Question

When 2.00 mol of SO₂Cl₂ is placed in a 2.00-L flask at 303 K, 56% of the SO₂Cl₂ decomposes to SO₂ and Cl₂:

SO₂Cl₂(g) SO₂(g) + Cl₂(g)

(a) Calculate K_c for this reaction at this temperature. (b) Calculate K_p for this reaction at 303 K. (c) According to Le Châtelier’s principle, would the percent of SO₂Cl₂ that decomposes increase, decrease or stay the same if the mixture were transferred to a 15.00-L vessel? (d) Use the equilibrium constant you calculated above to determine the percentage of SO₂Cl₂ that decomposes when 2.00 mol of SO₂Cl₂ is placed in a 15.00-L vessel at 303 K.