What is the molar entropy of a pure crystal at 0 K, and what is the significance of the answer?

Verified step by step guidance

1. Identify the concept: The problem is related to the Third Law of Thermodynamics.
2. Understand the Third Law of Thermodynamics: It states that the entropy of a perfect crystal at absolute zero temperature (0 K) is exactly zero.
3. Recognize the significance: At 0 K, a perfect crystal is in a state of perfect order, meaning there is only one possible microstate.
4. Explain the implication: Since entropy is a measure of disorder or the number of microstates, having only one microstate means the entropy is zero.
5. Conclude the significance: This concept helps in calculating absolute entropies of substances at temperatures above 0 K by providing a reference point.

Key Concepts

Third Law of Thermodynamics

The Third Law of Thermodynamics states that as the temperature of a perfect crystal approaches absolute zero (0 K), the entropy of the crystal approaches a constant minimum. For a perfect crystalline substance at 0 K, this minimum entropy is zero, indicating that the system is in a state of perfect order with no randomness.

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. Higher entropy indicates greater disorder, while lower entropy suggests more order, as seen in a pure crystal at absolute zero.

Significance of Molar Entropy at 0 K

The significance of the molar entropy of a pure crystal at 0 K lies in its implications for thermodynamic processes and the behavior of materials at low temperatures. It reinforces the concept of absolute zero as a theoretical limit and provides a foundation for understanding the thermodynamic properties of substances, influencing calculations in physical chemistry and materials science.