Final answer:
The student's question involves calculating the theoretical yield of H₂SO₃ from the reactants SO₂ and H₂O using stoichiometry. The exact theoretical yield cannot be provided without further calculations but would typically be expressed to three significant figures after performing these calculations.
Step-by-step explanation:
The student is asking how to calculate the theoretical yield of H₂SO₃ when 5.520 g SO₂ is mixed with 14.69 g H₂O. This problem involves the reactants SO₂ and H₂O reacting to form sulfurous acid (H₂SO₃), and the student needs to find the amount of product formed from given masses of reactants.
To solve this, we would begin by identifying the balanced chemical equation for the reaction, which is:
SO₂(g) + H₂O(l) → H₂SO₃(aq). Next, we calculate the moles of each reactant using their molar masses. The reactant that produces the least amount of product is the limiting reactant. From there, we use the mole ratio from the balanced equation to find the moles of product formed, which we then convert back into grams.
However, as the full stoichiometric calculations are not included here, I cannot provide the precise theoretical yield. Typically, the theoretical yield would be expressed to three significant figures based on the calculation and the precision of the given data.