What is the mass of $H_{2} O_{2}$ present in $1$ litre of a $2 M$ solution? Calculate the volume of oxygen at STP liberated upon the complete decomposition of $100 c m^{3}$ of the above solution.

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Solution

$1$ litre of $1 M$ solution of $H_{2} O_{2}$ contains $34 g$ of $H_{2} O_{2} [(2 H y d r o g e n = 2) + (2 O x y g e n = 32) = 34]$

$1$ litre of $2$ M solution of $H_{2} O_{2}$ contains $34 \times 2 = 68 g$ of $H_{2} O_{2}$

$1000$ ml of $2 M$ solution contains $68 g$ of $H_{2} O_{2}$

$100$ ml of $2 M$ solution contains $6.8 g$ of $H_{2} O_{2}$

$68 g$ of $H_{2} O_{2}$ will produce $22.4$ litre of $O_{2}$ at STP

$6.8$ g of $H_{2} O_{2}$ will produce $= 2.24$ litre of $O_{2}$ to STP.

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