Hydrazine, n2h4, is used as a rocket fuel. in the reaction below, if 80.1 g of n2h4 and 92.0 g of n2o4 are allowed to react, how many grams of excess reactant remain at the end of the reaction?

Question

Chemistry

Derek Sharp

21 June, 13:30

Hydrazine, n2h4, is used as a rocket fuel. in the reaction below, if 80.1 g of n2h4 and 92.0 g of n2o4 are allowed to react, how many grams of excess reactant remain at the end of the reaction?

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Answers (1)

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Kamila Villa · Answer 1

Answer is: excess of hydrazine is 16 grams.

Chemical reaction: N₂O₄ (l) + 2N₂H₄ (l) → 3N₂ (g) + 4H₂ O (g).

m (N₂H₄) = 80,1 g.

m (N₂O₄) = 92,0 g.

n (N₂H₄) = m (N₂H₄) : M (N₂H₄).

n (N₂H₄) = 80,1 g : 32 g/mol.

n (N₂H₄) = 2,5 mol.

n (N₂O₄) = 92 g : 92 g/mol.

n (N₂O₄) = 1 mol; limiting reactant.

From chemical reaction: n (N₂H₄) : n (N₂O₄) = 2 : 1.

n (N₂H₄) = 2 mol reacts.

Δn (N₂H₄) = 2,5 mol - 2 mol = 0,5 mol.

Δm (N₂H₄) = 0,5 mol · 32 g/mol = 16 g.