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Evaluation of reaction spontaneity for acidic and reductive dissolutions of corrosion metal oxides using HyBRID chemical decontamination

  • Byung-Chul LeeEmail author
  • Seon-Byeong Kim
  • Jei-Kwon Moon
  • Sang-Yoon Park
Article
  • 6 Downloads

Abstract

Complete sets of reaction mechanisms are proposed in the acidic and reductive dissolution of magnetite, nickel ferrite, and chromite using the HyBRID (Hydrazine Based Reductive metal Ion Decontamination) process for the decontamination of a primary coolant system of nuclear power plant. Hydrazine participated in the reaction pathway of reducing ferric ions to ferrous ions and simultaneously regenerating oxidized cupric ions into cuprous ions. The data of the heat capacity, the heat of formation, the entropy of formation, and the Gibbs energy of formation for all chemical species and ions were collected from the HSC Chemistry 9 database. The enthalpy, entropy, and Gibbs energy changes of reactions were calculated in the temperature range of 298.15–373.15 K for individual reactions. The degree of spontaneity decreased with the increase of the temperature. The reaction spontaneity was significantly enhanced by addition of hydrazine and slightly increased by further addition of copper sulfate.

Keywords

HyBRID decontamination Reductive dissolution Corrosion metal oxides Equilibrium constant Reaction spontaneity 

Notes

Acknowledgements

This work has been carried out under the Nuclear R&D Program (NRF-2018M2A8 A5024102 and NRF-2017M2A8A5015144) funded by Ministry of Science and ICT, South Korea.

References

  1. 1.
    Moon JK, Kim SB, Choi WK, Choi BS, Chung DY, Seo BK (2019) The status and prospect of decommissioning technology development at KAERI. J Nucl Fuel Cycle Waste Technol 17(2):139–165CrossRefGoogle Scholar
  2. 2.
    Technical Report Series No.395 (1999) State of the art technology for decontamination and dismantling of nuclear facilities. IAEA, ViennaGoogle Scholar
  3. 3.
    Technical Report Series No. 386 (1998) Decommissioning of nuclear facilities other than reactors. IAEA, ViennaGoogle Scholar
  4. 4.
    Won HJ, Lee WS, Jung CH, Park SY, Choi WK, Moon JK (2014) A feasibility study on the decontamination of type 304 stainless steel by N2H4 base solution. Asian J Chem 26(5):1327–1330CrossRefGoogle Scholar
  5. 5.
    Jung JY, Park SY, Won HJ, Kim SB, Choi WK, Moon JK, Park SJ (2015) Corrosion properties of inconel-600 and 304 stainless steel in new oxidative and reductive decontamination reagent. Met Mater Int 21(4):678–685CrossRefGoogle Scholar
  6. 6.
    Choi WK (2017) Development of advanced decontamination technology for nuclear facilities. KAERI Report No. 2012M2A8A5025655, Daejeon, KoreaGoogle Scholar
  7. 7.
    Choi WK, Won HJ, Park SY, Kim SB, Jung JY, Moon JK (2015) Chemical decommissioning of a primary coolant system using hydrazine-based solutions. In: Proceedings of waste management conference, 15–19 March 2015, Phoenix, Arizona, USA, paper no 15215Google Scholar
  8. 8.
    Won HJ, Lee WS, Jung CH, Park SY, Choi WK, Moon JK (2013) Dissolution of Fe3O4 by the N2H4 base solution. In: Proceedings of 7th international conference on multi-functional materials and applications, 22–23 November 2013, Huainan, ChinaGoogle Scholar
  9. 9.
    Kim SB, Park SY, Choi WK, Won HJ, Park JS, Seo BK (2018) Magnetite dissolution by copper catalyzed reductive decontamination. J Nucl Fuel Cycle Waste Technol 16(4):421–429CrossRefGoogle Scholar
  10. 10.
    White AF, Peterson ML, Hochella MF Jr (1994) Electrochemistry and dissolution kinetics of magnetite and ilmenite. Geochim Cosmochim Acta 58(8):1859–1875CrossRefGoogle Scholar
  11. 11.
    Brown DB, Donner JA, Hall JW, Wilson SR, Wilson RB, Hodgson DJ, Hatfield WE (1979) Interaction of hydrazine with copper(I1) chloride in acidic solutions: formation, spectral and magnetic properties, and structures of copper(II), copper(I), and mixed-valence species. Inorg Chem 18(10):2635–2641CrossRefGoogle Scholar
  12. 12.
    Heaton BT, Jacob C, Page P (1996) Transition metal complexes containing hydrazine and substituted hydrazines. Coordin Chem Rev 154:193–229CrossRefGoogle Scholar
  13. 13.
    Srivastava AK, Varshvey AL, Jain PC (1980) Complexes of copper(II) with substituted hydrazines. J Inorg Nucl Chem 42:47–50CrossRefGoogle Scholar
  14. 14.
    Outotec HSC Chemistry software. www.outotec.com
  15. 15.
    Bard AJ, Parsons R, Jordan J (1985) Standard potentials in aqueous solution. IUPAC, CRC Press, Boca RatonGoogle Scholar
  16. 16.
    Rumble JR (ed) (2018) CRC handbook of chemistry and physics, 99th edn. CRC Press, Boca RatonGoogle Scholar
  17. 17.
    Zemaitis JF Jr, Clark DM, Rafal M, Scrivner NC (1986) Handbook of aqueous electrolyte thermodynamics: theory and application. AIChE DIPPR, Wiley, New YorkCrossRefGoogle Scholar
  18. 18.
    Dean JA (1999) Lange’s handbook of chemistry, 15th edn. McGraw-Hill, New YorkGoogle Scholar
  19. 19.
    Puigdomenech I, Taxén C (2000) Thermodynamic data for copper, implications for the corrosion under repository conditions. Tech. Report TR-00-13, SKBGoogle Scholar
  20. 20.
    Barin I, Knacke O, Kubaschewski O (1973, supplement 1977) Thermodynamic properties of inorganic substances. Springer, BerlinGoogle Scholar
  21. 21.
    Wagman DD, Evans WH, Parker VB, Schumm RH, Halow I, Bailey SM, Churney KL, Nuttall RL (1982) The NBS tables of chemical thermodynamic properties, selected values for inorganic and C1 and C2 organic substances in SI units. J Phys Chem Ref Data 11: Suppl No 2Google Scholar

Copyright information

© Akadémiai Kiadó, Budapest, Hungary 2019

Authors and Affiliations

  • Byung-Chul Lee
    • 1
    Email author
  • Seon-Byeong Kim
    • 2
  • Jei-Kwon Moon
    • 2
  • Sang-Yoon Park
    • 2
  1. 1.Department of Advanced Materials and Chemical EngineeringHannam UniversityDaejeonSouth Korea
  2. 2.Decommissioning Technology Research DivisionKorea Atomic Energy Research InstituteDaejeonSouth Korea

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