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Ch.19 - Chemical Thermodynamics
Brown - Chemistry: The Central Science 14th Edition
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232당신이 사용하는 게 아니라요?교과서 변경
모든 교과서Brown 14th EditionCh.19 - Chemical Thermodynamics문제 42a
19장, 문제 42a

Predict the sign of ΔSsys for each of the following processes: (a) Molten gold solidifies.

검증된 단계별 안내
1
Step 1: Understand the concept of entropy (ΔS). Entropy is a measure of the disorder or randomness in a system. A positive ΔS indicates an increase in disorder, while a negative ΔS indicates a decrease in disorder.
Step 2: Consider the process described: molten gold solidifying. This process involves a phase change from liquid to solid.
Step 3: Recall that in general, the transition from a liquid to a solid results in a decrease in entropy. This is because the particles in a solid are more ordered and have less freedom of movement compared to those in a liquid.
Step 4: Predict the sign of ΔSsys. Since the process involves a decrease in disorder (from liquid to solid), ΔSsys is expected to be negative.
Step 5: Conclude that the sign of ΔSsys for the solidification of molten gold is negative, indicating a decrease in entropy.

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주요 개념

질문에 올바르게 답하기 위해 반드시 이해해야 하는 핵심 개념들은 다음과 같습니다.

Entropy (ΔS)

Entropy, denoted as ΔS, is a measure of the disorder or randomness in a system. In thermodynamics, a positive ΔS indicates an increase in disorder, while a negative ΔS signifies a decrease in disorder. Understanding how entropy changes during a process is crucial for predicting the spontaneity and direction of chemical reactions.
추천 영상:
가이드 코스
02:46
Entropy in Thermodynamics

Phase Changes

Phase changes refer to the transitions between solid, liquid, and gas states of matter. During these transitions, energy is absorbed or released, affecting the system's entropy. For example, when a substance solidifies, it typically moves from a more disordered liquid state to a more ordered solid state, which usually results in a decrease in entropy.
추천 영상:
가이드 코스
01:46
Entropy in Phase Changes

Spontaneity of Processes

The spontaneity of a process is determined by the changes in enthalpy (ΔH) and entropy (ΔS) according to the Gibbs free energy equation, ΔG = ΔH - TΔS. A process is spontaneous if ΔG is negative. In the case of molten gold solidifying, the decrease in entropy (negative ΔS) must be considered alongside the enthalpy change to assess the overall spontaneity of the process.
추천 영상:
가이드 코스
04:20
Spontaneity of Processes
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