Hydrazine (N2H4), a rocket fuel, reacts with oxygen to form nitrogen gas and water vapor. The reaction is represented with the equation: N2H4 (l) + O2 (

g. → N2 (

g. + 2H2O (

g. If 6 moles of hydrazine react with an excess of oxygen, how many moles of water will be produced?

Question

Wheeler

Chemistry

14 August, 19:44

Hydrazine (N2H4), a rocket fuel, reacts with oxygen to form nitrogen gas and water vapor. The reaction is represented with the equation: N2H4 (l) + O2 (

g. → N2 (

g. + 2H2O (

g. If 6 moles of hydrazine react with an excess of oxygen, how many moles of water will be produced?

+3

Answers (1)

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Cadence Pugh · Answer 1

Answer is: 12 moles of water will be produced.

Balanced chemical reaction: N₂H₄ + O₂ → N₂ + 2H₂O.

n (N₂H₄) = 6 mol.

From balanced chemical reaction: n (N₂H₄) : n (H₂O) = 1 : 2.

n (H₂O) = 2 · n (N₂H₄).

n (H₂O) = 2 · 6 mol.

n (H₂O) = 12 mol.

n - amount of substance.

Hydrazine (N2H4), a rocket fuel, reacts with oxygen to form nitrogen gas and water vapor. The reaction is represented with the equation: N2H4 (l) + O2 (g. → N2 (g. + 2H2O (g. If 6 moles of hydrazine react with an excess of oxygen, how many moles of water will be produced?

Hydrazine (N2H4), a rocket fuel, reacts with oxygen to form nitrogen gas and water vapor. The reaction is represented with the equation: N2H4 (l) + O2 (

g. → N2 (

g. + 2H2O (

g. If 6 moles of hydrazine react with an excess of oxygen, how many moles of water will be produced?