When ammonia reacts with oxygen, nitrogen monoxide and water are produced. The balanced equation for this reaction is: 4NH3 (g) + 5O2 (g) → 4NO (g) + 6H2O (g) If 16 moles of ammonia react, the reaction consumes 20 moles of oxygen. The reaction produces 16 moles of nitrogen monoxide and 24 moles of water
The Correct Answer and Explanation is:
Correct Answer:
Yes, the reaction consumes 20 moles of oxygen, produces 16 moles of nitrogen monoxide, and produces 24 moles of water when 16 moles of ammonia react.
Explanation
To determine if the numbers are correct, we begin with the balanced chemical equation for the reaction between ammonia and oxygen:
4NH₃ (g) + 5O₂ (g) → 4NO (g) + 6H₂O (g)
This equation tells us that 4 moles of ammonia (NH₃) react with 5 moles of oxygen (O₂) to produce 4 moles of nitrogen monoxide (NO) and 6 moles of water (H₂O).
This is a mole ratio. From the equation, for every 4 moles of NH₃, we need:
- 5 moles of O₂
- We produce 4 moles of NO
- We produce 6 moles of H₂O
Now, we scale the entire equation up based on the amount of ammonia given in the question, which is 16 moles.
Since 16 moles is 4 times the original 4 moles of NH₃ in the balanced equation, we must multiply every other substance in the equation by 4:
- O₂: 5 moles × 4 = 20 moles required
- NO: 4 moles × 4 = 16 moles produced
- H₂O: 6 moles × 4 = 24 moles produced
So, reacting 16 moles of ammonia would consume 20 moles of oxygen, produce 16 moles of nitrogen monoxide, and produce 24 moles of water.
The quantities in the question match exactly with the stoichiometry of the balanced equation. Therefore, the answer is correct, and the mole relationships are consistent with the balanced reaction. This example demonstrates how mole ratios from balanced equations can be used to predict the amounts of reactants and products in a chemical reaction.
