What must be true for a spontaneous process according to the 2nd law of thermodynamics?

For a process to be classified as spontaneous according to the second law of thermodynamics, it must result in an increase in the total entropy of the universe. The universe's entropy is defined as the sum of the entropy of the system in question and the entropy of its surroundings. When a spontaneous process occurs, the overall disorder of the universe (as measured by entropy) increases, indicating a natural tendency towards more disordered states.

This principle is essential because it highlights that spontaneous processes are directionally favored, naturally progressing from less probable, more ordered states to more probable, disordered states. The second law thereby underscores the directional nature of thermodynamic processes and the eventual trend towards equilibrium, where the total entropy reaches a maximum.

The correct understanding of this concept is fundamental in physical chemistry and thermodynamics, as it governs many processes observed in nature. The options suggesting an entropy of less than or equal to zero do not align with this principle of spontaneous transition towards higher entropy states. Additionally, the idea that a closed system must have greater entropy than its surroundings is not a requirement for spontaneity and stands separate from the overall increase in the universe's entropy. Thus, the assertion that the entropy of the universe is greater than zero accurately reflects the necessary condition for spontane