Abstract
Fission of U(233) leads to produce number of fission products and among them Sr is one of the high yield fission product which form stable fluoride, SrF2. High temperature interaction of SrF2 and UF4 leads to formation of single ternary compound, SrUF6(s). The Gibbs energy formation of SrUF6(s) has been experimentally measured using two different calcium fluoride solid electrolyte Galvanic cell setup with common sample electrode and different reference electrode:Cell 1: (−)Pt, U3O8(s) + UO2F2(s) + SrUF6(s) + SrF2(s) = CaF2(s) = NiO(s) + NiF2(s), Pt (+)Cell 2: (−)Pt, SrO(s) + SrF2(s) = CaF2(s) = U3O8(s) + UO2F2(s) + SrUF6(s) + SraF2(s), Pt (+)Heat capacity and enthalpy increment has been experimentally measured with Differential Scanning Calorimeter and high temperature Calvet type drop calorimeter, respectively. The pseudo-binary phase diagram of SrF2-UF4 system was calculated by minimization of Gibbs energies of the phases present in the system. Before phase diagram calculation the experimental thermodynamic data were optimized. The stability domain of SrUF6(s) has been calculated from the chemical potential diagram of Sr–U–F–O system at 873 K as oxygen is present as an impurity in molten fluoride salts. The isothermal ternary phase diagram of Sr–U–F2 system has also been calculated in order to determine the coexisting phases of SrUF6(s) at 873 K.
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