Which of the following is correct statement?

Engineering

Chemistry

Gibbs Free Energy Entropy and Spontaneity

Question

During a spontaneous process entropy of system will always increase.

In case of He(g) more heat has to be given as compared to C₂H₄(g) for same temperature change at constant volume.

Entropy of a closed system must increase in an irreversible adiabatic process.

ΔS is a state function.

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The correct statement is: ΔS is a state function.

Entropy change (ΔS) depends only on the initial and final states of a system, not the path taken. For any reversible process between two states, ΔS is defined as the integral of dq_rev/T.

$Δ S = \int_{1}^{2} \frac{d q_{rev}}{T}$

This makes it a state function, unlike heat (q) or work (w), which are path-dependent.

Final Answer: ΔS is a state function.