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Lorico [155]
3 years ago
7

The multistep smelting of ferric oxide to form elemental iron occurs at high temperatures in a blast furnace. In the first step,

ferric oxide reacts with carbon monoxide to form Fe₃O.₄ This substance reacts with more carbon monoxide to formiron(II) oxide, which reacts with still more carbon monoxide to form molten iron. Carbon dioxide is also produced in each step.
(a) Write an overall balanced equation for the iron-smelting process.
(b) How many grams of carbon monoxide are required to form 45.0 metric tons of iron from ferric oxide?
Chemistry
1 answer:
iVinArrow [24]3 years ago
3 0

Answer: a)  Fe_2O_3+3CO\rightarrow 2Fe+3CO_2

b) 33749996 grams

Explanation:

a) The balanced chemical reactions will be :

3Fe_2O_3+CO\rightarrow CO_2+2Fe_3O_4

2Fe_3O_4+2CO\rightarrow 6FeO+2CO_2

6FeO+6CO\rightarrow 6Fe+6CO_2

Overall equation : 3Fe_2O_3+9CO\rightarrow 6Fe+9CO_2

Overall balanced equation : Fe_2O_3+3CO\rightarrow 2Fe+3CO_2

b) Amount of iron = 45 metric ton = 45000 kg = 45000000g

To calculate the moles :

\text{Moles of solute}=\frac{\text{given mass}}{\text{Molar Mass}}    

\text{Moles of} Fe=\frac{45000000g}{56g/mol}=803571moles

Fe_2O_3+3CO\rightarrow 2Fe+3CO_2

According to stoichiometry :

2 moles of Fe are produced from=  3 moles of CO

Thus 803571 moles of Fe are produced from=\frac{3}{2}\times 803571=1205357moles  of CO

Mass of CO=moles\times {\text {Molar mass}}=1205357moles\times 28g/mol=33749996g

Thus 33749996 g of carbon monoxide are required to form 45.0 metric tons of iron from ferric oxide

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