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
State, in terms of the concentration of SO3(g), what occurs when more O2(g) is added to the reaction at equilibrium.
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