The overall reaction for the corrosion of iron by oxygen is given by the followi

Question

The overall reaction for the corrosion of iron by oxygen is given by the following reaction. 4Fe (s) + 3O2 (g) ?? 2Fe2O3 (s) Compound ?H

Explanation / Answer

That ?H is for the equation as written. 4 Moles of Fe(s) + 3 Moles of O2(g)----> 2 Moles of Fe2O3(s) Heat released is 1652 KJ a. Four moles of iron releases 1652 kJ b. 1652 for two moles of Fe2O3. One mole of Fe2O3. Half as much : 826 kJ c. Atomic weight of iron is 55.8 grams per mole. One gram of iron is 1 / 55.8 mole. ?H will be (1 / 55.8) * (1652 / 4) = 7.4 kJ d. Which one is limiting? Fe : 10 / 55.8 Moles = 0.18 O2 : 2 / 32 Moles. = 0.063 And remember that for every 4 moles of Fe, 3 moles of O2 are required. Ratio of 1.3 Ratio of Fe to O2 is 0.18 / 0.063 = 2.8 So it is the oxygen that is limiting. 0.063 moles of oxygen will react with 4/3 of 0.063 = 0.084 moles of Fe. There is plenty of iron. Heat released = 0.063 * 1652 / 3 = 34.7 kJ

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