The empirical formula of a gaseous compound is $C H_{2}$ . The density of the compound is 1.25 gm/lit.at S.T.P. The molecular formula of the compound is :

C_{2} H_{4}

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C_{3} H_{6}

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C_{6} H_{12}

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C_{4} H_{8}

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Solution

The correct option is C $C_{2} H_{4}$
Since, $1$ lite contains $1.25$ gms.
Hence $22.4$ litres contain $(1.25 \times 22.4) g m s \equiv 28 g m s .$
So molar mass $\equiv 28 g m s / m a s s = C_{2} H_{4} .$

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The empirical formula of a gaseous compound is CH2. The density of the compound is 1.25 gm/lit.at S.T.P. The molecular formula of the compound is :

The correct option is C C2H4Since, 1 lite contains 1.25 gms.Hence 22.4 litres contain(1.25×22.4)gms≡28gms.So molar mass ≡28gms/mass=C2H4.

The empirical formula of a gaseous compound is $C H_{2}$ . The density of the compound is 1.25 gm/lit.at S.T.P. The molecular formula of the compound is :

The correct option is C $C_{2} H_{4}$
Since, $1$ lite contains $1.25$ gms.
Hence $22.4$ litres contain $(1.25 \times 22.4) g m s \equiv 28 g m s .$
So molar mass $\equiv 28 g m s / m a s s = C_{2} H_{4} .$