Final answer:
Upon intense heating, sulfuric acid can decompose into water and sulfur trioxide, among other products. For low concentrations, the formation of sulfur trioxide is more likely, which is a concern for generating acid rain. Sulfuric acid is a strong oxidizing agent at higher concentrations and can release various sulfur-containing compounds.
Step-by-step explanation:
Reaction of H₂SO₄ to Heat
When sulfuric acid (H₂SO₄) is subjected to intense heating, it undergoes thermal decomposition and may release various products depending on the conditions such as concentration and the presence of reducing agents. For very low concentrations and intense heating, it is more likely that the sulfuric acid will decompose into water (H₂O) and sulfur trioxide (SO₃), which further reacts with water to form additional sulfuric acid. At higher concentrations and elevated temperatures, sulfuric acid can act as a strong oxidizing agent, potentially releasing sulfur dioxide (SO₂), hydrogen sulfite (HSO₃⁻), sulfite (SO₃²⁻), elemental sulfur (S), hydrogen sulfide (H₂S), or sulfide (S²⁻).
Since sulfur trioxide gas reacts vigorously with water to form sulfuric acid, which can further result in the formation of acid rain, it is a considerable fire and environmental hazard. The classic laboratory method for producing sulfur dioxide involves the action of a strong acid on sulfite or hydrogen sulfite salts, with the resultant sulfurous acid decomposing into sulfur dioxide and water. In larger-scale chemistry and industrial applications, sulfur dioxide may arise from the roasting of sulfide ores or the burning of sulfur.
It is important to note that during dilution of concentrated sulfuric acid, the protocol requires adding acid to water and not the reverse to prevent risk of splatter and burns due to the exothermic nature of the dissolution process.