Final answer:
To determine the heat produced when sulfur dioxide reacts with oxygen to form sulfur trioxide, we need to calculate the moles of sulfur dioxide, use the enthalpy change of the reaction, and identify the limiting reactant. Without the specific enthalpy change provided, we employ the known enthalpy release of 198 kJ per 2 moles of SO2 reacted.
Step-by-step explanation:
The reaction in question is an exothermic reaction where sulfur dioxide (SO2) reacts with oxygen (O2) to form sulfur trioxide (SO3). To determine the heat produced during this reaction, we will need to know the specific enthalpy change for the reaction, which is not provided in the question. However, based on the information provided in this scenario, we can calculate the amount of SO2 that reacts by dividing the mass of sulfur dioxide by its molar mass (64.066 g/mol).
Since the reaction is 2 SO2 + O2 ⇒ 2 SO3 and 198 kJ is released for every 2 moles of SO2, we can find the heat released by calculating how many moles of SO2 we have from the given 200 grams and then using proportional calculations based on the exothermic heat release of 198 kJ for 2 moles of SO2. It is important to check whether SO2 or O2 is the limiting reactant, although this information is not given in the question.