The heat of formation of `Fe_(2)O_(3)(s)` is -824.0 kJ.What will be the `Delta H` for thereaction:
`2Fe_(2)O_(3)(s) to 4Fe(s) + 3O_(2)(g)`

Explanation

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

\[ 2 \text{Fe}_2\text{O}_3(s) \rightarrow 4 \text{Fe}(s) + 3 \text{O}_2(g) \]

we start with the given heat of formation for iron(III) oxide (Fe₂O₃):

1. **Understanding Heat of Formation**: The heat of formation (ΔH_f) of Fe₂O₃(s) is given as -824.0 kJ. This value indicates that when 1 mole of Fe₂O₃ is formed from its elements (iron and oxygen), 824.0 kJ of energy is released.

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