pep asked in Science & MathematicsChemistry · 4 weeks ago

How much energy is evolved during the reaction of 57.3 g of Al, according to the reaction below? Assume that there is excess Fe2O3.?

How much energy is evolved during the reaction of 57.3 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

1 Answer

Relevance
  • 4 weeks ago

    Fe₂O₃(s) + 2 Al(s) → Al₂O₃(s) + 2 Fe(s) …… ΔH°rxn = -852 kJ

    When 2 moles of Al reacts, 852 kJ of energy is evolved.

    Molar mass of Al = 26.98 g/mol

    No. of moles of Al reacts = (57.3 g) × (1 mol / 26.98 g) = 2.124 mol

    Heat evolved = (852 kJ) × (2.124/2) = 905 kJ

    =====

    OR:

    (57.3 g Al) × (1 mol Al / 26.98 g Al) × (852 kJ heat evolved / 2 mol Al)

    = 905 kJ heat evolved

Still have questions? Get your answers by asking now.