Entropy to never decrease in an isolated system

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SUMMARY

The discussion centers on the concept of entropy in isolated systems, specifically addressing the confusion surrounding molecular self-assembly and its impact on entropy. It is established that while ordering can decrease entropy locally, it simultaneously increases entropy in the surrounding environment, thus adhering to the second law of thermodynamics. The example of humans consuming apples illustrates how energy transfer from the sun contributes to this process, emphasizing that true isolation must account for all interacting particles.

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  • Understanding of the second law of thermodynamics
  • Familiarity with concepts of entropy and energy transfer
  • Knowledge of molecular self-assembly processes
  • Basic principles of closed and isolated systems
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  • Explore molecular self-assembly and its implications on entropy
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Students of physics, chemists, and anyone interested in thermodynamics and the principles governing entropy and energy interactions in systems.

venomxx
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I considered entropy to never decrease in an isolated system, so I am a little confused when i read about how molecules 'self assemble' to lower interfacial energy which leads to an ordering of the system...

Is this ordering not a decrease in entropy violating the law that it always increases?

Im just a little confused, so if anyone can explain this id appreciate it!
 
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venomxx said:
Is this ordering not a decrease in entropy violating the law that it always increases?

Ordering decreases entropy for the thing that's being ordered, but it increases entropy elsewhere. You have to make sure that your 'closed system' includes ALL interacting particles etc.

Example, humans eat apples to order themselves by destroying the order of the apple. The apple became ordered by using energy from the sun etc.
 


It's not an isolated system.
 

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