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Solution


Q.

Consider the following reaction occurring in the blast furnace. 

Fe3O4(s)+4CO(g) → 3Fe(l)+4CO2(g)

'x' kg of iron is produced when 2.32×103 kg Fe3O4 and 2.8×102 kg CO are brought together in the furnace. The value of 'x' is _______ (nearest integer).                   

[Given:
Molar mass of Fe3O4=232 g mol-1
Molar mass of CO=28 g mol-1
Molar mass of Fe=56 g mol-1]                         [2025]

Ans.

(420)

Moles of Fe3O4(nFe3O4) =Given mass of Fe3O4Molar mass of Fe3O4

=2.32×103 kg232 g mol-1=2.32×103×103 g232 g mol-1=10000 mol

Moles of CO (nCO)=Given mass of COMolar mass of CO

=2.8×102 kg28 g mol-1=2.8×102×103 g28 g mol-1=10000 mol

Fe3O4+4CO⟶3Fe+4CO2

As per stoichiometry of the reaction, 10000 mol Fe3O4 needs 40000 mol of CO for complete reaction. But only 10000 mol CO is present. So CO is the limiting reagent.  
So amount of iron formed depends upon the amount of CO.

By reaction stoichiometry:

Fe3O4+4CO⟶3Fe+4CO2

nFe3=nCO4

nFe3=100004

nFe=3×100004=7500 mol

Mass of Fe =Fen×Molar mass of Fe=7500×56 g=420000 g=420 kg