Iron(III)oxide is used to produce iron by reacting it with carbon monoxide. If 2.70 kg Fe2O3 are available to react, how many moles of CO are needed?

2 Answers

justaguide's profile pic

justaguide | College Teacher | (Level 2) Distinguished Educator

Posted on

To produce iron from ferric oxide or iron(III) oxide, ferric oxide is reacted with carbon monoxide in a chemical reaction that has the following equation:

Fe2O3 + CO --> Fe + CO2

This equation is not balanced and balancing the chemical equation gives:

Fe2O3 + 3CO --> 2Fe + 3CO2

This shows that for each mole of Fe2O3 three moles of carbon monoxide (CO) are required. The molar mass of Fe2O3 is 159.69 g/mole. 2.7 kg of Fe2O3 is equivalent to 2700/159.69 = 16.9 moles.

The reaction with carbon monoxide requires thrice the number of moles of carbon monoxide or approximately 50.7 moles.

najm1947's profile pic

najm1947 | Elementary School Teacher | (Level 1) Valedictorian

Posted on

The balanced equation of the reaction of Ferric oxide with Carbon Mono-oxide is:

Fe2O3 (s) + 3CO (g) -> Fe (s) + 3CO2 (g)

1 Mole of Fe2CO3 requiress 3 Moles of CO to complete reaction

Molar mass of Fe2O3 = 159.6682 g

Mass of Fe2O3 available to react = 2.70Kg

Moles of Fe2O3 in 2.70Kg = 2.70*1000/159.6682 = 16.91 Mol

Mole of CO required = 3*16.91 = 50.73 Mol

50.73 Moles of CO are needed to convert 2.70 Kg of Fe2O3 in Fe