One can review the blast furnace from a simple viewpoint as a process in which t

Question

One can review the blast furnace from a simple viewpoint as a process in which the principle reaction is:

Fe 2 O 3 + 3C 2Fe + 3CO

But some other undesired side reactions occur, mainly:

Fe 2 O 3 + C 2FeO + CO

After mixing 600.0 lb of carbon with 1.00 ton of pure iron dioxide, Fe 2 O 3 ,
the process produces 1200.0 lb of pure iron, 183 lb FeO, and 85.0 lb of Fe 2 O 3 . Calculate the following items:

a. the percentage of excess carbon furnished, based on the principle reaction
b. the percentage conversion of Fe 2 O 3 to Fe
c. the pounds of carbon used up and the pounds of CO produced per ton of Fe 2 O 3 charged
d. what is the selectivity in this process (of Fe with respect to FeO)

Thanks for help.

Explanation / Answer

a. 1 ton (2000 lb) Fe2O3 reacts with 600 lb of C

1 mole of Fe2O3 produces 2 moles of Fe

moles of Fe2O3 = 2000/159.69 g/mol = 12.524 lb.mol

mass of C used = 12. 524 x 3 x 12.01 g/mol = 451.24 lb

excess C left = 600 - 451.24 = 148.76 lb

percentage of excess C funished = 148.76 lb x 100/600 lb = = 24.79%

b. percentage conversion of Fe2O3 to Fe

theoretical yield of Fe = 2 x 12.524 x 55.845 = 1398.80 lb

percentage conversion of Fe2O3 to Fe = 1200 lb x 100/1398.80 lb = 85.79%

c. lbs of C used

moles of Fe formed = 1200/55.845 = 21.50 lb.mol

mass of C used for Fe formation = 21.50 x 3 x 12.01/2 = 387.322 lb

moles of FeO formed = 183/71.844 = 2.55 lb.mol

mass of C used for FeO formation = 2.55 x 12.01/2 = 15.296 lb

Total pounds of C used up = 387.322 + 15.296 = 402.62 lb

Pounds of CO produced per ton of Fe2O3 = 12.524 x 28.01/1 = 350.80 lb

d. Selectivity of Fe/FeO = 85.79/10.17 = 8.43

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