09 - 10/8/09 Chapter 10 Ssolid<Sliquid<Sgas Examples:...

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10/8/09 Chapter 10 S solid <S liquid <<S gas Examples: 1) C (s) + CO 2(g) 2CO (g) ∆S system = + Whenever the products contain more moles of gas than the reactants, the change in entropy is always positive for the system 2) 2SO 2(g) + O 2(g) 2SO 3(g) ∆S system = - 3) N 2(g) + O 2(g) 2NO (g) ∆S system ~ 0 4) 4Fe (s) + 3O 2(g) 2 Fe 2 O 3(s) ∆S system = - We know this reaction is spontaneous. How can this be? 2 nd Law: Every spontaneous reaction is accompanied by an increase entropy of the system and surroundings ∆S total = ∆S system + ∆S surroudnings This reaction must be accompanied by a large increase in ∆S surroundings For this reaction: ∆H system = - Temperature of gas molecules in the surroundings increases Kinetic energy of the gas particles increases Disorder of the universe increases Calculation of ∆S Discuss reversible and irreversible processes Reversible Process: a cyclic process in which both the system and the surroundings are returned to
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09 - 10/8/09 Chapter 10 Ssolid&lt;Sliquid&lt;Sgas Examples:...

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