Question

Given an initial mass of 10.36 g SO₂, an excess of H₂O, and assuming that all of the reactant is converted to product(s), and none is lost, calculate the mass (g) of H₂SO₃ produced by the reaction?

Answer 1

To calculate the mass of H₂SO₃ produced, convert the initial mass of SO₂ to moles, use the ratio of coefficients from the balanced equation to determine the moles of H₂SO₃, and then convert the moles of H₂SO₃ to grams using the molar mass of H₂SO₃.

Step-by-step explanation:

To calculate the mass of H₂SO₃ produced, we need to determine the moles of SO₂ and then use the coefficients from the balanced chemical equation to convert to moles of H₂SO₃. From the equation given: 2H₂S (g) +30₂ (g) → 2SO₂ (g) + 2H₂O(g)

1. Convert the mass of SO₂ to moles using its molar mass: 10.36 g SO₂ / (64.06 g/mol SO₂) = 0.1614 mol SO₂
2. Use the ratio of coefficients from the balanced equation to determine the moles of H₂SO₃ produced: 0.1614 mol SO₂ × (1 mol H₂SO₃ / 2 mol SO₂) = 0.0807 mol H₂SO₃
3. Convert the moles of H₂SO₃ to grams using the molar mass of H₂SO₃: 0.0807 mol H₂SO₃ × (82.09 g/mol H₂SO₃) = 6.64 g H₂SO₃