What is the maximum amount (in grams) of CO2 that can be obtained from 454g of Fe2O3?

This is a logical extension of your first problem. Work it first, then we can tackle this one.

Convert 454 g Fe2O3 to mols.

Convert mos Fe2O3 to mol CO2.
Convert mols CO2 to grams CO2.

To find the maximum amount of CO2 that can be obtained from 454g of Fe2O3 (iron(III) oxide), we first need to determine the stoichiometry of the reaction between Fe2O3 and CO2. The balanced equation for the reaction is:

Fe2O3 + 3CO2 → 2Fe + 3CO2

From the equation, we can see that for every 1 mole of Fe2O3, we will produce 3 moles of CO2. To calculate the moles of Fe2O3, we can use its molar mass.

The molar mass of Fe2O3 can be calculated as follows:

2(atomic mass of Fe) + 3(atomic mass of O)
= 2(55.845 g/mol) + 3(16.00 g/mol)
= 159.69 g/mol

Now, we can calculate the number of moles of Fe2O3:

moles of Fe2O3 = mass of Fe2O3 / molar mass of Fe2O3
= 454 g / 159.69 g/mol
≈ 2.84 mol

According to the stoichiometry, 1 mole of Fe2O3 produces 3 moles of CO2. Therefore, the number of moles of CO2 that can be obtained from 2.84 moles of Fe2O3 is:

moles of CO2 = moles of Fe2O3 × (3 moles CO2 / 1 mole Fe2O3)
≈ 2.84 mol × (3 mol CO2 / 1 mol Fe2O3)
≈ 8.52 mol

Finally, to calculate the mass of CO2:

mass of CO2 = moles of CO2 × molar mass of CO2
= 8.52 mol × 44.01 g/mol
≈ 374.57 g

Therefore, the maximum amount of CO2 that can be obtained from 454g of Fe2O3 is approximately 374.57 grams.