For oxidation of iron.
`4Fe(s)+3O_(2)(g)rarr2Fe_(2)O_(3)(s)`
entropy change is`- 549.4 JK^(-1)mol^(-1)` at 298 K. Inspite of negative entropy change of this reaction, why is the reaction spontaneous?
`(Delta_(r)H^(Ө)` for this reaction is `-1648xx10^(3)J"mol"^(-1)`)

a) For the oxidation of iron 4 Fe_((s))+3O_(2(g))rightarrow2Fe_2O_(3(s)) , entropy change is -549.4 JK^-1mol^-1 at 298 K. Inspite of the negative entropy change of this reaction, why is the reaction spontaneous? ( DeltaH_r^0 for the reaction is - 1648xx10^3Jmol^-1 ). b) Write the difference between extensive and intensive properties. Give one example of each.

For oxidation of Fe 4Fe(s) + 3O_2(g) to 2Fe_2O_3(s) entropy change is -549.4 JK^-1mol^-1 at 298K. Inspite of negative entropy change of this reaction, why is the reaction spontaneous ? triangleH^@ = -1648xx10^3 J mol^-1

For the oxidation of iron 4Fc_((s))+3O_(2(g))to2Fe_((2))O_(3(s)) , the entropy change is -549.45 JK^(-1)mol^(-1) at 298 K. Though it has negative entropy change the reaction is spontaneous. Why? (Delta_(r)H^(theta)=-164xx10^(3)J ml^(-1))

The oxidation of iron occurs as: 4Fe(s) + 3 O_(2)(g) to 2Fe_(2)O_(3)(s) The enthalpy of formation of Fe_(2)O_(3) is - 824.2 kJ mol^(-1) and entropy change for the reaction is -549 J K^(-1) mol^(-1) at 298 K. Inspite of negative entropy change of this reaction, why is the reaction spontaneous at 298 K?