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
Determine the amount of heat released by the production of 1.0 mole of SO3(g)