A sample of air containing SO₂ as an impurity measures 1 kiloliter at STP. It is passed through excess of aqueous solution of H₂O2. The resultant solution required 20 ml of 0.1 N NaOH solution for complete neutralization. If mass of SO2 present is x. Then value of 1000x/8 is ?
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CaCO
3
⇌
Δ
CaO+CO
2
Let pure sample of CaCO
3
=x grams
Mass of CaO produced after decomposition =22.4 g
Molar mass of CaCO
3
=100 g/mol
and, Molar mass of CaO=56 g
If 100% is pure, then
100 g CaCO
3
⟶56 g of CaO
Also,y g of CaCO
3
⟶22.4 g of CaO
Dividing these two,
y
100
=
22.4
56
y=40 grams
∴ Percentage of purity =
Totalmassofimpure
Massofpuresample
×100=
50
40
×100=80%
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