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प्रश्न
Hydrogen sulphide gas burns in oxygen to yield 12.8 g of sulphur dioxide gas as under:
\[\ce{2H2S + 3O2 -> 2H2O + 2SO2}\]
Calculate the volume of hydrogen sulphide at STP. Also, calculate the volume of oxygen required at STP which will complete the combustion of hydrogen sulphide determined in litres.
उत्तर
\[\ce{2H2S + 3O2 -> 2H2O + 2SO2}\]
At S.T.P.
(i) 2 vol. of H2S = 2 × 22.4 = 44.8 litres
2SO2 = 2[32 + (2 × 16)] = 128 g
128 g of SO2 needs H2S = 44.8 litres
∴ 12.8 g of SO2 needs H2S = `(44.8 xx 12.8)/128`
= 4.48 litres
(ii) Also, 2 vols. of H2S require O2 = 3 volume
∴ 4.48 litres of H2S requires O2 = `3/2 xx 4.48`
= 6.72 litres
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