---
title: "A student places a sample of \\(1.00\\text{ mol}\\) of \\(\\text{CH}_4\\text{(g)}\\) and a sample of \\(1.00\\text{ mol}\\) of \\(\\text{SO}_2\\text{(g)}\\) into separate, rigid \\(2.45\\text{ L}\\) containers maintained at \\(298\\text{ K}\\). According to the ideal gas law, the pressure in each container should be approximately \\(10.0\\text{ atm}\\). Which of the following statements correctly compares the actual measured pressure of \\(\\text{SO}_2\\text{(g)}\\) to that of \\(\\text{CH}_4\\text{(g)}\\) and provides the best particulate-level justification?"
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url: "https://nerd-notes.com/ubq/121390/"
date_modified: "2026-08-23T05:02:02+00:00"
---

# A student places a sample of \(1.00\text{ mol}\) of \(\text{CH}_4\text{(g)}\) and a sample of \(1.00\text{ mol}\) of \(\text{SO}_2\text{(g)}\) into separate, rigid \(2.45\text{ L}\) containers maintained at \(298\text{ K}\). According to the ideal gas law, the pressure in each container should be approximately \(10.0\text{ atm}\). Which of the following statements correctly compares the actual measured pressure of \(\text{SO}_2\text{(g)}\) to that of \(\text{CH}_4\text{(g)}\) and provides the best particulate-level justification?

A student places a sample of \(1.00\text{ mol}\) of \(\text{CH}_4\text{(g)}\) and a sample of \(1.00\text{ mol}\) of \(\text{SO}_2\text{(g)}\) into separate, rigid \(2.45\text{ L}\) containers maintained at \(298\text{ K}\). According to the ideal gas law, the pressure in each container should be approximately \(10.0\text{ atm}\). Which of the following statements correctly compares the actual measured pressure of \(\text{SO}_2\text{(g)}\) to that of \(\text{CH}_4\text{(g)}\) and provides the best particulate-level justification?

- **A.** \(P_{\text{measured}}(\text{SO}_2) < P_{\text{measured}}(\text{CH}_4)\) because \(\text{SO}_2\) molecules have a greater molar mass than \(\text{CH}_4\) molecules, which results in a lower average molecular speed and fewer collisions per second with the container walls.
- **B.** \(P_{\text{measured}}(\text{SO}_2) < P_{\text{measured}}(\text{CH}_4)\) because \(\text{SO}_2\) molecules experience significant dipole-dipole attractions and stronger London dispersion forces than \(\text{CH}_4\) molecules, which decreases the force and frequency of collisions with the container walls.
- **C.** \(P_{\text{measured}}(\text{SO}_2) > P_{\text{measured}}(\text{CH}_4)\) because the larger molecular volume of \(\text{SO}_2\) reduces the free volume available in the container, significantly increasing the rate of collisions with the container walls.
- **D.** \(P_{\text{measured}}(\text{SO}_2) > P_{\text{measured}}(\text{CH}_4)\) because the polar bonds in \(\text{SO}_2\) cause mutual electrostatic repulsion between adjacent molecules, increasing the force exerted during wall collisions.

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/121390/*