---
title: "A student analyzes a sample of a pure carbohydrate and determines that its empirical formula is \\(\\text{CH}_2\\text{O}\\). In a separate measurement, a \\(0.0500\\text{ mol}\\) sample of the compound is found to have a mass of \\(9.01\\text{ g}\\). Based on these data, what is the molecular formula of the compound?"
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url: "https://nerd-notes.com/ubq/119928/"
date_modified: "2026-08-21T08:18:16+00:00"
---

# A student analyzes a sample of a pure carbohydrate and determines that its empirical formula is \(\text{CH}_2\text{O}\). In a separate measurement, a \(0.0500\text{ mol}\) sample of the compound is found to have a mass of \(9.01\text{ g}\). Based on these data, what is the molecular formula of the compound?

A student analyzes a sample of a pure carbohydrate and determines that its empirical formula is \(\text{CH}_2\text{O}\). In a separate measurement, a \(0.0500\text{ mol}\) sample of the compound is found to have a mass of \(9.01\text{ g}\). Based on these data, what is the molecular formula of the compound?

- **A.** \(\text{C}_2\text{H}_4\text{O}_2\)
- **B.** \(\text{C}_3\text{H}_6\text{O}_3\)
- **C.** \(\text{C}_6\text{H}_{12}	ext{O}_6\)
- **D.** \(\text{C}_{12}	ext{H}_{24}	ext{O}_{12}\)

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/119928/*