Problem: Dry chemical hand warmers utilize the oxidation of iron to form iron oxide according to the following reaction:4 Fe(s) + 3 O2(g) → 2 Fe2O3(s)Standard thermodynamic quantities for selected substances at 25oC Reactant or productΔH°f (kJ/mol)Fe(s)0.0O2(g)0.0Fe2O3(s)-824.2Calculate ΔH°rxn for this reaction and calculate how much heat is produced from a hand warmer containing 15.0 g of iron powder.

FREE Expert Solution

4 Fe(s) + 3 O2(g) → 2 Fe2O3(s)

We can use the following equation to solve for ΔH˚rxn:

ΔH°rxn=ΔH°f, prod-ΔH°f, react

ΔH°rxn=(2 mol Fe2O3)-824.2 kJ1 mol Fe2O3-(0+0

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Problem Details

Dry chemical hand warmers utilize the oxidation of iron to form iron oxide according to the following reaction:

4 Fe(s) + 3 O2(g) → 2 Fe2O3(s)

Standard thermodynamic quantities for selected substances at 25o

Reactant or productΔH°f (kJ/mol)
Fe(s)0.0
O2(g)0.0
Fe2O3(s)-824.2




Calculate ΔH°rxn for this reaction and calculate how much heat is produced from a hand warmer containing 15.0 g of iron powder.


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