The following reaction occurs in a blast furnace
Fe2O3 +3Co--------2Fe+3Co2
Calculate the mass of carbon monoxide needed to reduce 16 tones of iron (111) oxide
1. Convert 16 tonnes of Fe2O3 to grams.
2. Convert g Fe2O3 to mols. mols = grams/molar mass
3. Using the coefficients in the balanced equationk convert mols Fe2o3 o mols CO.
4. Convert mols CO to grams. grams CO = mols CO x molar mass CO
11.1g
To calculate the mass of carbon monoxide needed to reduce 16 tonnes of iron (III) oxide (Fe2O3), we need to use the stoichiometry of the balanced equation. In the given reaction:
Fe2O3 + 3Co -> 2Fe + 3Co2
We can see that 3 moles of carbon monoxide (Co) are required to react with 1 mole of iron (III) oxide (Fe2O3). The molar mass of carbon monoxide (Co) is approximately 28.01 g/mol, and the molar mass of iron (III) oxide (Fe2O3) is approximately 159.69 g/mol.
Step 1: Convert the mass of iron (III) oxide (Fe2O3) to moles.
Given: 16 tonnes of Fe2O3
1 tonne = 1000 kg
1 kg = 1000 g
Number of moles of Fe2O3 = Mass of Fe2O3 / Molar mass of Fe2O3
Number of moles of Fe2O3 = (16 tonnes) * (1000 kg/tonne) * (1000 g/kg) / (159.69 g/mol)
Note: Ensure that all units cancel out properly to reach the unit of moles.
Step 2: Calculate the moles of carbon monoxide (Co) required.
Since the stoichiometry of the balanced equation tells us that 3 moles of Co are required to react with 1 mole of Fe2O3, we can set up a ratio:
Moles of Co = Moles of Fe2O3 x (3 moles of Co / 1 mole of Fe2O3)
Step 3: Convert moles of carbon monoxide (Co) to grams.
Molar mass of Co = 28.01 g/mol
Mass of Co = Moles of Co x Molar mass of Co
Performing the calculations will give you the mass of carbon monoxide (Co) needed to reduce 16 tonnes of iron (III) oxide (Fe2O3).