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Question

For oxidation of iron,
4Fe(s)+3O2(g)2Fe2O3(s)
entropy change is - 549.4 JK1mol1 at 298 K. In spite of negative entropy change of this reaction, why is the reaction spontaneous?
(,H for this reaction is 1648×103Jmol1)

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Solution

For a spontaneous reaction, total entropy must be greater than zero i.e. positive
4Fe(s)+3O2(g)2Fe2O3(s)
Hf=1648 KJmol1
reaction is exothermic and surroundings absorbed 1648KJ of heat
Ssurr=HfT=1648298=5.53 KJmol1k1
=5530 Jmol1k1
Stotal=Ssystem+Ssurrounding
=549.4+5530
=4980.6 Jk1mol1

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