a) The following two unbalanced reactions are important in the blast furnace pro

Question

a) The following two unbalanced reactions are important in the blast furnace production of iron metal from iron ore, Fe2O3 .

C (s) + O2 (g) ? CO(g)

Fe2O3 (s) + CO(g) ? Fe + CO2

Balance the above reaction and write a net reaction. Using the balanced reaction, how many grams of O2 and Fe2O3 are required for the production of 5.00 kg of Fe

b) Sulfuric acid is produced by the following process:

FeS2 + O2 ? Fe2O3 + SO2

SO2 + O2 ? SO3

SO3 + H2O ? H2SO4

Balance each reaction and then write a balanced net reaction. How many moles of O2 and H2O will be needed when 10.0 kg of FeS2 reacts completely?

Explanation / Answer

a)

6C(s) + 3O2 (g) - - - - - > 6CO (g)

2Fe2O3(s) + 6CO (g) - - - - - - > 4Fe(s) + 6CO2(g)

Net reaction

2Fe2O3(g) + 6C(g) + 3O2(g) - - - - - - > 4Fe(s) + 6CO2(g)

stoichiometrically, to produce 4 moles of Fe, 2moles of Fe2O3 and 3moles of O2 are required

required moles of Fe = 5000g/55.85g/mol = 89.53

moles of Fe2O3 reuired = ( 2/4)×89.53mol = 44.77

moles of O2 required = (3/4) × 89.53mol = 67.15mol

mass of Fe2O3 required = 44.77mol × 159.7g/mol = 7150g

masss of O2 required = 67.15mol × 32g/mol = 2150g

b)

4FeS2 + 11O2 - - - - - - > 2Fe2O3 + 8SO2

8SO2 + 4O2 - - - - > 8SO3

8SO3 + 8H2O - - - - - > 8H2SO4

net reaction

4FeS2 + 8H2O + 15O2 - - - - - > 2Fe2O3 + 8H2SO4

stoichiometrically, 4moles of FeS2 react with 15moles of O2 and 8 moles of H2O

moles of FeS2 = 10000g/119.99mol = 83.34

moles of O2 required = (15/4)×83.34mol = 312.53mol

moles of H2O required = (8/4)×83.34mol = 166.68mol

Related Questions

Navigate

• Browse (All)
• Browse A
• Subjects

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.