In the reaction of 9.7 g of NH₃ witH₂ 4.6 g of O₂, a chemist isolates 8.0 g of H₂0. The other product is NO. What is the percent yield?

Question

Quizplus · Accepted Answer

The balanced equation for the reaction is 4NH₃ + 5O₂ → 4NO + 6H₂O. The molar mass of NH₃ is 17 g/mol, so 9.7 g is 0.57 mol. The molar mass of O₂ is 32 g/mol, so 4.6 g is 0.144 mol. O₂ is the limiting reactant. According to the stoichiometry, 0.144 mol of O₂ produces 0.1728 mol of H₂O (0.144 mol O₂ * (6 mol H₂O / 5 mol O₂)). The molar mass of H₂O is 18 g/mol, so the theoretical yield is 3.11 g. The percent yield is (8.0 g / 3.11 g) * 100% = 52%.

In the Reaction of 9