What will be the volume (in litres) of oxygen liberated (at STP) when 17 grams of $H_{2}$ $O_{2}$ decomposed on heating?

5.6 L

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22.7L

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11.35L

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45.4L

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Solution

The correct option is A
5.6 L

2 x 34 g of $H_{2}$ $O_{2}$ gives 22400 ml of $O_{2}$

So, 17 g of $H_{2}$ $O_{2}$ = $\frac{22400}{68}$ X 17 ml $O_{2}$ =5600ml=5.6 L

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