Textbook Question
Cyclopropane and propylene are isomers that both have the formula C3H6. Based on the molecular structures shown, which of these isomers would you expect to have the higher standard molar entropy at 25 °C?
Ch.19 - Chemical Thermodynamics
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970
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Table of contents
- Ch.1 - Introduction: Matter, Energy, and Measurement146
- Ch.2 - Atoms, Molecules, and Ions200
- Ch.3 - Chemical Reactions and Reaction Stoichiometry176
- Ch.4 - Reactions in Aqueous Solution155
- Ch.5 - Thermochemistry126
- Ch.6 - Electronic Structure of Atoms131
- Ch.7 - Periodic Properties of the Elements126
- Ch.8 - Basic Concepts of Chemical Bonding123
- Ch.9 - Molecular Geometry and Bonding Theories143
- Ch.10 - Gases147
- Ch.11 - Liquids and Intermolecular Forces91
- Ch.12 - Solids and Modern Materials122
- Ch.13 - Properties of Solutions126
- Ch.14 - Chemical Kinetics174
- Ch.15 - Chemical Equilibrium101
- Ch.16 - Acid-Base Equilibria139
- Ch.17 - Additional Aspects of Aqueous Equilibria146
- Ch.18 - Chemistry of the Environment72
- Ch.19 - Chemical Thermodynamics129
- Ch.20 - Electrochemistry142
- Ch.21 - Nuclear Chemistry101
- Ch.22 - Chemistry of the Nonmetals68
- Ch.23 - Transition Metals and Coordination Chemistry66
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry10
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970Not the one you use?Change textbook
Chapter 19, Problem 47
Predict which member of each of the following pairs has the greater standard entropy at 25°C: (a) Sc(s) or Sc(g). Use Appendix C to find the standard entropy of each substance. (b) NH3(g) or NH3(aq). Use Appendix C to find the standard entropy of each substance. (c) O2(g) or O3(g). Use Appendix C to find the standard entropy of each substance. (d) C(graphite) or C(diamond). Use Appendix C to find the standard entropy of each substance.
Verified step by step guidance1
Step 1: Understand the concept of standard entropy. Standard entropy is a measure of the amount of disorder or randomness in a system. Generally, gases have higher entropy than liquids, and liquids have higher entropy than solids due to the increased freedom of movement of particles.
Step 2: For part (a), compare Sc(s) and Sc(g). Recognize that the gaseous state (Sc(g)) typically has a higher entropy than the solid state (Sc(s)) because gas particles are more disordered and have more freedom of movement.
Step 3: For part (b), compare NH3(g) and NH3(aq). Consider that gases usually have higher entropy than aqueous solutions because gas molecules are more dispersed and have more freedom to move compared to when they are dissolved in water.
Step 4: For part (c), compare O2(g) and O3(g). Note that molecules with more atoms generally have higher entropy due to the increased number of ways they can arrange themselves. Therefore, O3(g) might have a higher entropy than O2(g) because it has more atoms.
Step 5: For part (d), compare C(graphite) and C(diamond). Recognize that graphite has a layered structure allowing more freedom of movement compared to the rigid, tightly bonded structure of diamond, suggesting that C(graphite) has a higher entropy than C(diamond).
Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Standard Entropy
Standard entropy is a measure of the disorder or randomness in a system at a specified temperature, typically 25°C. It is denoted as S° and is expressed in units of J/(mol·K). Higher entropy values indicate greater disorder, which often correlates with the number of microstates available to a substance. Understanding standard entropy is crucial for predicting the spontaneity of processes and the stability of different phases of matter.
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03:33
Standard Molar Entropy
Phase Changes and Entropy
The phase of a substance significantly affects its entropy. Gases generally have higher entropy than liquids, which in turn have higher entropy than solids due to the increased freedom of movement and greater number of microstates in gases. For example, comparing solid and gaseous states of the same element, the gas will have a greater standard entropy due to its higher disorder and molecular motion.
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Comparative Entropy of Solutions
When comparing the standard entropy of a solute in different states, such as gas versus aqueous solution, the solute in solution typically has a lower entropy than its gaseous form. This is because solvation restricts the movement of solute particles, leading to a more ordered arrangement. Thus, understanding how solvation affects entropy is essential for predicting which state will have a greater standard entropy.
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Related Practice
Textbook Question
Predict the sign of ΔSsys for each of the following processes: (c) Gaseous CO reacts with gaseous H2 to form liquid methanol, CH3OH.
Textbook Question
Predict the sign of ΔSsys for each of the following processes: (d) Calcium phosphate precipitates upon mixing Ca(NO3)2(aq) and (NH4)3PO4(aq).
Textbook Question
Using S° values from Appendix C, calculate ΔS° values for the following reactions. In each case, account for the sign of ΔS°.
(a) C2H4(g) + H2(g) → C2H6(g)
(b) N2O4(g) → 2 NO2(g)
(c) Be(OH)2(s) → BeO(s) + H2O(g)
(d) 2 CH3OH(g) + 3 O2(g) ⟶ 2 CO2(g) + 4 H2O(g)