Elemental sulfur can be converted to sulfur dioxide by combustion in air.Sulfur dioxide will react with water to form sulfurous acid (see balanced equation below) .
SO₂(g) + H₂O(l) → H₂SO₃(l)
What mass of sulfur dioxide is needed to prepare 29.36 g of H₂SO₃(l) ?

Question

Quizplus · Accepted Answer

The balanced chemical equation for the reaction between sulfur dioxide (SO2) and water (H2O) to form sulfurous acid (H2SO3) is:$$ \text{SO}_2(g) + \text{H}_2\text{O}(l) \rightarrow \text{H}_2\text{SO}_3(l) $$To find the mass of sulfur dioxide needed to prepare 29.36 g of H2SO3, we use the molar masses of SO2 and H2SO3. The molar mass of SO2 is approximately 64.07 g/mol, and the molar mass of H2SO3 is approximately 82.07 g/mol.Using stoichiometry:$$ \text{Mass of SO}_2 = \left( \frac{\text{Mass of H}_2\text{SO}_3}{\text{Molar mass of H}_2\text{SO}_3} \right) \times \text{Molar mass of SO}_2 $$$$ = \left( \frac{29.36 \, \text{g}}{82.07 \, \text{g/mol}} \right) \times 64.07 \, \text{g/mol} $$$$ \approx 22.91 \, \text{g} $$Therefore, 22.91 g of sulfur dioxide is needed to prepare 29.36 g of H2SO3.

Elemental Sulfur Can Be Converted to Sulfur Dioxide by Combustion