The mass of hydrazine (N₂H₄) required to produce 96 g of water (H₂O) is 85.4 g (Option C)
<h3>Balanced equation </h3>
N₂H₄ + O₂ —> N₂ + 2H₂O
Molar mass of N₂H₄ = (2×14) + (4×1) = 32 g/mol
Mass of N₂H₄ from the balanced equation = 1 × 32 = 32 g
Molar mass of H₂O = (2×1) + 16 = 18 g/mol
Mass of H₂O from the balanced equation = 2 × 18 = 36 g
SUMMARY
From the balanced equation above,
36 g of H₂O were produced by 32 g of N₂H₄
<h3>How to determine the mass of N₂H₄</h3>
From the balanced equation above,
36 g of H₂O were produced by 32 g of N₂H₄
Therefore,
96 g of H₂O will be produced by = (96 × 32) / 36 = 85.4 g of N₂H₄
Thus, 85.4 g of N₂H₄ is needed for the reaction
Learn more about stoichiometry:
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