Which of the following represents the chemical equation involved in the preparation of $H_{2} O_{2}$ from barium peroxide?

B a O_{2} .8 H_{2} O + H_{2} S O_{4} \to B a S O_{4} + H_{2} O_{2} + 8 H_{2} O

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C H_{3} C H O H C H_{3} \to C H_{3} C O O C H_{3} + H_{2} O_{2}

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B a O_{2} + C O_{2} + H_{2} O \to B a C O_{3} + H_{2} O_{2}

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B a_{3} (P O_{4})_{2} + 3 H_{2} S O_{4} \to 3 B a S O_{4} + 2 H_{3} P O_{4}

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Solution

The correct option is B $B a O_{2} .8 H_{2} O + H_{2} S O_{4} \to B a S O_{4} + H_{2} O_{2} + 8 H_{2} O$
Barium peroxide react with sulfuric acid to produce Hydrogen peroxide and Barium sulfate.

Isopropyl Alcohol oxidises to Acetone and water, and not hydrogen peroxide.

Barium peroxide react with $C O_{2}$ carbonic acid. It then racts with barium to form barium carbonate and hydrogen peroxide. Barium carbonate is insoluble and is easy to remove by filtration. This process is widely used to manufacture $H_{2} O_{2}$ .

Barium phosphate reacts with Sulphuric acid to form Barium sulfate and Phosphoric acid.

The correct option is C.

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Similar questions

B a O_{2} + H_{2} S O_{4} \to B a S O_{4} + H_{2} O_{2}

C O_{2}, H_{2} O

H_{2} O_{2}

H_{2} O_{2}

(I) H_{2} O_{2} + O_{3} \to H_{2} O + 2 O_{2}

(I I) H_{2} O_{2} + A g_{2} O \to 2 A g + H_{2} O + O_{2}

H_{2} O_{2} + O_{3} \to H_{2} O + 2 O_{2}

H_{2} O_{2} + A g_{2} O \to 2 A g + H_{2} O + O_{2}

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