Final answer:
To use up 32.6 grams of N₂, it takes 7.03 grams of H₂.
Step-by-step explanation:
To determine the grams of H₂ that will react with 32.6 grams of N₂, we need to use the balanced equation:
N₂ (g) + 3 H₂(g) → 2 NH₃ (g)
From the equation, we can see that 1 mole of N₂ reacts with 3 moles of H₂ to produce 2 moles of NH₃. Using the molar masses of N₂ (28.02 g/mol) and H₂ (2.02 g/mol),
we can calculate the number of moles of N₂ and H₂ in 32.6 grams of N₂:
32.6 g N₂ × (1 mol / 28.02 g) = 1.16 mol N₂
1.16 mol N₂ × (3 mol H₂ / 1 mol N₂) = 3.48 mol H₂
Therefore, we need 3.48 moles of H₂, which is equivalent to:
3.48 mol H₂ × (2.02 g / 1 mol) = 7.03 grams of H₂