A 14.01 g sample of N₂ reacts with 3.02 g of H₂ to form ammonia (NH₃). If ammonia is the only product, what mass of ammonia is formed? A) 17.03 g B) 1.10 g C) 14.01 g D) 3.02 g E) 23.07 g

Question

Quizplus · Accepted Answer

The balanced chemical equation is:N₂ + 3H₂ → 2NH₃From the stoichiometry of the balanced equation, we can see that 1 mole of N₂ reacts with 3 moles of H₂ to produce 2 moles of NH₃.The molar mass of N₂ is 28.02 g/mol, and the molar mass of H₂ is 2.02 g/mol.Therefore, 14.01 g of N₂ is equal to 14.01 g / 28.02 g/mol = 0.5 moles of N₂.3.02 g of H₂ is equal to 3.02 g / 2.02 g/mol = 1.5 moles of H₂.Since N₂ is the limiting reactant, we will use its moles to calculate the moles of NH₃ produced.From the stoichiometry of the balanced equation, we know that 1 mole of N₂ produces 2 moles of NH₃.Therefore, 0.5 moles of N₂ will produce 0.5 moles * 2 = 1.0 moles of NH₃.The molar mass of NH₃ is 17.03 g/mol.Therefore, 1.0 moles of NH₃ is equal to 1.0 moles * 17.03 g/mol = 17.03 g of NH₃.Therefore, the mass of ammonia formed is 17.03 g.

A 1401 G Sample of N2 Reacts with 3

A 1401 G Sample of N₂ Reacts with 3