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The overall reaction in a commercial heat pack involves the reaction of 4.00 moles of iron with excess [tex]O_2[/tex]. How much heat is released?

A. Depends on the specific reaction
B. 4.00 kJ
C. 8.00 kJ
D. 16.00 kJ

Answer :

Final answer:

The heat released for the reaction of 4.00 moles of iron with excess oxygen is calculated using the reaction's enthalpy change. Based on the provided reaction (808 kJ/mol for 1 mole of iron), 4.00 moles would release 3232 kJ, which is not indicated in the given options.

Explanation:

The question regarding the amount of heat released when 4.00 moles of iron react with excess oxygen refers to the exothermic reaction used in commercial heat packs. This is a stoichiometry and thermochemistry problem. From the given data, we know that when 1 mole of iron burns, 808 kJ of heat is released. Therefore, we can calculate the heat released for 4.00 moles as follows:

(808 kJ/mol) × (4.00 mol) = 3232 kJ

The correct answer would be that the heat released upon the reaction of 4.00 moles of iron with excess oxygen cannot be the options provided (b) 4.00 kJ, (c) 8.00 kJ, or (d) 16.00 kJ, as they are all too low. The amount of heat released would be significantly higher, based on the reaction provided in the reference information.

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