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. The reaction to produce sulfur trioxide reaches an equilibrium. 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. – 9023

One thought on “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. The reaction to produce sulfur trioxide reaches an equilibrium. 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. – 9023”

1. In set A, the equilibrium is reached faster because the temperature is higher. When the temperature is higher, the particles have more energy and move faster, so there are more frequent and successful collisions between the reacting particles. This increases the rate of reaction.

   In set B, the temperature is lower, so the particles have less energy, move slower, and collide less often, so it takes longer to reach equilibrium.

   Also, if the forward reaction is exothermic, then a lower temperature increases the yield because it favours the forward reaction. However, this happens more slowly, because the particles are less energetic. So although set B might give a higher yield, it will take longer.

   Set B also has a higher pressure, and higher pressure causes the molecules to be closer together, meaning more frequent collisions. This increases the rate at which equilibrium is reached.

   If the product side has fewer gas molecules than the reactant side, then increasing pressure favours the forward reaction, giving a higher yield in set B.

   A catalyst is also used in set B. A catalyst speeds up both the forward and backward reactions, so equilibrium is reached faster, but it does not change the yield because it doesn’t affect the position of equilibrium. However, it helps reduce the need for high temperatures, making the process more efficient.

   Reply