Oxidation of iron at 298 K is given by:
$4 F e (s) + 3 O_{2} (g) \to 2 F e_{2} O_{3} (s)$
$Δ H^{0} = - 1648 \times 1 0^{3} J m o l^{- 1}$ ,
and the entropy change is $- 549.4 J K^{- 1} m o l^{- 1}$ . Then, the correct statements consistent with the above data are:

Question

Oxidation of iron at 298 K is given by:

$4 F e (s) + 3 O_{2} (g) \to 2 F e_{2} O_{3} (s)$

$Δ H^{0} = - 1648 \times 1 0^{3} J m o l^{- 1}$ ,

and the entropy change is $- 549.4 J K^{- 1} m o l^{- 1}$ . Then, the correct statements consistent with the above data are:

TestHub · Accepted Answer

Δ S sys ​ = − 549.4 J K − 1 m o l − 1 Δ S s u r ​ = − T Δ H 0 ​ = − 298 1648 × 1 0 3 ​ = − 5530 J K − 1 m o l − 1 Δ S T o t a l ​ = − 4980.6 J K − 1 m o l − 1

Chemistry - Thermodynamics - II Question with Solution | TestHub

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