Sulfur dioxide, SO2(g), can react with oxygen to produce sulfur trioxide, SO2(g), by the reaction 2SO2(g) + O2(g)2 → SO3(g)

The standard enthalpies of formation for SO2(g) and SO3(g) are

ΔHf= [SO2(g)] = -296.8 kJ/mol
ΔHf= [SO2(g)] = -395.7 kJ/mol

Calculate the amount of energy in the form of heat that is produced when a volume of 1.64 L of SO2(g) is converted to 1.64 L of SO3(g) according to this process at a constant pressure and temperature of 1.00 bar and 25.0 °C . Assume ideal gas behavior.