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10 Nov 2019

the reaction of ferric oxide and carbon monoxide to form ironand carbon dioxide is one of the steps in refining iron ore

a)show the balance equation

b)what is the maximum of iron in grams that can be obtained from1 pounds of ferric oxide

c)what mass in grams of C02 is required to react with 1 pound offerric oxide to form iron metal..........thanks

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Patrina Schowalter
Patrina SchowalterLv2
20 Sep 2019

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Related questions

Iron is the most widely used metal in North America. It may be produced by the reaction of iron (III) oxide, from iron ore, with carbon monoxide to produce iron metal and carbon dioxide. What mass of iron (III) oxide is required to produce of iron? Show your work.

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) → 2CO (g)

In the second step, iron(III) oxide and carbon monoxide react to form iron and carbon dioxide: Fe2O3 (s) + 3CO (g) → 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.

4. Iron (III) oxide reacts with carbon monoxide to form iron metaland carbon dioxide gas. In a certain reaction, 5.00 g of iron (III)oxide is reacted with 5.00 g of carbon monoxide gas.
c. What is the limiting reactant?
d. Assuming complete reaction, what mass of iron metal isproduced?
e. If the percent yield is only 93%, what was the actualyield?

please show all work

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