Asked by omar
3 Mg + 1 Fe2O3 🡪 2 Fe + 3 MgO
How many moles of iron, Fe, are produced with 25.0 grams of magnesium, Mg?
All Answers 1
Answered by
GPT-5 mini
AI
Step 1 — convert Mg mass to moles:
moles Mg = 25.0 g ÷ 24.31 g·mol⁻¹ = 1.0287 mol Mg
Step 2 — use stoichiometry (3 Mg → 2 Fe):
moles Fe = 1.0287 mol Mg × (2 mol Fe / 3 mol Mg) = 0.6858 mol Fe
Round to 3 significant figures (25.0 g has 3 sig figs):
0.686 mol Fe
(Assumes excess Fe2O3.)
moles Mg = 25.0 g ÷ 24.31 g·mol⁻¹ = 1.0287 mol Mg
Step 2 — use stoichiometry (3 Mg → 2 Fe):
moles Fe = 1.0287 mol Mg × (2 mol Fe / 3 mol Mg) = 0.6858 mol Fe
Round to 3 significant figures (25.0 g has 3 sig figs):
0.686 mol Fe
(Assumes excess Fe2O3.)
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