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4] For the following equation determine which reactant is the limiting reactant and which reactant is in excess. The amounts of reagent used are shown. Show calculations to support your choices 3fe + 4h2o Fe3O4 + 4h2 40.0 g 16.0g the limiting reactant is the excess reactant is
Accepted Answer
To determine the limiting reactant, we need to convert the given masses of iron (Fe) and water (H₂O) to moles and compare their mole ratios to the stoichiometric ratio in the balanced equation:
1. Calculate moles of Fe:
- Molar mass of Fe = 55.845 g/mol
- Moles of Fe = 40.0 g / 55.845 g/mol = 0.716 mol
2. Calculate moles of H₂O:
- Molar mass of H₂O = 18.015 g/mol
- Moles of H₂O = 16.0 g / 18.015 g/mol = 0.888 mol
3. Determine the limiting reactant:
- The balanced equation shows that 3 moles of Fe react with 4 moles of H₂O.
- Mole ratio of Fe to H₂O required: 3/4 = 0.75
- Actual mole ratio of Fe to H₂O: 0.716 mol Fe / 0.888 mol H₂O = 0.807
- Since the actual mole ratio (0.807) is greater than the required ratio (0.75), Fe is in excess and H₂O is the limiting reactant.
4. Determine the excess reactant:
- Fe is the excess reactant.
Therefore, the limiting reactant is H₂O and the excess reactant is Fe.
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