The standard entropy change for the reaction
$4Fe\left(s\right) + 3{O}_{2}\left(g\right) \to 2{Fe}_{2}{O}_{3}\left(s\right)$ is $- 550J{K}^{- 1}$ at $298K$
[Given : The standard enthalpy change for the reaction is $- 165kJ{mol}^{- 1}$ ]. The temperature in $K$ at which the reaction attains equilibrium is (Nearest Integer)

Question

The standard entropy change for the reaction

$4Fe\left(s\right) + 3{O}_{2}\left(g\right) \to 2{Fe}_{2}{O}_{3}\left(s\right)$ is $- 550J{K}^{- 1}$ at $298K$

[Given : The standard enthalpy change for the reaction is $- 165kJ{mol}^{- 1}$ ]. The temperature in $K$ at which the reaction attains equilibrium is (Nearest Integer)

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4Fe(s) + 3 O _ 2 (g) → 3 Fe _ 2 O _ 3 (s) Δ S _ r = - 550J / K Δ S _ r = - 165kJ / mole At equilibrium Δ G = 0 T = ((Δ H)/(Δ S)) at equilibrium = - 165 × 10 ^ 3 - 550 = 300K

The standard entropy change for the reaction 4Fe(s) + 3 O _ 2 (g) →...

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