Calculate heat of the following reaction at constant pressure,
`F_(2)O(g)+H_(2)O(g)rarrO_(2)(g)+2HF(g)`
The heats of formation of `F_(2)O(g),H_(2)O(g)` and `HF(g)` are `5.5 kcal-57kcal` and `-64 kcal` repectively.

Explanation

To calculate the heat of the reaction at constant pressure for the given reaction:

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

we will use the heats of formation provided for each compound involved in the reaction. The formula to calculate the change in enthalpy (\(\Delta H\)) for the reaction is:

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