how many CO would be needed to reduce 19.1 grams of iron (III).
Fe2O3 + 3CO ==> 3CO2 + 2Fe
mols Fe2O3 = grams/molar mass = ?
Use the coefficients in the balanced equation to convert mols Fe2O3 to mols CO.
Now convert mols CO to grams. grams CO = mols CO x molar mass CO
To determine how many moles of CO (carbon monoxide) would be needed to reduce 19.1 grams of iron (III), you need to follow a few steps:
Step 1: Calculate the molar mass of iron (III) oxide (Fe2O3)
Start by finding the molar mass of iron (III) oxide. The molar mass of one iron (III) atom (Fe) is 55.845 g/mol, and since there are two atoms of iron in iron (III) oxide, the molar mass of iron (III) oxide is:
Molar mass of Fe2O3 = (2 × Molar mass of Fe) + Molar mass of O = (2 × 55.845 g/mol) + 16.00 g/mol = 159.69 g/mol
Step 2: Convert the given mass of iron (III) to moles
To determine the number of moles of iron (III), divide the given mass of iron (III) by its molar mass:
Moles of iron (III) = Mass of iron (III) / Molar mass of iron (III) = 19.1 g / 159.69 g/mol
Step 3: Write and balance the chemical equation for the reaction between iron (III) oxide and carbon monoxide
The balanced chemical equation for the reaction is:
Fe2O3 + 3CO → 2Fe + 3CO2
Step 4: Determine the stoichiometric ratio between iron (III) oxide and carbon monoxide
According to the balanced chemical equation, 3 moles of CO are required to react with 1 mole of Fe2O3.
Step 5: Calculate the moles of CO needed
To find the moles of CO needed to reduce 19.1 grams of iron (III), multiply the moles of iron (III) by the stoichiometric ratio:
Moles of CO = Moles of iron (III) × (3 moles of CO / 1 mole of Fe2O3)
By following these steps, you can find the number of moles of CO needed to reduce 19.1 grams of iron (III).