Let’s carefully examine each reaction option to find the one that correctly represents the formation of [tex]\( SO_2 \)[/tex] and the release of 296.8 kJ/mol of energy.
### Option A:
[tex]\[ S (s) + O_2 (g) \rightarrow SO_2 (g) + 296.8 \text{ kJ} \][/tex]
This reaction shows sulfur ([tex]\( S \)[/tex]) reacting with oxygen ([tex]\( O_2 \)[/tex]) to form sulfur dioxide ([tex]\( SO_2 \)[/tex]), and 296.8 kJ of energy is being released, indicating an exothermic reaction. This fits the condition given in the problem where the formation of [tex]\( SO_2 \)[/tex] releases 296.8 kJ/mol.
### Option B:
[tex]\[ S (s) + 2 O (g) + 296.8 \text{ kJ} \rightarrow SO_2 (g) \][/tex]
This reaction suggests that solid sulfur and two oxygen atoms react together, and 296.8 kJ is absorbed (as it is on the reactant side) to form sulfur dioxide. This does not match the given requirement, as it indicates energy absorption rather than release.
### Option C:
[tex]\[ S (s) + O_2 (g) + 296.8 \text{ kJ} \rightarrow SO_2 (g) \][/tex]
Here, sulfur reacts with molecular oxygen plus 296.8 kJ being absorbed (appearing on the reactant side) to form sulfur dioxide. This also does not fit the requirement because it implies energy is needed for the formation rather than being released.
### Option D:
[tex]\[ S (s) + O (g) \rightarrow SO_2 (g) + 296.8 \text{ kJ} \][/tex]
This reaction involves solid sulfur and a single oxygen atom forming sulfur dioxide while releasing 296.8 kJ of energy. Although it indicates exothermic release, the stoichiometry is incorrect as [tex]\( SO_2 \)[/tex] formation typically involves molecular oxygen [tex]\( O_2 \)[/tex], not a single oxygen atom.
Based on the analysis, the correct answer is:
Option A:
[tex]\[ S (s) + O_2 (g) \rightarrow SO_2 (g) + 296.8 \text{ kJ} \][/tex]
This option correctly represents the reaction where the formation of sulfur dioxide releases 296.8 kJ/mol.
