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A metallic oxide reacts with water to form its hydroxide, hydrogen peroxide and also liberates
oxygen. The metallic oxide could be
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oxygen. The metallic oxide could be
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Verified Answer
The correct answer is:
\( \mathrm{O} \mathrm{K} \mathrm{O}_{2} \)
Potassium Superoxide react with water to produce potassium hydroxide, hydrogen peroxide and oxygen. This reaction
takes place at a temperature near \( 0^{\circ} \mathrm{C} \). Whereas, other metal oxide reacts with water but does not produce peroxide.
\( 2 \mathrm{KO}_{2}+2 \mathrm{H}_{2} \mathrm{O} \rightarrow 2 \mathrm{KOH}+\mathrm{H}_{2} \mathrm{O}_{2}+\mathrm{O}_{2} \)
Reaction of other metal
\( \mathrm{Na}_{2} \mathrm{O}_{2}+2 \mathrm{H}_{2} \mathrm{O} \rightarrow 4 \mathrm{NaOH}(a q)+\mathrm{O}_{2}(g) \) \( \mathrm{CaO}+\mathrm{H}_{2} \mathrm{O} \rightarrow \mathrm{Ca}(\mathrm{OH})_{2} \) \( \mathrm{Li}_{2} \mathrm{O}+\mathrm{H}_{2} \mathrm{O} \rightarrow 2 \mathrm{LiOH} \)
takes place at a temperature near \( 0^{\circ} \mathrm{C} \). Whereas, other metal oxide reacts with water but does not produce peroxide.
\( 2 \mathrm{KO}_{2}+2 \mathrm{H}_{2} \mathrm{O} \rightarrow 2 \mathrm{KOH}+\mathrm{H}_{2} \mathrm{O}_{2}+\mathrm{O}_{2} \)
Reaction of other metal
\( \mathrm{Na}_{2} \mathrm{O}_{2}+2 \mathrm{H}_{2} \mathrm{O} \rightarrow 4 \mathrm{NaOH}(a q)+\mathrm{O}_{2}(g) \) \( \mathrm{CaO}+\mathrm{H}_{2} \mathrm{O} \rightarrow \mathrm{Ca}(\mathrm{OH})_{2} \) \( \mathrm{Li}_{2} \mathrm{O}+\mathrm{H}_{2} \mathrm{O} \rightarrow 2 \mathrm{LiOH} \)
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