Problem: The rusting of iron is spontaneous and is accompanied by a decrease in the entropy of the system (the iron and oxygen).What can we conclude about the entropy change of the surroundings?

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We are asked what we can conclude about the entropy change of surroundings accompanying the rusting of iron which is spontaneous and is accompanied by a decrease of entropy of the system (the iron and oxygen).

 4Fe(s) + 3O2(g) → 2Fe2O3(s)

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The rusting of iron is spontaneous and is accompanied by a decrease in the entropy of the system (the iron and oxygen).

What can we conclude about the entropy change of the surroundings?

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What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Second and Third Laws of Thermodynamics concept. If you need more Second and Third Laws of Thermodynamics practice, you can also practice Second and Third Laws of Thermodynamics practice problems.

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Based on our data, we think this problem is relevant for Professor Dixon's class at UCF.