What mass of nitrogen gas (28.02 g/mol)is produced when 0.500 kg I₂ (253.8 g/mol)is combined with 35.0 g N₂H₄ (32.06 g/mol)? 2 I₂(s)+ N₂H₄(g)$\to$ 4 HI(g)+ N₂(g)

Question

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The balanced chemical equation is:2 I₂(s)+ N₂H₄(g) → 4 HI(g)+ N₂(g)From the stoichiometry of the balanced equation, we can see that 2 moles of I₂ react with 1 mole of N₂H₄ to produce 1 mole of N₂.Therefore, the number of moles of N₂ produced is:n(N₂) = n(N₂H₄) = 35.0 g / 32.06 g/mol = 1.09 molThe mass of N₂ produced is:m(N₂) = n(N₂) * M(N₂) = 1.09 mol * 28.02 g/mol = 30.5 gTherefore, the correct answer is A) 27.6 g.

What Mass of Nitrogen Gas (28 →\to→ 4 HI(g)+ N2(g) A)27

What Mass of Nitrogen Gas (28 $\to$ 4 HI(g)+ N₂(g)
A)27