For the following stoichiometry problem, select ALL of the mole definitions you would need to solve the problem.

Problem: If 2.5 x 1024 atoms of iron are produced, how many liters of carbon monoxide can be produced? The reaction is:

Fe2O3 + 3C --> 2 Fe + 3CO

1 mol contains 6.022E23 atoms of Fe.

mols Fe = 2.5E24/6.022E23 = 4.15
mols CO produced = 4.15 mols Fe x (3 mols CO/2 mols Fe) = 6.22
1 mol gas at STP occupies 22.4 L so
6.22 mol CO x 22.4 L/mol = ?
You can figure out how many definitions I used.

Converting given data to moles typically uses ...

grams to moles => moles = mass(g) given/formula wt(g/mole)
particles to moles => moles = particle numbers given/Avogadro's Number
volume at STP (Liters) to moles => moles = Volume(L) given/22.4l/mole
solutions data (Molarity(M) & Volume(L) given) => moles = Molarity(M) x Volume(L)
energy values to moles => moles = energy value given/molar heat of rxn

To solve this stoichiometry problem, you need to use the following mole definitions:

1. The mole ratio between the reactant and product: This ratio is given by the balanced chemical equation and tells you the number of moles of each substance that react or are produced. In this case, you would need to use the mole ratio between Fe2O3 and CO.

2. The molar mass of the given substance: To convert the given amount (in atoms) to moles, you need to know the molar mass of the substance. In this case, you would need the molar mass of iron.

3. The molar volume at STP: To convert moles to volume, you need to use the molar volume, which is the volume occupied by one mole of a gas at standard temperature and pressure (STP). The molar volume at STP is 22.4 liters/mol.

So, in summary, to solve this stoichiometry problem, you need to use the mole ratios from the balanced chemical equation, the molar mass of iron, and the molar volume at STP.