Question

A fuel mixture consisting of hydrazine, N₂H4, and dinitrogen tetroxide, N₂O4, was used to launch a lunar module. These two compounds react to form nitrogen gas and water vapour. If 50.0 g 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) =50/32.0=1.56mol

According to the reaction equation:

n(N2) = 3/2n(N_2H_4) =3/2× 1.56 = 2.34 mol

M(N2) = 28.01 g/mol

m(N2) = 2.34 × 28.01 = 65.56 g = 2.34×28.01=65.56g

Answer: 65.56 g

Answer 2

Answer:

2N2H4 + N2O4 → 3N2 + 4H2O

M(N2H4) = 32.04 g/mol

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

32.04

50.0

=1.56mol

According to the reaction equation:

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

2

3

n(N

2

H

4

)=

2

3

×1.56=2.34mol

M(N2) = 28.01 g/mol

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

Answer: 65.56 g

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Explanation:

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