Question

Calculate how many moles of the product form when 0.048 mol of O₂ completely reacts. Assume that there is more than enough of the other reactant.

4Fe (s) + 3O₂ (g) ⟶ 2Fe₂O₃ (s)

a) 0.032 mol
b) 0.064 mol
c) 0.096 mol
d) 0.128 mol

Answer 1

0.048 mol of O₂ will react according to the balanced equation 4Fe + 3O₂ ⇒ 2Fe₂O₃ to produce 0.032 mol of Fe₂O₃.

Step-by-step explanation:

To calculate how many moles of the product form when 0.048 mol of O₂ completely reacts in the reaction 4Fe (s) + 3O₂ (g) ⇒ 2Fe₂O₃ (s), we need to use the stoichiometric mole ratio from the balanced chemical equation. The balanced equation tells us that 3 moles of O₂ react to form 2 moles of Fe₂O₃. Using this stoichiometric ratio, we set up the problem as follows:

(mol Fe₂O₃) = (mol O₂) × (2 mol Fe₂O₃ / 3 mol O₂)

Substituting the given moles of O₂:

(mol Fe₂O₃) = (0.048 mol O₂) × (2 mol Fe₂O₃ / 3 mol O₂) = 0.032 mol Fe₂O₃

Therefore, 0.048 mol of O₂ will completely react to form 0.032 mol of Fe₂O₃.