Sulfur trioxide decomposes at high temperatures according to the following reversible reaction:
2SO3(g)⇌2SO2(g)+O2(g)ΔH=+197 kJ mol−1 2\text{SO}_3\text{(g)} \rightleftharpoons 2\text{SO}_2\text{(g)} + \text{O}_2\text{(g)} \quad \Delta H = +197\text{ kJ mol}^{-1} 2SO3(g)⇌2SO2(g)+O2(g)ΔH=+197 kJ mol−1A 4.20 mol4.20\text{ mol}4.20 mol sample of SO3\text{SO}_3SO3 is placed in a closed container of volume 16.0 dm316.0\text{ dm}^316.0 dm3 and heated. When equilibrium is reached, the mixture contains 1.20 mol1.20\text{ mol}1.20 mol of SO3\text{SO}_3SO3.
Calculate the amount, in moles, of SO2\text{SO}_2SO2 and of O2\text{O}_2O2 in the equilibrium mixture.
Give an expression for KcK_cKc for this equilibrium.
Calculate the value of KcK_cKc. Give its units.
State and explain the effect of using a higher temperature on the equilibrium yield of sulfur dioxide.
Sulfur dioxide is a major air pollutant. State the environmental problem caused by sulfur dioxide in the atmosphere, and write a balanced equation to show how calcium oxide is used to remove it from power station flue gases.
