Sulfur dioxide gas (SO2) reacts with excess oxygen gas (O2) and excess liquid water (H2O) to form liquid sulfuric acid (H2SO4). In the laboratory, a chemist carries out this reaction with 67.2 L of sulfur dioxide and gets 250 g of sulfuric acid.

• Write a balanced equation for the reaction.

• Calculate the theoretical yield of sulfuric acid.

• Calculate the percent yield of the reaction. (One mole of any gas occupies 22.4 L under certain conditions of temperature and pressure. Assume those conditions for this question.)

Question

Chemistry

Glenn Pham

27 October, 23:47

Sulfur dioxide gas (SO2) reacts with excess oxygen gas (O2) and excess liquid water (H2O) to form liquid sulfuric acid (H2SO4). In the laboratory, a chemist carries out this reaction with 67.2 L of sulfur dioxide and gets 250 g of sulfuric acid.

• Write a balanced equation for the reaction.

• Calculate the theoretical yield of sulfuric acid.

• Calculate the percent yield of the reaction. (One mole of any gas occupies 22.4 L under certain conditions of temperature and pressure. Assume those conditions for this question.)

+4

Answers (1)

Know the Answer?

Lamar Myers · Answer 1

A. 2SO₂ + O₂ + 2H₂O → 2H₂SO₄

B. Moles of SO₂ = 67.2 / 22.4Moles of SO₂ = 3 molesMoles of H₂SO₄ = 3 molesMass of H₂SO₄ = 3 x 98Mass of H₂SO₄ = 294 grams

Assuming sulfuric acid to have the same density as water, density = 1000 g / LVolume = mass / densityVolume = 294 / 1000Volume = 0.29 liters of sulfuric acid