Open Question
A reaction has ΔH°rxn = -112 kJ and ΔS°rxn = 354 J/K. At what temperature is the change in entropy for the reaction equal to the change in entropy for the surroundings?
Ch.18 - Free Energy and Thermodynamics
Chapter 18, Problem 5
What is the molar entropy of a pure crystal at 0 K, and what is the significance of the answer?
Verified step by step guidance1
Identify the concept: The problem is related to the Third Law of Thermodynamics.
Understand the Third Law of Thermodynamics: It states that the entropy of a perfect crystal at absolute zero temperature (0 K) is exactly zero.
Recognize the significance: At 0 K, a perfect crystal is in a state of perfect order, meaning there is only one possible microstate.
Explain the implication: Since entropy is a measure of disorder or the number of microstates, having only one microstate means the entropy is zero.
Conclude the significance: This concept helps in calculating absolute entropies of substances at temperatures above 0 K by providing a reference point.
Related Practice
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Textbook Question
Two systems, each composed of two particles represented by circles, have 20 J of total energy. Which system, A or B, has the greater entropy? Why?
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