Sulfur dioxide, SO 2 ( g ) , SO2(g), can react with oxygen to produce sulfur trioxide, SO 3 ( g ) , SO3(g), by the reaction 2 SO 2 ( g ) + O 2 ( g ) ⟶ 2 SO 3 ( g ) 2SO2(g)+O2(g)⟶2SO3(g) The standard enthalpies of formation for SO 2 ( g ) SO2(g) and SO 3 ( g ) SO3(g) are Δ H ∘ f [ SO 2 ( g ) ] = − 296.8 kJ / mol ΔHf°[SO2(g)]=−296.8 kJ/mol Δ H ∘ f [ SO 3 ( g ) ] = − 395.7 kJ / mol ΔHf°[SO3(g)]=−395.7 kJ/mol Calculate the amount of energy in the form of heat that is produced when a volume of 1.97 L 1.97 L of SO 2 ( g ) SO2(g) is converted to 1.97 L 1.97 L of SO 3 ( g ) SO3(g) according to this process at a constant pressure and temperature of 1.00 bar 1.00 bar and 25.0 °C 25.0 °C . Assume ideal gas behavior.