Final answer:
The second law of thermodynamics states that the total entropy of a system does not decrease but may increase, reflecting the concept that usable energy is lost in energy transfers, contributing to the universe's increasing entropy.
Step-by-step explanation:
The question specifically pertains to the concept of entropy in systems, where the second law of thermodynamics states that the total entropy of a system either increases or remains constant; it never decreases. In the context of energy transfers, this law emphasizes that every transfer or transformation of energy results in a loss of some usable energy, thereby increasing the entropy of the universe. Consider the example wherein a person gathers scattered marbles into a cup, thus decreasing the system's entropy. However, the input of energy from the person ultimately contributes to an increase in the universe's total entropy. Living organisms, which maintain low-entropy states, continually take in energy to sustain themselves, but this process elevates the entropy of their surroundings. In essence, while local decreases in entropy are possible (like in the storage of solar energy by plants), they are offset by greater increases in the entropy of the surrounding environment, ensuring that the second law of thermodynamics is not violated.