In the given equation, \[ 4 \mathrm{Fe}(s)+3 \mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{Fe}_{2}...

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In the given equation,
\[
4 \mathrm{Fe}(s)+3 \mathrm{O}_{2}(g) \longrightarrow 2 \mathrm{Fe}_{2} \mathrm{O}_{3}(s)
\]
The entropy change is \( -549.4 \mathrm{JK}^{-1} \mathrm{~mol}^{-1} \) at \( 298 \mathrm{~K} \). \( \left(\Delta_{r} H^{\circ}=-1648 \times 10^{3} \mathrm{~J} \mathrm{~mol}^{-1}\right) \). The above reaction is
(a) spontaneous
(b) non-spontaneous
(c) non-spontaneous at \( 500 \mathrm{~K} \)
(d) None of these
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