---
title: "A 1.50 g sample of a pure organic compound containing only carbon, hydrogen, and oxygen is completely burned in excess oxygen gas. All of the carbon in the compound is converted to \\(\\text{CO}_2\\text{(g)}\\) and all of the hydrogen is converted to \\(\\text{H}_2\\text{O(g)}\\). The masses of the products collected are shown in the table below.  | Product | Mass (g) | |—|—| | \\(\\text{CO}_2\\text{(g)}\\) | 2.20 | | \\(\\text{H}_2\\text{O(g)}\\) | 0.90 |  Based on these data, what is the empirical formula of the compound?"
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url: "https://nerd-notes.com/ubq/119209/"
date_modified: "2026-08-19T12:39:21+00:00"
---

# A 1.50 g sample of a pure organic compound containing only carbon, hydrogen, and oxygen is completely burned in excess oxygen gas. All of the carbon in the compound is converted to \(\text{CO}_2\text{(g)}\) and all of the hydrogen is converted to \(\text{H}_2\text{O(g)}\). The masses of the products collected are shown in the table below.

| Product | Mass (g) |
|—|—|
| \(\text{CO}_2\text{(g)}\) | 2.20 |
| \(\text{H}_2\text{O(g)}\) | 0.90 |

Based on these data, what is the empirical formula of the compound?

A 1.50 g sample of a pure organic compound containing only carbon, hydrogen, and oxygen is completely burned in excess oxygen gas. All of the carbon in the compound is converted to \(\text{CO}_2\text{(g)}\) and all of the hydrogen is converted to \(\text{H}_2\text{O(g)}\). The masses of the products collected are shown in the table below.

| Product | Mass (g) |
|---|---|
| \(\text{CO}_2\text{(g)}\) | 2.20 |
| \(\text{H}_2\text{O(g)}\) | 0.90 |

Based on these data, what is the empirical formula of the compound?

- **A.** \(\text{C}_2\text{H}_4\text{O}\)
- **B.** \(\text{CH}_4\text{O}\)
- **C.** \(\text{CH}_2\text{O}\)
- **D.** \(\text{C}_2\text{H}_2\text{O}_3\)

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/119209/*