According to the second law of thermodynamics, which of the following is true?

• A. Energy conversions increase the order in the universe.
• B. The total amount of energy in the universe is constant.
• C. The entropy of the universe is constantly decreasing.
• D. All reactions produce some heat.
• E. The decrease in entropy associated with life must be compensated for by increased entropy in the environment in which life exists.

Answer: (E)

Verified step by step guidance

1. Understand the second law of thermodynamics: It states that the entropy of an isolated system always increases over time. Entropy is a measure of disorder or randomness.
2. Recognize that energy conversions in biological systems are not perfectly efficient, and some energy is always lost as heat, contributing to increased entropy.
3. Consider the concept of entropy in the universe: While local decreases in entropy can occur (such as in living organisms), they must be offset by increases in entropy elsewhere, maintaining the overall trend of increasing entropy.
4. Evaluate the options given: The statement that 'The decrease in entropy associated with life must be compensated for by increased entropy in the environment in which life exists' aligns with the second law of thermodynamics.
5. Conclude that the correct understanding of the second law is that while life can create order locally, it does so at the expense of increasing disorder in the surrounding environment, thus increasing the universe's overall entropy.