British bituminous coal has a high sulfur content and produces much smoke when burned. In 1952, the burning of this coal in London led to elevated levels of smog containing high concentrations of sulfur dioxide, a lung irritant, and more than 4000 people died. Sulfur dioxide emissions can be converted to SO3and ultimately to H2SO4, which is the cause of acid rain. The initial reaction is 2SO2(g) + O2(g) ⇌ 2SO3(g), for which Kp = 44. Given this Kp, are products or reactants favored in this reaction? What is the partial pressure of each species under equilibrium conditions if the initial pressure of each reactant is 0.50 atm? Would an increase in pressure favor the formation of products or reactants? Why?

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