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title: "At \\(298\\text{ K}\\) and \\(1\\text{ atm}\\), bromine exists primarily as a reddish-brown liquid, \\(\\text{Br}_2(l)\\), in equilibrium with a small amount of bromine vapor, \\(\\text{Br}_2(g)\\). Which of the following statements correctly compares the standard molar entropy, \\(S^\\circ\\), of \\(\\text{Br}_2(g)\\) to that of \\(\\text{Br}_2(l)\\) at \\(298\\text{ K}\\), and provides the correct justification?"
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url: "https://nerd-notes.com/ubq/120002/"
date_modified: "2026-08-21T08:31:48+00:00"
---

# At \(298\text{ K}\) and \(1\text{ atm}\), bromine exists primarily as a reddish-brown liquid, \(\text{Br}_2(l)\), in equilibrium with a small amount of bromine vapor, \(\text{Br}_2(g)\). Which of the following statements correctly compares the standard molar entropy, \(S^\circ\), of \(\text{Br}_2(g)\) to that of \(\text{Br}_2(l)\) at \(298\text{ K}\), and provides the correct justification?

At \(298\text{ K}\) and \(1\text{ atm}\), bromine exists primarily as a reddish-brown liquid, \(\text{Br}_2(l)\), in equilibrium with a small amount of bromine vapor, \(\text{Br}_2(g)\). Which of the following statements correctly compares the standard molar entropy, \(S^\circ\), of \(\text{Br}_2(g)\) to that of \(\text{Br}_2(l)\) at \(298\text{ K}\), and provides the correct justification?

- **A.** \(S^\circ\) is greater for \(\text{Br}_2(g)\) than for \(\text{Br}_2(l)\) because gaseous molecules have significantly greater freedom of translational motion, resulting in a larger number of accessible microstates.
- **B.** \(S^\circ\) is greater for \(\text{Br}_2(g)\) than for \(\text{Br}_2(l)\) because the covalent \(\text{Br}-\text{Br}\) bonds are weaker in the gas phase than in the liquid phase.
- **C.** \(S^\circ\) is greater for \(\text{Br}_2(l)\) than for \(\text{Br}_2(g)\) because the presence of intermolecular attractions in the liquid allows for a greater variety of molecular orientations.
- **D.** \(S^\circ\) is greater for \(\text{Br}_2(l)\) than for \(\text{Br}_2(g)\) because liquid bromine has a higher density, leading to more particles per unit volume and greater total entropy.

*The answer key and step-by-step explanation are available to logged-in users at https://nerd-notes.com/ubq/120002/*