Several steps are involved in the industrial production of

Last updated: 7/29/2022

Several steps are involved in the industrial production of sulfuric acid. One step involves the oxidation of sulfur dioxide gas to form sulfur trioxide gas. A catalyst is used to increase the rate of production of sulfur trioxide gas. In a rigid cylinder with a movable piston, this reaction reaches equilibrium, as represented by the equation below. 2SO₂(g) + O₂(g) →2SO3(g) + 392 kJ A. Explain in terms of collision theory, why increasing the pressure of the gases in the cylinder increases the rate of the forward reaction. B. State, in terms of the concentration of SO3(g), what occurs when the following changes are made to the equilibrium mixtures. i. More O₂(g) is added. ii. SO3(g) is removed. C. If 40 grams of sulfur trioxide gas, SO3(g) was passed through 250 mL of water, determine the olarity of sulfuric acid formed.