Add time:08/10/2019         Source:sciencedirect.com

The enthalpy of neutralization of aqueous hydrazine with hydrofluoric acid was determined to be −13.4 kcal mol−1 at 25 °C. The enthalpy of solution ΔHs of hydrazinium monofluoride in water is 0.832 kcal mol−1, whereas ΔHs for hydrazinium difluoride in the same solvent is 9.64 kcal mol−1. To complete the results on hydrazinium halides ΔHs for N2H5I has been determined to be 7.33 kcal mol−1. From these values the standard enthalpies of formation of crystalline N2H5F, N2H6F2, and N2H5I were derived to be −82.1, −167.5, and −23.11 kcal mol−1 respectively. Some experiments were performed in anhydrous hydrazine as solvent and the results obtained were compared with those obtained in aqueous solution. The enthalpy of solvation of N2H5F was found to be some 1 to 2 kcal mol−1 higher in water than in anhydrous hydrazine.

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