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In one of the practice problems I was doing, I noticed that although heat is conserved from the system to the surroundings: delta H (system) = - (delta H surroundings), the same idea does not apply for entropy. For example, although enthalpy is conserved, the entropy lost by a system and gained by the surroundings are completely different. Why is change in entropy not conserved as well?
Conservation of anything implies that it cannot be created nor destroyed. However, Entropy is not conserved because it's something that is generated from the "disorder" of systems. Also note that the second law of Thermodynamics states that entropy within an isolated system will keep increasing.
Enthalpy is a state property and entropy is not.
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