[tex]\tt{\huge{\red{Solution:}}}[/tex]
Based on the balanced chemical equation, 2 moles of SO₂ is stoichiometrically equivalent to 2 moles of H₂SO₄. Note that the molar masses of SO₂ and H₂SO₄ are 64.07 g/mol and 98.09 g/mol, respectively.
[tex]\begin{aligned} \text{mass of} \: \text{SO}_2 & = 200. \: \cancel{\text{g} \: \text{H}_2\text{SO}_4} \times \frac{1 \: \cancel{\text{mol} \: \text{H}_2\text{SO}_4}}{98.09 \: \cancel{\text{g} \: \text{H}_2\text{SO}_4}} \times \frac{2 \: \cancel{\text{mol} \: \text{SO}_2}}{2 \: \cancel{\text{mol} \: \text{H}_2\text{SO}_4}} \times \frac{\text{64.07 g} \: \text{SO}_2}{1 \: \cancel{\text{mol} \: \text{SO}_2}} \\ & = \boxed{\text{131 g} \: \text{SO}_2} \end{aligned}[/tex]
Hence, the minimum mass of SO₂ needed is 131 g.
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