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The heats of the following reactions were measured directly in an electrically calibrated flame calorimeter operated at one atm pressure and 303 °K.    OF  2   (  g  )  +  2   H  2   (  g  )  +  99   H  2   O  (  l  )  →  2   [   HF  ⋅  50   H  2   O   ]   (  l  )F  2   (  g  )  +   H  2   (  g  )  +  100   H  2   O  (  1  )  →  2   [   HF  ⋅  50   H  2   O   ]   (  l  )1  2        O  2   (  g  )  +   H  2   (  g  )  →   H  2   O  (  l  )   The reactants and products were analyzed for each of the reactions. From these heats we calculated the corresponding heats of formation, as follows:    OF  2   (  g  )     Δ   H   f  298.15   °   =  +  24.52  ±  1.59   kJ    mol   -  1(   +  5.86  ±  0.38   kcal     mol    -  1)HF  ⋅  50   H  2   O  (  l  )     Δ   H   f  298.15   °   =  -  320.83  ±  0.38   kJ    mol   -  1(   -  76.68  ±  0.09   kcal     mol    -  1)H  2   O  (  l  )     Δ   H   f  298.15   °   =  -  285.85  ±  0.33   kJ    mol   -  1(   -  68.32  ±  0.08   kcal     mol    -  1)    The uncertainties indicated are the estimates of the overall experimental errors. The value of the average O - F bond energy in OF 2 was calculated to be 191.29 kJ mol -1 (45.72 kcal mol -1 ).

Constant pressure flame calorimetry with fluorine. II. The heat of formation of oxygen difluoride