The combustion of ammonia in the presence of excess oxygen yields NO₂ and H₂O: 4 NH₃ (g) + 7 O₂ (g) → 4 NO₂ (g) + 6 H₂O (g)
The combustion of 57.6 g of ammonia consumes __________ g of oxygen.

Question

Quizplus · Accepted Answer

The molar mass of NH₃ is 17.03 g/mol, so 57.6 g of NH₃ is 3.38 mol. According to the balanced equation, 4 mol of NH₃ requires 7 mol of O₂. Therefore, 3.38 mol of NH₃ requires 5.915 mol of O₂. The molar mass of O₂ is 32.00 g/mol, so 5.915 mol of O₂ is 189 g.

The Combustion of Ammonia in the Presence of Excess Oxygen