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.

it's all four options.

b. accuracy of the data matters alot more than its number of digits, organization or amount of detail. quantitative observation is more accepted than the qualitative observation.