The reaction of iron (III) oxide with carbon monoxide produces iron and carbon dioxide. Fe2O3(s) + 3C0(9) - 2Fe(s) + 3CO (9)
How many grams of Fe2O3 are required to produce 4.65g Fe? You must show your work to receive full credit.

6.65 grams of Fe₂O₃ are required to produce 4.65g Fe.

Explanation:

The balanced reaction is:

Fe₂O₃ + 3 CO → 2 Fe + 3 CO₂

By reaction stoichiometry (that is, the relationship between the amount of reagents and products in a chemical reaction), the following amounts of moles of each compound participate in the reaction:

The molar mass of each compound is:

Then, by reaction stoichiometry, the following mass quantities of each compound participate in the reaction:

Then you can apply the following rule of three: if by stoichiometry 111.7 grams of Fe are produced from 159.7 grams of Fe₂O₃, 4.65 grams of Fe are produced from how much mass of Fe₂O₃?

mass of Fe₂O₃= 6.65 grams

6.65 grams of Fe₂O₃ are required to produce 4.65g Fe.

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