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Ch.18 - Free Energy and Thermodynamics
Tro - Chemistry: A Molecular Approach 4th Edition
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831Not the one you use?Change textbook
All textbooksTro 4th EditionCh.18 - Free Energy and ThermodynamicsProblem 53b
Chapter 18, Problem 53b

Rank each set of substances in order of increasing standard molar entropy (S°). Explain your reasoning. b. H2O(s); H2O(l); H2O(g)

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Start by understanding the concept of standard molar entropy (S°), which is a measure of the amount of disorder or randomness in a system.
Recognize that the state of matter affects entropy: gases have higher entropy than liquids, and liquids have higher entropy than solids.
Identify the substances given: H2O(s) is solid water (ice), H2O(l) is liquid water, and H2O(g) is gaseous water (steam).
Rank the substances based on their states: H2O(s) has the lowest entropy, followed by H2O(l), and H2O(g) has the highest entropy.
Conclude that the order of increasing standard molar entropy is: H2O(s) < H2O(l) < H2O(g).

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Standard Molar Entropy

Standard molar entropy (S°) is a measure of the amount of disorder or randomness in a system at standard conditions (1 bar, 25°C). It quantifies the energy dispersal in a substance, with higher values indicating greater disorder. Entropy increases with temperature and the number of microstates available to a substance.
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Standard Molar Entropy

Phase Changes and Entropy

The phase of a substance significantly affects its entropy. Generally, gases have higher entropy than liquids, which in turn have higher entropy than solids due to the increased freedom of movement and arrangement of particles. As a substance transitions from solid to liquid to gas, its entropy increases due to the greater molecular motion and disorder.
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Comparative Entropy of Water Phases

In the case of water, the standard molar entropies of its phases can be ranked based on their molecular arrangements. Ice (H2O(s)) has the lowest entropy due to its ordered crystalline structure, followed by liquid water (H2O(l)), which has more disorder, and finally water vapor (H2O(g)), which has the highest entropy due to the greatest molecular freedom and disorder in the gaseous state.
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Related Practice
Textbook Question

For each pair of substances, choose the one that you expect to have the higher standard molar entropy (S°) at 25 °C. Explain your choices. a. CO(g); CO2(g) b. CH3OH(l); CH3OH(g) c. Ar(g); CO2(g) d. CH4(g); SiH4(g) e. NO2(g); CH3CH2CH3(g) f. NaBr(s); NaBr(aq)

Textbook Question

Rank each set of substances in order of increasing standard molar entropy (S°). Explain your reasoning. a. I2(g); F2(g); Br2(g); Cl2(g) b. H2O(g); H2O2(g); H2S(g) c. C(s, graphite); C(s, diamond); C(s, amorphous)

Textbook Question

Rank each set of substances in order of increasing standard molar entropy (S°). Explain your reasoning. a. NH3(g); Ne(g); SO2(g); CH3CH2OH(g); He(g) c. CH4(g); CF4(g); CCl4(g)

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Textbook Question

For each pair of substances, choose the one that you expect to have the higher standard molar entropy (S°) at 25 °C. Explain your choices. a. NaNO3(s); NaNO3(aq) b. CH4(g); CH3CH3(g) c. Br2(l); Br2(g) d. Br2(g); F2(g) e. PCl3(g); PCl5(g) f. CH3CH2CH2CH3(g); SO2(g)

Textbook Question

Use data from Appendix IIB to calculate ΔS°rxn for each of the reactions. In each case, try to rationalize the sign of ΔS°rxn . b. C(s) + H2O(g) → CO(g) + H2(g)