What willl be the mass of oxygen liberated by decomposition of 200 mL hydrogen peroxide solution with a strength of 34 g per litre?

25.5g

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3.0g

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3.2g

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4.2g

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Solution

The correct option is B 3.2g
Strength of the solution $= 34$ g/L.
1 L (or 1000 mL) of the solution contains 34 g of $H_{2} O_{2}$
200 mL of the solution contains $\frac{34}{1000} \times 200 = 6.8$ g of $H_{2} O_{2}$
$2 H_{2} O_{2} \to 2 H_{2} O + O_{2}$
2 moles of $H_{2} O_{2}$ gives 1 mole of $O_{2}$
68g of $H_{2} O_{2}$ gives $32$ g of $O_{2}$
6.8g of $H_{2} O_{2}$ gives $\frac{32}{68} \times 6.8 = 3.2$ g of $O_{2}$

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What willl be the mass of oxygen liberated by decomposition of 200 mL hydrogen peroxide solution with a strength of 34 g per litre?

The correct option is B 3.2gStrength of the solution =34 g/L.1 L (or 1000 mL) of the solution contains 34 g of H2O2200 mL of the solution contains 341000×200=6.8 g of H2O22H2O2→2H2O+O22 moles of H2O2 gives 1 mole of O268g of H2O2 gives 32 g of O26.8g of H2O2 gives 3268×6.8=3.2 g of O2