🤓 Based on our data, we think this question is relevant for Professor Marohn's class at CORNELL.
Sulfur dioxide, SO2(g), can react with oxygen to produce sulfur trioxide, SO3(g), by the following reaction
2SO2(g) + O2(g) → 2SO3(g)
The standard enthalpies of formation for SO2(g) and SO3(g) are
ΔH°f [SO2(g)] = -296.8 kJ/mol
ΔH°f [SO3(g)] = -395.7 kJ/mol
Calculate the amount of energy in the form of heat (kJ) that is produced when a volume of 3.24 L of SO2(g) is converted to 3.24 L of SO3(g) according to this process at a constant pressure and temperature of 1.00 atm and 25.0°C. Assume ideal gas behavior.