Textbook Question
Two different gases occupy the two bulbs shown here. Consider the process that occurs when the stopcock is opened, assuming the gases behave ideally. (d) How does the process affect the entropy of the surroundings?
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Ch.19 - Chemical Thermodynamics
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970
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Table of contents
- Ch.1 - Introduction: Matter, Energy, and Measurement111
- Ch.2 - Atoms, Molecules, and Ions166
- Ch.3 - Chemical Reactions and Reaction Stoichiometry138
- Ch.4 - Reactions in Aqueous Solution127
- Ch.5 - Thermochemistry104
- Ch.6 - Electronic Structure of Atoms109
- Ch.7 - Periodic Properties of the Elements107
- Ch.8 - Basic Concepts of Chemical Bonding102
- Ch.9 - Molecular Geometry and Bonding Theories120
- Ch.10 - Gases122
- Ch.11 - Liquids and Intermolecular Forces79
- Ch.12 - Solids and Modern Materials102
- Ch.13 - Properties of Solutions99
- Ch.14 - Chemical Kinetics153
- Ch.15 - Chemical Equilibrium83
- Ch.16 - Acid-Base Equilibria109
- Ch.17 - Additional Aspects of Aqueous Equilibria117
- Ch.18 - Chemistry of the Environment60
- Ch.19 - Chemical Thermodynamics109
- Ch.20 - Electrochemistry113
- Ch.21 - Nuclear Chemistry79
- Ch.22 - Chemistry of the Nonmetals52
- Ch.23 - Transition Metals and Coordination Chemistry57
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry7
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970Not the one you use?Change textbook
Chapter 19, Problem 3b
b. If energy can flow in and out of the system to maintain a constant temperature during the process, what can you say about the entropy change of the surroundings as a result of this process?
Verified step by step guidance1
Identify the type of system and process: The system allows energy exchange to maintain constant temperature, indicating it's an isothermal process.
Understand the concept of entropy: Entropy is a measure of the disorder or randomness in a system. In thermodynamics, it's also a measure of energy dispersal at a specific temperature.
Relate energy flow and entropy: When energy flows out of the system (as heat) to maintain constant temperature, it increases the entropy of the surroundings because the energy is dispersed into a larger environment.
Apply the second law of thermodynamics: This law states that the total entropy of an isolated system can never decrease over time. Since the system is not isolated but can exchange heat with its surroundings, the entropy of the surroundings must increase if the system's entropy decreases or remains constant.
Conclude about the entropy change of the surroundings: Since the system maintains a constant temperature by exchanging heat with its surroundings, and based on the second law of thermodynamics, the entropy of the surroundings increases as a result of this process.
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Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Entropy
Entropy is a measure of the disorder or randomness in a system. In thermodynamics, it quantifies the amount of energy in a physical system that is not available to do work. When energy is transferred between a system and its surroundings, the change in entropy can indicate whether the process is spontaneous or requires external energy input.
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Entropy in Thermodynamics
Thermodynamic Equilibrium
Thermodynamic equilibrium occurs when a system's macroscopic properties, such as temperature and pressure, are uniform throughout and do not change over time. In the context of the question, maintaining a constant temperature implies that the system is in thermal equilibrium with its surroundings, allowing for energy exchange without a net change in temperature.
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Second Law of Thermodynamics
The Second Law of Thermodynamics states that the total entropy of an isolated system can never decrease over time. It implies that processes occur in a direction that increases the total entropy of the universe. In the scenario described, if energy flows in and out of the system while maintaining constant temperature, the entropy change of the surroundings will increase, reflecting the energy exchange and the tendency towards greater disorder.
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Related Practice
Textbook Question
The accompanying diagram shows how entropy varies with temperature for a substance that is a gas at the highest temperature shown. (c) If this substance is a perfect crystal at T = 0 K, what is the value of S at this temperature?
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Textbook Question
Predict the signs of ΔH and ΔS for this reaction. Explain your choice.
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