Disproportionation Reactions

Chemistry ⇒ Redox Reactions and Electrochemistry

Disproportionation Reactions starts at 11 and continues till grade 12. QuestionsToday has an evolving set of questions to continuously challenge students so that their knowledge grows in Disproportionation Reactions. How you perform is determined by your score and the time you take. When you play a quiz, your answers are evaluated in concept instead of actual words and definitions used.

See sample questions for grade 11

Describe the changes in oxidation state for the element sulfur in the disproportionation of thiosulfate ion (S₂O₃^2-) to sulfate (SO₄^2-) and sulfite (SO₃^2-).

Describe the role of oxidation states in identifying disproportionation reactions.

Explain why chlorine gas reacts with cold, dilute NaOH to give both NaCl and NaClO in a disproportionation reaction.

Explain why fluorine does not undergo disproportionation reactions.

Explain why potassium permanganate (KMnO₄) does not undergo disproportionation in acidic medium.

Explain why the oxidation state of the element in the reactant must be intermediate between those in the products in a disproportionation reaction.

Explain why the reaction 2Fe³⁺ + 2I^- → 2Fe²⁺ + I₂ is not a disproportionation reaction.

In the disproportionation of NO₂ in alkaline medium, what are the oxidation states of nitrogen in the reactant and products?

In the reaction: 2HNO₂ → HNO₃ + NO + H₂O, what are the oxidation states of nitrogen in the reactant and products?

In the reaction: 2MnO₄^2- + 2H₂O → MnO₄^- + MnO₂ + 4OH^-, what are the oxidation states of manganese in the reactant and products?

In the reaction: 3Cl₂ + 6NaOH → 5NaCl + NaClO₃ + 3H₂O, which species is oxidized and which is reduced?

Write the balanced chemical equation for the disproportionation of chlorine in cold, dilute NaOH.

Write the balanced equation for the disproportionation of hypochlorous acid (HClO) in basic solution.

Write the half-reactions for the disproportionation of chlorine in water.

Write the half-reactions for the disproportionation of hydrogen peroxide.