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.
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
2 answers
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
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
2 answers