Question

How many grams of CO would be required to generate 635 g CO2?

Fe2O3 + 3CO → 2Fe + 3CO2 CO: 28.01 g/mol CO2: 44.01 g/mol
[?] g CO₂

Answer 1

To generate 635 g of CO₂, 13.22 grams of CO are required to react with 25.13 grams of Fe₂O3.

Step-by-step explanation:

To determine the mass of CO required to react with 25.13 g of Fe₂O3 according to the equation Fe2O3 + 3CO → 2Fe + 3CO₂, we need to use the molar ratio between CO and Fe₂O3. From the balanced equation, we can see that 3 moles of CO are required to react with 1 mole of Fe₂O3. Let's calculate the moles of Fe₂O3 first by dividing its mass by its molar mass:

1. Mass of Fe₂O3 = 25.13 g
2. Molar mass of Fe₂O3 = 159.69 g/mol
3. Moles of Fe₂O3 = Mass of Fe₂O3 / Molar mass of Fe₂O3
4. Moles of Fe₂O3 = 25.13 g / 159.69 g/mol
5. Moles of Fe₂O3 = 0.1574 mol

Now we can use the molar ratio to find the moles of CO required:

1. Moles of CO = Moles of Fe₂O3 × (3 moles of CO / 1 mole of Fe₂O3)
2. Moles of CO = 0.1574 mol × (3 mol CO / 1 mol Fe₂O3)
3. Moles of CO = 0.4722 mol CO

Finally, we can calculate the mass of CO by multiplying the moles of CO by its molar mass:

1. Mass of CO = Moles of CO × Molar mass of CO
2. Mass of CO = 0.4722 mol × 28.01 g/mol
3. Mass of CO = 13.22 g

So, 13.22 grams of CO are required to react with 25.13 grams of Fe₂O3.