---
title: "A student conducts a reaction to synthesize ammonia gas according to the balanced equation below.  \\[\\text{N}_2\\text{(g)} + 3\\text{H}_2\\text{(g)} \\rightarrow 2\\text{NH}_3\\text{(g)}\\]  The student combines \\(56 \\text{ g}\\) of \\(\\text{N}_2\\text{(g)}\\) and \\(9.0 \\text{ g}\\) of \\(\\text{H}_2\\text{(g)}\\) in a closed reaction vessel and allows the reaction to proceed to completion. Assuming a 100% yield, what is the theoretical yield of \\(\\text{NH}_3\\text{(g)}\\) produced?"
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/119272/"
date_modified: "2026-08-19T12:39:36+00:00"
---

# A student conducts a reaction to synthesize ammonia gas according to the balanced equation below.

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

The student combines \(56 \text{ g}\) of \(\text{N}_2\text{(g)}\) and \(9.0 \text{ g}\) of \(\text{H}_2\text{(g)}\) in a closed reaction vessel and allows the reaction to proceed to completion. Assuming a 100% yield, what is the theoretical yield of \(\text{NH}_3\text{(g)}\) produced?

A student conducts a reaction to synthesize ammonia gas according to the balanced equation below.

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

The student combines \(56 \text{ g}\) of \(\text{N}_2\text{(g)}\) and \(9.0 \text{ g}\) of \(\text{H}_2\text{(g)}\) in a closed reaction vessel and allows the reaction to proceed to completion. Assuming a 100% yield, what is the theoretical yield of \(\text{NH}_3\text{(g)}\) produced?

- **A.** \(26 \text{ g}\)
- **B.** \(34 \text{ g}\)
- **C.** \(51 \text{ g}\)
- **D.** \(68 \text{ g}\)

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/119272/*