Oxygen difluoride is an unstable molecule that reacts readily with water. calculate the bond energy of the o–f bond using the standard enthalpy of reaction and the bond energy data provided. just enter a number (no units). of2(g) + h2o(g) \longrightarrow⟶ o=o(g) + 2hf(g) \deltaδh° = –318 kj bond: o–h o=o h–f bond energy (kj/mol): 467 498 565

The bond dissociation enthalpy of O-F bond is 188 kJ/mol.

Explanation:

Total bond energies of the reactant :

Total bond energies of the product:

Standard enthalpy of reaction :

=Total bond energies of the reactants - Total bond energies of the products

The bond dissociation enthalpy of O-F bond is 188 kJ/mol.

in the analysis of systems that involve fluid flow, we frequently encounter the combination of properties u and pv.