To find the volume of CO required to convert 200g of Fe2O3 to Fe, we need to determine the number of moles of Fe2O3 and then use the stoichiometry of the balanced equation to find the volume of CO.
1. Calculate the number of moles of Fe2O3:
Molar mass of Fe2O3 = 2(55.85) + 3(16) = 159.7 g/mol
Number of moles = Mass / Molar mass
Number of moles = 200g / 159.7 g/mol = 1.252 moles
2. Use the stoichiometry of the balanced equation to determine the volume of CO:
From the balanced equation: 1 mol Fe2O3 reacts with 3 mol CO
Therefore, 1.252 moles of Fe2O3 will react with 3 x 1.252 = 3.756 moles of CO
3. Use the ideal gas law to determine the volume of CO at STP:
Volume at STP = Number of moles x 22.4 L/mol
Volume at STP = 3.756 moles x 22.4 L/mol = 84.1 L
Therefore, 84.1 liters of CO at STP will be required to convert 200g of Fe2O3 to Fe.
From the balanced equation of Fe2O3 + 3CO = 2Fe + 3CO, what is the volume of CO at s.t.p will be required to convert 200g of Fe2O3 to Fe?
1 answer