Which of the following reactions correctly depicts the formation of Sulfur Trioxide (SO3)?

The formation of Sulfur Trioxide (SO3) involves the chemical reaction between sulfur and oxygen. In this case, the correct reaction is represented by the equation 2S + 3O2 > 2SO3.

This reaction indicates that two moles of sulfur react with three moles of oxygen to produce two moles of sulfur trioxide. This is important because the stoichiometry shows the exact ratio of sulfur to oxygen needed for the reaction to proceed efficiently.

Sulfur typically exists in its elemental form (S) and needs sufficient oxygen to react fully to form SO3. The coefficients in the balanced reaction reflect the conservation of mass, which stipulates that the number of atoms of each element must be equal on both sides of the equation.

When examining the other choices, some do not maintain that balance or imply incorrect stoichiometric relationships. For example, the first option suggests that only two moles of sulfur and one mole of oxygen are sufficient to produce SO3, which is not accurate since more oxygen is required for complete combustion. The third option also portrays an insufficient amount of oxygen for full SO3 production. The fourth option incorrectly suggests an incorrect amount of sulfur in relation to oxygen needed to produce SO3.