Given the three-step Contact process for manufacturing sulfuric acid,H₂SO₄: S(s)+ O₂(g)→ SO₂(g)
2 SO₂(g)+ O₂(g)→ 2 SO₃(g)
SO₃(g)+ H₂O(l)→ H₂SO₄(aq)
What mass of sulfuric acid is produced from the reaction of 25.0 g of sulfur?

Question

Quizplus · Accepted Answer

First, calculate the moles of sulfur used using its molar mass (32.06 g/mol). For 25.0 g of sulfur: moles = 25.0 g / 32.06 g/mol = 0.780 moles. The stoichiometry of the reaction shows that 1 mole of sulfur produces 1 mole of H₂SO₄. Therefore, 0.780 moles of sulfur will produce 0.780 moles of H₂SO₄. The molar mass of H₂SO₄ is approximately 98.08 g/mol, so the mass of H₂SO₄ produced is 0.780 moles * 98.08 g/mol = 76.5 g, which rounds to 76.4 g for the answer.

Given the Three-Step Contact Process for Manufacturing Sulfuric Acid,H₂SO₄: S(s)