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?
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.
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