Sulfur trioxide is produced industrially via the equilibrium reaction
2 SO2(g) + O2(g) ⇌ 2 SO3(g)
A rigid 5.00 L reaction vessel at 800 K is loaded with 1.00 mol SO2(g) and 0.500 mol O2(g); no SO3 is present initially. When equilibrium is established at the same temperature, the amount of O2 present is found to be 0.200 mol.
(a) Calculate the equilibrium molar concentration of each species in the vessel.
(b) Determine the value of Kc for the reaction at 800 K.
(c) Calculate Kp for the reaction at 800 K.
(d) Industrial reactors often operate under pressures greater than 1 atm. Using Le Châtelier’s principle and the numerical value of Kp obtained in part (c), discuss how increasing the total pressure would be expected to influence the equilibrium yield of SO3 at 800 K.