Domanda del libro di testo
The normal boiling point of Br2(𝑙) is 58.8 °C, and its molar enthalpy of vaporization is Δ𝐻vap=29.6kJ/mol. (b) Calculate the value of Δ𝑆 when 1.00 mol of Br2(𝑙) is vaporized at 58.8 °C.
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Ch.19 - Chemical Thermodynamics
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232
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TOC.tableOfContents
- Ch.1 - Introduction: Matter, Energy, and Measurement177
- Ch.2 - Atoms, Molecules, and Ions231
- Ch.3 - Chemical Reactions and Reaction Stoichiometry216
- Ch.4 - Reactions in Aqueous Solution189
- Ch.5 - Thermochemistry175
- Ch.6 - Electronic Structure of Atoms168
- Ch.7 - Periodic Properties of the Elements150
- Ch.8 - Basic Concepts of Chemical Bonding177
- Ch.9 - Molecular Geometry and Bonding Theories200
- Ch.10 - Gases179
- Ch.11 - Liquids and Intermolecular Forces113
- Ch.12 - Solids and Modern Materials154
- Ch.13 - Properties of Solutions157
- Ch.14 - Chemical Kinetics199
- Ch.15 - Chemical Equilibrium128
- Ch.16 - Acid-Base Equilibria164
- Ch.17 - Additional Aspects of Aqueous Equilibria163
- Ch.18 - Chemistry of the Environment105
- Ch.19 - Chemical Thermodynamics164
- Ch.20 - Electrochemistry171
- Ch.21 - Nuclear Chemistry122
- Ch.22 - Chemistry of the Nonmetals82
- Ch.23 - Transition Metals and Coordination Chemistry79
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry16
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Non è quello che usi tu?Cambia libro di testo
Capitolo 19, Problema 25c
Indicate whether each statement is true or false. (c) In a certain spontaneous process the system undergoes an entropy change of 4.2 J/K; therefore, the entropy change of the surroundings must be -4.2 J/K.
Guida verificata passo dopo passo1
insert step 1> Understand the concept of entropy and the second law of thermodynamics. Entropy is a measure of the disorder or randomness in a system, and the second law of thermodynamics states that the total entropy of an isolated system can never decrease over time.
insert step 2> Recognize that in a spontaneous process, the total entropy change (ΔS_total) of the universe (system + surroundings) must be greater than zero.
insert step 3> Identify that the given problem states the system undergoes an entropy change (ΔS_system) of 4.2 J/K.
insert step 4> Recall that the entropy change of the surroundings (ΔS_surroundings) is related to the heat exchange with the system and can be calculated using the formula ΔS_surroundings = -ΔS_system if the process is isothermal and reversible.
insert step 5> Evaluate whether the given statement that ΔS_surroundings must be -4.2 J/K is consistent with the requirement that ΔS_total = ΔS_system + ΔS_surroundings > 0 for a spontaneous process.
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Entropy
Entropy is a measure of the disorder or randomness in a system. In thermodynamics, it quantifies the number of microscopic configurations that correspond to a thermodynamic system's macroscopic state. A positive change in entropy indicates an increase in disorder, while a negative change suggests a decrease. Understanding entropy is crucial for analyzing spontaneous processes, as they tend to favor states of higher entropy.
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Percorso guidato
02:46
Entropy in Thermodynamics
Second Law of Thermodynamics
The Second Law of Thermodynamics states that in any spontaneous process, the total entropy of an isolated system will always increase over time. This law implies that energy transformations are not 100% efficient, and some energy is always lost as heat, contributing to the overall increase in entropy. It also establishes the relationship between the entropy changes of the system and its surroundings, which is essential for evaluating the truth of statements regarding entropy changes.
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00:48Second Law of Thermodynamics Example
Entropy Change of the Surroundings
The entropy change of the surroundings is related to the heat exchanged with the system during a process. For a spontaneous process, the total change in entropy (system plus surroundings) must be positive. If a system experiences an entropy change of +4.2 J/K, the surroundings must experience a corresponding change that ensures the total entropy increases, which may not necessarily be -4.2 J/K, depending on the heat exchange and the nature of the process.
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00:53Entropy of Surroundings Formula
Pratica correlata
Domanda del libro di testo
The element gallium (Ga) freezes at 29.8 °C, and its molar enthalpy of fusion is ΔHfus = 5.59 kJ/mol. (a) When molten gallium solidifies to Ga(s) at its normal melting point, is ΔS positive or negative?
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Domanda del libro di testo
The element gallium (Ga) freezes at 29.8 °C, and its molar enthalpy of fusion is ΔHfus = 5.59 kJ/mol. (b) Calculate the value of ΔS when 60.0 g of Ga(l) solidifies at 29.8 °C.
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Domanda del libro di testo
(c) During a certain reversible process, the surroundings undergo an entropy change, ΔSsurr = -78 J/K. What is the entropy change of the system for this process?
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Domanda del libro di testo
(a) Does the entropy of the surroundings increase for spontaneous processes?
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Domanda del libro di testo
(b) In a particular spontaneous process the entropy of the system decreases. What can you conclude about the sign and magnitude of ΔSsurr?
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