Consider the following reaction:
3NO2(g) + H2O(l) → HNO3(l) + NO(g)
How many moles of the excess reactant remain if 2.00 moles of H2O(l) and 5.00 moles of NO2(g) are used?
Consider the following reaction: 3NO2(g) + H2O(l) → HN....?
2017-05-09 1:51 pm
回答 (1)
2017-05-09 6:04 pm
3NO₂(g) + H₂O(l) → HNO₃(l) + NO(g)
Mole ratio NO₂ : H₂O = 3 : 1
Initial number of moles of NO₂ = 5.00 mol
Initial number of moles of H₂O = 2.00 mol
When 5.00 mol of NO₂ completely reacts :
Number of moles of H₂O needed = (5.00 mol) × (1/3) = 1.67 mol < 2.00 mol
Hence, H₂O is in excess, and NO₂ completely reacts.
Number of moles of excess H₂O = (2.00 - 1.67) mol = 0.33 mol
Mole ratio NO₂ : H₂O = 3 : 1
Initial number of moles of NO₂ = 5.00 mol
Initial number of moles of H₂O = 2.00 mol
When 5.00 mol of NO₂ completely reacts :
Number of moles of H₂O needed = (5.00 mol) × (1/3) = 1.67 mol < 2.00 mol
Hence, H₂O is in excess, and NO₂ completely reacts.
Number of moles of excess H₂O = (2.00 - 1.67) mol = 0.33 mol
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