Which of the following is/are true for a reversible process at equilibrium?
I. $\Delta$ S_univ = 0
II. $\Delta$ S_sys = 0
III. $\Delta$ G_sys = 0

Question

Which of the following is/are true for a reversible process at equilibrium? I.$\Delta$S_univ = 0 II.$\Delta$S_sys = 0 III.$\Delta$G_sys = 0

Quizplus · Accepted Answer

For a reversible process at equilibrium, both the system and the surroundings are in a state of constant entropy, which means that ΔSsystem = ΔSsurroundings = 0. Therefore, the first and second equations are true: I. F1F1F1S1F1F1F10S_univ = 0 (where U1B1univ stands for the total internal energy of the universe) II. F1F1F1S1F1F1F10S_sys = 0 (where U1B1sys stands for the internal energy of the system) However, the third equation is not true because the Gibbs free energy change of a reversible process at equilibrium can only be equal to zero if the process occurs at constant temperature and pressure. Therefore, we cannot assume that ΔG = 0 for a reversible process at equilibrium without specifying these conditions.

Which of the Following Is/are True for a Reversible Process Δ\DeltaΔ

Which of the Following Is/are True for a Reversible Process $\Delta$