The key reversible step in the industrial manufacture of sulfuric acid (the Contact Process) is represented by the following chemical equation:
2SO2(g)+O2(g)⇌2SO3(g) 2\text{SO}_2\text{(g)} + \text{O}_2\text{(g)} \rightleftharpoons 2\text{SO}_3\text{(g)} 2SO2(g)+O2(g)⇌2SO3(g)Identify the industrial source from which each reactant is obtained:
The graph shows the percentage yield of sulfur trioxide at equilibrium at different temperatures and pressures.
State the conditions of temperature and pressure from those shown on the graph that produce the largest percentage yield of sulfur trioxide.
Find the percentage yield of sulfur trioxide at equilibrium at a pressure of 300 atm300\text{ atm}300 atm and a temperature of 450 ∘C450\ ^\circ\text{C}450 ∘C.
Suggest why, in the actual industrial process, the percentage yield of sulfur trioxide per pass over the catalyst is lower than the equilibrium percentage yield at these conditions.
