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9 October, 08:31

How much energy is evolved during the reaction of 48.7 g of Al, according to the reaction below? Assume that there is excess Fe2O3. Fe2O3 (s) + 2 Al (s) → Al2O3 (s) + 2 Fe (s) ΔH°rxn = - 852 kJ

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  1. 9 October, 09:39
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    From the reaction, we see that for every 2 moles of Al reacted, 852 kJ of energy is released. So convert the mass given to moles:

    moles Al = 48.7 g / (26.98 g/mol)

    moles Al = 1.805 mol

    So the energy evolved is:

    Energy = - 852 kJ / 2 mol * 1.805 mol

    Energy = - 769 kJ
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