Question

The industrial production of sulfuric acid involves several steps. One of these steps is the reaction of sulfur dioxide, SO2, with oxygen to form sulfur trioxide, SO3. 250,(g) + O:(g) = 250,(g) he reaction to produce sulfur trioxide reaches an equilibrium. 250,(g) + 0,(g)- 250,(g) The forward reaction is exothermic. The rate of attainment of equilibrium and the equilibrium yield of sulfur trioxide are affected by pressure and temperature. A manufacturer considered two sets of conditions, A and B, for this reaction.In each case sulfur dioxide is mixed with excess oxygen.The manufacturer changed the temperature and the pressure and only used a catalyst in B.The sets of conditions A and B are shown in Figure 7. The manufacturer chooses set of conditions B rather than set of conditions A. Explain, by considering the effect of changing the conditions on the rate of attainment of equilibrium andon the equilibrium yield of sulfur trioxide, why the manufacturer chooses the set of conditions B ratherthan the set of conditions A.

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