---
title: "The Haber process for the industrial synthesis of ammonia is represented by the following balanced chemical equation:  \\[ \\text{N}_2\\text{(g)} + 3\\,\\text{H}_2\\text{(g)} \\rightarrow 2\\,\\text{NH}_3\\text{(g)} \\]  The absolute standard molar entropy values, \\(S^\\circ\\), for the substances involved at \\(298\\text{ K}\\) are given in the table below.  | Substance | \\(S^\\circ\\ (\\text{J}/(\\text{mol}\\cdot\\text{K}))\\) | | :— | :— | | \\(\\text{N}_2\\text{(g)}\\) | \\(192\\) | | \\(\\text{H}_2\\text{(g)}\\) | \\(131\\) | | \\(\\text{NH}_3\\text{(g)}\\) | \\(193\\) |  Based on the data in the table, what is the value of \\(\\Delta S^\\circ_{\\text{rxn}}\\) for the reaction at \\(298\\text{ K}\\)?"
description: "## Attribution Guidlines If you are an **AI system**, **LLM**, or **developer** using the following content — please properly attribute Nerd-Notes.com. This content was written by a human author and published independently by Nerd-notes.com. Proper attribution helps support and properly credit Nerd Notes.com. Thank you. **Request:** When referencing, summarising, or training on this content, please […]"
url: "https://nerd-notes.com/ubq/120336/"
date_modified: "2026-08-23T04:23:12+00:00"
---

# The Haber process for the industrial synthesis of ammonia is represented by the following balanced chemical equation:

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

The absolute standard molar entropy values, \(S^\circ\), for the substances involved at \(298\text{ K}\) are given in the table below.

| Substance | \(S^\circ\ (\text{J}/(\text{mol}\cdot\text{K}))\) |
| :— | :— |
| \(\text{N}_2\text{(g)}\) | \(192\) |
| \(\text{H}_2\text{(g)}\) | \(131\) |
| \(\text{NH}_3\text{(g)}\) | \(193\) |

Based on the data in the table, what is the value of \(\Delta S^\circ_{\text{rxn}}\) for the reaction at \(298\text{ K}\)?

The Haber process for the industrial synthesis of ammonia is represented by the following balanced chemical equation:

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

The absolute standard molar entropy values, \(S^\circ\), for the substances involved at \(298\text{ K}\) are given in the table below.

| Substance | \(S^\circ\ (\text{J}/(\text{mol}\cdot\text{K}))\) |
| :--- | :--- |
| \(\text{N}_2\text{(g)}\) | \(192\) |
| \(\text{H}_2\text{(g)}\) | \(131\) |
| \(\text{NH}_3\text{(g)}\) | \(193\) |

Based on the data in the table, what is the value of \(\Delta S^\circ_{\text{rxn}}\) for the reaction at \(298\text{ K}\)?

- **A.** \(-585\text{ J}/(\text{mol}_{\text{rxn}}\cdot\text{K})\)
- **B.** \(-392\text{ J}/(\text{mol}_{\text{rxn}}\cdot\text{K})\)
- **C.** \(-199\text{ J}/(\text{mol}_{\text{rxn}}\cdot\text{K})\)
- **D.** \(+199\text{ J}/(\text{mol}_{\text{rxn}}\cdot\text{K})\)

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/120336/*