NH₃ is produced according to the following reaction: N₂(g) + 3H₂(g)→ 2NH₃(g). In an experiment, 0.25 mol of NH₃ is formed when 0.5 mol of N₂ is reacted with 0.5 mol of H₂. What is the % yield?
Correct answer: A. 75%
- A. 75%
- B. 50%
- C. 33%
- D. 25%
Explanation
With the given reactants, H₂ is the limiting reactant. The theoretical yield of NH₃ from 0.5 mol of H₂ is 0.333 mol. The percent yield is calculated as (actual yield / theoretical yield) × 100 = (0.25 / 0.333) × 100 = 75%
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Mole calculations connect mass, number of particles and Avogadro's number, while balanced equations provide the mole ratios used in stoichiometry. Questions cover limiting and excess reactants, theoretical yield and percentage yield, including identifying which reactant is consumed first and comparing the actual product with the maximum possible product.
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