The chemical equation below represents sulfur trioxide (SO₃) in the atmosphere mixing with rainwater to form sulfuric acid (H₂SO₄) , which is a major component of acid rain:
SO₃(g) + H₂O(I) → H₂SO_4(I)
The molar mass of SO₃ is 80.1 g/mol and the molar mass of H₂SO₄ is 98.1 g/mol. How much H₂SO₄ is produced when 128.0 g of SO₃ mixes with rainwater?

Question

Quizplus · Accepted Answer

128.0 g of SO₃ is 1.6 moles (128.0 g / 80.1 g/mol). Since the reaction is a 1:1 molar ratio, 1.6 moles of H₂SO₄ are produced. 1.6 moles of H₂SO₄ is 157 g (1.6 moles * 98.1 g/mol).

The Chemical Equation Below Represents Sulfur Trioxide (SO3) in the Atmosphere

The Chemical Equation Below Represents Sulfur Trioxide (SO₃) in the Atmosphere