What does the equation ∆S(system) + ∆S(surroundings) = ∆S(universe) ≥ 0 imply?

The equation ∆S(system) + ∆S(surroundings) = ∆S(universe) ≥ 0 reflects the Second Law of Thermodynamics, which states that the entropy of the universe tends to increase over time for spontaneous processes. This indicates that for any spontaneous process, the total change in entropy of the universe (which is the sum of the change in entropy of the system and the change in entropy of the surroundings) will be greater than or equal to zero.

A positive ∆S(universe) suggests that the process is spontaneous, meaning it occurs naturally without external intervention. When considering a process that is at equilibrium, the entropy change will equal zero, which means the process is not spontaneous. The important takeaway here is that the overall entropy change for spontaneous processes is always positive or zero, directly relating to your selected answer.

Understanding this principle is crucial in thermodynamics as it helps us predict the direction of chemical reactions and physical changes in matter. Hence, the statement reinforces the idea that as processes occur in the universe, there is an overall tendency toward an increase in entropy, aligning with the physical principles governing spontaneous reactions.