The reduction of iron(III) oxide (Fe203) to pure iron during the first step of s

Question

The reduction of iron(III) oxide (Fe203) to pure iron during the first step of steelmaking, 2 Fe,03s)- 4Fe(s) 30,(e) is driven by the high-temperature combustion of coke, a purified form of coal: Cs)+ 08) CO2(8) Suppose at the temperature of a blast furnace the Gibbs free energies of formation ??, of CO2 and Fe2O3 are-437. kJ/mol and-842. kJ/mol, respectively. Calculate the maximum mass of pure iron that can be produced by the combustion of 6500. kg of coke. Round your answer to 2 significant digits 10

Explanation / Answer

the reactions are 2Fe2O3(s) -------->4Fe(s)+3O2(g) (1)

and C(s)+ O2(g) -------------->CO2, (2)

Eq.1+3*Eq.2 elemiates the presence of oxygen.

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

Maxium mass will be produced as per the theoretical yield of the reaction which states that

3 moles of C ( from Coke) gives rise to 4 moles of Fe

atomic weight of C=12 and Fe= 56 g/mole

mole= mass/atomic weight

mass = moles* atomic weight

so 3 moles of C= 3*12 =36 gm of C and 4 moles of Fe= 4*56= 224 gm of Fe

36 gm of Coke gives a maxium iron of 224 gm

6500 kg of Coke gives 6500Kg* 224 gm/36 gm =40444.44 kg of Fe

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