Final answer:
To calculate the amount of H₂SO₄ formed by the reaction of 6.0 L of SO₃ gas with sufficient water at STP, we need to determine the stoichiometry of the reaction.
Step-by-step explanation:
To calculate the amount of H₂SO₄ formed by the reaction of 6.0 L of SO₃ gas with sufficient water at STP, we need to determine the stoichiometry of the reaction. From the balanced equation:
2H₂S + SO₂ → 2H₂O + S (unbalanced)
It can be seen that 2 moles of H₂S produce 2 moles of H₂O. Therefore, the moles of H₂S produced can be calculated as follows:
6.0 L of SO₃ gas at STP is equal to 6.0 moles of SO₃ (using the ideal gas law).
Therefore, 6.0 moles of SO₃ will produce 6.0 moles of H₂O and 3.0 moles of S.