The reaction that occurs in heat packs that are used to treat
sports injuries is:
4Fe(s) + 3O2(g) Ò
2Fe2O3(s) ΔH = -1652
kJ
How much heat is released when 1.0 gram of Fe(s) is reacted with
excess O2(g)?
Not sure how to solve this. The more thorough the better.
The balanced chemical reaction taking place is
The enthalpoy change for the reaction is
.
The sign of enthalpy change indicates that heat is being released.
Molar mass of Fe = 55.85 g/mol.
As evident by the balanced reaction, when 4 moles of Fe is completely reacting with O2, the amount of heat released is 1652 kJ.
Mass of 4 moles of Fe =
Since 223.4 g of Fe produces 1652 kJ of heat.
Heat released by 1 g of Fe is
Hence, the heat released by 1 g of Fe when reacting with excess O2 is 7.394 kJ.
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