---
title: "The synthesis of ammonia is represented by the following balanced equation:  \\(\\text{N}_2\\text{(g)} + 3\\text{H}_2\\text{(g)} \\rightarrow 2\\text{NH}_3\\text{(g)}\\)  Which of the following best predicts the sign of the standard entropy change, \\(\\Delta S^\\circ\\), for the reaction and provides the correct justification?"
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url: "https://nerd-notes.com/ubq/119293/"
date_modified: "2026-08-19T12:39:41+00:00"
---

# The synthesis of ammonia is represented by the following balanced equation:

\(\text{N}_2\text{(g)} + 3\text{H}_2\text{(g)} \rightarrow 2\text{NH}_3\text{(g)}\)

Which of the following best predicts the sign of the standard entropy change, \(\Delta S^\circ\), for the reaction and provides the correct justification?

The synthesis of ammonia is represented by the following balanced equation:

\(\text{N}_2\text{(g)} + 3\text{H}_2\text{(g)} \rightarrow 2\text{NH}_3\text{(g)}\)

Which of the following best predicts the sign of the standard entropy change, \(\Delta S^\circ\), for the reaction and provides the correct justification?

- **A.** \(\Delta S^\circ < 0\), because the reaction results in a net decrease in the number of moles of gas.
- **B.** \(\Delta S^\circ < 0\), because energy is released as new chemical bonds form in the products.
- **C.** \(\Delta S^\circ > 0\), because two different element species combine to form a compound with greater structural complexity.
- **D.** \(\Delta S^\circ > 0\), because the total mass and total number of atoms are conserved during the reaction.

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/119293/*