Question Detail
Question
For the reaction: N₂(g) + 3H₂(g) ⇌ 2NH₃(g), Kc = 0.50 at a certain temperature. In a 2.00 L container, 0.20 mol N₂, 0.60 mol H₂, and 0.10 mol NH₃ are mixed. Is the system at equilibrium?
Correct Answer
Option C is the correct answer.
Detailed Explanation
[N₂] = 0.20/2 = 0.10 M, [H₂] = 0.60/2 = 0.30 M, [NH₃] = 0.10/2 = 0.050 M. Q = (0.050)²/(0.10 × (0.30)³) = 0.0025/(0.10 × 0.027) = 0.0025/0.0027 = 0.93. Since Q (0.93) > Kc (0.50), the reaction will shift left to reach equilibrium. Wait recalc: 0.30³=0.027, 0.10×0.027=0.0027, 0.050²=0.0025, 0.0025/0.0027=0.926. Q=0.93 > 0.50, so shift left. But the original pattern had a similar question with a different answer. Based on this, the system is not at equilibrium and will shift left.
Hint
Calculate Q and compare to K. If Q > K, reaction shifts left; if Q < K, shifts right.