---
title: "A student injects a \\(2.20\\text{ g}\\) sample of an unknown volatile liquid into a rigid, evacuated \\(0.500\\text{ L}\\) container. The container is heated to \\(300\\text{ K}\\), at which point all of the liquid completely vaporizes. The pressure of the gas inside the container is measured to be \\(2.46\\text{ atm}\\). Assuming ideal gas behavior, what is the molar mass of the unknown substance?"
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url: "https://nerd-notes.com/ubq/119566/"
date_modified: "2026-08-21T06:53:50+00:00"
---

# A student injects a \(2.20\text{ g}\) sample of an unknown volatile liquid into a rigid, evacuated \(0.500\text{ L}\) container. The container is heated to \(300\text{ K}\), at which point all of the liquid completely vaporizes. The pressure of the gas inside the container is measured to be \(2.46\text{ atm}\). Assuming ideal gas behavior, what is the molar mass of the unknown substance?

A student injects a \(2.20\text{ g}\) sample of an unknown volatile liquid into a rigid, evacuated \(0.500\text{ L}\) container. The container is heated to \(300\text{ K}\), at which point all of the liquid completely vaporizes. The pressure of the gas inside the container is measured to be \(2.46\text{ atm}\). Assuming ideal gas behavior, what is the molar mass of the unknown substance?

- **A.** \(11\text{ g/mol}\)
- **B.** \(22\text{ g/mol}\)
- **C.** \(44\text{ g/mol}\)
- **D.** \(88\text{ g/mol}\)

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/119566/*