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21 August, 15:07

Dry chemical hand warmers utilize the oxidation of iron to form iron oxide according to the following reaction: 4Fe (s) + 3O2 (g) →2Fe2O3 (s) Standard thermodynamic quantities for selected substances at 25 ∘C Reactant or product ΔH∘f (kJ/mol) Fe (s) 0.0 O2 (g) 0.0 Fe2O3 (s) - 824.2 Calculate ΔH∘rxn for this reaction.

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  1. 21 August, 18:43
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    -1648.4 kJ/mol

    Explanation:

    Based on Hess's law:

    ΔHr = ∑n*ΔH°f (products) - ∑n*ΔH°f (reactants)

    In the reaction:

    4Fe (s) + 3O₂ (g) → 2Fe₂O₃ (s)

    ΔHr = 2 ΔH°f {Fe₂O₃} - (4ΔH°f {Fe (s) } + 3ΔH°f{O₂ (g) }

    As:

    ΔH°f {Fe₂O₃} = - 824.2kJ/mol

    ΔH°f {Fe (s) } = 0.0kJ/mol

    ΔH°f{O₂ (g) } = 0.0kJ/mol.

    Thus,

    ΔHr = 2 ₓ - 824.2kJ/mol =

    -1648.4 kJ/mol
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