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The thermochemical equations for the formation of iron (ii) oxide and iron (iii) oxide are given below:rn (1) 2 fe (s) + O2(g) → 2 FeO (s) Δh= -63.7 kcal rn(2) 4 fe (s) + 3o2(g) → 2fe2o3 (s) Δh= -393.0 kcal rnfrom these data, Calculate the heat of reaction Δh for the change:rn 4 FeO(s) + O2(g) → 2fe2o3 (s)
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Sure, here is the requested calculation:
From the given thermochemical equations, we can determine the heat of reaction for the desired change as follows:
(1) 2 Fe (s) + O2(g) --→ 2 FeO (s) ΔH= -63.7 kcal
(2) 4 Fe (s) + 3O2(g) --→ 2Fe2O3 (s) ΔH= -393.0 kcal
To obtain the target equation, we must multiply equation (1) by 2 and then add the result to equation (2) as shown below:
4 Fe (s) + 2O2(g) --→ 4 FeO (s) ΔH= -127.4 kcal
4 Fe (s) + 3O2(g) --→ 2Fe2O3 (s) ΔH= -393.0 kcal
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8 Fe (s) + 5O2(g) --→ 4 Fe2O3 (s) ΔH= -520.4 kcal
Therefore, the heat of reaction for the change 4 FeO(s) + O2(g) --→ 2Fe2O3 (s) is ΔH = -520.4 kcal.
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