Calculate the weight of sulphur present in $1.5$ moles of hydrogen sulphide.

48 g

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50 g

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60 g

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70 g

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Solution

The correct option is A $48 g$
given that
$1.5$ moles of $H_{2} S O_{4}$
atomic weight of sulphur $= 32 g / m o l$
Moles of sulphur $= 1 \times 1.5$
$= 1.5 m o l e s$
sulphide gram weight $=$ moles $\times$ atomic weight
$= 1.5 \times 32$
$= 48 g$

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Hydrogen sulphide gas burns in oxygen to yield 12.8 g of sulphur dioxide gas as under:
$2 H_{2} S + 3 O_{2} \to 2 H_{2} O + 2 S O_{2}$
(i). calculate the volume of hydrogen suulphide at STP.
Also, (ii). calculate the volume of oxygen required at STP. Which will complete the combustion of hydrogen sulphide determined in litres.