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

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$C_{2} H_{4}$

$C_{3} H_{6}$

$C_{6} H_{12}$

$C_{4} H_{8}$

answer is A.

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Detailed Solution

Molecular Formula from Empirical Formula and Density

Empirical formula: CH₂

Empirical formula mass: 14 g/mol (12 + 2 × 1)

Density at STP: 1.25 g/L

Molar volume at STP: 22.4 L/mol

Molecular mass = Density × Molar volume = 1.25 × 22.4 = 28 g/mol

Number of empirical units in molecular formula = 28 ÷ 14 = 2

Molecular formula X = (CH₂)₂ = C₂H₄

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