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)`)

Explanation

To determine why the oxidation of iron is spontaneous despite a negative entropy change, we can analyze the thermodynamic principles involved.

### Step-by-Step Solution:

1. **Identify the Given Data:**
- The reaction is:
\[
4Fe(s) + 3O_2(g) \rightarrow 2Fe_2O_3(s)
...