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The thermochemical equations for the formation of iron (ii) oxide and iron (iii) oxide are given below: (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 From these data, Calculate the heat of reaction Δh for the change: 4 FeO(s) + O2(g) → 2fe2o3 (s)
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(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 determine the heat of reaction for the change:
4FeO (s) + O2 (g) → 2Fe2O3 (s)
We can combine the two given reactions in a way that cancels out the 4 FeO on the left-hand side and the 4Fe on the right-hand side, leaving only the desired reaction:
(1) 2 Fe (s) + O2(g) → 2 FeO (s) ΔH= -63.7 kcal
(3) 2 Fe2O3 (s) → 4 Fe (s) + 3O2(g) ΔH= 393.0 kcal
Now we can add the two equations to find the overall reaction :
(4) 4FeO (s) + O2 (g) → 2Fe2O3 (s) ΔH= -329.3 kcal
Therefore, the heat of reaction for the change 4FeO (s) + O2 (g) → 2Fe2O3 (s) is -329.3 kcal.
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