected measurements of NaF at 100{degrees}C. In addition, the solubility ofmore » gibbsite was measured in mixed NaOH-NaNO{sub 3} solutions to determine the reliability of existing thermodynamic models of aluminum hydroxide solubility when applied to concentrated nitrate. In general the final model proposed here is valid from dilute solution to salt saturation over the temperature range 25-100{degrees}C. The accuracy of the model is tested by comparisons of the model predictions with experimental data in selected common-ion ternary systems. When necessary a few commonion ternary ion interaction parameters for the Pitzer model were developed.« less