The second law of thermodynamics leads us to conclude that

Question

BlackTom AI · Accepted Answer

The prompt presents a question about the second law of thermodynamics and asks what conclusion follows from it.

First, it is important to recall the core idea: the second law states that the total entropy of an isolated system can never decrease over time, and in many processes, entropy increases. This leads to a tendency toward greater disorder or more probabilistic configurations as time progresses.

In this specific item, the provided answer option is: "disorder in the universe is increasing with the passage of time." This aligns with the common interpretation of entropy increasing in an isolated system, which is a hallmark of the second law.

Since no other answer choices are present to evaluate, we cannot compare alternatives, but we can examine the given statement for consistency with the second law. If the system under consideration is effectively isolated and undergoing natural processes, the entropy increase interpretation is consistent with the law.

Potential misinterpretations to watch for include confusing entropy with energy or assuming that order can never appear locally; local decreases in entropy are possible if compensated by greater increases elsewhere, so the global trend remains toward higher entropy.

In sum, the statement that disorder (entropy) in the universe increases over time reflects the standard consequence of the second law for isolated or approximately isolated systems, which is what this question targets.

The second law of thermodynamics leads us to conclude that 单项选择题

类似问题

As moisture from the air condenses on the outside of a cold glass of water, the entropy of the condensing moisture

Which of the following is a FALSE statement?

Question at position 6 How do energy transfers affect the universe?decrease entropyincrease entropy

Entropy definition implies that systems tend to disorder, which is against organized life. However, life is maintaned. Choose from below the incorrect answer:

Thermodynamics: A closed system is thermally isolated from the surroundings. The cycle consists of 2 processes:Process 1-2 is irreversible and adiabatic ( Q12=0 ) Process 2-1 is reversible but not adiabatic ( Q21≠0 ). Which of the following statements is/are true?

Which of the following statements is(are) true? I. The entropy change of a system is equal and opposite to the surroundings for any irreversible process. II. The entropy of the system must increase in any spontaneous process.

Which of the two Laws of Thermodynamics states that randomness and disorder are increasing in the universe.

The change of entropy caused by heat addition to system is defined as:

更多留学生实用工具

智能学习助手

风格化写作助手

论文查重助手

文献引用助手

课堂转译助手

课堂笔记助手

Quiz搜索助手

学校历年真题

智能刷题助手

智能匹配练习

希望你的学习变得更简单