The Haber Process for the production of ammonia is represented by:
3 H₂(g) + N₂(g) → 2 NH₃(g)
If a mixture of 30 g of hydrogen with 10 g of nitrogen produced 8.4 g of ammonia,what was the percent yield?

Question

Quizplus · Accepted Answer

To determine the percent yield, we first need to calculate the theoretical yield of ammonia based on the balanced chemical equation. From the equation, we can see that 3 moles of hydrogen react with 1 mole of nitrogen to produce 2 moles of ammonia. 
Moles of hydrogen = 30 g / 2.01588 g/mol = 14.90 mol
Moles of nitrogen = 10 g / 28.0134 g/mol = 0.357 mol
Since nitrogen is the limiting reagent, its moles will determine the maximum amount of product that can be formed. Therefore, theoretical yield of ammonia = 0.357 mol x (2 mol of NH3 / 1 mol of N2) x (17.03 g/mol) = 12.22 g
Percent yield = (actual yield / theoretical yield) x 100% = (8.4 g / 12.22 g) x 100% = 68.7% ≈ 69%

The Haber Process for the Production of Ammonia Is Represented