Final answer:
12.6 moles of oxygen were required to produce 8.40 moles of sulfur dioxide based on the stoichiometry of the chemical equation 2H₂S (g) + 3O₂ (g) → 2SO₂ (g) + 2H₂O(g).
Step-by-step explanation:
To determine how many moles of oxygen were required to produce 8.40 moles of sulfur dioxide, we must use the chemical reaction provided and apply stoichiometry principles:
2H₂S (g) + 3O₂ (g) → 2SO₂ (g) + 2H₂O(g)
According to the reaction, it takes 3 moles of oxygen (O₂) to produce 2 moles of sulfur dioxide (SO₂). To find out the amount of oxygen needed for 8.40 moles of SO₂, we set up a proportion based on the coefficients in the balanced equation:
(3 moles O₂ / 2 moles SO₂) = x moles O₂ / 8.40 moles SO₂
Solving for x, we find that:
x = (3/2) * 8.40 moles SO₂
x = 12.6 moles O₂
Therefore, 12.6 moles of oxygen were required to produce 8.40 moles of sulfur dioxide.