Answer to Question #249692 in General Chemistry for Kim

Question

A fuel mixture consisting of hydrazine, N2H4, and dinitrogen tetroxide, N204,was used to launch a lunar module. These two compounds react to form nitrogen gas and water vapour. If 50.0g of hydrazine reacts with sufficient dinitrogen tetroxide, what mass of nitrogen gas is formed?

Answer 1

2N₂H₄ + N₂O₄ → 3N₂ + 4H₂O

M(N₂H₄) = 32.04 g/mol

n(N₂H₄) $= \frac{50.0}{32.04} = 1.56 \;mol$

According to the reaction equation:

n(N₂) $= \frac{3}{2}n(N_2H_4) = \frac{3}{2} \times 1.56 = 2.34 \;mol$

M(N₂) = 28.01 g/mol

m(N₂) $= 2.34 \times 28.01 = 65.56 \;g$

Answer: 65.56 g