A reaction that produces heat for welding and incendiary bombs is the thermite reaction: iron (III) oxide...

Question

A reaction that produces heat for welding and incendiary bombs is the thermite reaction: iron (III) oxide reacts with aluminum to produce aluminum oxide and iron. How many grams of iron (III) oxide can be converted to aluminum oxide by the reaction of 47.1 g of aluminum?

SnapAndSolve AI · Accepted Answer

To solve this stoichiometry problem, we need to use the balanced chemical equation for the thermite reaction:

Fe₂O₃ + 2Al → 2Fe + Al₂O₃

Calculate the molar mass of aluminum (Al):
Al = 26.98 g/mol
Calculate the moles of aluminum:
Moles of Al = 47.1 g / 26.98 g/mol = 1.746 moles
Use the stoichiometry of the reaction to find moles of iron (III) oxide (Fe₂O₃):
According to the balanced equation, 2 moles of Al react with 1 mole of Fe₂O₃.
Moles of Fe₂O₃ = 1.746 moles Al × (1 mole Fe₂O₃ / 2 moles Al) = 0.873 moles Fe₂O₃
Calculate the molar mass of iron (III) oxide (Fe₂O₃):
Fe₂O₃ = (2 × 55.85) + (3 × 16.00) = 159.7 g/mol
Calculate the grams of iron (III) oxide:
Grams of Fe₂O₃ = 0.873 moles × 159.7 g/mol = 139.4 g

Therefore, 139.4 grams of iron (III) oxide can be converted to aluminum oxide by the reaction of 47.1 g of aluminum.

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A reaction that produces heat for welding and incendiary bombs is the thermite reaction: iron (III) oxide...

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