Question

A company has ordered 91.4 pounds of iron metal. How many grams of carbon monoxide would be needed to produce 91.4 pounds of iron metal, knowing that the reaction only has a 33.2% yield. The reaction that occurs here is:

Fe₂O₃ + CO ----> Fe + CO

Answer 1

To find the mass of CO required to react with Fe₂O₃, you need to use stoichiometry. Follow the steps outlined in the detailed answer to calculate the mass of CO required. The mass of CO required is 13.19 grams.

Step-by-step explanation:

To find the mass of CO required to react with Fe₂O₃ , we need to use stoichiometry, which is the relationship between the moles of different substances in a chemical reaction.

From the balanced equation Fe₂O₃ + 3CO → 2Fe + 3CO₂, we can see that one mole of Fe₂O₃ reacts with 3 moles of CO.

First, we convert the given mass of Fe₂O₃ to moles using its molar mass. Then, we use the stoichiometric ratio to find the number of moles of CO needed. Finally, we convert the moles of CO to grams using its molar mass.

Given: mass of Fe₂O₃ = 25.13 g

Molar mass of Fe₂O₃ = 159.70 g/mol

Molar mass of CO = 28.01 g/mol

1. Convert mass of Fe₂O₃to moles: moles of Fe₂O₃= mass/molar mass = 25.13 g/159.70 g/mol = 0.1572 mol
2. Use the stoichiometric ratio to find moles of CO: moles of CO = 3 * moles of Fe₂O₃= 3 * 0.1572 mol = 0.4716 mol
3. Convert moles of CO to grams: mass of CO = moles * molar mass = 0.4716 mol * 28.01 g/mol = 13.19 g
   

The mass of CO required to react with 25.13 g of Fe₂O₃ is 13.19 grams.