Abstract
The activity of NiO in NiO−MnO solid solutions has been measured using the cell Ni, NiO |Zr0.85 Ca0.15 O1.85|Ni, [NiO]s.s. in the temperature range 900° to 1200°C for compositions between 0 and 80 mol pct NiO. The activity-composition relationships for MnO have been determined by integration of the Gibbs-Duhem equation, and the partial and integral thermodynamic quantities for the system have been calculated. The system exhibits a positive deviation from ideal behavior with a maximum heat of mixing of 850±150 cals per mole, and a positive excess entropy of mixing of 0.24±0.1 cal per mole °C was detected at the equimolar composition.
Similar content being viewed by others
References
W. C. Hahn, Jr. and A. Muan:J. Phys. Chem. Solids, 1961, vol. 19, p. 388.
R. A. Rapp and F. Maak:Acta Met., 1962, vol. 10, p. 63.
C. M. Sellars and F. Maak:Trans. TMS-AIME, 1966, vol. 236, p. 457.
A. Kubik and C. B. Alcock:Met. Sci. J., 1967, vol. 1, p. 19.
H. J. Engel:Z. Phys. Chem. (Frankfurt), 1962, vol. 35, p. 192.
K. Schwerdtfeger and A. Muan:Trans. TMS-AIME, 1967, vol. 239, p. 1114.
I. V. Gordeev, Yu. D. Tret’yakov, and K. G. Komayakov:Vestn. Mosk. Univ., Ser. II, Khim., 1963, vol. 18, p. 59.
S. Seetharaman and K. P. Abraham:Trans. Inst. Min. Met., 1968, vol. C77, p. 209.
L. S. Darken and R. W. Gurry:Physical Chemistry of Metals, McGraw-Hill Book Co., New York, 1953.
L. S. Darken:Trans. TMS-AIME, 1967, vol. 239, p. 80.
W. H. McCoy and W. E. Wallace:J. Am. Chem. Soc., 1956, vol. 78, p. 5995.
W. T. Barrett and W. E. Wallace:J. Am. Chem. Soc., 1954, vol. 76, p. 370.
Author information
Authors and Affiliations
Rights and permissions
About this article
Cite this article
Cameron, D.J., Unger, A.E. The measurement of the thermodynamic properties of NiO−MnO solid solutions by a solid electrolyte cell technique. Metall Trans 1, 2615–2621 (1970). https://doi.org/10.1007/BF03038393
Received:
Issue Date:
DOI: https://doi.org/10.1007/BF03038393