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How many moles of carbon monoxide are required to reduce 5.0 moles of iron from iron(III)oxide? Fe2O3 + 2CO=2Fe + 2CO2

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13 Dec 2019
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Related questions

Blast furnaces extract pure iron from the iron(III) oxide in iron ore in a two step sequence.

In the first step, carbon and oxygen react to form carbon monoxide: 2C (s) + O2 (g) รขย†ย’ 2CO (g)

In the second step, iron(III) oxide and carbon monoxide react to form iron and carbon dioxide: Fe2O3 (s) + 3CO (g) รขย†ย’ 2Fe (s) + 3CO2 (g)

Write the net chemical equation for the production of iron from carbon, oxygen and iron(III) oxide. Be sure your equation is balanced.

Iron(III) oxide, Fe2O3, otherwise known as rust, can react with pure carbon to reform solid iron and carbon monoxide. A balanced chemical equation for this reaction is included below. Fe2O3(s) + 3C(s) ? 2Fe(s) + 3CO(g)

a) Assuming you have 635 g of iron(III) oxide and 185 g of carbon, which of these reagents would be considered the limiting reagent? You must show all your work, including dimensional analysis, to receive credit for this problem!

b) What is the theoretical yield of Fe for this reaction (in g)?

Iron (III) oxide may be reduced to pure iron either with carbonmonoxide or with coke (pure carbon). Suppose that 150kg of ferricoxide are available. How many kilograms of carbon monoxide would berequired to reduce the oxide? How many kilograms of coke would beneeded? In each case, how many kilograms of pure iron would beproduced?

The equations are:
Fe2O3 3CO --> 2Fe 3CO2

2Fe2O3 3C --> 4Fe 3CO2

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