Which of the following is a FALSE statement?

Question

BlackTom AI · Accepted Answer

The task asks us to identify which statement is FALSE among the given options. 
Option: 'The entropy of an isolated system is conserved, i.e., constant.' This claim is not generally true. In thermodynamics, the Second Law states that the entropy of an isolated system tends to increase or, for ideal reversible processes, remain constant. In real, irreversible processes, entropy increases because of irreversibilities like friction, mixing, and heat transfer. Therefore, asserting that entropy is conserved (constant) for an isolated system is false in most natural scenarios.
If one were to consider a perfectly reversible (ideal) process within an isolated system, the entropy would remain constant, but this is a special case, not the general rule. Consequently, the statement as given is false in the broad context of thermodynamics.
A helpful way to view this is to recall that entropy is a measure of disorder or the number of accessible microstates. In an isolated system undergoing unrestricted (irreversible) evolution, the number of accessible microstates typically increases, raising the entropy, which contradicts the idea of constant entropy.
Thus, the single listed statement is false because it incorrectly generalizes entropy behavior in isolated systems beyond the reversible case.

Which of the following is a FALSE statement? Single choice

Similar Questions

The second law of thermodynamics leads us to conclude that

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

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:

More Practical Tools for Students Powered by AI Study Helper

Homework AI Solver

Stylized AI Paper Writer

Plagiarism Checker Assistant

Citation AI Academic Writing Tool

In-Class Translation Assistant

AI Note Generator

AI Quiz Answers

Past Exam Questions from University Test Bank

Smart Practice Assistant

Adaptive Practice

Making Your Study Simpler