Which of the following is a FALSE statement?

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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.

SPHY001 Practice Quiz - Unit 15 | LA055

Which of the following is a FALSE statement?

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