Question

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 negative entropy change of this reaction , why is the reaction spontaneous ? `( Delta H ^(@)` for this reaction is `- 1648 xx 10^(3) J mol^(-1))`

Answer 1

Proceed as in Solved Problem on page `6 // 87` by either method (Prove that `DeltaG^(@) ` is `-ve` or `DeltaS_("total") ` is `+`ve).