Complete the exercises below. Indicate whether each of the following statements is true or false. 2SO₂ (g) + O₂ (g) → 2SO₃ (g) is an example of a disproportionation reaction.

Verified step by step guidance

1. Step 1: Understand the concept of a disproportionation reaction. A disproportionation reaction is a type of redox reaction in which a single substance is simultaneously oxidized and reduced, forming two different products.
2. Step 2: Analyze the given chemical equation: 2SO₂ (g) + O₂ (g) → 2SO₃ (g). Identify the reactants and products in the reaction.
3. Step 3: Determine the oxidation states of sulfur in the reactants and products. In SO₂, sulfur has an oxidation state of +4, and in SO₃, sulfur has an oxidation state of +6.
4. Step 4: Check if the same element is both oxidized and reduced. In this reaction, sulfur in SO₂ is only oxidized to form SO₃, and there is no reduction of sulfur occurring.
5. Step 5: Conclude whether the reaction is a disproportionation reaction. Since sulfur is only oxidized and not reduced, this reaction is not a disproportionation reaction.