Consider the following equilibrium:
4NH₃(g) + 3O₂(g)
2N₂(g) + 6H₂O(g)
Suppose 0.30 mol of NH₃ and 0.40 mol of oxygen are added to a 5.0-L container.If x mol of water is present at equilibrium,how many moles of ammonia will remain at equilibrium?

Question

Consider the following equilibrium:
4NH₃(g) + 3O₂(g)

Consider the following equilibrium: 4NH<sub>3</sub>(g) + 3O<sub>2</sub>(g) 2N<sub>2</sub>(g) + 6H<sub>2</sub>O(g) Suppose 0.30 mol of NH<sub>3</sub> and 0.40 mol of oxygen are added to a 5.0-L container.If x mol of water is present at equilibrium,how many moles of ammonia will remain at equilibrium? A) 0.30 - x B) 0.30 - x C) 0.30 - x D) 0.40 - x E) x

2N₂(g) + 6H₂O(g)
Suppose 0.30 mol of NH₃ and 0.40 mol of oxygen are added to a 5.0-L container.If x mol of water is present at equilibrium,how many moles of ammonia will remain at equilibrium?

Quizplus · Accepted Answer

The balanced equation shows that 4 moles of NH₃ reacts with 3 moles of oxygen to form 6 moles of water and 2 moles of ammonia. Therefore, the ratio of NH₃ to NH3 is 4:2 or 2:1. If x moles of water is formed, then the number of moles of ammonia formed is also x/2. Initially, there are 0 moles of NH3 but 0.30 moles of NH₃. At equilibrium, 2x/6 moles of NH3 will be formed. Therefore, the number of moles of NH3 remaining at equilibrium is 0.30 - 2x/6 or 0.30 - x/3, which is closest to choice C.

Consider the Following Equilibrium