Question

Oxides of sulfur are important in atmospheric pollution, arising particularly from burning coal. Use the thermodynamic data at 25oC given in the appendix to answer the following questions. (a) In air, the oxidation of SO2 can occur: 1⁄2 O2(g) + SO2 (g) → SO3 (g). Calculate ∆Gorxn,298. (b) Find the equilibrium ratio of partial pressures of SO3 (g) to SO2(g) in air at 25oC. The partial pressure of O2(g) is 0.21 bar. (c) SO3(g) can react with H2O (g) to form sulfuric acid, H2SO4 (g). Air that is in equilibrium with liquid water at 25oC has a partial pressure of H2O (g) of 0.031 bar. Find the equilibrium ratio of partial pressures of H2SO4 (g) to SO3 (g) in air at 25oC.

Answer 1