The unbalanced equation is Fe2O3 + H2 = Fe + H2O.
What mass of hyrdogen gas, H2 must be consumed to produce 10.0 g of iron metal??
Also
What mass of Fe2O3 must be consumed to prepare 2.5 g of iron metal
Iron (III) oxide Fe2O3 reacts with hydrogen gas H2 at elevated temperatures to produce iron metal and water.?
2016-06-09 6:10 pm
回答 (1)
2016-06-09 6:31 pm
From Wikipedia :
Molar mass of H₂ = 1.008 × 2 g/mol = 2.016 g/mol
Molar mass of Fe = 55.845 g/mol
Molar mass of Fe₂O₃ = 159.69 g/mol
The balanced equation :
Fe₂O₃ + 3H₂ → 2Fe + 3H₂O
When 10.0 g of Fe is produced :
[(10 g Fe) / (55.845 g Fe / 1 mol Fe)] × (3 mol H₂ / 2 mol Fe) × (2.016 g H₂ / 1 mol H₂) = 0.541 g H₂
Mass of H₂ consumed = 0.541 g
When 2.5 g of Fe is prepared :
[(2.5 g Fe) / (55.845 g Fe / 1 mol Fe)] × (1 mol Fe₂O₃ / 2 mol Fe) × (159.69 g Fe₂O₃ / 1 mol) = 3.57 g Fe₂O₃
Mass of Fe₂O₃ consumed = 3.57 g
Molar mass of H₂ = 1.008 × 2 g/mol = 2.016 g/mol
Molar mass of Fe = 55.845 g/mol
Molar mass of Fe₂O₃ = 159.69 g/mol
The balanced equation :
Fe₂O₃ + 3H₂ → 2Fe + 3H₂O
When 10.0 g of Fe is produced :
[(10 g Fe) / (55.845 g Fe / 1 mol Fe)] × (3 mol H₂ / 2 mol Fe) × (2.016 g H₂ / 1 mol H₂) = 0.541 g H₂
Mass of H₂ consumed = 0.541 g
When 2.5 g of Fe is prepared :
[(2.5 g Fe) / (55.845 g Fe / 1 mol Fe)] × (1 mol Fe₂O₃ / 2 mol Fe) × (159.69 g Fe₂O₃ / 1 mol) = 3.57 g Fe₂O₃
Mass of Fe₂O₃ consumed = 3.57 g
收錄日期: 2021-04-18 14:59:04
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