Question

In the given equation, "2SO₃ → S + 3O₂", the correct representation with subscript and superscript is as follows: Is the reaction 2SO₃ → S + 3O₂ endothermic or exothermic?

Answer 1

Without specific bond energy or enthalpy change data, it's difficult to definitively classify the decomposition of sulfur trioxide (2SO₃ → S + 3O₂) as an endothermic or exothermic reaction. Generally, bond breaking suggests an endothermic reaction.

Step-by-step explanation:

The reaction you've described, 2SO₃ → S + 3O₂, is an example of a decomposition reaction, where a single complex substance (in this case, sulfur trioxide) breaks down into its component elements (sulfur and oxygen). To determine whether this reaction is endothermic (absorbing heat) or exothermic (releasing heat), we need to consider the energies involved in the breaking and forming of chemical bonds.

In general, breaking a chemical bond requires energy (an endothermic process), while forming a bond releases energy (an exothermic process). In this case, the bonds in the SO₃ molecules are being broken, which would require energy input and suggest an endothermic reaction. However, without more specific information like bond energies or enthalpy change data, we cannot definitively say whether the reaction is endothermic or exothermic.

Learn more about endothermic and exothermic reactions