🤓 Based on our data, we think this question is relevant for Professor Bindell's class at UCF.

We are asked to find the enthalpy of formation of SO_{2} under these conditions.

The oxidization of sulfur to SO_{3} is the formation reaction for SO_{3}. Therefore, the enthalpy of reaction is the enthalpy of formation for SO_{3}.

Balanced reaction:

2 SO_{2(g)} + O_{2(g)} → 2 SO_{3(g)}

$\overline{){\mathbf{\Delta H}}{{\mathbf{\xb0}}}_{{\mathbf{rxn}}}{\mathbf{=}}{\mathbf{\Delta H}}{{\mathbf{\xb0}}}_{\mathbf{f}\mathbf{,}\mathbf{}\mathbf{prod}}{\mathbf{-}}{\mathbf{\Delta H}}{{\mathbf{\xb0}}}_{\mathbf{f}\mathbf{,}\mathbf{}\mathbf{react}}}$

Note that we need to *multiply each ΔH˚ _{f} by the stoichiometric coefficient* since ΔH˚

Also, note that ΔH˚_{f} for elements in their standard state is 0.

Under certain nonstandard conditions, oxidation by O_{2}(g) of 1 mol of SO_{2}(g) to SO_{3}(g) absorbs 89.6 kJ. The heat of formation of SO_{3}(g) is –204.1 kJ/mol under these conditions. Find the heat of formation of SO_{2}(g).