Sulfuryl chloride, SO₂Cl₂, is used as a reagent in the synthesis of organic compounds. When heated to a sufficiently high temperature, it decomposes to SO₂ and Cl₂.

(a) A 10.0-L flask containing 6.70 g of SO₂Cl₂ is heated to 375°C. What is the concentration of each of the compounds in the system when equilibrium is achieved? What fraction of SO₂Cl₂ has dissociated?
(b) What are the concentrations of SO₂Cl₂, SO₂,and Cl₂ at equilibrium in the 10.0-L flask at 375°C if you begin with a mixture of SO₂Cl₂(6.70 g) and Cl₂ (0.10 atm)? What fraction of SO₂Cl₂ has dissociated?
(c) Compare the fractions of SO₂Cl₂ in parts (a)and (b). Do they agree with your expectations based on Le Chatelier’s principle?

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SO₂Cl₂(g) → SO₂(g) + Cl₂(g) K = 0.045 at 375 °C