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For oxidation of iron, 4Fe(s) + 3O(2)(g)...

For oxidation of iron, `4Fe(s) + 3O_(2)(g) rarr 2Fe_(2)O_(3) (s)` entrop change is `-549.4 J K^(-1)mol^(-1)` at 298K. In spite of negative entropy change of this reaction, why is the reaction spontaneous? (`Delta_(r ) H^(theta)` for this reaction is -1648 kJ `mol^(-1)`)

Text Solution

Verified by Experts

`DeltaS_("total") = +4980.6 JK^(-1) mol^(-1)`
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