for the given equation the change in entropy is positive or negative? WHY? Fe(400k)-------->Fe(300k)

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Q. Change in entropy is negative for:

Q. For the oxidation of iron, the entropy change is -549.45J/K.mol at 298K. Though it has negative entropy change, the reaction is spontaneous. Why?
The reaction is
4Fe+3O₂ gives 2Fe₂O₃

For the reaction Hg ---------> Hg (), the entropy change will have the sign:

For oxidation of iron,

4 F e (s) + {3 O}_{2} (g) \to 2 {F e}_{2} O_{3} (s)

entropy change is - 549.4

{J K}^{- 1} {m o l}^{- 1}

at 298 K. In spite of negative entropy change of this reaction, why is the reaction spontaneous?

(

△, H^{⊝}

for this reaction is

- 1648 \times 10^{3} J {m o l}^{- 1}

)

The enthalpy change for a given reaction at 298 K is $- x J m o l^{- 1}$ (x being positive). If the reaction occurs spontaneously at 298 K, the entropy change at that temperature

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