Answer:
Given reaction is
2Fe(s) + (3/2)O2(g) ----------> Fe2O3(s)
Enthalpy, ∆Hrxn=sum of ∆H°f products - sum of ∆H°f reactants
∆Hrxn=(1 mol x ∆H°f Fe2O3 (s)) - [(2 mol x∆H°f Fe(s)) + ((3/2 mol) x ∆H°f O2(g))]
∆H°f Fe2O3 (s)=-824.248 kJ/mol
∆H°f Fe(s)=0 and ∆H°f O2(g)=0.
∆Hrxn=( 1 mol x -824.248 kJ/mol) -[(2 mol x 0) + (3/2 molx 0)]
∆Hrxn=-824.248 kJ
Therefore reaction enthalpy=-824.2 kJ
(c) is correct.
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