For oxidation of iron,, 4Fe(s) + 3O_(2)(g) rarr 2Fe_(2)O_(3)(s),entropy change is - 549 .4 JK^(-1) mol^(-1) at 298 K . Inspite of the negativeentropy change of this reaction , why is the reaction spontaneous ? ( Delta H ^(@) for this reaction is - 1648 xx 10^(3) J mol^(-1))

For oxidation of iron,, 4Fe(s) + 3O_(2)(g) rarr 2Fe_(2)O_(3)(s),entrop

1.	For oxidation of iron,, 4Fe(s) + 3O_(2)(g) rarr 2Fe_(2)O_(3)(s),entropy change is - 549 .4 JK^(-1) mol^(-1) at 298 K . Inspite of the negativeentropy change of this reaction , why is the reaction spontaneous ? ( Delta H ^(@) for this reaction is - 1648 xx 10^(3) J mol^(-1))
Answer» SOLUTION :Proceed as in Solved PROBLEM on page `6 // 87` by either method (Prove that `DELTAG^(@) ` is `-ve` or `DeltaS_("total") ` is `+`ve).