How many moles of water are produced when 40 g of pure hydrazine is ignited in the presence of 62 g of pure oxygen?
2016-05-23 3:28 pm
How many moles of water are produced when 40 g of pure hydrazine is ignited in the presence of 62 g of pure oxygen? Answer in units of mol. N2H4(l) + O2(g) → N2(g) + 2 H2O(g) .
回答 (1)
2016-05-23 3:59 pm
Molar mass of N₂H₄ = 14.01×2 + 1.008×4 = 32.05 g/mol
Molar mass of O₂ = 16.00×2 = 32.00 g/mol
N₂H₄(l) + O₂(g) → N₂(g) + 2H₂O(g)
Initial number of moles of N₂H₄ = 40/32.05 = 1.25 mol
Initial number of moles of O₂ = 62/32.00 = 1.94 mol > 1.25 mol
As Mole ratio N₂H₄ : O₂ = 1 : 1, O₂ is in excess, and N₂H₄ is the limiting reactant (completely reacts).
Mole ratio N₂H₄ : H₂O = 1 : 2
Number of moles of N₂H₄ reacted = 1.25 mol
Number of moles of H₂O produced = (1.25 mol) × 2 = 2.5 mol
Molar mass of O₂ = 16.00×2 = 32.00 g/mol
N₂H₄(l) + O₂(g) → N₂(g) + 2H₂O(g)
Initial number of moles of N₂H₄ = 40/32.05 = 1.25 mol
Initial number of moles of O₂ = 62/32.00 = 1.94 mol > 1.25 mol
As Mole ratio N₂H₄ : O₂ = 1 : 1, O₂ is in excess, and N₂H₄ is the limiting reactant (completely reacts).
Mole ratio N₂H₄ : H₂O = 1 : 2
Number of moles of N₂H₄ reacted = 1.25 mol
Number of moles of H₂O produced = (1.25 mol) × 2 = 2.5 mol
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