Under appropriate conditions, nitrogen and hydrogen undergo a combination reaction to yield ammonia: N₂ (g) + 3H₂ (g) → 2NH₃ (g)
If the reaction yield is 87.5%, how many moles of N₂ are needed to produce 3.00 mol of NH₃?

Question

Quizplus · Accepted Answer

To produce 3.00 mol of NH₃ with an 87.5% yield, calculate the theoretical moles of NH₃ needed: 3.00 mol / 0.875 = 3.43 mol. From the balanced equation, 1 mol of N₂ produces 2 mol of NH₃, so 3.43 mol NH₃ requires 3.43 / 2 = 1.71 mol of N₂.

Under Appropriate Conditions, Nitrogen and Hydrogen Undergo a Combination Reaction