---
title: "In an industrial chemical plant, ammonia gas is synthesized from nitrogen and hydrogen gases in a rigid reactor at a constant temperature according to the following equation:  \\[ \\text{N}_2(g) + 3\\,\\text{H}_2(g) \\rightleftharpoons 2\\,\\text{NH}_3(g) \\]  After the system reaches chemical equilibrium, \\(\\text{NH}_3(g)\\) is continuously removed from the reactor by condensation. Which of the following best predicts the effect of this removal on the system and provides the correct justification?"
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url: "https://nerd-notes.com/ubq/119998/"
date_modified: "2026-08-21T08:31:44+00:00"
---

# In an industrial chemical plant, ammonia gas is synthesized from nitrogen and hydrogen gases in a rigid reactor at a constant temperature according to the following equation:

\[ \text{N}_2(g) + 3\,\text{H}_2(g) \rightleftharpoons 2\,\text{NH}_3(g) \]

After the system reaches chemical equilibrium, \(\text{NH}_3(g)\) is continuously removed from the reactor by condensation. Which of the following best predicts the effect of this removal on the system and provides the correct justification?

In an industrial chemical plant, ammonia gas is synthesized from nitrogen and hydrogen gases in a rigid reactor at a constant temperature according to the following equation:

\[ \text{N}_2(g) + 3\,\text{H}_2(g) \rightleftharpoons 2\,\text{NH}_3(g) \]

After the system reaches chemical equilibrium, \(\text{NH}_3(g)\) is continuously removed from the reactor by condensation. Which of the following best predicts the effect of this removal on the system and provides the correct justification?

- **A.** The system will favor the reverse reaction to restore total pressure because the partial pressure of \(\text{NH}_3(g)\) decreases, making \(Q_p > K_p\).
- **B.** The system will favor the forward reaction to produce more \(\text{NH}_3(g)\) because removing product shifts the equilibrium by increasing the value of \(K_p\).
- **C.** The system will favor the forward reaction to produce more \(\text{NH}_3(g)\) because the decrease in the partial pressure of \(\text{NH}_3(g)\) causes \(Q_p < K_p\), resulting in a forward reaction rate that exceeds the reverse reaction rate.
- **D.** The system will favor the reverse reaction to replace lost gas particles because decreasing the total pressure always shifts an equilibrium toward the side with more moles of gas.

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/119998/*