On being placed in water, sodium peroxide not only produces an alkaline solution but also some bubbles. If we assume that the peroxide ion picks up two protons from water to produce a compound that can be seen as the dibasic conjugate acid of peroxide ion and then this compound undergoes a redox disproportion. Using the above information complete the following equation. ${Na}_{2} O_{2} (s) + H_{2} O (l) ⟶ (A) + (B)$ . (A) and (B) are respectively

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H₂O₂ and NaOH

H₂O and O₂

NaOH and O₂

Na₂O and NaOH

answer is C.

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Detailed Solution

From the given information, we can see that the reaction proceeds via formation of H₂O₂ (which is dibasic conjugate acid of peroxide ion), H₂O₂ then disproportionates into water and oxygen.

$\begin{array}{l} {Na}_{2} O_{2} (s) + H_{2} O (l) ⟶ 2 NaOH (aq) + H_{2} O_{2} (aq) \\ H_{2} O_{2} (aq) ⟶ H_{2} O (l) + \frac{1}{2} O_{2} (g) \end{array}$