A quantity of $1.4 g$ of a hydrocarbon gives $1.8 g$ water on complete combustion. The empirical formula of hydrocarbon is :

C H

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C H_{2}

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C H_{3}

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C H_{4}

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Solution

The correct option is B $C H_{2}$
$%$ of Hydrogen $= \frac{2}{18} \times \frac{m a s s o f H_{2} O}{m a s s o f o r g a n i c c o m p o u n d} \times 100$

$= \frac{2}{18} \times \frac{1.8}{1.4} \times 100$

$= 14.28 %$

$%$ of carbon $= 100 - 14.28$
$= 85.71 %$

$∴$ moles of $H = \frac{14.28}{1} = 14.28$
moles of $C = \frac{85.71}{12} = 7.14$

$C : H$
$\frac{7.14}{7.14} : \frac{14.28}{7.14} = 1 : 2$

empirical formula $= C H_{2}$
option $" B "$ correct

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