Find `DeltaH` of the following reaction:
`OF_(2)(g) +H_(2)O(g) rarr O_(2)(g)+2HF (g)`, average bond energies of `O -F, O-H, O =O`, and `H - F` are `44,111, 118`, and `135 kcal mol^(-1)`, respectively.

Explanation

To find the change in enthalpy (ΔH) for the reaction:

\[ \text{OF}_2(g) + \text{H}_2\text{O}(g) \rightarrow \text{O}_2(g) + 2\text{HF}(g) \]

we will use the average bond energies provided for the bonds involved in the reaction. The bond energies given are:
- O-F: 44 kcal/mol
- O-H: 111 kcal/mol
- O=O: 118 kcal/mol
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