Question

The overall reaction in a commercial heat pack can be represented as

4 Fe(s) + 3O₂(g) + 2FeO₃(s) AH = -1652 kJ

a. How much heat is released when 4.40 moles of iron are reacted with excess O₂?

Answer 1

When 4.40 moles of iron react with excess oxygen in a heat pack reaction, 1817.2 kJ of heat is released.

Step-by-step explanation:

The student is asking about the amount of heat released when 4.40 moles of iron react with excess oxygen according to the given thermochemical equation for a heat pack reaction.

The thermochemical equation provided is:
4 Fe(s) + 3O₂(g) → 2Fe₂O₃(s) ΔH = -1652 kJ

To find the amount of heat released, we need to determine the heat released per mole of iron and use that to calculate the total heat for 4.40 moles.

It is given that the total ΔH for 4 moles of Fe is -1652 kJ, so the ΔH per mole of Fe is -1652 kJ / 4 moles = -413 kJ/mol. Then, for 4.40 moles of iron, the heat released is: 4.40 moles × (-413 kJ/mol) = -1817.2 kJ.

Therefore, when 4.40 moles of iron are reacted with excess oxygen, 1817.2 kJ of heat is released.