Question

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.

Answer 1

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

Step-by-step 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:

• Fe₂O₃: 1 mole
• CO: 3 moles
• Fe: 2 moles
• CO₂: 3 moles

The molar mass of each compound is:

• Fe₂O₃: 159.7 g/mole
• CO: 28 g/mol
• Fe: 55.85 g/mole
• CO₂: 44 g/mole

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

• Fe₂O₃: 1 mole* 159.7 g/mole= 159.7 grams
• CO: 3 moles* 28 g/mol= 84 grams
• Fe: 2 moles* 55.85 g/mole= 111.7 grams
• CO₂: 3 moles* 44 g/mole= 132 grams

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 Fe_(2) O_(3) =(4.65 grams of Fe*159.7 grams of Fe_(2) O_(3))/(111.7grams of Fe)`

mass of Fe₂O₃= 6.65 grams

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